Download FORMULA WRITNG

FORMULA WRITNG
Problem Set 8.1
Name: ______________________________
Hour: _____ Date: _____
Three basic rules in writing formulas:
1. Positive ion first, negative ion second.
2. Total positive charges much equal total negative charge.
3. The parentheses are used ONLY when a polyatomic ion is used more than once.
Basic rules is naming ionic compounds.
1. Name the positive ion (usually a metal) first.
(Use roman numerals to indicate charge only if there is more than one charge possible.)
2. Name the negative ion (anion) second (dropping the ending and adding –ide for monatomic ions or simply naming the
polyatomic ion.)
Correct, if necessary, the following formulas, then name.
1. BaI
________________________________ 9. (NH4) 2I
________________________________
2. Zn(NO2)
________________________________ 10. CaCl
________________________________
3. Ba(ClO4)
________________________________ 11. (NH4)(SO3) ________________________________
4. (CrO4)Li
________________________________ 12. AgS
________________________________
5. Ca(PO4)
________________________________ 13. OAl
________________________________
6. SAl
________________________________ 14. CaCO3
________________________________
7. MgBr
________________________________ 15. K(Cr2O7)
________________________________
8. Al(CH3COO) ________________________________ 16. Li(SO3)
________________________________
Write the correct formula for the following compounds.
17. Sodium Phosphate
____________________
18. Iron (III) Chloride
____________________
19. Potassium Carbonate
____________________
20. Copper (I) Hypochlorite
____________________
21. Lithium Permanganate ____________________
22. Mercuric Hydroxide
____________________
23. Zinc Bicarbonate
24. Ferrous Chloride
____________________
____________________
25. Galium (III)Hydrogen Carbonate
26. Manganese (IV) sulfide
____________________
____________________
These use the old naming system for metal ions with
more than one charge. Use the ion chart on your desks
to answer these.
Name the following compounds:
27. PbCl4
____________________________
28. CaSO4
____________________________
29. AgNO3
____________________________
30. MnF2
____________________________
31. Be(NO2) 2 ____________________________
32. ZnS
____________________________
33. Li2S
____________________________
34. Al2O3
____________________________
35. FeCl3
____________________________
36. K3N
____________________________
Write the Lewis dot structure for the most stable ion for each of the following:
37. Potassium ________
38. Sulfur
________
39. Nitrogen
________
40. Beryllium
________
41. Oxygen
________
42. Galium
________ (losing all valence e-)
43. Fluorine
________
44. Selenium
________
45. Barium
________
Write the correct formula if Calcium were to combine with the following polyatomic ions:
46. Nitrate
________________
47. Carbonate
________________
48. Dichromate ________________
49. Sulfate
________________
50. Sulfite
________________
51. Permanganate
________________
52. Phosphate
________________
53. Chlorate
________________
54. What type of compounds are we naming on this worksheet? ________________________
55. How do we recognize that they are this type of compound by looking at the formula? ___________________________
56-61. Fill in the blanks on the table below:
Number of protons
Number of Electrons
Net Charge
6
6
______
8
10
______
20
_____
+2
9
_____
-1
____
18
-1
____
18
+1
Problem Set 9.1
1) Name the following acids and identify them as either oxyacids or binary acids.
a. HCl
_____________________
______________________
b. HBr
_____________________
______________________
c. HNO3
_____________________
______________________
d. H2SO4
_____________________
______________________
e. H3PO4
_____________________
______________________
2. Name the following compounds:
1) Li2O
____________________ 6) Ca(NO2) 2 ____________________
2) Mg(OH) 2 ____________________ 7) SrSO4 ____________________
3.
3) N2O
____________________ 8) P2O5 ____________________
4) Be3N2
____________________ 9) SF6 ____________________
5) CO2
____________________ 10) SO2 ____________________
Write the formula for the following compounds:
1) Beryllium nitride
__________
6) dibromine pentaiodide ____________
2) diiodine tetraoxide
__________
7) Lead (II) sulfate
3) Copper (I) chloride
__________
8) Magnesium chromate ____________
4) Nitrogen hexafluoride
__________
9) Sodium sulfide
____________
____________
5) Manganese (III) phosphate ____________
4. Draw Lewis dot structures for each of the following compounds. (Remember that the structures for ionic compounds must
include charges for any ions and covalent compounds must have any shared electrons encircles or represented by a bond.)
a. BeF2
b. O2
c. CO2
d. Na2O
e. KF
f. PBr3
5.
a. Name 7 properties of metals.
b. The properties listed in (a) are due to metallic bonding. Describe the “electron-sea model” of metallic bonding.
c. What is an alloy?
d. Give two examples of alloys.
8.
a. Describe the difference between ionic and covalent bonding.
b. How does the difference between ionic and covalent bonding account for the difference in their properties?
9. Classify each of the following compounds as ionic, polar covalent, or nonpolar covalent.
a. CO2 ____________________________
b. Na2O ____________________________
c. N2 ____________________________
d. PCl5 ____________________________
e. CsCl ____________________________
f. CF4 ____________________________
10. Draw the lewis dot structure for the following compounds:
a. C3H8
b. C2H6
c. C2H5OH
d. N2H4
e. C2H4
e. CH3OCH3
Supplement 10.1
1) Balance the following equations:
a. __ C3H8 + __ O2  __ CO2 + __ H2O
b. __ C4H10 + __ O2  __ CO2 + __ H2O
c. __ Pb(NO3)2  __ PbO + __ NO2 + __ O2
d. __(NH4)2S + __ Ba(NO3)2  __ BaS + __ NH4NO3
e. __ NH4Cl + __ AgNO3  __ AgCl + __ NH4NO3
f. __ (NH4)2Cr2O7  __ Cr2O3 + __ N2 + __ H2O
2) Write the dissolving equation for each of the following compounds: (include subnotations- s, l, g, aq)
a. sodium bromide
b. iron (III) chloride
c. manganese (II) nitrate
d. silver sulfate
3) Indicate if each of the following compounds is soluble (S) or insoluble (I)
_____ a. barium chloride
_____ e. sodium sulfide
_____ b. silver chloride
_____ f. calcium phosphate
_____ c. barium sulfate
_____ g. ammonium carbonate
_____ d. copper (II) bromide
_____ h. magnesium hydroxide
4) Write balanced equations for the following double-replacement reactions. Include subnotations (s, l, aq, g).
a. Solutions of magnesium nitrate and sodium hydroxide are mixed.
b. Solutions of barium chloride and silver nitrate are mixed.
c. Solutions of barium hydroxide and copper (II) sulfate.
d. Solutions of ammonium sulfide and iron (III) chloride.
5) Write balanced equations for the following single-replacement reactions. If no reaction occurs, write NR.
a. Magnesium ribbon is placed into a solution of copper (II) chloride.
b. Calcium shavings are placed into a solution of magnesium nitrate.
c. Silver strips are placed into a solution of aluminum chloride.
d. Aluminum metal is placed into a solution of hydrochloric acid.
e. Lithium chunks are placed into a beaker of water.
6)
(a) When sodium metal is dropped into water, a vigorous reaction occurs. Write the balanced equation for this reaction.
(Hint: Think of H2O as HOH).
(b) What type of reaction is this?
(c) Write the equation representing the reaction of Cs with H2O.
(d) The reactions in (a) and (b) can be dangerous. Looking at your balanced equations, why do you think this is so?
(e) Why does knowing the equation for the reaction between sodium and water allow you to write equations for the reactions
between potassium and water, rubidium and water, and cesium and water?
7) Write the electron dot structures (Lewis dot structures) for the compounds made from the following elements: (Be sure to write
the structures for compounds according to whether they are ionic or covalent.)
a. Rb and O
b. Mg and S
c. C and F
d. Se and F
8) Hydrogen is considered in a family of its own. It is sometimes placed above the alkali metals and sometimes above the
halogens on the periodic table.
a) Explain how the following reaction shows how hydrogen can act like an alkali metal.
H2 (g) + Cl2 (g) 2 HCl (g)
b) Explain how the following reaction shows how hydrogen can act like a halogen.
H2 (g) + 2 Li (s) 2 LiH (s)
Supplement 10.2
1) Write balanced equations (molecular, total ionic, and net ionic) for the reaction between each of the following solutions. If no
reaction occurs, write “NR” for No Reaction.
a. barium nitrate and sodium phosphate
molecular:
total ionic:
net ionic:
b. silver nitrate and sodium sulfide
molecular:
total ionic:
net ionic:
c. Solutions of barium hydroxide and copper (II) sulfate are mixed.
molecular:
total ionic:
net ionic:
d. cesium sulfide and aluminum hydroxide
molecular:
total ionic:
net ionic:
e. Solutions of calcium chloride and copper (II) nitrate are mixed.
molecular:
total ionic:
net ionic:
Continued Back Side 
2) Write balanced equations (molecular, total ionic, and net ionic) for the following single replacement reactions. Remember to use
the activity series and include subnotations (s), (l), (aq), or (g). If there is no reaction write “NR” for no reaction.
a. Potassium metal is placed into a beaker of water.
molecular:
total ionic:
net ionic:
b. Calcium shavings are placed into a solution of copper (II) nitrate.
molecular:
total ionic:
net ionic:
c. Balls of aluminum foil are placed into a solution of lithium chloride.
molecular:
total ionic:
net ionic:
d. Aluminum metal is placed into a solution of hydrochloric acid.
molecular:
total ionic:
net ionic:
e. Zinc shot is placed into a solution of gold (III) nitrate.
molecular:
total ionic:
net ionic:
f. Aluminum metal is placed into a solution of zinc nitrate.
molecular:
total ionic:
net ionic:
Continued next page 
3) Several elements are described as follows:
Answer a-d given clues 1-5 below. (Hint: Determine to what group each element 1-5 belongs. By knowing the group you can
determine in what ratio it will react with other elements, if at all.
(a) Write the formula for the most ionic substance that can be formed from the elements shown. ___________
(b) Write the formula for a covalent compound that can be formed from any two of the above five elements. __________
(c) Would you expect compound LZ to be a solid, liquid, or gas? An ionic or covalent substance? _________, ________
(d) Write a formula for a compound formed between elements M and X; elements L and P; elements Z and X. _________
_________
_________
(1) Element M: Silvery gray in color; can be drawn into wires and rolled into sheets; first ionization energy = 175 kcal/mole;
second ionization energy = 345 kcal/mole; third ionization energy = 1,840 kcal/mole; does not react with cold water.
(2) Element P: Red solid; exist as powder; first ionization energy 252 kcal/mole; second ionization energy = 454 kcal/mole;
third ionization energy = 690 kcal/mole; fourth ionization energy 1,175 kcal/mole.
(3) Element X: Yellowish gas; very irritating when inhaled; first ionization energy 400 kcal/mole; one mole of X gas will
react with one mole of H2 to give two moles HX. Following data available: X(g) e-  X- + energy.
(4) Element Z: Colorless, flammable gas; very light; a balloon filled with molecules of the element Z will rise rapidly; first
ionization potential = 313 kcal/mole; no second ionization potential yet reported.
(5) Element L: A very light, silvery substance that floats on water and reacts violently with water; tarnishes quite rapidly in
air; first ionization energy = 99 kcal/mole; second ionization energy = 732 kcal/mole.
Supplement 10.3 (Homework Option: Short 1-6; Long 1-7)
1) (a) Write the formulas for the fluorides formed by Li, C, Na Cs, Be, K.
(b)Write the formulas for the compounds when hydrogen combines with O, N, and F.
2) Write the synthesis of each of the following compounds from their elements.
a. sodium bromide
b. potassium nitride
c. sodium carbonate
3) Write the decomposition of each of the following compounds into their elements.
a. barium iodide
b. copper (II) oxide
c. magnesium nitrate
4) Write balanced equations for each of the following:
a. synthesis of calcium phosphate from its elements
b. decomposition of iron (III) oxide into its elements
c. synthesis of ammonia (NH3) from its elements
5) Write the balanced equation for the complete combustion of each of the following:
a. ethene, C2H4
b. hexane, C6H14
c. sodium
d. aluminum
6) Write balanced equations for each of the following:
a. synthesis of lithium sulfate from its elements
b. decomposition of nickel (II) sulfide into its elements
c. solutions of potassium iodide and lead (II) nitrate are mixed
d. complete combustion of butane, C4H10
e. synthesis of diphosphorus pentoxide from its elements
f. solutions of silver nitrate and calcium bromide are mixed
7) Write balanced equations for the following: (Review of Reactions)
(a) propane gas (C3H8), which is used for heating, is burned with insufficient oxygen, the flame is yellow and smoky because
the products are elemental carbon and water vapor.
(b) Potassium chloride is synthesized from its elements
(c) Nitrogen monoxide plus oxygen gas gives nitrogen dioxide gas
(d) Copper metal is placed in a solution of magnesium fluoride.
(e) Ammonia gas burns in air to give nitrogen and water vapor (ammonia is NH3)
(f) Magnesium ribbon is placed in a solution of copper (II) chloride.
(g) Hydrogen gas and fluorine gas are allowed to mix.
(h) Hydrogen gas and chlorine gas are illuminated with ultraviolet light.
(i) Rubidium is mixed with chlorine
(j) Barium metal reacts with hydrogen gas
(k) Solutions of calcium hydroxide and copper (II) nitrate are mixed.
(l) Solutions of sodium chloride and lead (II) nitrate are mixed.
Problem Set 20.1 (Options 1-7 or 1-11)
1)
What is the main characteristic of oxidation-reduction reactions?
2) a. In terms of electrons, what happens when an atom is oxidized?
b. In terms of electrons, what happens when an atom is reduced?
3) Identify the oxidation numbers for each ATOM in the following:
a.
KBr
b. Na3PO4
c. PBr3
d. N2O4
e. NH3
4) Complete the following table:
Reaction
What is
oxidized?
What is
reduced?
What is the
oxidizing
agent?
What is the
reducing
agent?
H2S + Cl2  2 HCl + S
Cu + 2 AgNO3  2 Ag + Cu(NO3)2
N2 + 3 H2  2 NH3
2 K + Cl2  2 KCl
5) Identify the half reaction as either oxidation or reduction.
a)
Al  Al3+ + 3 e-
b) Cu2+ + 2 e-  Cu
c) Cl2 + 2 e-  2 Cld) Zn  Zn2+ + 2 e6) Which of the following reaction is NOT a redox reaction?
i)
CO + I2O5  I2 + CO2
ii) Ca + ZnCl2  Zn + CaCl2
iii) CO2 + H2O  H2CO3
iv) Mg + O2  MgO
7) Identify the oxidation number of nitrogen in each of the following compounds or ions.
a) NH3
b) N2H4
c) N2O
d) KCN
e) NO3f) NF3
8) Identify the oxidation number of sulfur in each of the following compounds or ions.
a)
SF6
b) SO42-
c) SO32-
d) Na2SO4
e) SO2
f) SF2
9) Identify the oxidation numbers for each ATOM in the following:
a) K2CrO4
b) Na2Cr2O7
c) SF6
d) PbO2
e) NaNO3
10) Complete the following table:
What is
oxidized?
Reaction
What is the
oxidizing
agent?
What is
reduced?
What is the
reducing
agent?
3 Br2 + 2 Ga  2 GaBr3
Mg + 2 HCl  H2 + MgCl2
CH4 + 2 O2  CO2 + 2 H2O
PbS + O2  PbO + SO2
11) Identify the reducing agent in each of the following:
a)
4 NH3 + 5 O2  4 NO + 6 H2O
b) Na + H2O  NaOH + ½ H2
c) 2 Ag + S  Ag2S
12) Complete the following concept map using the following terms: decreases, half-reactions, gain electrons,
reduction, lose electrons, redox reaction, oxidation, increases.
1.
consists of two
1.
2.
2.
called
3.
4.
in which atoms
5.
6.
and the oxidation number
7.
8.
3.
4.
5.
6.
7.
8.
Extra Practice Equations
Write the balanced chemical equation for the following:
1)
Ca(OH) 2 + H3PO4 ---->
Ca3(PO4) 2 + H2O
2)
C3H7OH +
CO2 + H2O
O2 ---->
3) Synthesize aluminum chloride from its elements.
4) Decompose Iron (III) sulfide into its elements
5) Toluene C7H8, is burned completely in air.
6) Aqueous sodium phosphate reacts with aqueous silver nitrate
Write a balance equation (reactants and products) for each of the following:
7.
Synthesis of Lithium chloride from its elements
8.
Decomposition of sodium nitride into its elements
9.
Synthesis of iron (III) sulfide from its elements
10.
Complete combustion of methane, CH4
11.
Incomplete combustion of propane, C3H8, yielding carbon monoxide and water
12.
Ba(s) + LiNO3(aq) 
13.
Au(s)
+ CuO(aq) 
14.
KI(aq)
+ Pb(NO3) 3 (aq)
15.
A solution of silver nitrate reacts with aqueous strontium chloride
16.
A solution of calcium hydroxide is mixed with a solution of iron (III) sulfide
17.
A piece of magnesium ribbon is placed in hydrochloric acid.
18.
Solid gold is placed in a solution of copper (II) chloride.
19.
Magnesium carbonate is placed in hydrofluoric acid.

Write the correct dissolving equations for each of the following solid ionic compounds:
20.
KCl
21.
K2SO4
22.
BaCl2
23.
Al2(SO4)3