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DANYLO HALYTSKY LVIV NATIONAL MEDICAL UNIVERSITY
DEPARTMENT of GENERAL, BIOINORGANIC, PHYSICAL and
COLLOIDAL CHEMISTRY
V.V. Ogurtsov, O.M. Roman, O.V. Klenina
MULTIPLY CHOICE QUESTIONS
ON INORGANIC CHEMISTRY
(Module 2. Inorganic Chemistry)
For the 1st year students
оf pharmaceutical faculty
L’VIV – 2012
Chapter 1. General characteristic of s-elements. Hydrogen
and its compounds
1.1. Solutions of alkalis react with the
following simple matters:
А. Zn, Cu, Mn
B. C O2, P
C. Cl2, S N2
D. Cl2, P, Zn
E. Si, Al, Cu
1.2. Hydrogen peroxide can take part
in all listed reactions, the
exception is only:
А. to be as a oxidizing agent
B. production of hydrogen
C. production of oxygen
D. E. to be as a reducing agent
1.3. Presence of what salts predefines
temporal hardness in water?
А. CaCO3 and MgCO3
B. Mg(HCO3)2 and Ca(HCO3)2
C. KHCO3 and NaHCO3
D. Na2SO4 and CaSO4
E. KHCO3 and Ca(HCO3)2
1.4. Which of the listed salts can
predefine permanent hardness of
water?
А. Mg(HCO3)2
B. Na2SO4
C. NaCl
D. Ca(HCO3)2
E. K2SO4
1.5. Which one of the given elements
forms peroxide at the reaction
with oxygen?
А. potassium
B. sodium and potassium
C. all alkaline metals
D. sodium
E. lithium
1.6. From elements of the IIA group
amphoteric property has:
А. calcium
B. beryllium
C. magnesium
D. all elements of IIA group
E. beryllium and magnesium
1.7. As a result of hydrolysis of
magnesium silicide such products
of reaction forms:
А. complex compound
B. silane and magnesium
hydroxide
C. silicium oxide, magnesium
oxide and hydrogen
D. silicon, magnesium oxide and
hydrogen
E. silane and magnesium oxide
1.8. Between the molecules of water
there are the following types of
connections:
А. ionic
B. covalent
C. hydrogenic
D. metallic
E. covalent and ionic
1.9. Sodium hydrogen carbonate is
used as:
А. cholagogue
B. laxative
C. diuretic
D. sedative
E. antacidic
1.10. Sodium iodide is used in medicine
as:
А. diuretic
B. antacidic
C. source to the microelement of
iodine
D. sedative
E. 1.11. Which one of the given
carbonates is stable at the heating?
А. magnesium carbonate
B. copper carbonate
C. silver carbonate
D. calcium carbonate
E. sodium carbonate
1.12. Which of the listed salts can
predefine permanent hardness of
water?
А. MgCl2
B. Mg(HCO3)2
C. KCl
D. Na3PO4
E. Ca(HCO3)2
1.13. Which of the given compounds
can be used for softening of
water?
А. CaCO3, Ca(OH)2
B. MgSO4, H2SO4
C. Na3PO4, CaCl2
D. Na2CO3, NaCl
E. Na2CO3, NAOH
1.14. Natural water always contains
dissolved salts. Which of the
listed salts can predefine temporal
hardness of water?
А. Mg(HCO3)2
B. CaÑl2
C. NaCl
D. MgCl2
E. Ca3(PO4)2
1.15. Which from the given reactions is
used for laboratory preparation of
hydrogen?
А. Fe + H2O → Fe3O4 + H2
B. CH4 + 2H2O → CO2 + 4H2
C. Zn + 2HCl → ZnCl2 + H2
D. CH4 → C + 2H2
E. C + H2O → CO + H2
1.16. The ions of what chemical
element influence on electrolyte
balance of brain and what salt of
this element is used for treatment
of psychical diseases:
А. Mg, MgSO4
B. I, KI
C. Cl, NaCl
D. Li, Li2CO3
E. Ca, CaCl2
1.17. Salts of this alkaline metal are
used in psychiatry. Burning on air
or in the atmosphere of oxygen it
forms the oxide E2O. What metal
is the question about?
А. Na
B. Rb
C. Li
D. Cs
E. K
1.18. What is the type of connection in
the molecule of NaCl?
А. covalently arctic
B. Ionic
C. metallic
D. covalently unpolar
E. hydrogenic
1.19. The reaction is between sodium
and water:
А. exothermic, connection
B. endotermic
C. exothermic, substitution
D. exothermic, exchange
E. endothermic, substitution
1.20. Sodium hydrogen carbonate reacts
with hydrochloric acid with
forming a gas of:
А.
B.
C.
D.
E.
CH4
CO2
H2
Cl2
CO
1.21. Which one from the given
formulas corresponds to sodium
thiosulphate?
А. Na2S2O4
B. NaHSO4
C. Na2S2O5
D. Na2S2O3
E. Na2SO3
1.22. At heating oxygen reacts only as
exception with:
А. Cl2
B. Ne
C. N2
D. Au
E. Cu
1.23. Temporal hardness of water is
predefined by a presence in water
of next salts of calcium and
magnesium
А. chlorides
B. sulfides
C. sulfates
D. nitrates
E. hydrogen carbonates
1.24. Which of the listed chemical
reactions can be used for the
preparation of hydrogen?
А. Zn + HNO3
B. Zn + NAOH
C. Fe + KOH
D. Mg + HNO3
E. Cu + H2SO4
1.25. Whish one of the given methods
can be used foe preparation of
metallic sodium?
А. -
B. hydrometallurgy
C. electrolysis of fusions of salts
D. aluminothermy
E. electrolysis of solutions of
salts
1.26. Chouse the formula which is
named lime:
А. Ca(OH)2
B. CaO2
C. CaCO3
D. CaCl2
E. CaO
1.27. Which one from the simple
matters reacts with water at the
room temperature?
А. Copper
B. Nitrogen
C. Chlorine
D. Silicon
E. Gold
1.28. Which element reacts with oxygen
to produce peroxide?
А. Al
B. Na
C. Cu
D. Fe
E. K
1.29. NaNO2 shows reducing properties
in relation with:
А. NH3
B. KMnO4
C. H2S
D. NaHCO3
E. KI
1.30. What element most widely
distributed on the earth?
А. Silicon
B. Oxygen
C. Nitrogen
D. Carbon
E. Hydrogen
1.31. Which of the given elements
corresponds to s–elements?
А. P, S, Cr
B. Be, Mg, Al
C. S, P, Cl
D. Mn, Br, Mo
E. K, Ca, Sc
1.32. Which compounds react to give as
a product only Fe(OH)3?
А. FeO and H2O
B. Fe(OH)2 and H2O2
C. Fe and H2O
D. Fe2O3 and H2O
E. Fe and O2
1.33. Which one of the given reactants
is used for identification of Ca2+
cation?
А. (NH4)2C2O4
B. HNO3
C. KCl
D. HCl
E. NaBr
1.34. Which one from the resulted
reactions is used in submarine
boats for the regeneration of air?
А. 2Na2O2 + 2CO2 = 2Na2CO3 +
O2
B. 2KClO3 = 2KCl + 3O2
C. 2NaNO3 = 2NaNO2 + O2
D. 2H2O2 = 2H2O + O2
E. 2KMnO4 = K2MnO4 + MnO2
+ O2
1.35. Hydrogen in the periodic system
of elements disposes in:
А. VIIB and IA groups
B. IIA group
C. IB group
D. IA and VIIA groups
E. VIIA group
1.36. Hydrogen in compounds shows
the following oxidation numbers:
А. 0, +1, +2
B. +1
C. -1, 0, +1
D. 0, -1
E. +1, +2
1.37. Which one of the listed reaction is
possible at the room temperature?
А. Au + HCl →
B. Na + H2O →
C. Cr2O3 + H2 →
D. Cu + H2O →
E. Fe + H2SO4 (conc.) →
1.38. Which one from the given salts
does not hydrolyze:
А. KNO2
B. CrCl3
C. Al2(SO4)3
D. ZnSO4
E. KI
1.39. In solution [OH–] = 1•10–6 mol/L.
What is the pH of solution?.
А. 8
B. 1
C. 4
D. 7
E. 6
Chapter 2. s-Elements of the І group of the Periodic Table.
Alkali metals
2.1. What is the electronic
configuration of Lithium atom?
А. 1s22s1
B. 1s22s22p63s23p64s1
C. 1s22s22p63s1
D. 1s12s1
E. 1s22s2
2.2. Electronic formula of Sodium
atom.
А. 1s22s1
B. 1s22s22p63s1
C. 1s22s22p63s23p64s1
D. 1s22s22p63s23p64s2
E. 1s22s22p63s2
2.3. Electronic formula of Potassium
atom.
А. 4s1
B. 1s22s22p63s23p64s23d105s1
C. 1s22s22p62d103s1
D. 1s22s22p63s1
E. 1s22s22p63s23p64s1
2.4. Electronic formula of Rubidium
atom.
А. 1s22s22p63s1
B. 1s22s22p62d103s1
C. 1s22s1
D. 5s1
E. 1s22s22p63s23p64s23d104p65s1
2.5. Electronic configuration of
external level of Cesium atom :
А. 6s1
B. 6s2
C. 1s22s1
D. 6s1
E. 1s22s22p63s23p64s23d105s1
2.6. Electronic formula of Lithium
cation:
А. 1s12s1
B. 1s22s22p63s1
C. 1s22s2
D. 1s2
E. 1s1
2.7. Electronic formula of Sodium
cation:
А. 4s1
B. 1s22s22p5
C. 1s22s22p63s1
D. 1s22s1
E. 1s22s22p6
2.8. Electronic formula of Potassium
cation:
А. 3s23p64s1
B. 5s1
C. 1s22s22p63s23p64s1
D. 1s22s22p63s23p6
E. 3s23p6
2.9. Electronic formula of Rubidium
cation:
А. 1s22s22p63s23p64s23d10
B. 4s23d104p6
C. 5s1
D. 1s22s22p63s23p64s23d105s1
E. 1s22s22p63s23p64s23d104p6
2.10. By a Lithium to Cesium atomic
radii of elements:
А. decreases
B. increased to Potassium, and
then decreases
C. does not change
D. increases
E. decreases to Potassium, and
then increased
2.11. By a Lithium to Cesium ion radii
of the elements E +:
А. does not change
B. decreases to Potassium, and
then increased
C. increased to Potassium, and
then decreases
D. decreases
E. increases
2.12. By a Lithium to Cesium atom
ionization energy:
А. decreases to Sodium, and then
increased
B. decreases
C. increases
D. increased to Sodium, and then
decreases
E. does not change
2.13. Value of standard electrode
potential from Lithium to Cesium:
А. decreases to Sodium, and then
increased
B. increased to Sodium, and then
decreases
C. increased
D. does not change
E. decreases
2.14. The most negative value of
standard electrode potential has:
А. Lithium
B. Potassium
C. Sodium
D. Rubidium
E. Cesium
2.15. Among alkaline metals more
active is:
А. Rubidium
B. Potassium
C. Cesium
D. Lithium
E. Sodium
2.16. Lithium with properties similar
to:
А. Calcium
B. Sodium
C. Beryllium
D. Potassium
E. Magnesium
2.17. Chemical formula of halite.
А. LiAlPO4F
B. NaCl
C. Na2SO4·10H2O
D. KCl·MgCl2·6H2O
E. NaCl·KCl
2.18. Chemical formula of sylvinite.
А. NaCl
B. Na2SO4·10H2O
C. LiAlPO4F
D. NaCl·KCl
E. KCl·MgCl2·6H2O
2.19. Chemical formula to carnallite.
А. LiAlPO4F
B. NaCl·KCl
C. Na2SO4·10H2O
D. NaCl
E. KCl·MgCl2·6H2O
2.20. Chemical formula of ambligonite.
А. NaCl·KCl
B. NaCl
C. Na2SO4·10H2O
D. KCl·MgCl2·6H2O
E. LiAlPO4F
2.21. Chemical formula Glauber salt:
А. NaCl
B. KCl·MgCl2·6H2O
C. LiAlPO4F
D. NaCl·KCl
E. Na2SO4·10H2O
2.22. To the macroelements belong:
А. Sodium and Lithium
B. Lithium and Potassium
C. Sodium and Rubidium
D. Sodium and Potassium
E. Cesium and Lithium
2.23. Which of the listed methods are
used for preparation of metallic
sodium?
А. method of hydrometallurgy
B. method of carbothermy
C. method of aluminothermy
D. electrolysis of fusions of salts
E. electrolysis of solutions of
salts
2.24. Which of the listed methods are
used for preparation of metallic
lithium?
А. electrolysis of fusions of salts
B. electrolysis of solutions of
salts
C. method of hydrometallurgy
D. method of aluminothermy
E. method of carbothermy
2.25. Which of the alkaline metals can
be obtained by the following
reaction?
MeCl + Na → Me + NaCl
А. rubidium and lithium
B. potassium and rubidium
C. lithium and францій
D. potassium and lithium
E. lithium and cesium
2.26. With the direct interaction with
oxygen peroxide forms:
А. rubidium
B. sodium and potassium
C. sodium
D. potassium
E. lithium
2.27. With the direct interaction with
oxygen oxide forms:
А. sodium and potassium
B. lithium
C. potassium
D. cesium
E. sodium
2.28. With the direct interaction with
oxygen supperoxide forms:
А. sodium and potassium
B. sodium and lithium
C. potassium and rubidium
D. sodium and rubidium
E. cesium and lithium
2.29. Under normal conditions, nitrogen
reacts with:
А. potassium
B. sodium
C. lithium
D. cesium
E. sodium and potassium
2.30. The oxidation number of
hydrogen in hydrides of alkali
metals is:
А. +2
B. -2
C. +1
D. –1
E. 0
2.31. The oxidation number of Oxygen
in the alkali metal peroxides is:
А. 0
B. –2
C. +1
D. –½
E. –1
2.32. The oxidation number of Oxygen
in the alkali metal supperoxides
is:
А. 0
B. –1
C. –2
D. –½
E. +1
2.33. What type of chemical bonds
present in the hydrides of alkali
metals?
А. B. nonpolar covalent
C. polar covalent
D. ionic
E. metallic
2.34. What alkaline metal, burning on
air or in the atmosphere of oxygen
forms the oxide of E2O?
А. K
B. Rb
C. Na
D. Li
E. Cs
2.35. When dissolved in water alkaline
oxide is formed:
А. alkalis and water
B. alkalis and hydrogen
C. alkalis
D. alkalis and oxygen
E. hydride of metal and oxygen
2.36. When dissolved in water alkaline
peroxide is formed:
А. hydride of metal and oxygen
B. alkalis
C. alkalis and water
D. alkalis and hydrogen
E. alkalis and oxygen
2.37. When dissolved in water alkaline
superoxide is formed:
А. alkalis and oxygen
B. alkalis and water
C. alkalis
D. hydride of metal and oxygen
E. alkalis and hydrogen
2.38. Which of the alkali metal
hydroxide has the worst solubility
in water?
А. sodium
B. cesium
C. lithium
D. rubidium
E. potassium
2.39. Which one of the given reactants
is used for identification of the ion
of K+.
А. NaH2SbO4
B. NaHC4H4O6
C. Na2S
D. Na2CO3
E. (NH4)2C2O4
2.40. Which one of the given reactants
is used for identification of the ion
Na+.
А. H2S
B. NH4SCN
C. KH2SbO4
D. NH4Cl
E. NaH2PO4
2.41. Chemical formula of soda is:
А. K2CO3
B. Na2CO3
C. Na2CO3·10H2O
D. NaHCO3
E. NaOH
2.42. Chemical formula of drinking
(baking) soda is:
А. Na2CO3·10H2O
B. NaOH
C. K2CO3
D. NaHCO3
E. Na2CO3
2.43. Chemical formula of crystalline
soda is:
А. NaOH
B. NaHCO3
C. Na2CO3
D. Na2CO3·10H2O
E. K2CO3
2.44. Chemical formula of potassium
carbonate is:
А. Na2CO3·10H2O
B. NaHCO3
C. K2CO3
D. Na2CO3
E. NaOH
2.49. Solutions of alkalis react with the
following simple matters:
А. C O2, P
B. Cl2, S N2
C. Zn, Cu, Mn
D. Cl2, P, Zn
E. Si, Al, Cu
2.45. Which of the following reactions
are used in submarines for air
regeneration?
А. 2Na2O2 + 2CO2 = 2Na2CO3 +
O2
B. 2KMnO4 = K2MnO4 + MnO2 +
O2
C. 2NaNO3 = 2NaNO2 + O2
D. 2H2O2 = 2H2O + O2
E. 2KClO3 = 2KCl + 3O2
2.50. Sodium iodide is used in medicine
as:
А. B. diuretic
C. sedative
D. antacidic
E. source to the microelement of
iodine
2.46. Chemical formula of caustic soda
is:
А. K2CO3
B. NaOH
C. Na2CO3
D. NaHCO3
E. Na2CO3·10H2O
2.47. Sodium hydrogen carbonate is
used as:
А. sedative
B. antacidic
C. diuretic
D. cholagogue
E. laxative
2.48. The ions of what chemical
element influence on electrolyte
balance of brain and what salt of
this element is used for treatment
of psychical diseases:
А. I, KI
B. Rb, RbCl2
C. Li, LiCl
D. Li, Li2CO3
E. Cl, NaCl
2.51. Mass percentage of sodium
chloride in hypertonic solution is:
А. 0,9 %
B. 0,18 %
C. 5 %
D. 1 %
E. 0,09 %
2.52. Which of the given compounds
can be used for softening of
water?
А. CaCO3, Ca(OH)2
B. MgSO4, H2SO4
C. Na3PO4, CaCl2
D. Na2CO3, NaOH
E. Na2CO3, NaCl
2.53. What is the type of bonds in the
molecule of NaCl?
А. polar covalent
B. ionic
C. nonpolar covalent
D. metallic
E. hydrogenic
2.54. The reaction is between sodium
and water:
А. endothermic, substitution
B. exothermic, substitution
C. endothermic
D. exothermic, connection
E. exothermic, exchange
2.55. Which one from the given
formulas corresponds to sodium
thiosulphate?
А. Na2S2O4
B. NaHSO4
C. Na2SO3
D. Na2S2O3
E. Na2S2O5
2.56. Which of the given elements
corresponds to s-elements?
А. Mn, Br, Mo
B. P, S, Cr
C. K, Ca, Cs
D. S, P, Cl
E. Be, Mg, Al
2.57. Which one of the listed reaction is
possible at the room temperature?
А. Au + HCl →
B. Cr2O3 + H2 →
C. Fe + H2SO4 (conc.) →
D. Na + H2O →
E. Cu + H2O →
2.58. Which one from the given salts
does not hydrolyze:
А. ZnSO4
B. KI
C. Al2(SO4)3
D. KNO2
E. CrCl3
2.59. The concentration of [OH–] =
1•10–6 mol/L. What is the pH of
this solution?
А. 8
B. 6
C. 7
D. 1
E. 4
Chapter 3. s-Elements of the ІІ groups of the Periodic Table.
Beryllium, Magnesium, and Alkaline earth metals
3.1. What is the electronic
configuration of Beryllium atom
А. 1s12s1
B. 1s22s2
C. 1s22s22p63s1
D. 1s22s0
E. 1s22s22p63s23p64s1
3.2. Electronic formula of Magnesium
atom.
А. 1s22s22p63s23p64s2
B. 1s22s22p63s2
C. 1s22s22p63s1
D. 1s22s22p63s23p64s2
E. 1s22s2
3.3. Electronic formula of Calcium
atom.
А. 4s1
B. 1s22s22p63s23p64s2
C. 1s22s22p63s23p64s23d105s1
D. 1s22s22p63s1
E. 1s22s22p62d103s1
3.4. Electronic formula of Strontium
atom.
А. 1s22s22p63s23p64s23d104p65s2
B. 1s22s22p63s2
C. 1s22s1
D. 5s1
E. 1s22s22p62d103s1
3.5. Electronic configuration of
external level of Barium atom.
А. 1s22s22p63s23p64s23d105s1
B. 1s22s1
C. 6s1
D. 6s1
E. 6s2
3.6. Electronic formula of Beryllium
cation.
А. 1s12s1
B. 1s22s22p63s1
C. 1s22s2
D. 1s1
E. 1s2
3.7. Electronic formula of Magnesium
cation.
А. 1s22s22p63s1
B. 1s22s22p6
C. 4s1
D. 1s22s22p5
E. 1s22s1
3.8. Electronic formula of Calcium
cation.
А. 5s1
B. 3s23p6
C. 1s22s22p63s23p64s1
D. 1s22s22p63s23p6
E. 3s23p64s1
3.9. Electronic formula of Strontium
cation.
А. 1s22s22p63s23p64s23d10
B. 4s23d104p6
C. 5s1
D. 1s22s22p63s23p64s23d104p6
E. 1s22s22p63s23p64s23d105s1
3.10. Atomic radius from Beryllium to
Barium of elements:
А. increases
B. decreases to Calcium, and then
increases
C. increases to Calcium, and then
decreases
D. does not change
E. decreases
3.11. Ionic radius of ions from
Beryllium to Barium of E2+ of
elements:
А. decreases
B. decreases to Calcium, and then
increases
C. does not change
D. increases to Calcium, and then
decreases
E. increases
3.12. Ionization energy From
Beryllium to Barium atom:
А. decreases to Calcium, and then
increases
B. decreases
C. increases to Calcium, and then
decreases
D. does not change
E. increases
3.13. Metallic properties from
Beryllium to Barium:
А. does not change
B. increases
C. decreases to Calcium, and then
increases
D. decreases
E. increases to Calcium, and then
decreases
3.14. Value of standard electrode
potential from Beryllium to
Radium:
А. decreases
B. increases
C. does not change
D. increases to Calcium, and then
decreases
E. decreases to Calcium, and then
increases
3.15. The most negative value of
standard electrode potential has:
А. Barium
B. Magnesium
C. Strontium
D. Beryllium
E. Calcium
3.16. Among the metals of IIA group
radioactive is:
А. Calcium
B. Beryllium
C. Strontium
D. Radium
E. Magnesium
3.17. Magnesium with its properties
reminds alkali metal:
А. Lithium
B. Potassium
C. Rubidium
D. Sodium
E. Cesium
3.18. Beryllium with its properties
similar to:
А. sodium
B. boron
C. lithium
D. potassium
E. aluminum
3.19. Alkaline earth metals are:
А. Ba, Sr, Ra
B. Mg, Sr, Ra
C. Be, Sr, Mg
D. Ca, Sr, Ba
E. Be, Ra, Mg
3.20. Which one of the listed elements
of IIA group shows amphotheric
property:
А. Magnesium
B. all elements of IIA group
C. Calcium
D. Beryllium and Magnesium
E. Beryllium
3.21. Chemical formula of magnesite;
А. MgSO4·10H2O
B. MgCO3·СaCO3
C. KCl·MgCl2·6H2O
D. MgCl2·KCl
E. MgCO3
3.22. Chemical formula of dolomite:
А. MgSO4·10H2O
B. MgCO3·СaCO3
C. MgCl2·CaCl2
D. KCl·MgCl2·6H2O
E. Mg3(PO4)2
3.23. Chemical formula of chalk;
А. СaCO3
B. MgCO3
C. Mg3(PO4)2
D. CaCl2
E. СаSO4
3.24. Chemical formula of anhydrite:
А. СaCO3
B. CaCl2
C. MgCO3
D. СаSO4
E. Mg3(PO4)2
3.25. Chemical formula of limestone:
А. СaO
B. СaCO3
C. Ca(OH)2
D. CaCl2
E. СаSO4
3.26. Chemical formula of calcite;
А. СaCO3
B. Ca(OH)2
C. СaO
D. CaCl2
E. СаSO4
3.27. Chemical formula of celestite;
А. SrSO4
B. SrCO3
C. CaSO4
D. СaCO3
E. KCl·MgCl2·6H2O
3.28. Chemical formula of gypsum:
А. KCl·MgCl2·6H2O
B. СaCO3
C. СаSO4·2Н2О
D. SrCO3
E. CaSO4
3.29. Chemical formula of fluorite:
А. KF·MgF2·6H2O
B. CaSO4
C. CaF2
D. SrF2
E. СaCO3
3.30. Chemical formula of barite:
А. ВаSO4
B. ВаCl2
C. СaCO3
D. SrSO4
E. ВaCO3
3.31. Chemical formula of lime:
А. Ca(OH)2
B. CaO
C. CaCl2
D. CaO2
E. CaCO3
3.32. Which of the listed methods are
used for preparation of metallic
beryllium?
А. hydrometallurgy
B. aluminothermy
C. electrolysis of fusions of salts
D. electrolysis of solutions of
salts
E. carbothermy
3.33. Which of the listed methods are
used for preparation of metallic
magnesium?
А. method of carbothermy
B. electrolysis of solutions of
salts
C. method of aluminothermy
D. electrolysis of fusions of salts
E. method of hydrometallurgy
3.34. At the reaction with oxygen
elements of IIA group form the
oxides of the following
composition:
А. МеО and Ме2О
B. Me2O
C. MeO
D. Ме2О3
E. Ме3О4
3.35. What metal of IIA group at
reaction with oxygen can form
peroxide?
А. beryllium
B. calcium
C. barium
D. magnesium
E. strontium
3.36. What metal of IIA of group does
not react with hydrogen?
А. calcium
B. beryllium
C. magnesium
D. strontium
E. barium
3.37. What metal of IIA of group does
not react with water?
А. magnesium
B. beryllium
C. strontium
D. calcium
E. barium
3.38. Basic properties of hydroxides
from Be(ОН)2 to Ba(ОН)2:
А. decreases to Magnesium, and
then increases
B. increases to Magnesium, and
then decreases
C. does not change
D. increases
E. decreases
3.39. Under ordinary conditions with
water does not react:
А. magnesium
B. calcium
C. barium
D. strontium
E. radium
3.40. The concentrated sulfuric acid
passive:
А. strontium
B. magnesium
C. beryllium
D. barium
E. calcium
3.41. The concentrated
passive:
А. calcium
B. beryllium
C. barium
D. strontium
E. magnesium
nitric
acid
3.42. What is the pH of water solution
of calcium sulfide?
А. basic
B. weak basic
C. acidic
D. neutral
E. strongly acidic
3.43. What reagent is used for the
identification of Ca2+ ion?
А. HNO3
B. H2S
C. NH4SCN
D. HCl
E. (NH4)2C2O4
3.44. What reagent is used for the
identification of Mg2+ ion?
А. HCl
B. H2S
C. NaH2PO4
D. NaHC4H4O6
E. KH2SbO4
3.45. What reagent is used for the
identification of Ba2+ ion?
А. НI
B. Н2C2O4
C. Н2SO4
D. НNO3
E. НCl
3.46. What reagent is used for the
identification of Sr2+ ion?
А. HCl
B. K2CrO4
C. NaHC4H4O6
D. H2S
E. (NH4)2C2O4
3.47. Do the ions of Ca2+ paint the
flame in what color?
А. reddish-orange
B. green
C. violet
D. yellow
E. greenish-yellow
3.48. Do the ions of Ba2+ paint the
flame in what color?
А. violet
B. yellow green
C. yellow
D. reddish-orange
E. red
3.49. Do the ions of Sr 2+ paint the
flame in what color?
А. reddish-orange
B. carmine-red
C. yellow
D. greenish-yellow
E. violet
3.50. Complete and balance the
equation of the reaction. Point out
the sum of the coefficient in the
equation.
Sr + H2 →
the sum of the coefficient in the
equation.
Ca + P →
А. 7
B. 4
C. 8
D. 6
E. 5
3.54. Complete and balance the
equation of the reaction. Point out
the sum of the coefficient in the
equation.
Mg + F2→
А. 6
B. 4
C. 8
D. 5
E. 3
3.51. Complete and balance the
equation of the reaction. Point out
the sum of the coefficient in the
equation.
Be + C →
А. 7
B. 5
C. 4
D. 6
E. 8
А. 6
B. 4
C. 3
D. 8
E. 5
3.55. Complete and balance the
equation of the reaction. Point out
the sum of the coefficient in the
equation.
Mg + S→
3.52. Complete and balance the
equation of the reaction. Point out
the sum of the coefficient in the
equation.
Mg + N2 →
А. 7
B. 8
C. 9
D. 5
E. 6
3.53. Complete and balance the
equation of the reaction. Point out
А. 8
B. 5
C. 3
D. 4
E. 6
3.56. Complete and balance the
equation of the reaction. Point out
the sum of the coefficient in the
equation.
Ca + C →
А. 8
B. 4
C. 7
D. 5
E. 6
3.57. Complete and balance the
equation of the reaction. Point out
the sum of the coefficient in the
equation.
Ca + H2O →
А. 6
B. 7
C. 4
D. 8
E. 5
Mg + NH4Cl (conc.) →
3.58. Complete and balance the
equation of the reaction. Point out
the sum of the coefficient in the
equation.
Mg + HCl (dil) →
А. 5
B. 8
C. 4
D. 7
E. 6
А. 8
B. 6
C. 9
D. 4
E. 5
3.62. Complete and balance the
equation of the reaction. Point out
the sum of the coefficient in the
equation.
Be + HF (conc.) →
3.59. Complete and balance the
equation of the reaction. Point out
the sum of the coefficient in the
equation.
Be + HCl (dil) →
А. 6
B. 4
C. 7
D. 8
E. 5
А. 7
B. 6
C. 4
D. 8
E. 5
3.63. Complete and balance the
equation of the reaction. Point out
the sum of the coefficient in the
equation.
BeО + HNO3 (conc.) →
3.60. Complete and balance the
equation of the reaction. Point out
the sum of the coefficient in the
equation.
Be + NaOH (conc.) →
А. 5
B. 7
C. 8
D. 4
E. 6
3.61. Complete and balance the
equation of the reaction. Point out
the sum of the coefficient in the
equation.
А. 6
B. 8
C. 7
D. 4
E. 5
3.64. Complete and balance the
equation of the reaction. Point out
the sum of the coefficient in the
equation.
Be(ОН)2 +HNO3 (conc.) →
А. 7
B. 6
C. 5
D. 4
E. 8
3.65. Complete and balance the
equation of the reaction. Point out
the sum of the coefficient in the
equation.
Ca(ОН)2 +HNO3 (conc.) →
А. 7
B. 6
C. 4
D. 8
E. 9
3.66. Complete and balance the
equation of the reaction. Point out
the sum of the coefficient in the
equation.
CaO + HNO3 (conc.) →
А. 7
B. 8
C. 5
D. 4
E. 6
3.67. Complete and balance the
equation of the reaction. Point out
the sum of the coefficient in the
equation.
CaCO3 + HNO3 (conc.) →
А. 8
B. 7
C. 5
D. 4
E. 6
3.68. Complete and balance the
equation of the reaction. Point out
the sum of the coefficient in the
equation.
Mg(ОН)2 + HNO3 (conc.) →
А. 5
B. 4
C. 6
D. 8
E. 7
3.69. The presence of which salts in
water predefines temporal
hardness of water?
А. CaCO3 and MgCO3
B. Mg(HCO3)2 and Ca(HCO3)2
C. KHCO3 and NaHCO3
D. Na2SO4 and CaSO4
E. KHCO3 and Ca(HCO3)2
3.70. The presence of what salts in
water predefines permanent
hardness of water?
А. СаSO4
B. Ca(HCO3)2
C. Mg(HCO3)2
D. K2SO4
E. NaCl
3.71. The presence of which salts in
water predefines permanent
hardness of water?
А. Mg(HCO3)2
B. Na3PO4
C. KCl
D. Ca(HCO3)2
E. MgCl2
3.72. The presence of which salts in
water predefines temporal
hardness of water?
А. MgCl2
B. NaCl
C. Ca3(PO4)2
D. Mg(HCO3)2
E. CaСl2
3.73. Temporary hardness is caused by
the presence in water alcium and
magnesium:
А. chlorides
B. sulfides
C. nitrates
D. hydrogencarbonates
E. sulfates
3.74. To the macroelements belongs
biotmetals:
А. Barium and Magnesium
B. Barium and Radium
C. Beryllium and Magnesium
D. Calcium and Magnesium
E. Strontium and Radium
3.75. Which one of the given salts is
used for the X-ray examination of
the gastrointestinal tract?
А. calcium chloride
B. strontium sulfate
C. magnesium sulfate
D. barium sulfate
E. magnesium oxide
3.76. Choose the formula of Epson salt
which has sedative, spasmolytic
and laxative effect.
А. MgSO4·7H2O
B. (MgOH)2CO3
C. CaSO4·2H2O
D. Na2CO3·10H2O
E. CaSO4·0,5H2O
3.77. Chemical formula of medical
hypsus:
А. CaSO4·3H2O
B. CaSO4·2H2O
C. CaSO4·5H2O
D. CaSO4·H2O
E. CaSO4·0,5H2O
3.78. The radio-nuclidess of what
element adsorbed by the body and
causes damage of blood-forming
organs and formation of cancer
cells?
А. beryllium
B. barium
C. calcium
D. magnesium
E. strontium
3.79. The high toxic action show
compounds of:
А. calcium
B. –
C. magnesium
D. strontium
E. beryllium
3.80. The high toxic action show
soluble compounds of:
А. barium
B. calcium
C. strontium
D. magnesium
E. –
Chapter 4. General characteristic of p-Elements. Boron and
Alluminium
4.1. Which of the given metals react
with hydrochloric acid releasing
hydrogen gas?
А. Hg
B. Au
C. Cu
D. Al
E. Pt
4.2. Which of the given metals does
not react with concentrated nitric
acid?
А. Al
B. Hg
C. Ag
D. Na
E. Cu
4.3. Which of the given metals react
with sulfuric acid releasing
hydrogen gas?
А. Hg
B. Pt
C. Ag
D. Al
E. Cu
4.4. What is the рН of aluminum
chloride AlCl3 solution?
А. pH=7
B. pH=9
C. pH=8
D. pH<7
E. pH>7
4.5. What is the рН of aluminum
nitrate solution Al(NO3)3?
А. pH=8
B. pH=9
C. pH>7
D. pH=7
E. pH<7
4.6. What is the рН of aluminum
sulfate solution Al2(SO4)3?
А. pH=7
B. pH=9
C. pH>7
D. pH=8
E. pH<7
4.7. Concentrated nitric acid HNO3
will react with:
А. Cu
B. Fe
C. Cr
D. Au
E. Al
4.8. Aluminum in the reactions with
other compounds:
А. gains 2 electrons
B. gains 3 electrons
C. loses 2 electrons
D. loses 1 electron
E. loses 3 electrons
4.9. Point out the sum of the
coefficients in the equation
between aluminum Al and sodium
hydroxide solution NaOH:
А. 18
B. 16
C. 20
D. 15
E. 17
4.10. Calculate a molar mass of gas
which is evolved at the hydrolysis
of aluminum Al2S3 sulfide:
А. 64
B. 34
C. 32
D. 80
E. 2
4.11. What is the product of hydrolysis
of aluminum chloride AlCl3 on the
first stage:
А. AlOHCl2
B. Al(OH)2Cl
C. Al(OH)3
D. Al2O3
E. [Al(H2O)6]Cl3
4.12. What is the product of hydrolysis
of aluminum nitrate Al(NO3)3 on
the second stage:
А. Al(OH)2NO3
B. [Al(H2O)6](NO3)3
C. Al2O3
D. AlOH(NO3)2
E. Al(OH)3
4.13. What is the product of hydrolysis
of aluminum sulfate Al2(SO4)3 on
the first stage:
А. AlOHSO4
B. Al(HSO4)3
C. Al(OH)3
D. (Al(OH)2)SO4
E. Al2O3
4.14. Which of the given salts have the
acidic medium?
А. CaCO3, BaSO4
B. NaCl, KNO3
C. KCl, Na3PO4
D. CaCl2, Na2CO3
E. FeCl2, Al(NO3)3
4.15. Choose the true statement for
aluminum hydroxide Al(OH)3?
А. dissolves in water
B. does not dissolve in in alkalis
C. does not decompose at heating
D. does not has oxidizingreduction properties
E. does not dissolve in acids
4.16. Al2(SO4)3 does not form as a result
of reaction between:
А. Al + SO3 →
B. Al + H2SO4 →
C. Al2O3 + H2SO4 →
D. Na3[Al(OH)6]+ H2SO4 →
E. Al(OH)3 + H2SO4 →
4.17. What product forms under the
reaction (precipitate) between
aluminum chloride AlCl3 and
sodium carbonate Na2CO3?
А. B. Al(OH)
C. Al2(CO3)3
D. Al2O3
E. NaAlO2
4.18. What product forms under the
reaction (precipitate) between
aluminum sulfate solution
Al2(SO4)3 and ammonium sulfide
(NH4)2S ?
А. Al2O3
B. Al(OH)3
C. (NH4)2SO4
D. Al2S3
E. AlOHSO4
4.19. What product forms under the
reaction (precipitate) between
aluminum chloride AlCl3 solution
and sodium sulfide Na2S?
А. Al2S3
B. Al2O3
C. AlOHSO4
D. Al2(SO4)3
E. Al(OH)3
4.20. Which one of the listed elements
has oxidation and reducing
properties:
А. Tl
B. Al
C. In
D. Ga
E. B
4.21. Which one of the listed oxides has
acidic properties only?
А. In2O3
B. Tl2O3
C. Al2O3
D. B2O3
E. Ga2O3
4.22. Which of the listed oxides has
basic properties only?
А. In2O3
B. Ga2O3
C. Al2O3
D. B2O3
E. Tl2O3
4.23. What mass of chlorine Cl2 will
react with aluminum Al. Mass of
aluminum equal 9 g?
А. 1,42
B. 35,5
C. 0,355
D. 0,71
E. 71
4.24. Which of the listed compounds of
boron is found in nature?
А. B2O3
B. H3BO3
C. B2H6
D. Mg3B2
E. NaBO2
4.25. The oxide of boron has the
properties:
А. B. acidic
C. basic
D. Mixed
E. amphoteric
4.26. The oxide of boron when
dissolved in water forms:
А. amphoteric hydroxide
B. does not form acids or bases
C. metaboric acid
D. ortoboric acid
E. tetraboric acid
4.27. In which compounds boron has
the oxidation state –3?
А. NaBO2
B. H3BO3
C. Mg3B2
D. Na2B4O7
E. B2O3
4.28. Which one of the given oxides
does not dissolve in alkalis?
А. In2O3
B. Al2O3
C. Tl2O3
D. B2O3
E. Ga2O3
4.29. Which one of the given
hydroxides has the basic
properties?
А. Tl(OH)3
B. Al(OH)3
C. B(OH)3
D. In(OH)3
E. Ga(OH)3
4.30. Which one of the given
hydroxides has the acidic
properties?
А. Al(OH)3
B. Ga(OH)3
C. B(OH)3
D. Tl(OH)3
E. In(OH)3
4.31. Which of the given hydroxides
have the amphoteric properties?
А. Tl(OH)3, Ba(OH)2
B. Ga(OH)3, In(OH)3
C. Mg(OH)2, Tl(OH)3
D. Fe(OH)2, B(OH)3
E. Ga(OH)3, B(OH)3
4.32. Which of the given oxides have
the amphoteric properties?
А. FeO, NO2
B. B2O3, BaO
C. CaO, SO3
D. BeO, Al2O3
E. MgO, P2O3
4.33. What volume of hydrogen H2 (L)
will be released at the reaction of
aluminum Al by mass 9 г with the
diluted sulfuric acid H2SO4?
А. 5,6
B. 22,4
C. 67,2
D. 44,8
E. 11,2
4.34. What metals react with solutions
of alkalis?
А. Ca, Fe
B. Cr, К
C. Hg, Cd
D. Mn, Na
E. Zn, Al
4.35. Which of the listed hydroxides
have amphoteric properties?
А. LiOH, Sr(OH)2
B. Mg(OH)2, KOH
C. Ca(OH)2, NaOH
D. Al(OH)3, Cr(OH)3
E. Cr(OH)2, Fe(OH)2
4.36. Which of the listed compounds
can not exist in the same solution
simultaneously?
А. AlCl3, Ca(NO3)2
B. NaCl, Al(NO3)3
C. Na2SO4, Al(NO3)3
D. Na2SO3, Al2(SO4)3
E. NaCl, AlCl3
4.37. What will be one of the products
of the reaction between
aluminium Al and concentrated
sulfuric acid H2SO4?
А. H2S
B. SO2
C. SO3
D. S
E. H2
4.38. Reducing properties of simple
substances from B to Tl:
А. B. decrease
C. does not change
D. decrease at first, then increase
E. increase
4.39. What metals do not react with
concentrated sulfuric acid H2SO4:
А. Fe, Cr, Al
B. Al, Zn, Be
C. Fe, Cr, Zn
D. Cr, Na, Mg
E. Al, К, Mg
4.40. From the listed pair of hydroxides
choose insoluble in water, but
soluble in acids and alkalis:
А. Ca(OH)2, Bi(OH)3
B. Mg(OH)2, Cu(OH)2
C. Al(OH)3, Zn(OH)2
D. Mg(OH)2, Sn(OH)2
E. Cr(OH)2, Fe(OH)2
4.41. Which of the listed electronic
configurations corresponds to 13Al
atom?
А. [Ne] 3s03p0
B. [Ne] 3s23p1
C. [Ne] 3s23p3
D. [Ne] 3s23p4
E. [Ne] 3s13p0
4.42. Which of the listed electronic
configurations corresponds to 5B
atom?
А. [He] 2s22p4
B. [He] 2s22p3
C. [He] 2s22p1
D. [He] 2s22p5
E. [He] 2s22p2
4.43. Which of the listed electronic
configurations corresponds to Al3+
ion?
А. [Ne] 3s23p1
B. [Ne] 3s03p0
C. [Ne] 3s13p0
D. [Ne] 3s23p4
E. [Ne] 3s23p3
Chapter 5. р-Elements of IVА Group. Carbon, Silicon
5.1. Which of the listed substances are
not allotropes of carbon?
А. diamond
B. anthracite
C. carbine
D. graphite
E. fullerene
5.2. Why properties of allotropes of
carbon substantially differ
between themselves?
А. they have different values of
Gibs’s free energy
B. they consist of different
isotopes of carbon
C. they have different aggregate
state
D. they have different heats of
formation
E. they have different structure of
crystalline grate
5.3. Which reagent is used for
determination of СО in air?
А. silver nitrate
B. PdCl2
C. Nesler reagent
D. –
E. bromine water
5.4. Which crystalline grate is in the
structure of diamond?
А. ionic
B. atomic
C. molecular
D. –
E. metallic
5.5. What allotrope modification of
carbon is the most hardness?
А. fullerene
B. carbine
C. graphite
D. diamond
E. –
5.6. What is the activated charcoal?
А. charcoal heating at the
temperature 500-6000С
B. charcoal cleaned by heating
with steam
C. brown coal cleaned by acid
D. charcoal cleaned by mineral
acid
E. –
5.7. An activated charcoal has a high
adsorbtivity, because it has:
А. solubility in water
B. high chemical activity of this
compound
C. low density
D. low chemical activity of this
compound
E. a large surface area
5.8. Which of the listed electronic
configurations corresponds to the
р-elements of IVA groups?
А. ns2np3
B. ns2np1
C. ns2np2
D. ns2np0
E. ns1np3
5.9. What oxidation states are the most
typical for carbon and silicon?
А. –2, –4
B.
C.
D.
E.
+2, –4
+2, +4
only +4
+4, –4
5.10. To what group of oxides carbon
(ІІ) oxide CO belongs?
А. B. basic
C. acidic
D. that cannot forms the salts
E. amphoteric
5.11. For the obtaining of carbon (ІІ)
oxide in laboratory is used such
compounds:
А. CH3OH, HCOOH
B. CH3COOH, HCOOH
C. СаСО3 MgCO3
D. НСООН, Н2С2О4
E. СаСО3⋅MgCO3, FeCO3
5.12. Carbonates are natural compounds
of carbon. Which of the listed
mineral does not belongs to this
group?
А. dolomite
B. malachite
C. carnelian
D. magnesite
E. shalk
5.13. Activated charcoal is used in
medical practice at those cases:
А. B. at poisonings and gastric
diseases
C. at an alkalosis (increasing of
рН blood)
D. at аcidosis (decreasing of рН
blood)
E. at the sepsis
5.14. What gas is formed as a result of
reaction between CaC2 and
water?
А. acetylene
B. ethylidene
C. methanol
D. ethane
E. methane
5.15. What is the “dry ice”?
А. carbonic acid in the hard state
B. carbon (IV) oxide in the hard
state
C. saturated solution of СО2 in
water
D. carbon (ІІ) oxide in the hard
state
E. concentrated carbonic acid
5.16. Mixture of СО + Н2 is named:
А. B. water gas
C. coke gas
D. generator gas
E. smeech gas
5.17. What concentration of СО in air is
mortal for a human?
А. 0.25%.
B. 0.5%.
C. 0.05%.
D. 0.01%.
E. 0.2%.
5.18. What compounds are the main air
pollutions?
А. oxides of all non-metals
B. oxides of sulfur and all
halogens
C. oxides of carbon, sulfur and
nitrogen
D. compounds of hydrogen with
carbon, sulfur and nitrogen
E. halogens
5.19. Which salt of carbonic acid
(H2CO3) does not hydrolyze:
А. (NH4)2CO3
B. MgCO3
C. K2CO3
D. Na2CO3
E. NaHCO3
5.20. Which one of the given salts does
not decompose at heating?
А. СаCO3
B. NH4НCO3
C. Са(НCO3)2
D. K2CO3
E. КНCO3
5.21. Compounds of Fe, Ni, Co, with
СО are named:
А. carbides
B. carboniles
C. hydrogen carbonates
D. carbonates
E. methanides
B. 1, 3, 5
C. 1, 4
D. 2, 4, 5
E. 4, 5
5.25. Determination of carbonate-ion
СО32– is:
А. decomposition of carbonates at
heating
B. formation of basic medium at
a hydrolysis
C. evolving of CO2 at action of
strong acids
D. evolving of CO2 at action of
alkalis
E. obtaining of a precipitate at
action of mineral acids
5.22. What is the optimum
concentration of СО2 in air:
А. 0.3%
B. 0.02%
C. 0.5%
D. 0.03%
E. 0.2%
5.26. Aluminium carbide Al4C3 reacts
with water releasing:
А. water gas
B. carbon dioxide
C. acetylene
D. ethane
E. methane
5.23. Carbonic acid corresponds to:
А. strong, polyprotic
B. monoprotic, stable
C. very weak, polyprotic
D. weak, polyprotic, unstable
E. monoprotic
5.27. Complete and balance the reaction
of the hydrolysis of aluminium
carbide Al4C3.
5.24. Which of the listed reactions
corresponds to redox reaction?
1. CO2 + NaOH → NaHCO3
2. CO2 + 2Mg → 2MgO + C
3. C + 2H2 → CH4
4. CO2 + H2O → H2CO3
5. CS2 + Na2S → Na2CS3
А. 2, 3
Point out the sum of the
coefficients in the equation.
А. 17
B. 14
C. 20
D. 16
E. 18
5.28. Complete and balance the reaction
of the hydrolysis of calcium
carbide CaC2
Point out the sum of the
coefficients in the equation.
А. 6
B.
C.
D.
E.
5
9
8
7
5.29. Write molecular equation of
transformation of sodium
hydrogencarbonate NaHCO3 into
a sodium carbonate Na2CO3 at
heating. Point out the sum of the
coefficients in the equation:
А. 4
B. 7
C. 8
D. 6
E. 5
5.30. Write molecular equation of
transformation of calcium
carbonate CaCO3 into a calcium
hydrogencarbonate Ca(HCO3)2.
Point out the sum of the
coefficients in the equation:
А. 7
B. 4
C. 6
D. 5
E. 8
5.31. Silicon reacts with such
compounds:
1. HCl
2. NaOH
3. HNO3
4. H2O
5. HF + HNO3
6. HCl + HNO3
А. 2, 3, 4
B. 2, 4, 5
C. 1, 2, 3
D. 5, 6
E. 1, 3, 5
5.32. Silicon dioxide (IV) SiO2
corresponds to the acidic oxides,
but it reacts with the next acid:
А. nitric acid (conc.) HNO3
B. nitric acid (dil.) HNO3
C. fluoric acid HF
D. phosphoric acid
E. hydrochloric acid HCl
5.33. Amorphous silicon does not react
even at heating with:
А. hydrogen
B. oxygen
C. carbon
D. metals
E. nitrogen
5.34. How to get silicon in industry?
А. reduction of its oxide by
carbon (IV) oxide
B. method of electrolysis
C. method of hydrometallurgy
D. E. reduction of its oxide SiO2 by
active metals
5.35. How do silanes burn?
А. with the releasing of silicic
acid H2SiO3 and water
B. with the releasing of water,
silicon dioxide and heat
C. with the releasing of hydrogen,
silicon SiO2 dioxide and heat
D. with absorption of heat,
formation of water and silicon
dioxide
E. with the releasing of water,
silicon and heat
5.36. What number of hydrochloric acid
needs to be taken for the complete
decomposition of 2.5 mole of
calcium silicide?
А. 4 moles
B. 15 moles
C. 10 moles
D. 0,1 mole
E. 8 moles
5.37. Silicagel is an effective adsorbent.
Choose the correct formula of
silicagel?
А. dimetasilicic acid H2Si2O5
B. silicic acid H2SiO3
C. micronized quartz
D. mixture of polysilicic acids
E. powder of SiO2
5.38. Complete and balance the reaction
of the hydrolysis of silicon
tetrachloride SiCl4.
Point out the sum of the
coefficients in the equation.
А. 5
B. 7
C. 9
D. 8
E. 10
5.39. Complete and balance the reaction
of the melting of silicon Si with
alkali NaOH. Point out the sum of
the coefficients in the equation.
А. 6
B. 9
C. 10
D. 7
E. 8
5.40. Silicic acid can be obtained by the
reaction:
А. Si + H2O → H2SiO3
B. CaSiO3 + H2 → H2SiO3 + Ca
C. SiO2 + H2O → H2SiO3
D. Na2SiO3 + 2HCl → H2SiO3 +
2NaCl
E. SiO2 + H2O→ H2SiO3
5.41. What volume of hydrogen at STP
will be released at dissolving of
silicon Si (mass of Si = 14 g) in
alcali?
А. 18,4 L
B. 5,6 L
C. 22,4 L
D. 11,2 L
E. 10,5 L
5.42. What is the pH of potassium
silicate solution K2SiO3?
А. week acidic
B. neutral
C. basic
D. week basic
E. acidic
Chapter 6. р-Elements of IVА Group. Germanium family
elements (Germanium, Tin, and Lead)
6.1. β - modification (white tin) can be
transformed into α - modification
(grey tin) at the condition of:
А. increased temperature
B. treating with an alkali
C. treating with an acid
D. constant temperature
E. decreased temperature
6.2. What is the behavior of Ge, Sn, Pb
elements at the normal conditions
in the presence of water and the
air:
А. do not react
B. react forming corresponding
hydroxides
C. form oxides
D. react releasing a gas
E. react
6.3. What is the product of the
reaction between tin and НСl
concentrated?
А. Н2[SnС14]
B. SnCl 4
C. SnO
D. SnCl 2
E. SnO2
6.4. Which elements of the Germanium
family are situated behind
Hydrogen in the electrochemical
series of metals?
А. Sn
B. Pb
C. Sn, Pb
D. Ge, Pb
E. Ge
forming:
А. basic salts
B. hydroxides
C. hydroxocomplex compounds
D. mixed oxides
E. neutral salts
6.8. Select the formulas of oxides
which are forming when the
Germanium family elements are
heating in the air:
А. GeO2, SnO, Рb2О3
B. GeO, SnO, РbО2
C. GeO2, SnO2, РbО2
D. GeO, SnO, РbО
E. GeO2, SnO2, РbО
6.9. What is the behavior of Ge, Sn, Pb
oxides in water?
А. slightly soluble
B. react releasing a gas
C. react vigorously
D. form hydroxocomplexes with
water
E. well soluble
6.5. Which elements of the Germanium
family do not react with nonoxidizer acids?
А. Ge, Pb
B. Ge
C. Sn
D. Sn, Pb
E. Pb
6.10. What are the products of the
reaction between РbО2 and
H2SO4 concentrated?
А. Pb3О4, Н2О
B. SO3, PbО, Н2О
C. PbO, О2, Н2О
D. PbSO4, Н2О
E. PbSO4, О2, Н2О
6.6. What are the products of the
reaction between lead and
HNO3 concentrated?
А. Pb(NO3)2 + NO
B. Na2[Pb(OH)4] + H2O
C. Pb(NO3)2 + NO
D. Na2[Pb(OH)4]
E. Pb(NO3)2 + NO2
6.11. What are the products of the
reaction При взаємодії РbО2 +
NaOH + Н2 О?
А. Na4[Рb(ОН)6]
B. Na[Рb(ОН)4]
C. Na4[Рb(ОН)4]
D. Na2[Рb(ОН)6 ]
E. Na2[Рb(ОН)4]
6.7. Sn і Pb can react with alkalis
aqueous solutions under heating
6.12. α - stannic and β - stannic acids
(H2SnO3) can be prepared
according to the following
reaction:
А. SnO2 + 4Н2О; Sn +
HNO3(conc.)
B. SnCl4 + NH3 +·H2O; Sn +
HNO3(conc.)
C. SnO2 + хН2О; SnО +
HNO3(conc.)
D. SnO2 + хН2О; SnO2 +
HNO3(conc.)
E. SnCl2 + 2Н2О; Sn +
HNO3(conc.)
6.13. Select the proper formulas of
german, Stannan and Plumban.
А. Ge3N4,Sn3N4, Рb3N4
B. GeO, SnO, РbО2
C. GeO2, SnO2, РbО2
D. GeH4, SnH4, РbН4
E. GeO2, SnO, Рb2О3
6.14. What are the products of the
reaction between the Germanium
family elements with chlorine?
А. GeCl2; SnCl2; РbС14
B. GeCl4; SnCl4; РbС12
C. GeCl4; SnCl4; РbС14
D. GeCl4; SnCl2; РbС12
E. GeCl2; SnCl4; РbС12
6.15. Which of the Germanium family
elements can be dissolved in
aqueous alkalis solutions?
А. Ge, Sn, Pb
B. Sn, Pb
C. Ge, Pb
D. Pb
E. Ge, Sn
6.16. What is the product of SnCl2
hydrolysis?
А. H2[Sn(OH)4]
B. [Sn(H2O)4]2+
C. Sn(OH)2
D. Sn(OH)Cl
E. SnO
6.17. What is the product of SnCl4
hydrolysis?
А. Sn(OH)2
B. [Sn(OH)(H2O)3]Cl3
C. Sn(OH)Cl3
D. H2SnO3
E. Sn(OH)2Cl2
6.18. Select the proper general formulas
of the Germanium family elements
existing oxides.
А. ЕО and Е2О3
B. ЕО2
C. Е2О3 and ЕО2
D. ЕО and ЕО2
E. ЕО
6.19. The acidic properties of the elements
hydroxides become stronger in the
following sequence:
А. Pb(OH)4– Ge(OH)4– Sn(OH)4
B. Sn(OH)4– Ge(OH)4– Pb(OH)4
C. Sn(OH)4– Pb(OH)4– Ge(OH)4
D. Pb(OH)4–Sn(OH)4– Ge(OH)4
E. Ge(OH)4–Sn(OH)4–Pb(OH)4
6.20. The basic properties of the elements
hydroxides become stronger in the
following sequence:
А. Sn(OH)2– Pb(OH)2– Ge(OH)2
B. Sn(OH)2– Ge(OH)2– Pb(OH)2
C. Pb(OH)2– Ge(OH)2– Sn(OH)2
D. Ge(OH)2–Sn(OH)2–Pb(OH)2
E. Pb(OH)2–Sn(OH)2– Ge(OH)2
6.21. Select the strongest oxidation agent
through the listed compounds:
А. PbO
B. PbO2
C. GeO2
D. SnO
E. SnO2
6.22. Select the strongest reduction agent
through the listed ions:
А. Ge2+
B. Sn2+
C. Sn4+
D. Ge4+
E. Pb2+
6.23. Select the formulas of all oxides lead
can form
А. PbO, Pb3O4, PbO2
B. Pb3O4, PbO2
C. PbO, PbO2
D. PbO, Pb3O4
E. PbO, Pb3O4, PbO3
6.24. α-stannic acid in contrast to βstannic acid:
А. is a strong acid
B. can dissolve in acids and alkalis
C. can dissolve in alkalis
D. can dissolve in acids
E. is insoluble in water
6.25. Which of the Germanium family
elements can react with nonoxidizer acids?
А. Sn, Ge
B. Ge, Sn, Pb
C. Pb
D. Ge, Pb
E. Sn, Pb
6.26. What is the electronic
configuration of Pb2+ ion?
А. [Xe] 6s26p1
B. [Xe] 6s26p2
C. [Xe] 6s16p0
D. [Xe] 6s16p1
E. [Xe] 6s26p0
6.27. What is the electronic
configuration of Pb4+ ion?
А. [Xe] 6s16p1
B. [Xe] 6s26p0
C. [Xe] 6s06p0
D. [Xe] 6s16p0
E. [Xe] 6s16p0
Chapter 7. р-Elements of VА Group. Nitrogen and its
compounds in the negative oxidation states
7.1. Water solution of ammonia
shows:
А. reducing and acidic
B. reducing and weak basic
C. oxidizing and strong acidic
D. oxidizing, weak basic
E. oxidizing і acidic
7.2. The degree of dissociation of
ammonia increases with:
А. concentration of solution
B. adding of the salt of ammonia
C. adding of alkali
D. dilution of solution
E. cooling of solution
7.3. Specify the formula of compound
that has both ionic and covalent
bonds:
А. N2O5
B. NH4NO3
C. Са2N3
D. NH3
E. NCl3
7.4. For which of the following
compounds most characteristic
hydrogen bonds?
А. NH3
B. PH3
C. AsH3
D. CaH2
E. NaH
7.5. One of the products of hydrazine
combustion under normal
conditions are:
А. NO2
B. NH3
C. NO
D. N2O
E. N2
7.6. Nitric acid diluted HNO3 at the
reaction with one of the given
metals forms compound of
nitrogen with oxidation number 3:
А. Cu
B. Mg
C. Pt
D. Pb
E. Ag
7.7. Ammonium hydrogencarbonate
decomposes with formation of
mixture of gases:
А. N2O, CO
B. NO, CO2
C. NH3, CO2
D. NO2, CO2
E. NH3, CO
7.8. What will be the product of
reduction of nitrogen at the
reaction of nitric acid HNO3 (very
diluted) with magnesium Mg?
А. N2
B. N2O
C. NO
D. NH4NO3
E. NO2
7.9. Which one of the given metals
does not react with concentrated
nitric acid at the ordinary
conditions?
А. K
B. Ca
C. Mn
D. Fe
E. Co
7.10. At the boiling of ammonium
chloride solution with magnesium
powder following gases are
released:
А. NН3 and Н2
B. NH3
C. Н2
D. NO2 and NH3
E. NО and Н2
7.11. Very diluted nitric acid HNO3
reduces by active metals to such
compound:
А. NO2
B. NO
C. NH4NO3
D. N2O
E. N2
7.12. At the interaction of ammonia
with sodium hypochlorite one of
the products is:
А. N2H4
B. HN3
C. N2O
D. N2
E. NH2OH
7.13. Specify the reaction of medium in
an aqueous solution of
hidrazonium salt N2H5Cl.
А. acidic
B. alkaline
C. weak alkaline
D. strongly alkaline
E. neutral
7.14. What properties more typical for
hydrazine and its derivatives?
А. strong acidic
B. acidic
C. reducing and oxidizing
D. oxidizing
E. reducing
7.15. Specify the formula of substance
that can be used for draining of
ammonia.
А. Н2SO4(dil)
B. СаCl2(anhydrous)
C. Н2SO4(conc.)
D. Р2О3(solid)
E. Р2О5(solid)
7.16. Which one of the listed
compounds has the oxidation
number of nitrogen -2?
А. N2H4
B. HCN
C. NH3
D. NH4Cl
E. NH2OH
7.17. Nitrogen is formed at
decomposition of such salt of
ammonium:
А. NH4HCO3
B. .(NH4)2CO3
C. NH4NO3
D. NH4Cl
E. NH4NO2
7.18. Which of the listed electronic
configurations corresponds to the
atom of Nitrogen?
А. 1s22s22p4
B. 1s22s22p63p1
C. 1s22s22p2
D. 1s22s22p3
E. 1s22s22p5
7.19. At decomposition of what salt is
possible to get ammonia NH3?
А. NaNO3
B. NH4NO2
C. NaNO2
D. NH4HCO3
E. NH4NO3
7.20. Which one of the listed
compounds has the oxidation
number of nitrogen -1?
А. N2O
B. NH2OH
C. N2H4
D. NH4OH
E. NaNO2
7.21. As a result of decomposition of
what salt it is possible to get
nitrogen N2?
А. AgNO3
B. NH4NO3
C. KNO3
D. NH4Cl
E. NH4NO2
7.22. What from the given reactions is
the reaction of substitution?
А. NH3 + HCl →
B. Na + NH3 →
C. NH3 + CuO →
D. Cl2 + NH3 →
E. NH3 + СuSO4 →
7.23. Ammonia NH3 can burn in the
presence of the catalyst with
forming:
А. NO2
B. NO
C. N2
D. N2O
E. N2O3
7.24. Ammonia NH3 can burn in the
atmosphere of oxygen with
forming:
А. NO
B. NO2
C. N2
D. NH3
E. N2O
7.25. What is the product of reduction
of nitric acid very diluted when it
reacts with calcium: Сa + HNO3
(very diluted) →?
А. NO
B. NO2
C. N2
D. N2O
E. NH4NO3
7.26. Which one from the resulted
reactions is the reaction of
connection?
А. NO2 + NH3
B. NH3 + CuSO4
C. NH3 + Na
D. NO + H2
E. NH3 + O2
7.27. Which of the listed nitrates
hydrolyses in a water solution?
А. KNO3
B. NaNO3
C. Sr(NO3)2
D. Ba(NO3)2
E. NH4NO3
7.28. Which of the given formulas
corresponds to hydroxilamine?
А. NH2OH
B. N2H4
C. HN3
D. NaNH2
E. NH4OH
7.29. Which of the given equation
describes reaction of
hydroxilamine NH2OH with
water?
А. NH2OH+HOH=NH3 + 2OHB. NH2OH+HOH= NH4+ +2OHC. NH2OH+HOH=[NH3OH]+OHD. NH2OH+HOH=NH2+ + 2OHE. NH2OH+HOH= NH3OH+ + H+
7.30. Water solution of hydroxilamine
NH2OH has the properties:
А. weak basic
B. strong acidic
C. amphoteric
D. strong basic
E. weak acidic
Chapter 8. р-Elements of VА Group. Nitrogen and its
compounds in the positive oxidation states
8.1. In which of the resulted reactions
it is impossible to get NaNO3?
А. Cu(NO3)2 + NAOH
B. Na2CO + HNO3
C. NAOH + HNO3
D. NaCl + HNO3
E. NAOH + NO2 + NO + O2
8.2. Which of the given nitrates
decomposes with formation of a
metal?
А.
B.
C.
D.
E.
Al(NO3)2
AgNO3
Cа(NO3)2
NaNO3
Pb(NO3)2
8.3. Nitric acid diluted reacts without
formation of gaseous products of
reaction with:
А. S
B. Cu
C. Mg
D. P
E. Pb
8.4. NaNO2 has the reduction
properties when reacts with:
А. KMnO4
B. NaHCO3
C. KI
D. H2S
E. NH3
8.5. Which one of the given metals
does not react with nitricHNO3
acid?
А. Pt
B. Mg
C. Pb
D. Cо
E. Cu
8.6. Nitric acid diluted HNO3 at the
reaction with one of the given
metals forms compound of
nitrogen with oxidation number 3:
А. Pb
B. Cu
C. Ag
D. Mg
E. Pt
8.7. Choose from the following
equations one that characterizes
the property of nitrate acid form
the reaction of exchanging:
А. 5HNO3 + 3P + 2H2O =
3H3PO4 + 5NO
B. CaCO3 + 2HNO3 = Ca(NO3) 2
+ CO2 + H2O
C. 4Ca + 10HNO3 = 4Ca(NO3) 2
+ N2O + 5H2O
D. Cu2O + 6HNO3 = Cu(NO3) 2 +
2NO2 + 3H2O
E. Cu + 4HNO3 = Cu(NO3) 2
+2NO2 + 2H2O
8.8. Nitrogen released during thermal
decomposition of such ammonium
salt:
А. NH4HCO3
B. NH4NO2
C. NH4Cl
D. NH4NO3
E. .(NH4)2CO3
8.9. Which one of the given metals
does not react with concentrated
nitric acid at the ordinary
conditions?
А. Co
B. K
C. Fe
D. Mn
E. Ca
8.10. What is the product of reduction
of nitric acid diluted when it
reacts with phosphorus?
А. NO2
B. N2O
C. NH3
D. N2
E. NO
8.11. Very diluted nitric acid HNO3
reduces by active metals to such
compound:
А. N2
B. NO
C. NO2
D. N2O
E. NH4NO3
8.12. Which of the listed oxides is an
anhydride of nitric acid HNO3?
А. N2O
B. N2O3
C. N2O5
D. NO
E. NO2
8.13. Which of the listed oxides is an
anhydride of nitrous acid HNO2?
А. NO
B. NO2
C. N2O3
D. N2O4
E. N2O5
8.14. Oxides which have an acidic
properties are in a row:
А. N2O, N2O3, N2O5
B. N2O3, NO2, N2O5
C. NO, N2O3, N2O5
D. NO, N2O3, N2O5
E. N2O, NO, NO2
8.15. Concentrated nitric acid does not
react with a following simple
substance:
А. sulfur
B. phosphorus
C. carbon
D. copper
E. gold
8.16. Which one of the given metals
does not react with concentrated
nitric acid?
А. Cr
B. Zn
C. Na
D. Mg
E. Cu
8.17. What gas forms in a result of
action of the concentrated nitric
acid HNO3 on a sulfur?
А. N2O
B. N2O
C. NO2
D. NO
E. N2O
8.18. Which of the given oxides can be
oxidizing agents only:
А. NO
B. N2O4
C. NO2
D. N2O5
E. N2O3
8.19. Which of the given compounds of
nitrogen has the oxidizingreduction properties:
А. NO2
B. HNO3
C. NH3
D. NH4Cl
E. N2O5
8.20. What oxide can be obtained in the
result of reaction of nitrogen with
oxygen?
А. N2O5
B. NO
C. NO2
D. N2O5
E. N2O
8.21. Nitrogen has a positive value of
the oxidation state in the
compounds with:
А. magnesium
B. calcium
C. hydrogen
D. chlorine
E. potassium
8.22. Which of the given compounds of
nitrogen can be oxidizing agents
only?
А.
B.
C.
D.
E.
NH3
HNO3
HNO2
N2O
NO2
8.23. Choose the formula of nitrogen
oxide, which is used for
anesthesia?
А. N2O
B. NO2
C. NO
D. N2O4
E. N2О3
8.24. Which of the listed electronic
configurations corresponds to the
atom of Nitrogen?
А. 1s22s22p2
B. 1s22s22p5
C. 1s22s22p4
D. 1s22s22p63p1
E. 1s22s22p3
8.25. Nitrogen has a positive oxidation
number in compounds with:
А. calcium
B. hydrogen
C. lithium
D. oxygen
E. magnesium
8.26. What is the “royal water”?
А. Mixture of HCl and HNO3
B. Mixture of HCl and HNO2
C. Mixture of HF and HNO3
D. Mixture of HCl and HN3
E. Mixture of H2SO4 and HNO3
8.27. Decomposition of which of the
listed salts can be obtained
ammonia?
А. NH4NO3
B.
C. NaNO2
D. NH4HCO3
E. NaNO3
8.28. What nitrate is decomposed at
heating with formation of nitrite?
А. NaNO3
B. AgNO3
C. Hg(NO3)2
D. Ca(NO3)2
E. Cu(NO3)2
8.29. Nitrogen (ІІ) oxide NO
corresponds to the oxides which
are:
А. amphoteric
B. does not forming a salt
C. D. basic
E. acidic
8.30. What is the product of reduction
of nitric acid very diluted when it
reacts with calcium: Сa + HNO3
(very diluted) →?
А. NO2
B. N2O
C. N2
D. NH4NO3
E. NO
8.31. What is the product of reaction of
mercury Hg with surplus of
concentrated nitric acid HNO3?
H2O
А. Hg(NO3)2 + NO2 +
B. Hg2(NO3)2 + N2O5 + H2O
C. Hg2(NO3)2 + NO + H2O
D. Hg(NO3)2 + NO + H2O
E. Hg(NO3)2 + N2O + H2O
8.32. What is the product of reduction
of nitric acid concentrated when it
reacts with magnesium Mg?
А. N2O
B. NH3
C. NO2
D. NO
E. N2O5
8.33. What is the product of oxidation
of sulfur S with HNO3
concentrated?
А. H2SO3
B. SO2
C. S
D. H2S
E. H2SO4
8.34. Which one of the given nitrates
decomposes with formation of
oxide of metal?
А. KNO3
B. NaNO3
C. Pb(NO3)2
D. Hg(NO3)2
E. AgNO3
8.35. Choose the compound in which
nitrogen can be an oxidizing agent
only:
А. NO2
B. HNO2
C. N2O
D. KNO3
E. NH3
to give corresponding compounds:
А. Ag, NO2, O2
B. AgO, NO2
C. AgNO2, O2
D. Ag, NO2
E. AgO, N2O3
8.37. Which of the listed electronic
configurations corresponds to the
atom of nitrogen in a nitrogen
oxide (ІІІ) N2O3?
А. [He] 2s22p0
B. [He] 2s22p2
C. [He] 2s22p3
D. [He] 2s12p1
E. [He] 2s22p1
8.38. Which of the listed electronic
configurations corresponds to the
atom of nitrogen in a nitric acid
HNO3?
А. [He] 2s12p2
B. [He] 2s22p3
C. [He] 2s02p0
D. [He] 2s12p1
E. [He] 2s22p2
8.36. Silver nitrate AgNO3 decomposes
Chapter 9. р-Elements of VА Group. Phosphorus and its
compounds
9.1. What is the color of
phenolphtalien in solution of
potassium orthophosphate?
А. raspberry
B. red
C. yellow
D. colourless
E. dark blue
9.2. What is the equivalent mass of
orthophosphoric acid?
А. 32.67
B. 49
C. 24.5
D. 98
E. 49.65
9.3. Pyrophosphoric acid is prepared
by heating of orthophosphoric
acid. Which chemical formula
through the listed ones
corresponds to pyrophosphoric
acid?
А. H2[HPO3]
B. H4P2O7
C. H3PO4
D. H[H2PO2]
E. HPO3
9.4. Which chemical formula through
the listed ones corresponds to a
salt of orthophosphoric acid?
А. –
B. NaPO3
C. Na2[PO3H]
D. NaH2PO4
E. NaH2PO2
9.5. What is the oxidation state of
Phosphorus in hypophosphorus
acid?
А. +3
B. +1
C. –3
D. +5
E. +4
9.6. What is the oxidation state of
Phosphorus in phosphoric acid?
А. +4
B. –3
C. +3
D. +1
E. +5
9.7. What is the oxidation state of
Phosphorus in phosphorus acid?
А. –3
B. +3
C. +1
D. +4
E. +5
9.8. In how many stages does
dihydrogenphosphate ion
dissociate?
А. in two stages: after the first –
completely, after the second –
partly
B. in two stages: after the first –
partly, after the second –
completely
C. in two stages, after each –
partly
D. in one stage – partly
E. in one stage – completely
9.9. Which acid through the listed
ones is monoprotic?
А. phosphorus
B. pyrophosphoric
C. hypophosphorus
D. sulfuric
E. phosphoric
9.10. What ions are present in the
highest amount is the aqueous
solution of orthophosphoric acid?
А. OH–
B. HPO42–
C. H2PO4–
D. H+
E. PO43–
9.11. What products are forming when
phosphorus has been dissolving in
solution of NaOH?
А. PH3 and NaH2PO2
B. PH3 and Na2HPO3
C. PH3 and NaН2PO4
D. PH3 and Na2НPO4
E. PH3 and Na3PO4
9.12. What is the product of phosphine
oxidation with the acidic solution
of potassium permanganate?
А. –
B.
C.
D.
E.
H3PO4
HPO3
H3PO3
H3PO2
9.13. What are the products of PCl3
hydrolysis?
А. H3PO4 and HCl
B. H3PO3 and HCl
C. H3PO4 and HClO
D. H3PO2 and HCl
E. PH3 and HCl
9.14. What are the products of PCl5
hydrolysis?
А. H3PO2 and HCl
B. H3PO3 and HCl
C. H3PO4 and HClO
D. PH3 and HCl
E. H3PO4 and HCl
9.15. The is the product of
hypophosphorus acid oxidation?
А. metaphosphoric acid
B. orthophosphoric acid
C. pyrophosphoricacid
D. –
E. phosphorus acid
9.16. What are the products of the selfoxidation self-reduction reaction
of hypophosphorus acid?
А. H3PO4 and Р
B. H3PO3 and Н3РО4
C. H3PO4 and РН3
D. H3PO3 and Р
E. H3PO3 and РН3
9.17. What are the products of the selfoxidation self-reduction reaction
of phosphorus acid?
А. H3PO2 and Н3РО4
B. H3PO4 and Р
C. H3PO4 and РН3
D. H3PO2 and РН3
E. H3PO2 and Р
9.18. What compound forms when
phosphorus trioxide P2O3 is acted
by the excess of sodium
hydroxide?
А. Na3PO3
B. NaH2PO4
C. Na2HPO3
D. Na2HPO4
E. Na3PO4
9.19. What electronic configuration
corresponds to Arsenic (As)
atom?
А. [Ar]3d104s24p3
B. [Kr] 4d105s25p3
C. [Ne] 3s23p3
D. [He] 2s223
E. [Xe] 4f145d106s26p3
Chapter 10. р-Elements of VА Group. Arsenic family
elements (Arsenic, Antimony, and Bismuth)
10.1. What electronic configuration
corresponds to Antimony (Sb)
atom?
А. [Ne] 3s23p3
B. [He] 2s223
C. [Ar]3d104s24p3
D. [Kr] 4d105s25p3
E. [Xe] 4f145d106s26p3
10.2. What electronic configuration
corresponds to Bismuth (Bi)
atom?
А. [Kr] 4d105s25p3
B. [Ar]3d104s24p3
C. [He] 2s223
D. [Xe] 4f145d106s26p3
E. [Ne] 3s23p3
10.3. What electronic configuration
corresponds to Arsenic As (+3)?
А. [Ar]3d104s24p0
B. [Ar]3d104s14p1
C. [Ar]3d94s14p3
D. [Ar]3d104s24p6
E. [Ar]3d74s24p3
10.4. What electronic configuration
corresponds to Arsenic As (–3)?
А. [Ar]3d104s24p0
B. [Ar]3d94s14p3
C. [Ar]3d104s14p1
D. [Ar]3d74s24p3
E. [Ar]3d104s24p6
10.5. What electronic configuration
corresponds to Antimony Sb
(+3)?
А. [Kr] 4d105s25p6
B. [Kr] 4d95s25p1
C. [Kr] 4d85s15p3
D. [Kr] 4d95s05p3
E. [Kr] 4d105s25p0
10.6. What electronic configuration
corresponds to Bismuth Bi (+3)?
А. [Xe] 4f145d76s26p3
B. [Xe] 4f145d106s06p2
C. [Xe] 4f145d106s26p6
D. [Xe] 4f145d106s26p0
E. [Xe] 4f115d106s26p3
10.7. What electronic configuration
corresponds to Antimony Sb (–
3)?
А. [Kr] 4d95s25p1
B. [Kr] 4d95s05p3
C. [Kr] 4d105s25p6
D. [Kr] 4d105s25p0
E. [Kr] 4d85s15p3
10.8. What electronic configuration
corresponds to Arsenic As (+5)?
А. [Xe] 4f145d106s26p6
B. [Xe] 4f115d106s26p3
C. [Xe] 4f145d76s26p3
D. [Xe] 4f145d106s26p0
E. [Xe] 4f145d106s06p2
10.9. As, Sb, Bi can react with the
following acids:
А. H3PO4, HNO3, H2SO4 (diluted)
B. CH3COOH, HCl, H2SO4 conc)
C. HNO3, H2SO4 conc), HClO3
D. HCl, H3PO4, CH3COOH
E. H3PO4, HNO3, H2SO4
10.10. What is the product of Antimony
treating with concentrated
sulfuric acid?
А. H[Sb(OH)6]
B. HSbO3
C. H2S
D. Sb2(SO4)3
E. Sb2O3
10.11. What is the product of Arsenic
oxidation with concentrated
nitric acid?
А. H3AsO3
B. H3AsO4
C. As2O5
D. As2O3
E. HAsO2
10.12. What is the product of Bismuth
treating with concentrated
sulfuric acid?
А. HBiO3
B. Bi2O3
C. H2S
D. Bi2(SO4)3
E. SO3
10.13. Which of the given elements
does not react with concentrated
nitric acid?
А. S
B. Sb
C. P
D. As
E. Bi
10.14. What is the molar mass (in
g/mole) of the gas which is
releasing under the reaction of
Bismuth with diluted nitric acid?
А. 44
B. 28
C. 64
D. 32
E. 30
10.15. Which of the given oxides can
dissolve in water and sodium
hydroxide?
А. As2O3
B. Sb2O3
C. Bi2O3
D. Sb2O5
E.
10.16. Which of the given oxides series
can dissolve in water?
А. Sb2O3, Sb2O5
B. Bi2O3, Sb2O5
C. Bi2O3, Sb2O3
D. As2O3, Sb2O3
E. As2O3, As2O5
10.17. What properties Bismuth(ІІІ)
oxide posses?
А. amphoteric
B. acidic
C. those which can not form
salts
D. basic
E. combined
10.18. What properties Arsenic (ІІІ)
oxide posses?
А. basic
B. amphoteric with acidic
properties prevailing
C. amphoteric with basic
properties prevailing
D. acidic
E. those which can not form
salts
10.19. What properties Antimony(ІІІ)
oxide posses?
А. those which can not form
salts
B. amphoteric
C. acidic
D. combined
E. basic
10.20. What is the change of the
electrons donor ability of
molecules in the consequence
NH3 – PH3 – AsH3 – SbH3 –
BiH3 ?
А. −
B. increases
C. does not change
D. decreases
E. changes without any
regularity
10.21. Which of the given compounds
is the less stable and its
molecules are the less polar?
А. PH3
B. SbH3
C. NH3
D. AsH3
E. BiH3
E. Sb2S3
10.22. Which of the given compounds
posses the strongest electrons
donation ability?
А. SbH3
B. BiH3
C. AsH3
D. PH3
E. NH3
10.27. What are the products of As(III)
and Sb(III) sulfides with
ammonium sulfide interaction?
А. As2S5, Sb2S5
B. (NH4)3AsS3, (NH4)3SbS3
C. (NH4)3AsS4, Sb2S5
D. As2S5, (NH4)3SbS4
E. (NH4)3AsS4, (NH4)3SbS4
10.23. In which of the given oxides the
mass percentage of Oxygen is
the least?
А. P2O5
B. Cl2O5
C. N2O5
D. As2O5
E. Sb2O5
10.28. What are he products of
ammonium thioarsenate
treatment with hydrochloric
acid?
А. As2S5, Н2S
B. As2S3, Н2S
C. As2О5, Н2S
D. NH3, SO2
E. As2О5, SО3
10.24. In which of the given sulfides the
mass percentage of Sulfur is the
least?
А. Bi2S3
B. Sb2S3
C. As2S3
D. Al2S3
E. P2S3
10.25. In which of the given oxides the
mass percentage of Oxygen is
the least?
А. As2O3
B. Bi2O3
C. P2O3
D. N2O3
E. Sb2O3
10.26. The mixture of the elements
suldides was treated with Na2S
solution. Which of the given
sulfides does not dissolve?
А. Bi2S3
B. As2S3
C. As2S5
D. Sb2S5
10.29. What are the products of
ammonium thioarsenite
treatment with hydrochloric
acid?
А. As2S5, Н2S
B. NH3, SO2
C. As2О3, SО3
D. As2S3, Н2S
E. As2О3, Н2S
10.30. The Marsh’ reaction is based on
the following property of the
elements compounds:
А. the solubility of Arsenic
oxides in water
B. the ability of bismuthates to
posses oxidation properties
C. The interaction of Arsenic
(III) oxide with hydrochloric
acid
D. the solubility of Arsenic
sulfides in concentrated nitric
acid HNO3
E. the ability of arsin to
decompose under heating
10.31. What is the change of acidic
properties for the compounds
consequence: As(OH)3 –
Sb(OH)3 – Bi(OH)3?
А. do not change
B. −
C. change without any regularity
D. decrease
E. increase
10.32. Which of the given hydroxides
have amphoteric properties?
А. Sb(OH)3, Cr(OH)3
B. Ca(OH)2, Bi(OH)3
C. Mg(OH)2, As(OH)3
D. Bi(OH)3, As(OH)3
E. Fe(OH)2, Bi(OH)3
10.33. Which of the given hydroxides
are insoluble in water but are
soluble in acids and alkalis?
А. Bi(OH)3, Fe(OH)2
B. Bi(OH)3, As(OH)3
C. Cr(OH)3, Sb(OH)3
D. Ba(OH)2, Cu(OH)2
E. As(OH)3, Ca(OH)2
10.34. What is the product of
Antimony(III) chloride
hydrolysis reaction?
А. Sb(OH)3
B. Sb(OH)2Cl
C. SbOHCl2
D. Sb2O3
E. SbOCl
10.35. What is the product of
Antimony(III) nitrate hydrolysis
reaction?
А. Sb(OH) 2NO3
B. SbOH(NO3)2
C. Sb(OH)3
D. SbONO3
E. Sb2O3
10.36. What is the product of
Bismuth(III) chloride hydrolysis
reaction?
А. Bi(OH)2Cl
B. Bi2O3
C. BiOHCl2
D. Bi(OH)3
E. BiOCl
10.37. What is the product of
Bismuth(III) nitrate hydrolysis
reaction?
А. Bi(OH) 2NO3
B. Bi2O3
C. Bi(OH)3
D. BiOH(NO3)2
E. BiONO3
10.38. What is the molar mass (in
g/mole) of the gas which is
releasing under the hydrolysis of
calcium arsenide?
А. 92
B. 32
C. 46
D. 64
E. 78
10.39. What are the oxidation numbers
of Arsenic in the following
compounds: AsH3, Na3AsO4,
H3AsO3?
А. –3, +5, +3
B. +5, –3, +3
C. +3, +5, –3
D. +5, +3, –3
E. –3, +3, +5
10.40. What are the oxidation numbers
of Antimony in the following
compounds: Mg3Sb2,
Na[Sb(OH)6], Sb2(SO4)3?
А. –3, +3, +5
B. +5, –3, +3
C. –3, +5, +3
D. +3, +5, –3
E. +5, +3, –3
10.41. What are the oxidation numbers
of Bismuth in the following
compounds: Ca3Bi2, NaBiO3,
BiONO3?
А. +5, –3, +3
B. –3, +3, +5
C. +5, +3, –3
D. –3, +5, +3
E. +3, +5, –3
10.42. What is the change of oxidation
ability for the compounds
consequence: As+5 – Sb+5 – Bi+5
?
А. −
B. does not change
C. changes without any
regularity
D. decreases
E. increases
10.43. What is the change of reduction
ability for the compounds
consequence: As+3 – Sb+3 – Bi+3
?
А. increases
B. changes without any
regularity
C. decreases
D. does not change
E. −
the reduction agent and the sum
of the coefficients in the
following reaction:
As2O3 + Zn + HCl →
А. –1, 30
B. 0, 30
C. –1, 19
D. 0, 29
E. 0, 20
10.45. Point out the oxidation state of
the oxidation agent and the sum
of the coefficients in the
following:
K3AsO4 + KI + H2SO4 →
А. –1, 8
B. +5, 8
C. +5, 7
D. +6, 8
E. +6, 6
10.46. Point out the oxidation state of
the reduction agent and the sum
of the coefficients in the
following reaction:
Na3AsO3 + I2 + KOH →
А. +3, 8
B. +3, 6
C. 0, 8
D. 0, 10
E. +3, 7
10.44. Point out the oxidation state of
Chapter 11. р-Elements of VІІА Group. Halogens
11.1. What electronic configuration
corresponds to Bromine atom in
potassium bromate?
А. 4s24p3
B.
C.
D.
E.
4s24p5
4s24p0
4s14p6
4s04p5
11.2. What electronic configuration
corresponds to Chlorine atom in
potassium perchlorate?
А. 3s13p5
B. 3s23p0
C. 3s03p0
D. 3s1p6
E. 3s23p5
11.3. What electronic configuration
corresponds to Chlorine atom in
chlorous acid?
А. 3s23p5
B. 3s1p6
C. 3s23p2
D. 3s13p5
E. 3s23p0
11.4. What electronic configuration
corresponds to Bromine atom in
potassium hypobromite?
А. 4s24p0
B. 5s25p5
C. 5s25p4
D. 4s24p4
E. 4s24p5
11.5. What is the electronic
configuration of І– ion?
А. 6s26p4
B. 6s26p5
C. 5s25p5
D. 5s25p6
E. 5s25p4
11.6. What is the electronic
configuration of F– ion?
А. 2s02p6
B. 2s22p4
C. 2s22p5
D. 2s02p5
E. 2s22p6
11.7. What is the electronic
configuration of Br– ion?
А. 5s25p6
B. 4s14p6
C. 4s04p5
D. 4s24p6
E. 4s24p5
11.8. What is the regularity in the
oxidation properties changing in
the elements consequence F2Cl2-Br2-I2?
А. decrease
B. increase, then decrease
C. increase
D. don’t change
E. decrease, then increase
11.9. The reduction properties in the
compounds consequence HCl –
HBr – HI will:
А. decrease, then increase
B. increase, then decrease
C. decrease
D. don’t change
E. increase
11.10. The atomic radii of the elements
in the elements consequence F –
Cl – Br – I – At will:
А. increase
B. increase, then decrease
C. don’t change
D. decreaseз
E. decrease, then increase
11.11. The electronegativity of the
elements in the consequence F –
Cl – Br – I – At will:
А. decrease
B. increase
C. decrease, then increase
D. increase, then decrease
E. don’t change
11.12. The non-metallic properties of
the elements in the consequence
F – Cl – Br – I – At will:
А. decrease, then increase
B. increase
C. increase, then decrease
D. don’t change
E. decrease
11.13. Which of the given elements can
easily transform into the gaseous
state?
А. Cl
B. Br
C. At
D. F
E. I
11.14. Which of the given elements can
have only one oxidation number
in its compounds?
А. Br
B. I
C. Cl
D. F
E. At
11.15. What is the type of chemical
binding in Cl2 molecule?
А. metallic
B. hydrogen
C. covalent polar
D. ionic
E. covalent unpolar
11.16. What is the type of chemical
binding in HBr molecule?
А. ionic
B. covalent polar
C. hydrogen
D. donor-acceptor
E. covalent unpolar
11.17. The strength of the acids in the
consequence HF – HCl – HBr –
HI will:
А. decreases
B. doesn’t change
C. increases
D. —
E. changes without any
correlation
11.18. The strength and stability of the
acids in the consequence HClO –
HClO2 – HClO3 – HClO4 will:
А. decrease
B. don’t change
C. —
D. change without any
correlation
E. increase
11.19. The oxidation ability of he acids
in the row HClO – HClO2 –
HClO3 – HClO4:
А. decreases
B. doesn’t change
C. —
D. change without any
correlation
E. increases
11.20. In a compound with which of the
elements Oxygen has oxidation
+2 ?
А. F
B. Br
C. N
D. S
E. Cl
11.21. The destrouction of a glass is
based on the reaction:
А. 2HF + KOH → KHF2 + H2O
B. SiO2 + 2NaOH → Na2SiO3 +
H2O
C. SiO2 + 6HF → H2[SiF6] +
2H2O
D. SiO2 + Na2CO3 → Na2SiO3 +
CO2
E. SiO2 + 2Mg → Si + 2MgO
11.22. Hydrogen chloride may be
prepared under the reaction:
А. NaCl(solid) + H2SO4(dil) →
B. NaCl(solution) + H2SO4(conc) →
C. all reaction may be used
D. NaCl(solid) + H2SO4(conc) →
E. NaCl(solution) + H2SO4(dil) →
11.23. The industrial preparation of
chlorine is based on:
А. HClconc + MnO2 →
B. electrolysis of NaCl solution
C. HClconc + PbO2 →
D. HCldilute + MnO2 →
E. electrolysis of molten NaCl
11.24. The reaction Cl2 + H2O → HCl +
HClO belongs to the following
type of redaction-oxidation
reactions:
А. intermolecular
B. it’s not red-ox reactiopn
C. intra-molecular
D. self-oxidation self-reduction
E. −
11.25. Which of the given salts doesn’t
hydrolyze?
А. AlCl3
B. FeCl2
C. BiCl3
D. ZnCl2
E. NaClO4
11.26. The acidic solution may be
obtained by dissolving in water:
А. NaCl
B. KClO4
C. KBr
D. FeCl3
E. KI
11.27. It is possible to increase the
percent of alumunium chloride
hydrolysis by adding:
А. NaCl
B. Na2CO3
C. NH4Cl
D. ZnCl2
E. HCl
11.28. For which of the given salts the
pH of its aqueous solution is less
than 7?
А. NaBr
B. SnCl2
C. KClO4
D. KBr
E. NaCl
11.29. What products will form when
aqueous solutions of aluminium
chloride and sodium sulfide will
be mixed?
А. Al(OH)3 + H2S
B. Al2S3 + H2O
C. Al(OH)2Cl + H2S
D. AlOHCl2 + NaHS
E. Al(OH)3 +NaHS
11.30. What products will form when
aqueous solutions of CrCl3 and
Na2CO3 will be mixed?
А. CrOHCl2 + NaHCO3
B. Cr(OH)2Cl + NaHCO3
C. Cr2(CO3)3 + NaHCO3
D. Cr(OH)3 + H2CO3
E. Cr(OH)3 + NaHCO3
11.31. Which equation should be used
for calculating the hydrolysis
constant for ZnCl2?
А.
К Н 2О
Кh =
К base ⋅ К acid
B.
Кh =
10 −7
К base
C.
Кh =
D.
Кh =
E.
Кh =
10 −7
К acid
К Н 2О
К acid
10 −14
К base
11.32. Which equation should be used
for calculating the constant of
hydrolysis for ammonium
bromide?
А.
К Н 2О
h=
С salt
К
B. h = Н О
11.34. Chose the solubility product
constant expression for PbCl2
salt.
А. [Pb]·[Cl]
B. [Pb]·[Cl]2
C. [Pb2+]·[Cl–]2
D. [Pb2+]·[2Cl–]
E. [Pb2+]·2[Cl–]2
11.35. Chose the expression for
calculation the solubility of
PbCl2 salt in mol/l.
А.
K
S = 4 sp
27
B.
K sp
S =3
4
2
К base
C. h =
D.
E.
h=
Кh
Сsalt
11.33. Which equation should be used
for calculating the constant of
hydrolysis for FeCl3?
А.
10 −7
Кh =
К acid
B. К = 10 −7
h
K base
C. К = К Н 2О
h
К base ⋅ К acid
Кh =
S =5
Кh
Кh
h=
С salt
D.
C.
10 −14
К acid
E. Кh = К Н О
2
К base
K sp
108
D. S =
K sp
E.
K sp
S=
4
11.36. Chose the expression for
calculation the solubility of
AgBr salt in mol/l.
А.
K sp
S =4
27
B. S = K
sp
C.
S =3
D.
S=
E.
S =5
K sp
4
K sp
4
K sp
108
11.37. Calculate the volume of oxygen
which may be obtained under the
thermal decomposition of 1 mole
KClO3?
А. 44.8
B. 33.6
C. 11.2
D. 22.4
E. 67.2
11.38. How many liters of chlorine may
be prepared under the reaction of
3 moles of MnO2 with HCl?
А. 33.6
B. 67.2
C. 22.4
D. 11.2
E. 44.8
11.39. How many liters of chlorine may
be prepared under the reaction of
1 mole of KMnO4 with HCl?
А. 22.4
B. 44.8
C. 56
D. 67.2
E. 33.6
11.40. How many liters of chlorine may
be prepared under the reaction of
2 moles of PbO2 with HCl?
А. 67.2
B. 44.8
C. 56
D. 33.6
E. 22.4
11.41. How many liters of chlorine may
be prepared under the reaction of
0.1 mol of potassium dichromate
with HCl?
А. 6.72
B. 44.8
C. 4.48
D. 22.4
E. 11.2
Chapter 12. General characteristic of d-Elements. dElements of IВ Group. Copper, Silver, Gold
12.1. Which of the listed electronic
configurations corresponds to
Cd2+ ion?
А. [Kr]4d95s0
B. [Kr]4d105s1
C. [Kr]4d105s2
D. [Kr]4d85s2
E. [Kr]4d105s0
12.2. Which of the listed electronic
configurations corresponds to
Hg1+ ion?
А. [Xe]4f145d106s1
B. [Xe]4f145d106s1
C. [Xe]4f145d86s1
D. [Xe]4f145d96s2
E. [Xe]4f145d106s0
12.3. Which of the listed electronic
configurations corresponds to
29Сu atom?
А. [Ar] 3d10 4s1
B. [Ar] 3d8 4s2
C. [Ar] 3d7 4s2
D. [Ar] 3d9 4s2
E. [Ar] 3d6 4s2
12.4. Which of the listed electronic
configurations corresponds to
Cu2+ ion ?
А. [Ar]3d104s2
B. [Ar]3d94s0
C. [Ar]3d84s2
D. [Ar]3d84s1
E. [Ar]3d104s1
12.5. Which of the listed electronic
configurations corresponds to
47Ag atom?
А. [Kr]4d105s1
B. [Kr]4d85s1
C. [Kr]4d95s2
D. [Kr]4d85s2
E. [Kr]4d105s0
12.6. What is the electronic
configuration of Ag+ ion?
А. [Kr]4d105s0
B. [Kr]4d105s2
C. [Kr]4d85s1
D. [Kr]4d95s1
E. [Kr]4d85s2
12.7. Which of the listed electronic
configurations corresponds to
79Au atom?
А. [Xe]4f145d106s2
B. [Xe]4f145d86s2
C. [Xe]4f145d96s2
D. [Xe]4f145d106s1
E. [Xe]4f145d96s1
12.8. What electronic configuration of
ion Au3+?
А. [Xe]4f145d86s0
B. [Xe]4f145d86s1
C. [Xe]4f145d96s2
D. [Xe]4f145d96s1
E. [Xe]4f145d106s0
12.9. What is the mass percentage of
mercury in mercury (I) chloride
(calomel)?
А. 79%
B. 91%
C. 85%
D. 48%
E. 52%
12.10. The most important minerals of
copper are chalcocite and
malachite. What are the chemical
formulas of these minerals?
А. Cu2S, (CuOH)2CO3
B. CuO, Cu(NO3)2
C. CuS CuCl2
D. (CuOH)2CO3, CuF2
E. CuFeS2, Cu2O
12.11. What is the chemical formula of
the natural mineral cinnabar?
А. ZnS
B. CdS
C. HgS
D. Hg2S2
E. Hg2S
12.12. What metal through the listed
ones exists in a liquid state at
STP:
А. cadmium
B. zinc
C. none of the listed metals
D. mercury
E. all listed metals
12.13. What oxidation states are the
most typical for cadmium:
А. +2, +3
B. +1
C. +2, +1
D. +2
E. +3
12.14. What coordination numbers are
common for zinc in coordination
compounds?
А. 2, 4
B. 2, 6
C. 4, 5
D. 4, 6
E. 3,6
12.15. What oxidation states are the
most typical for copper in its
compounds?
А. +1, +4
B. +1, +2
C. +1, +3
D. +2, +4
E. +2, +3
12.16. What oxidation state is the most
typical for gold in its
compounds?
А. +2, +3
B. +1, +2
C. +2, +5
D. +1, +3
E. +3, +4
12.17. What oxidation state is the most
typical for silver in its
compounds?
А. +3
B. +1
C. +4
D. +5
E. +2
12.18. The chemical activity of
substances in the consequence
Cu–Ag–Au will:
А. increase firstly, then decrease
B. decrease
C. decrease firstly, then increase
D. do not change
E. increase
12.19. Silver and copper can not
dissolve in:
А. concentrated sulfuric acid
B. aqua regia (a mixture of
hydrochloric and nitric acids)
C. diluted hydrochloric and
sulfuric acids
D. diluted nitric acid
E. concentrated nitric acid
12.20. Which metal can not be oxidized
on air, even at strong heating:
А. nickel
B. zinc
C. copper
D. gold
E. iron
12.21. In what acids through the listed
ones silver may be dissolved?
А. HCl, HNO3(conc.)
B. HNO3(dil.), H2SO4(dil.),
C. H2SO4(conc.), HCl
D. H2SO4(conc.), HNO3(dil.)
E. HCl, HNO3(dil.)
12.22. What are the products of the
reaction of gold dissolving in
aqua regia (a mixture of
hydrochloric and nitric acids):
А. Au(NO3)3, AuCl3, H2O
B. AuCl3, NO2, H2O
C. H[AuCl4], NO2, H2O
D. H2[AuOCl3], NO, H2O
E. H[AuCl4], NO, H2O
12.23. What will be the product of
reduction of diluted nitric acid
HNO3 by zinc?
А. NH4NO3
B. N2O
C. NO
D. N2
E. NO2
12.24. What will be one of the products
of the reaction between zinc and
diluted sulfuric acid?
А. H2
B. H2S
C. SO3
D. SO2
E. S
12.25. What will be the product of
reduction of concentrated sulfuric
acid H2SO4 by zinc?
А. S or H2S
B. SO2 or H2S
C. H2
D. S
E. SO2 or S
12.26. Which IIB group metals through
the listed ones do not react with
alkalis?
А. Zn, Cd
B. Cd, Hg
C. Cd
D. Zn, Hg
E. Zn, Hg, Cd
12.27. What compounds (listed in pairs)
have amphoteric properties?
А. Cu(OH)2, Au(OH)3
B. Cu2O, Ag2O
C. Au2O3, Ag2O
D. Cu2O, Au(OH)3
E. Cu(OH)2, AuOH
12.28. The concentration of H+ ions in
copper nitrate Cu(NO3)2 solution
is 1·10–5 mol/l. What is the рН of
this solution?
А. 13
B. 1
C. 7
D. 5
E. 9
12.29. What products are forming under
the hydrolysis of copper sulfate
CuSO4?
А. the salt does not hydrolyze
B. acidic salt and basic salt
C. basic salt and acid
D. acidic salt and base
E. base and acid
12.30. What product forms under the
reaction between copper sulfate
CuSO4 and the excess of
potassium hydroxide KOH?
А. K2[Cu(OH)4]
B. [Cu(OH)2(H2O)2]
C. the reaction does not occur
D. [Cu(H2O)4](OH)2
E. K[Cu(OH)3]
12.31. What product forms under the
reaction between copper sulfate
CuSO4 and the excess of
ammonium hydroxide NH4OH?
А. [Cu(OH)2(NH3)2]
B. [Cu(NH3)4]SO4
C. [Cu(NH3)2](OH)2
D. Cu(OH)2
E. [Cu(NH3)2(H2O)2]SO4
12.32. What reagent should be used for
identification Cu2+ ions in
solution?
А. K2[HgI4]
B. NaCl
C. Na3[Ag(S2O3)2]
D. NаOH(excess)
E. NH4OH(excess)
12.33. What are the products of the
reaction between silver nitrate
AgNO3 and solution of sodium
hydroxide NaOH?
А. Ag2O, NaNO3, H2
B. Ag2O, NaNO3, H2O
C. AgOH NaNO3
D. the reaction does not occur
E. AgNO2, Na, H2O
12.34. Complete and balance the
reaction of a coordination
compound formation:
D.
AgBr + Na2S2O3(excess) → ... .
Point out the sum of the
coefficients in the equation.
А. 8
B. 7
C. 5
D. 6
E. 4
E.
12.35. What products are forming in the
reaction of an Ag(I) compound
with formaldehyde (reaction of
“silver mirror”):
А. Ag, HCOOH
B. Ag H2CO3
C. Ag2O, СН3OН
D. Ag CO2, H2O
E. Ag2CO3, H2O
12.36. What is the molecular formula of
diammindithiocyanocopper (II)?
А. [Cu(NH3)2(SCN)2]
B. [Cu(NH3)2(CN)2]
C. (NH4)2[Cu(SCN)4]
D. [Cu(NH3)4](CN)2]
E. (NH4)2[Cu(CN)4]
12.37. Which equation through the
listed ones is the mathematical
expression for the ionization
constant of [Au(OH)Cl3]+
complex ion?
А.
[Au(OH)Cl 3 ] +
Кн =
[Au 3+ ] ⋅ [OH − ] ⋅ [Cl − ] 3
B.
[ Au 3+ ] ⋅ [ Au( OH)Cl 3 ] +
Кн =
[OH − ] ⋅ [Cl − ] 3
C.
[OH − ] ⋅ [Cl − ] 3
Кн =
[ Au 3+ ] ⋅ [ Au(OH)Cl 3 ] +
Кн =
Кн =
[Au 3+ ] ⋅ [OH − ] ⋅ [Cl − ]
[Au(OH)Cl 3 ] +
[Au 3+ ] ⋅ [OH − ] ⋅ [Cl − ]3
[Au(OH)Cl 3 ]+
12.38. What will be the color of methyl
orange indicator in the gold(III)
chloride AuCl3 solution?
А. blue
B. yellow
C. orange
D. pink
E. purple
12.39. What are the oxidation numbers
of the central metal ions in the
coordination compounds
[Cu(NH3)4]SO4 and H[AuCl4],
respectively?
А. +3, +2
B. +2, +3
C. +3, +1
D. +1, +2
E. +2, +1
12.40. What coordination numbers are
the most typical for Cu2+ as a
central metal ion in coordination
compounds?
А. 6, 8
B. 4, 6
C. 2, 4
D. 4, 8
E. 2, 6
12.41. What ІІВ group elements have
amphoteric properties?
А. zinc and cadmium
B. cadmium and mercury
C. zinc only
D. mercury only
E. all elements
12.42. Which ion through the listed ones
will form under the reaction of
zinc dissolving in alkalis?
А. ZnO22–
B. [Zn(H2O)4]2+
C. [Zn(NH3)4]2+
D. [Zn(OH)4]2–
E. [ZnCl4]2–
12.43. What are the products of the
reaction between mercury(II)
nitrate Hg(NO3)2 and solution of
potassium hydroxide KOH?
А. Hg+KNO3+H2O
B. HgO+KNO3+H2O
C. HgNO3+KNO2+H2O
D. HgNO3+KNO3+H2O
E. Hg+KNO2+H2O
12.44. What products are forming under
the hydrolysis of zinc sulfate
ZnSO4?
А. base and acid
B. acidic salt and base
C. basic salt and acid
D. acidic salt and basic salt
E. the salt does not hydrolyze
12.45. What will be the color of methyl
orange indicator in zinc sulfate
ZnSO4 solution?
А. purple
B. colourless
C. orange
D. yellow
E. pink
12.46. Mercury forms compounds in
which it has oxidation numbers
+1 or +2. In which of the listed
compounds mercury has +2
oxidation state?
А. Hg2Cl2
B. Hg2(NO3)2•2H2O
C. Hg2O
D. Hg2SO4
E. K2[HgI4]
12.47. What ion through the listed ones
is the central ion in the
coordination compound
K2[HgI4]?
А. K+
B. I–
C. HgI42–
D. Hg2+
E. K2[HgI4]
12.48. Complete and balance the
equation of the reaction:
AgNO3 + KOH → ... . Point out
the sum of the coefficients in the
equation.
А. 9
B. 12
C. 6
D. 8
E. 11
12.49. Complete and balance the
equation of the reaction:
Hg(NO3)2 + NaOH → ... . Point
out the sum of the coefficients in
the equation.
А. 12
B. 8
C. 6
D. 7
E. 9
12.50. Complete and balance the
equation of the reaction:
Hg2(NO3)2 + NaOH → ... . Point
out the sum of the coefficients in
the equation.
А. 9
B. 12
C. 8
D. 11
E. 6
Chapter 13. d-Elements of IІВ Groups. Zinc, Cadmium,
Mercury
13.1. Which of the listed electronic
configurations corresponds to
Cd2+ ion?
А. [Kr]4d105s0
B. [Kr]4d105s1
C. [Kr]4d105s2
D. [Kr]4d85s2
E. [Kr]4d95s0
13.2. Which of the listed electronic
configurations corresponds to
Hg1+ ion?
А. [Xe]4f145d106s1
B. [Xe]4f145d86s1
C. [Xe]4f145d106s1
D. [Xe]4f145d96s2
E. [Xe]4f145d106s0
13.3. What is the mass percentage of
mercury in mercury (I) chloride
(calomel)?
А. 52%
B. 48%
C. 79%
D. 91%
E. 85%
13.4. What is the chemical formula of
the natural mineral cinnabar?
А. Hg2S2
B. ZnS
C. HgS
D. Hg2S
E. CdS
13.5. What metal through the listed
ones exists in a liquid state at
STP:
А. none of the listed metals
B. cadmium
C. mercury
D. all listed metals
E. zinc
13.6. What oxidation states are the
most typical for cadmium:
А. +3
B. +2, +3
C. +2
D. +1
E. +2, +1
13.7. What coordination numbers are
common for zinc in coordination
compounds?
А. 4, 5
B. 2, 6
C. 3,6
D. 2, 4
E. 4, 6
13.8. What will be the product of
reduction of diluted nitric acid
HNO3 by zinc?
А. NO2
B. N2O
C. N2
D. NH4NO3
E. NO
13.9. What will be one of the products
of the reaction between zinc and
diluted sulfuric acid?
А. SO2
B. S
C. SO3
D. H2
E. H2S
13.10. What will be the product of
reduction of concentrated
sulfuric acid H2SO4 by zinc?
А. SO2 or H2S
B. S
C. S or H2S
D. SO2 or S
E. H2
13.11. Which IIB group metals through
the listed ones do not react with
alkalis?
А. Zn, Cd
B. Zn, Hg, Cd
C. Cd, Hg
D. Cd
E. Zn, Hg
13.12. What ІІВ group elements have
amphoteric properties?
А. zinc only
B. cadmium and mercury
C. mercury only
D. zinc and cadmium
E. all elements
13.13. Which ion through the listed
ones will form under the reaction
of zinc dissolving in alkalis?
А. [Zn(H2O)4]2+
B. [Zn(NH3)4]2+
C. [ZnCl4]2–
D. ZnO22–
E. [Zn(OH)4]2–
13.14. What are the products of the
reaction between mercury(II)
nitrate Hg(NO3)2 and solution of
potassium hydroxide KOH?
А. HgNO3+KNO2+H2O
B.
C.
D.
E.
HgNO3+KNO3+H2O
Hg+KNO2+H2O
HgO+KNO3+H2O
Hg+KNO3+H2O
13.15. What products are forming under
the hydrolysis of zinc sulfate
ZnSO4?
А. basic salt and acid
B. acidic salt and basic salt
C. acidic salt and base
D. base and acid
E. the salt does not hydrolyze
13.16. What will be the color of methyl
orange indicator in zinc sulfate
ZnSO4 solution?
А. yellow
B. orange
C. colourless
D. purple
E. pink
13.17. Mercury forms compounds in
which it has oxidation numbers
+1 or +2. In which of the listed
compounds mercury has +2
oxidation state?
А. Hg2O
B. Hg2SO4
C. Hg2Cl2
D. K2[HgI4]
E. Hg2(NO3)2•2H2O
13.18. What ion through the listed ones
is the central ion in the
coordination compound
K2[HgI4]?
А. K+
B. Hg2+
C. I–
D. K2[HgI4]
E. HgI42–
13.19. Complete and balance the
equation of the reaction:
Hg(NO3)2 + NaOH → ... . Point
out the sum of the coefficients in
the equation.
А. 7
B. 9
C. 6
D. 12
E. 8
Hg2(NO3)2 + NaOH → ... . Point
out the sum of the coefficients in
the equation.
А. 8
B. 9
C. 12
D. 11
E. 6
13.20. Complete and balance the
equation of the reaction:
Chapter 14. d-Elements of VІВ Group. Chromium elements
family
14.1. Which of the listed electronic
configurations corresponds to
Cr6+ ion?
А. [Ar]3d04s1
B. [Ar]3d44s0
C. [Ar]3d54s0
D. [Ar]3d54s0
E. [Ar]3d04s0
14.2. Which of the listed electronic
configurations corresponds to
Cr3+ ion?
А. [Ar]3d44s1
B. [Ar]3d54s0
C. [Ar]3d34s0
D. [Ar]3d54s1
E. [Ar]3d44s0
14.3. Which of the listed electronic
configurations corresponds to
Cr2+ ion?
А. [Ar]3d34s0
B. [Ar]3d24s0
C. [Ar]3d44s0
D. [Ar]3d54s0
E. [Ar]3d44s1
14.4. Which of the listed electronic
configurations corresponds to the
atom of Chromium?
А. [Ar]3d64s1
B. [Ar]3d44s2
C. [Ar]3d54s1
D. [Ar]3d44s1
E. [Ar]3d54s2
14.5. Which of the listed electronic
configurations corresponds to
Molybdenum atom?
А. [Kr]3d54s2
B. [Kr]3d44s1
C. [Kr]3d54s1
D. [Kr]3d64s1
E. [Kr]3d44s2
14.6. Which of the listed electronic
configurations corresponds to the
atom of Tungsten?
А. [Xe]4d55s1
B.
C.
D.
E.
[Xe]4d45s2
[Xe]4d45s1
[Xe]4d65s1
[Xe]4d55s2
14.7. Chromium can form stable
compounds in which it has the
following oxidation numbers:
А. +1; +5; +6
B. +1; +2; +6
C. +2; +4; +6
D. +2; +3; +6
E. +2; +3; +4
14.8. What oxidation state is the most
typical for Molybdenym?
А. +6
B. +4
C. +5
D. +3
E. +2
14.9. What oxidation state is the most
typical for Tungsten?
А. +6
B. +3
C. +4
D. +5
E. +2
14.10. The reduction properties of the
elements in the consequence of
Cr–Mo–W will:
А. the most typical for Mo
B. increase from W to Cr
C. increase
D. do not change
E. decrease
14.11. What are the products of the
oxidation reaction of Cr and Mo
by the oxygen of the air?
А. Cr2O3, Mo2O3
B. CrO3, MoO3
C. Cr2O3, MoO3
D. CrO, Mo2O3
E. CrO, MoO3
14.12. What are the products of the
oxidation reaction of Cr and W
by the oxygen of the air?
А. CrO, W2O3
B. CrO, WO3
C. Cr2O3, W2O3
D. Cr2O3, WO3
E. CrO3, WO3
14.13. Which one of the following
metals may be prepared by the
reduction its oxide with
aluminium?
А. Re
B. Tc
C. W
D. Mo
E. Cr
14.14. What compounds of
Molybdenum should be reduced
with hydrogen to get metallic
Molybdenum?
А. MoO3 or Na2MoO4
B. Mo2O3 or MoF6
C. MoO3 or MoF6
D. Mo2O3 or MoO3
E. Na2MoO4 or MoF6
14.15. What compounds of Tungsten
should be reduced with hydrogen
to get metallic Tungsten?
А. Na2WO4 or WF6
B. WO3 or Na2WO4
C. WO3 or WF6
D. W2O3 or WF6
E. W2O3 or WO3
14.16. In which of the listed acids
chromium dissolves at room
temperature?
А. HCl, H2SO4
B. HCl, H2SO4(conc.)
C. HNO3 (conc.), H2SO4(conc.)
D. HCl, HNO3 (conc.)
E. HNO3, H2SO4(conc.)
14.17. Chromium can be dissolved in:
А. HNO3 (dilut.)
B. HNO3
C. H2SO4 (conc.)
D. H2SO4
E. HNO3 (conc.)
14.18. What oxidation numbers does
Chromium have in its
compounds with Oxygen?
А. +1; +2; +3; +6
B. +2; +3; +4; +6
C. +2; +3; +4; +5
D. +2; +3; +6
E. +3; +6
14.19. Specify, in what manner the
acid-base properties of the
compounds change in the
following row CrO–Cr2O3–
CrO3?
А. acidic properties decrease
B. basic properties increase
C. acid-base properties do not
change
D. acidic properties increase
E. –
C. +2
D. +4
E. +3
14.22. Which compounds of Chromium
through the listed ones have
amphoteric properties?
А. Cr2O3 and Cr(OH)3
B. CrO and Cr2O3
C. CrO and Cr(OH)3
D. CrO3 and Cr(OH)3
E. CrO and Cr(OH)2
14.23. Which compound of Chromium
through the listed ones has
amphoteric properties:
А. CrO3
B. Cr2O3
C. K2CrO4
D. Cr(OH)2
E. CrO
14.24. What will be the products of the
reaction between Na2S and CrCl3
solutions?
А. Cr(OH)3, H2S and Na2Cl
B. Cr(HS)3 and NaCl
C. –
D. Cr2S3 and NaCl
E. CrS, S and NaCl
14.20. Which of the listed compounds
of Chromium have basic
properties only?
А. CrO and Cr(OH)2
B. CrO and Cr2O3
C. Cr2O3 and Cr(OH)3
D. CrO and Cr(OH)3
E. CrO3 and Cr(OH)3
14.25. Which compounds of Chromium
through the listed ones have
acidic properties?
А. CrO
B. CrO2
C. CrO2 and CrO3
D. CrO3
E. Cr2O3
14.21. In what oxidation state should be
the atom of Chromium in its
compounds for they will be
strong reducing agents?
А. +6
B. +2 and +3
14.26. Which compound of Chromium
through the listed ones can act as
the oxidation agent only in redox reactions?
А. Cr2(SO4)3
B. K2Cr2O7
C. CrCl2
D. FeSO4
E. KI
14.27. The chemical transformation of
Cr3+ → Cr2O72– is the process of:
А. reduction in basic solution
B. reduction in acidic solution
C. oxidation in acidic solution
D. none
E. oxidation in basic solution
14.28. The chemical transformation of
Cr+3 → CrO42– is the process of:
А. reduction in basic solution
B. oxidation in acidic solution
C. reduction in neutral solution
D. oxidation in basic solution
E. reduction in acidic solution
14.29. Complete and balance the
equation of the reaction:
K2CrO4 + H2SO4 → . .
Point out the sum of the
coefficients in the equation.
А. 6
B. 5
C. 8
D. 7
E. 4
14.30. Complete and balance the
equation of the reaction:
K2Cr2O7 + KOH → . .
Point out the sum of the
coefficients in the equation.
А. 4
B. 6
C. 5
D. 7
E. 8
Chapter 15. d-Elements of VІІВ Group. Manganese elements
family
15.1. Which of the listed electronic
configurations corresponds to
Mn6+ ion?
А. [Ar]3d04s1
B. [Ar]3d54s0
C. [Ar]3d54s0
D. [Ar]3d44s1
E. [Ar]3d04s2
15.2. Which of the listed electronic
configurations corresponds to
Mn4+ ion?
А. [Ar]3d44s1
B. [Ar]3d44s0
C. [Ar]3d24s2
D. [Ar]3d14s2
E. [Ar]3d24s1
15.3. Which of the listed electronic
configurations corresponds to
Mn 7+ ion?
А. [Ar]3d04s0
B. [Ar]3d54s0
C. [Ar]3d04s1
D. [Ar]3d44s0
E. [Ar]3d54s1
15.4. Which of the listed electronic
configurations corresponds to
Mn2+ ion?
А. [Ar]3d24s1
B. [Ar]3d04s2
C. [Ar]3d44s1
D. [Ar]3d34s2
E. [Ar]3d54s0
15.5. Which of the listed electronic
configurations corresponds to
atom of Mn?
А. [Ar]3d44s2
B. [Ar]3d64s1
C. [Ar]3d34s2
D. [Ar]3d54s2
E. [Ar]3d44s1
15.6. Which of the listed electronic
configurations corresponds to
atom of Technetium?
А. [Kr]4d44s1
B. [Kr]4d44s2
C. [Kr]4d34s2
D. [Kr]4d64s1
E. [Kr]4d54s2
15.7. Which of the listed electronic
configurations corresponds to
atom of Rhenium?
А. [Xe]5d65s1
B. [Xe]5d55s2
C. [Xe]5d55s1
D. [Xe]5d45s2
E. [Xe]5d45s1
15.8. Manganese forms a stable
compounds in the following
oxidation states:
А. +2; +3; +4; +6; +7
B. +2; +3; +4
C. +1; +5; +6; +7
D. +2; +4; +5; +7
E. +1; +2; +6
15.9. What oxidation state is the most
typical for Technetium?
А. +2
B. +5
C. +7
D. +6
E. +4
15.10. What oxidation state is the most
typical for Rhenium?
А. +3
B. +6
C. +7
D. +4
E. +5
15.11. Point out in what oxidation state
Manganese and Chlorine have
similar chemical properties:
А. +7
B. +2
C. +3
D. 0
E. +4
15.12. How does ionization energy
change in the row Mn–Tc–Re?
А. increases
B. Increases from Re to Tc
C. the least for Tc
D. diminishes
E. The greatest for Tc
15.13. In the electrochemical series of
metals left-of-hydrogen is
situated:
А. Technetium
B. Manganese and Technetium
C. Rhenium
D. Technetium and Rhenium
E. Manganese
15.14. In the electrochemical series of
metals right-of-hydrogen is
situated:
А. Manganese
B. Manganese and Technetium
C. Technetium and Rhenium
D. Technetium
E. Rhenium
15.15. Industrial method of manganese
obtaining is reduction of:
А. Mn2O3
B. MnO
C. MnO3
D. MnO2
E. Mn2O7
15.16. Pure Rhenium is obtained by the
reduction (with the help of
hydrogen) of the compound:
А. ReO
B. KReO4
C. ReO2
D. ReO3
E. ReO2 або ReO3
15.17. What substances are used in
industrial method of manganese
obtaining as reducing agents?
А. Si
B. H2 або Si
C. Si або C
D. H2 або C
E. H2
15.18. What substance is used in
industrial method of Rhenium
obtaining as reducing agent?
А. H2
B. Si або C
C. H2 або Si
D. Si
E. H2 або C
15.19. Coordination number of VIB
group elements is:
А. 6
B. 4 і 6
C. 2
D. 4
E. 2 і 4
15.20. When oxidized with oxygen
Manganese forms:
А. MnO
B. MnO3
C. Mn2O3
D. Mn2O3
E. MnO2
15.21. Technetium and Rhenium are
burnt down with the forming of:
А. Tc2О3, Re2О7
B. Tc2О3, Re2О3
C. Tc2О7, Re2О7
D. TcО3, ReО3
E. Tc3О4, Re3О4
15.22. When Rhenium is dissolved in
nitric acid it forms:
А. Re2O7
B. ReO3
C. HReO4
D. Re(NO3)4
E. Re(NO3)2
15.23. When Manganese is dissolved in
nitric acid it forms:
А. MnO3
B. HMnO4
C. MnO2
D. Mn(NO3)2
E. Mn(NO3)4
15.24. Which of the Manganese
compounds displays amphoteric
properties?
А. MnO
B. MnO3
C. Mn2O3
D. Mn2O7
E. MnO2
15.25. Which of the Manganese
compounds display basic
properties?
А. MnO і Mn2O3
B. Mn2O3 і MnO2
C. MnO2 і MnO3
D. MnO3 і Mn2O7
E. MnO2
15.26. Which of the Manganese
compounds display acidic
properties?
А. Mn2O3 і MnO2
B. MnO і Mn2O3
C. MnO3 і Mn2O7
D. MnO2 і MnO3
E. MnO2
15.27. Changing of acid-basic
properties in compounds MnO –
MnO2 – Mn2O7 corresponds to
such rule:
А. acidic properties intensify
B. acid-basic properties don’t
change
C. no answer is right
D. acidic properties decreases
E. basic properties intensify
15.28. Which of the listed Manganese
compounds can undergo selfreduction self-oxidation reaction
in solution?
А. K2MnO4
B. KMnO4
C. MnCl2
D. Mn(NO3)2
E. MnO2
15.29. Which of the listed Manganese
compounds can’t be isolated in
free state?
А. HMnO4
B. MnO
C. H2MnO4
D. Mn2O3
E. MnO2
15.30. What Manganese compound is
formed in the reaction of
potassium permanganate
reduction in basic solution?
А. MnO2
B. Mn(OH)4
C. К2MnO4
D. MnO
E. MnSO4
15.31. What Manganese compound is
formed in the reaction of
potassium permanganate
reduction in acidic solution?
А. Mn(OH)2
B. К2MnO4
C. MnO
D. MnO2
E. MnSO4
15.32. What Manganese compound is
formed in the reaction of
potassium permanganate
reduction in neutral solution?
А. MnSO4
B. MnO2
C. MnO
D. Mn(OH)2
E. К2MnO4
15.33. Which one of the listed
compounds displays only
oxidizing properties in redox
processes?
А. Mn2O3
B. K2MnO4
C. KMnO4
D. MnCl2
E. MnO2
15.34. According to standard redox
potentials values find the
reaction where Manganese is the
strongest oxidizer:
А. MnO2 + 4H+ + 2e– = Mn2+ +
2H2O; E0 = 1,28 V
B. MnO4– + 4 H2O + 3e– =
Mn(ОH)4 + 4OH– ; E0 = 0,57
V
C. MnO4– + 8H+ + 5e– = Mn2+
+ 4H2O; E0 = 1,51 V
D. MnO4– + e– = MnO42– (alkali
medium); Е0 = 0,54 V
E. MnO42– + 4H2O + 2e– =
Mn(OH)4 + 4OH– ; E0 =
0,71 V
15.35. What substance is obtained in
the reaction of thermal
decomposition of potassium
permanganate?
А. O2
B. KOH
C. H2
D. H2O2
E. Mn(OH)2
А. Reduction in acidic solution
B. Reduction in basic solution
C. Reduction in neutral solution
D. Oxidation in acidic solution
E. Oxidation in basic solution
15.37. Complete equation of
reaction and balance it
the
Mn + O2 → ... .
Point out sum of the coefficients
in the equation.
А. 6
B. 4
C. 7
D. 5
E. 3
15.36. Explain the transformation
MnO4– → MnO2
Chapter 16. d-Elements of VІІІВ Group. Cobalt and Nickel
compounds. Platinum metals
16.1. Which of the listed electronic
configurations corresponds to
Fe3+ion
А. [Ar] 3d5 4s1 4p1
B. [Ar] 3d5 4s0
C. [Ar] 3d3 4s2
D. [Ar] 3d3 4s1 4p1
E. [Ar] 3d4 4s1
16.2. What is the oxidization number
of central ion in coordination
compounds Na2[Fe(CN)5NO]?
А. 0
B. +3
C. +2
D. +1
E. +6
16.3. Which of the listed electronic
configurations corresponds to Fe
atom?
А. 3d84s2
B. 3d74s2
C. 3d54s1
D. 4d65s2
E. 3d64s2
16.4. Which of the listed electronic
configurations corresponds to
Co2+ ion?
А. 3d74s0
B. 3d64s2
C. 4d75s2
D. 3d54s2
E. 3d74s2
16.5. Which of the listed electronic
configurations corresponds to Ni
atom?
А. 3d64s2
B. 4d85s2
C. 3d74s2
D. 3d84s2
E. 3d84s0
16.9. What is the maximal oxidization
number of Fe in its compounds?
А. 2
B. 6
C. 8
D. 4
E. 3
16.10. Complete and balance the
equation of the reaction:
0
16.6. Which of the following
equations represents the process
of corrosion of iron:
А. 4Fe + 8H2O + 3O2 →
4Fe(OH)3
B. Fe + 2H2O → Fe(OH)2
C. 4Fe + 2H2O → 2Fe2O3
D. 2Fe + O2 → 2FeO
E. 3Fe + 4H2O → Fe3O4 + 4H2
16.7. Complete and balance the
equation of the reaction:
Ni + CO
t
→
Point out the sum of the
coefficients in the equation.
А. 6
B. 12
C. 8
D. 5
E. 9
16.11. Complete and balance the
equation of the reaction:
Fe(OH)3 + NaOH →
K4[Fe(CN)6]+ Cl2 →
Point out the sum of the
coefficients in the equation.
А. 10
B. 3
C. 5
D. 6
E. 4
Point out the sum of the
coefficients in the equation.
А. 7
B. 6
C. 5
D. 9
E. 11
16.8. Complete and balance the
equation of the reaction:
16.12. Complete and balance the
equation of the reaction:
FeCl2 + K3[Fe(CN)6] →
FeSO4 + KCN →
Point out the sum of the
coefficients in the equation.
А. 6
B. 5
C. 9
D. 10
E. 12
Point out the sum of the
coefficients in the equation.
А. 15
B. 8
C. 9
D. 11
E. 6
16.13. Which one of the listed element
has the following electronic
configurations: 3d74s2?
А. Rh
B. Mn
C. Ni
D. Fe
E. Co
16.14. A mineral cobalt glance or
cobaltite has the following
structure:
А. CoS
B. CoAs
C. Co2O3
D. CoAsS
E. CoO
16.15. The most stable complexes with
amino carbonic acids form ions
of:
А. Mn, Mg, Zn
B. Mn, Ni, Fe
C. Cu, Zn, Co
D. Fe, Mn, Mg
E. Co, Fe, Zn
16.16. In which of the following
reactions it is possible to get the
iron(ІІІ) chloride:
А. Fe(NO3) 3 + HCl→
B. Fe(OH)3 + HCl →
C. Fe2O3 + Cl2 →
D. Fe + HCl →
E. Fe2(SO4) 3 + HCl →
16.17. An iron-stone - hematite has the
following structure:
А. FeO
B. FeO(OH)
C. Fe2O3
D. FeS2
E. Fe3O4
16.18. The products of igniting a pyrite
are:
А. Fe + SO3
B. Fe + SO2
C. Fe3O4 + SO2
D. FeO + SO2
E. Fe2O3 + SO2
16.19. Iron forms a carbide with
metallic conductivity, which has
the following composition:
А. FeC3
B. FeC
C. Fe3C4
D. Fe2C
E. Fe3C
16.20. An iron-stone - magnetite has
the following structure:
А. FeO
B. Fe3O4
C. FeS2
D. FeO(OH)
E. Fe2O3
16.21. Which compounds can form
iron(ІІІ) hydroxide as a product
of reaction?
А. Fe2O3 + H2O
B. Fe + NaOH
C. Fe2O3 and NaOH
D. FeCl3 and NaOH
E. FeCl3 + H2O
16.22. Pyrite is:
А. Fe2O3
B. FeSO4⋅7H2O
C. Fe3O4
D. FeS2
E. FeS
16.23. Which of the listed acid
dissolves iron at a room
temperature and forms the salts
of Fe(III)
А. HNO3 diluted
B. H2SO4 diluted
C. HCl
D. HNO3 conc
E. H2SO4 conc
16.24. For analytical determination of
the Fe2+ ions red prussiate of
potash salt is used. Its formula:
А. K4[Fe(CN)6]
B. K4[Fe(OH)6]
C. KFe[Fe(CN)6]
D. K3[Fe(CN)6]
E. K4[Fe(CNS) 6]
16.25. Which one of the given
compounds is used as a reagent
on the ions of iron (ІІІ)?
А. K3[Fe(CN)6] and NH4CNS
B. K3[Fe(CN)6] and KCNS
C. KFe[Fe(CN)6] and NH4CNS
D. KCNS and HNO3
E. K4[Fe(CN)6] and KCNS
16.26. Co can force other metals out of
solutions of salts:
А. CaCl2
B. NiSO4
C. Zn(NO3)2
D. KNO3
E. AlCl3
16.27. The expression of the solubility
product constant Ksp for
Co(OH)2:
А. Ksp= [ Co2+]⋅[OH–]2
B. Ksp= [Co2+]⋅[OH–]
C. Ksp= Co2+]+2[OH–]
D. Ksp= [Co2+]⋅2[OH–]
E. Ksp= [Co]⋅[OH]2
16.28. The expression of the solubility
product constant Ksp for
Fe(OH)2:
А. Ksp= [Fe2+]+2[OH–]
B. Ksp= [Fe]⋅[OH]2
C. Ksp= [Fe2+]⋅2[OH–]
D. Ksp= [Fe2+]⋅[OH–]
E. Ksp= [Fe2+]⋅[OH–]2
16.29. The expression of the solubility
product constant Ksp for the salt
Fe2S3:
А. Ksp= 2[Fe3+]⋅3[S2–]
B. Ksp= [Fe3+]3⋅[S2–]2
C. Ksp= [Fe]2⋅[S]3
D. Ksp= [Fe3+]⋅[S2–]
E. Ksp= [Fe3+]2⋅[S2–]3
16.30. The expression of the solubility
product constant Ksp for
Ni(OH)2:
А. Ksp= [Ni2+]⋅[OH–]
B. Ksp= [Ni]⋅[OH]2
C. Ksp=[Ni2+]⋅[OH–]2
D. Ksp= [Ni2+]+2[OH–]
E. Ksp= [Ni2+]⋅2[OH–]
16.31. The red prussiate of potash
K3[Fe(CN)6] is a reagent on:
А. FeO2– ions
B. Fe3+ ions
C. Ca2+ ions
D. Fe2+ ions
E. FeO42– ions
16.32. The yellow prussiate of potash
K4[Fe(CN)6] is a reagent on:
А. Fe2+ ions
B. Fe3+ ions
C. Ca2+ ions
D. FeO42– ions
E. FeO2– ions
16.33. What is the medium of solution
of the salt FeCl2?
А. acidic
B. weak acidic
C. neutral
D. weak alkaline
E. alkaline
16.34. What is the medium of solution
of the salt CoCl2?
А. acidic
B. weak alkaline
C. alkaline
D. neutral
E. weak acidic
E. Kd =
[Co 2+ ] ⋅ [ NH 3 ]6 ⋅ [Cl − ] 2
[[Co( NH 3 ) 6 ]Cl 2 ]
16.35. What is the medium of solution
of the Ni(NO3)2 salt?
А. alkaline
B. weak acidic
C. neutral
D. acidic
E. weak alkaline
16.36. Expression of dissociation
constant Kd of complex ion
K4[Fe(CN)6]:
А. Kd = [Fe 2+ ] ⋅ [CN − ] 6
[[Fe(CN) 6 ] 4− ]
+ 4
4−
B. K = [K ] ⋅ [[Fe(CN) 6 ] ]
d
[[Fe(CN) 6 ] 4− ]
2+
−
C. Kd = [Fe ] ⋅ 6[CN ]
[[Fe(CN) 6 ] 4− ]
D. K = [[ Fe(CN ) 6 ]4− ]
d
[[ Fe(CN ) 6 ] 4− ]
E. Kd = [ K + ]4 + [[ Fe(CN ) 6 ]4− ]
[[ Fe(CN ) 6 ] 4− ]
16.37. Expression of dissociation
constant Kd of complex ion
[Со(NН3)6]Cl2:
А. K = [Co 2+ ] + [ NH 3 ] 6
d
B.
Kd =
[[Co( NH 3 ) 6 ] 2+ ]
[Co 2+ ] ⋅ [ NH 3 ] 6
[[Co( NH 3 ) 6 ] 2+ ]
C. K = [[Co( NH 3 ) 6 ] 2+ ] ⋅ [Cl − ] 2
d
[[Co ( NH 3 ) 6 ]Cl 2 ]
D.
2+
Kd = [Co ] ⋅ 6[ NH 3 ]
[[Co( NH 3 ) 6 ] 2+ ]
16.38. The Mor salt is:
А. basic salt
B. complex salt
C. double salt
D. acidic salt
E. middle salt
16.39. Fe(OH)3 has the amphoteric
properties because:
А. reacts only with acids
B. C. reacts only with bases
D. reacts with acids and bases
E. decomposes at heating
16.40. The hydrolysis of what salt is
described by ionic equation:
Fe2+ + H2O ⇄ FeOH+ + H+?
А. Fe sulfide
B. Fe sulfate
C. Fe sulfite
D. E. Fe acetate
16.41. Iron reacts with hydrochloric
acid and forms the salt:
А. FeOHCl2
B. FeCl3
C. Fe(OH)2Cl
D. FeOHCl
E. FeCl2
16.42. The hydrolysis of what salt is
described by ionic equation:
Ni2+ + H2O ⇄ NiOH+ + H+?
А. Ni nitrite
B. C. Ni chloride
D. Ni sulfide
E. Ni acetate
16.43. The color of litmus in the
solution FeCl2:
А. red
B. violet
C. colourless
D. raspberry
E. dark blue
Chapter 17. d-Elements of VІІІВ Group. Iron and its
compounds
17.1. The Mor salt is:
А. middle salt
B. basic salt
C. double salt
D. acidic salt
E. complex salt
17.2. Fe(OH)3 has the amphoteric
properties because:
А. decomposes at heating
B. C. reacts with acids and bases
D. reacts only with acids
E. reacts only with bases
17.3. The hydrolysis of what salt is
described by ionic equation:
Fe2+ + H2O ⇄ FeOH+ + H+?
А. B. Fe acetate
C. Fe sulfite
D. Fe sulfide
E. Fe sulfate
17.4. Iron reacts with hydrochloric
acid and forms the salt:
А. FeOHCl
B. FeCl3
C. FeOHCl2
D. Fe(OH)2Cl
E. FeCl2
17.5. The hydrolysis of what salt is
described by ionic equation:
Ni2+ + H2O ⇄ NiOH+ + H+?
А. Ni chloride
B. Ni acetate
C. Ni nitrite
D. Ni sulfide
E. 17.6. The color of litmus in the
solution FeCl2:
А. red
B. dark blue
C. colourless
D. raspberry
E. violet
17.7. Expression of dissociation
constant Kd of complex ion
K4[Fe(CN)6]:
А. Kd = [Fe 2+ ] ⋅ 6[CN − ]
[[Fe(CN) 6 ] 4− ]
B. Kd = [ K + ]4 + [[ Fe(CN ) 6 ]4− ]
[[ Fe(CN ) 6 ]4 − ]
C. Kd =
[[Fe(CN ) 6 ]4 − ]
[[Fe(CN ) 6 ]4 − ]
D. Kd =
[Fe 2 + ] ⋅ [CN − ] 6
[[Fe(CN) 6 ] 4− ]
E. Kd = [K + ] 4 ⋅ [[Fe(CN) 6 ] 4− ]
4−
[[Fe(CN) 6 ] ]
17.8. The red prussiate of potash
K3[Fe(CN)6] is a reagent on:
А. FeO42– ions
B. FeO2– ions
C. Fe2+ ions
D. Ca2+ ions
E. Fe3+ ions
17.9. The yellow prussiate of potash
K4[Fe(CN)6] is a reagent on:
А. FeO42– ions
B. Fe3+ ions
C. Ca2+ ions
D. FeO2– ions
E. Fe2+ ions
17.10. What is the medium of solution
of the salt FeCl2?
А. weak acidic
B. acidic
C. alkaline
D. neutral
E. weak alkaline
17.11. The red prussiate of potash
K3[Fe(CN)6] is a reagent on:
А. Fe3+ ions
B. FeO42– ions
C. Fe2+ ions
D. FeO2– ions
E. Ca2+ ions
17.12. The expression of the solubility
product constant Ksp for
Fe(OH)2:
А. Ksp= [Fe2+]⋅2[OH–]
B. Ksp= [Fe2+]+2[OH–]
C. Ksp= [Fe]⋅[OH]2
D. Ksp= [Fe2+]⋅[OH–]2
E. Ksp= [Fe2+]⋅[OH–]
17.13. The expression of the solubility
product constant Ksp for the salt
Fe2S3:
А. Ksp= [Fe3+]3⋅[S2–]2
B. Ksp= [Fe3+]⋅[S2–]
C. Ksp= [Fe]2⋅[S]3
D. Ksp= [Fe3+]2⋅[S2–]3
E. Ksp= 2[Fe3+]⋅3[S2–]
17.14. In which of the following
reactions it is possible to get the
iron(ІІІ) chloride:
А. Fe(OH)3 + HCl →
B. Fe(NO3) 3 + HCl→
C. Fe2O3 + Cl2 →
D. Fe2(SO4) 3 + HCl →
E. Fe + HCl →
17.15. An iron-stone - hematite has the
following structure:
А. FeO
B. FeO(OH)
C. Fe3O4
D. FeS2
E. Fe2O3
17.16. The products of igniting a pyrite
are:
А. FeO + SO2
B. Fe3O4 + SO2
C. Fe + SO2
D. Fe2O3 + SO2
E. Fe + SO3
17.17. Iron forms a carbide with
metallic conductivity, which has
the following composition:
А. Fe3C4
B. FeC3
C. Fe2C
D. Fe3C
E. FeC
17.18. An iron-stone - magnetite has the
following structure:
А. FeS2
B. Fe3O4
C. FeO(OH)
D. FeO
E. Fe2O3
17.19. Which compounds can form
iron(ІІІ) hydroxide as a product
of reaction?
А. Fe + NaOH
B. Fe2O3 and NaOH
C. FeCl3 and NaOH
D. Fe2O3 + H2O
E. FeCl3 + H2O
17.20. Pyrite is:
А. Fe3O4
B. Fe2O3
C. FeS
D. FeS2
E. FeSO4⋅7H2O
17.21. Which of the listed electronic
configurations corresponds to
Fe3+ion
А. [Ar] 3d5 4s0
B. [Ar] 3d3 4s2
C. [Ar] 3d5 4s1 4p1
D. [Ar] 3d3 4s1 4p1
E. [Ar] 3d4 4s1
17.22. What is the oxidization number
of central ion in coordination
compounds Na2[Fe(CN)5NO]?
А. +1
B. 0
C. +2
D. +3
E. +6
17.23. Which of the listed electronic
configurations corresponds to Fe
atom?
А. 3d54s1
B. 4d65s2
C. 3d74s2
D. 3d84s2
E. 3d64s2
17.24. Which of the following
equations represents the process
of corrosion of iron:
А. 4Fe + 8H2O + 3O2 →
4Fe(OH)3
B. 3Fe + 4H2O → Fe3O4 + 4H2
C. Fe + 2H2O → Fe(OH)2
D. 4Fe + 2H2O → 2Fe2O3
E. 2Fe + O2 → 2FeO
17.25. Complete and balance the
equation of the reaction:
Fe(OH)3 + NaOH →
Point out the sum of the
coefficients in the equation.
А. 10
B. 6
C. 4
D. 3
E. 5
17.26. Complete and balance the
equation of the reaction:
FeCl2 + K3[Fe(CN)6] →
Point out the sum of the
coefficients in the equation.
А. 5
B. 10
C. 9
D. 6
E. 12
17.27. What is the maximal oxidization
number of Fe in its compounds?
А. 3
B. 6
C. 8
D. 4
E. 2
1.1.
1.2.
1.3.
1.4.
1.5.
1.6.
1.7.
1.8.
1.9.
1.10.
1.11.
1.12.
1.13.
1.14.
1.15.
1.16.
1.17.
1.18.
1.19.
1.20.
1.21.
1.22.
1.23.
1.24.
1.25.
1.26.
1.27.
1.28.
1.29.
1.30.
1.31.
1.32.
1.33.
1.34.
1.35.
1.36.
1.37.
1.38.
1.39.
2.1.
2.2.
D
B
B
B
D
B
B
C
E
C
E
A
E
A
C
D
C
B
C
B
D
E
E
B
C
A
C
B
B
E
E
B
A
A
D
C
B
E
A
A
B
2.3.
2.4.
2.5.
2.6.
2.7.
2.8.
2.9.
2.10.
2.11.
2.12.
2.13.
2.14.
2.15.
2.16.
2.17.
2.18.
2.19.
2.20.
2.21.
2.22.
2.23.
2.24.
2.25.
2.26.
2.27.
2.28.
2.29.
2.30.
2.31.
2.32.
2.33.
2.34.
2.35.
2.36.
2.37.
2.38.
2.39.
2.40.
2.41.
2.42.
2.43.
E
E
A
D
E
D
E
D
E
B
B
A
C
E
B
D
E
E
E
D
D
A
B
C
B
C
C
D
E
D
D
D
C
E
A
C
B
C
B
D
D
2.44.
2.45.
2.46.
2.47.
2.48.
2.49.
2.50.
2.51.
2.52.
2.53.
2.54.
2.55.
2.56.
2.57.
2.58.
2.59.
3.1.
3.2.
3.3.
3.4.
3.5.
3.6.
3.7.
3.8.
3.9.
3.10.
3.11.
3.12.
3.13.
3.14.
3.15.
3.16.
3.17.
3.18.
3.19.
3.20.
3.21.
3.22.
3.23.
3.24.
3.25.
C
A
B
B
D
D
E
C
D
B
B
D
C
D
B
A
B
B
B
A
E
E
B
D
D
A
E
B
B
A
A
D
A
E
D
E
E
B
A
A
B
3.26.
3.27.
3.28.
3.29.
3.30.
3.31.
3.32.
3.33.
3.34.
3.35.
3.36.
3.37.
3.38.
3.39.
3.40.
3.41.
3.42.
3.43.
3.44.
3.45.
3.46.
3.47.
3.48.
3.49.
3.50.
3.51.
3.52.
3.53.
3.54.
3.55.
3.56.
3.57.
3.58.
3.59.
3.60.
3.61.
3.62.
3.63.
3.64.
3.65.
3.66.
A
A
C
C
A
A
C
D
C
C
B
B
D
A
C
B
A
E
C
C
B
A
B
B
E
C
D
D
C
C
B
B
A
E
B
C
A
E
B
B
C
3.67.
3.68.
3.69.
3.70.
3.71.
3.72.
3.73.
3.74.
3.75.
3.76.
3.77.
3.78.
3.79.
3.80.
4.1.
4.2.
4.3.
4.4.
4.5.
4.6.
4.7.
4.8.
4.9.
4.10.
4.11.
4.12.
4.13.
4.14.
4.15.
4.16.
4.17.
4.18.
4.19.
4.20.
4.21.
4.22.
4.23.
4.24.
4.25.
4.26.
4.27.
E
C
B
A
E
D
D
D
D
A
E
E
E
A
D
A
D
D
E
E
A
E
D
B
A
A
A
E
D
A
B
B
E
E
D
E
B
B
B
D
C
4.28.
4.29.
4.30.
4.31.
4.32.
4.33.
4.34.
4.35.
4.36.
4.37.
4.38.
4.39.
4.40.
4.41.
4.42.
4.43.
5.1.
5.2.
5.3.
5.4.
5.5.
5.6.
5.7.
5.8.
5.9.
5.10.
5.11.
5.12.
5.13.
5.14.
5.15.
5.16.
5.17.
5.18.
5.19.
5.20.
5.21.
5.22.
5.23.
5.24.
5.25.
C
A
C
B
D
E
E
D
D
E
E
A
C
B
C
B
B
E
B
B
D
B
E
C
E
D
D
C
B
A
B
B
E
C
B
D
B
D
D
A
C
5.26.
5.27.
5.28.
5.29.
5.30.
5.31.
5.32.
5.33.
5.34.
5.35.
5.36.
5.37.
5.38.
5.39.
5.40.
5.41.
5.42.
6.1.
6.2.
6.3.
6.4.
6.5.
6.6.
6.7.
6.8.
6.9.
6.10.
6.11.
6.12.
6.13.
6.14.
6.15.
6.16.
6.17.
6.18.
6.19.
6.20.
6.21.
6.22.
6.23.
6.24.
6.25.
6.26.
6.27.
E
C
B
E
B
B
C
A
E
B
C
E
C
E
D
C
C
E
A
A
E
B
E
C
E
A
E
E
B
D
B
B
D
D
D
D
D
B
B
A
B
E
E
C
7.1.
7.2.
7.3.
7.4.
7.5.
7.6.
7.7.
7.8.
7.9.
7.10.
7.11.
7.12.
7.13.
7.14.
7.15.
7.16.
7.17.
7.18.
7.19.
7.20.
7.21.
7.22.
7.23.
7.24.
7.25.
7.26.
7.27.
7.28.
7.29.
7.30.
8.1.
8.2.
8.3.
8.4.
8.5.
8.6.
8.7.
8.8.
8.9.
8.10.
8.11.
8.12.
8.13.
8.14.
B
D
B
A
E
B
C
D
D
A
C
A
A
E
B
A
E
D
D
B
E
B
B
C
E
B
E
A
C
A
D
B
C
A
A
D
B
B
C
E
E
C
C
B
8.15.
8.16.
8.17.
8.18.
8.19.
8.20.
8.21.
8.22.
8.23.
8.24.
8.25.
8.26.
8.27.
8.28.
8.29.
8.30.
8.31.
8.32.
8.33.
8.34.
8.35.
8.36.
8.37.
8.38.
9.1.
9.2.
9.3.
9.4.
9.5.
9.6.
9.7.
9.8.
9.9.
9.10.
9.11.
9.12.
9.13.
9.14.
9.15.
9.16.
9.17.
9.18.
9.19.
10.1.
E
A
C
D
A
B
D
B
A
E
D
A
D
A
B
D
A
A
E
C
D
A
A
C
A
A
B
D
B
E
B
C
C
D
A
B
B
E
B
C
C
C
A
D
10.2.
10.3.
10.4.
10.5.
10.6.
10.7.
10.8.
10.9.
10.10.
10.11.
10.12.
10.13.
10.14.
10.15.
10.16.
10.17.
10.18.
10.19.
10.20.
10.21.
10.22.
10.23.
10.24.
10.25.
10.26.
10.27.
10.28.
10.29.
10.30.
10.31.
10.32.
10.33.
10.34.
10.35.
10.36.
10.37.
10.38.
10.39.
10.40.
10.41.
10.42.
10.43.
10.44.
10.45.
D
A
E
E
D
C
A
C
B
B
D
E
E
A
E
D
B
B
D
E
E
E
A
B
A
B
A
D
E
D
A
C
E
D
E
E
E
A
C
D
E
C
B
B
10.46.
11.1.
11.2.
11.3.
11.4.
11.5.
11.6.
11.7.
11.8.
11.9.
11.10.
11.11.
11.12.
11.13.
11.14.
11.15.
11.16.
11.17.
11.18.
11.19.
11.20.
11.21.
11.22.
11.23.
11.24.
11.25.
11.26.
11.27.
11.28.
11.29.
11.30.
11.31.
11.32.
11.33.
11.34.
11.35.
11.36.
11.37.
11.38.
11.39.
11.40.
11.41.
12.1.
12.2.
A
C
C
C
D
D
E
D
A
E
A
A
E
E
D
E
B
C
E
A
A
C
D
B
D
E
D
B
B
A
D
E
D
E
C
B
B
B
B
C
B
A
E
A
12.3.
12.4.
12.5.
12.6.
12.7.
12.8.
12.9.
12.10.
12.11.
12.12.
12.13.
12.14.
12.15.
12.16.
12.17.
12.18.
12.19.
12.20.
12.21.
12.22.
12.23.
12.24.
12.25.
12.26.
12.27.
12.28.
12.29.
12.30.
12.31.
12.32.
12.33.
12.34.
12.35.
12.36.
12.37.
12.38.
12.39.
12.40.
12.41.
12.42.
12.43.
12.44.
12.45.
12.46.
A
B
A
A
D
A
C
A
C
D
D
D
B
D
B
B
C
D
D
E
A
A
B
B
A
D
C
A
C
E
B
C
A
A
E
D
B
B
C
D
B
C
E
E
12.47.
12.48.
12.49.
12.50.
13.1.
13.2.
13.3.
13.4.
13.5.
13.6.
13.7.
13.8.
13.9.
13.10.
13.11.
13.12.
13.13.
13.14.
13.15.
13.16.
13.17.
13.18.
13.19.
13.20.
14.1.
14.2.
14.3.
D
D
D
C
A
A
E
C
C
C
E
D
D
A
C
A
E
D
A
E
D
B
A
A
E
C
C
14.4.
14.5.
14.6.
14.7.
14.8.
14.9.
14.10.
14.11.
14.12.
14.13.
14.14.
14.15.
14.16.
14.17.
14.18.
14.19.
14.20.
14.21.
14.22.
14.23.
14.24.
14.25.
14.26.
14.27.
14.28.
14.29.
14.30.
C
C
B
D
A
A
E
C
D
E
C
C
A
D
B
D
A
C
A
B
A
D
B
C
D
A
B
15.1.
15.2.
15.3.
15.4.
15.5.
15.6.
15.7.
15.8.
15.9.
15.10.
15.11.
15.12.
15.13.
15.14.
15.15.
15.16.
15.17.
15.18.
15.19.
15.20.
15.21.
15.22.
15.23.
15.24.
15.25.
15.26.
15.27.
A
D
A
D
D
E
B
A
C
C
A
C
E
C
D
B
C
A
B
E
C
C
D
E
A
C
A
15.28.
15.29.
15.30.
15.31.
15.32.
15.33.
15.34.
15.35.
15.36.
15.37.
16.1.
16.2.
16.3.
16.4.
16.5.
16.6.
16.7.
16.8.
16.9.
16.10.
16.11.
16.12.
16.13.
16.14.
16.15.
16.16.
16.17.
A
C
C
E
B
C
C
A
C
E
B
B
E
A
D
A
C
B
B
A
A
C
E
D
C
B
C
16.18.
16.19.
16.20.
16.21.
16.22.
16.23.
16.24.
16.25.
16.26.
16.27.
16.28.
16.29.
16.30.
16.31.
16.32.
16.33.
16.34.
16.35.
16.36.
16.37.
16.38.
16.39.
16.40.
16.41.
16.42.
16.43.
17.1.
E
E
B
D
D
A
D
E
B
A
E
E
C
D
B
A
A
D
A
B
C
D
B
E
C
A
C
17.2.
17.3.
17.4.
17.5.
17.6.
17.7.
17.8.
17.9.
17.10.
17.11.
17.12.
17.13.
17.14.
17.15.
17.16.
17.17.
17.18.
17.19.
17.20.
17.21.
17.22.
17.23.
17.24.
17.25.
17.26.
17.27.
C
E
E
A
A
D
C
B
B
C
D
D
A
E
D
D
B
C
D
A
D
E
A
E
A
B
CONTENTS
Chapter 1. General characteristic of s-elements. Hydrogen and its compounds .......... 2
Chapter 2. s-Elements of the І group of the Periodic Table. Alkali metals ................. 6
Chapter 3. s-Elements of the ІІ groups of the Periodic Table. Beryllium,
Magnesium, and Alkaline earth metals .................................................... 11
Chapter 4. General characteristic of p-Elements. Boron and Alluminium ................ 19
Chapter 5. р-Elements of IVА Group. Carbon, Silicon ............................................ 24
Chapter 6. р-Elements of IVА Group. Germanium family elements
(Germanium, Tin, and Lead) ................................................................... 28
Chapter 7. р-Elements of VА Group. Nitrogen and its compounds in the
negative oxidation states .......................................................................... 31
Chapter 8. р-Elements of VА Group. Nitrogen and its compounds in the
positive oxidation states ........................................................................... 34
Chapter 9. р-Elements of VА Group. Phosphorus and its compounds ...................... 38
Chapter 10. р-Elements of VА Group. Arsenic family elements (Arsenic,
Antimony, and Bismuth) ......................................................................... 40
Chapter 11. р-Elements of VІІА Group. Halogens.................................................... 45
Chapter 12. General characteristic of d-Elements. d-Elements of IВ Group.
Copper, Silver, Gold ................................................................................ 50
Chapter 13. d-Elements of IІВ Groups. Zinc, Cadmium, Mercury............................ 56
Chapter 14. d-Elements of VІВ Group. Chromium elements family ........................ 58
Chapter 15. d-Elements of VІІВ Group. Manganese elements family ...................... 61
Chapter 16. d-Elements of VІІІВ Group. Cobalt and Nickel compounds.
Platinum metals ....................................................................................... 65
Chapter 17. d-Elements of VІІІВ Group. Iron and its compounds ............................ 70