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CHAPTER 2: ATOMS, MOLECULES AND IONS
Objectives
Part I: Sections 2.1 - 2.3
1.
2.
3.
4.
5.
6.
7.
8.
9.
10.
11.
12.
Describe the early developments of atomic theory.
State the laws of conservation of mass, definite proportions, and multiple proportions, and explain
the basis of each.
Describe Dalton’s atomic theory.
Describe Thomson’s cathode ray experiments that lead to his “Plum Pudding” model of the atom.
Contrast Dalton’s model of the atom with Thomson’s model.
Describe Rutherford’s Gold Foil experiment and explain how it leads to the discovery of the
nucleus.
Differentiate among the electron, proton, and neutron, and indicate the electrical charge and
relative mass associated with each particle.
Define atomic number and mass number and their relationship to isotopes.
Define isotope, nucleon, and nuclide.
Given the atomic number and mass number, list the number of protons, neutrons, and electrons in
an atom, or given the number of particles, determine the atomic number and mass number.
Describe the structure of the Periodic Table; identify the groups (families) and the periods.
Discriminate between the main, transition and rare earth elements. Locate the alkali, alkaline-earth
, halogen, and noble gas groups in the Periodic Table.
Differentiate between the properties of metals, nonmetals, and metalloids.
Part II: Sections 2.4 - 2.6
13.
14.
15.
16.
17.
18.
19.
20.
21.
22.
List the names and symbols for the common elements.
Given a formula, state the number of atoms of each element present.
Differentiate between chemical symbols and chemical formulas.
Differentiate between subscripts and coefficients.
Define, recognize, and give examples of formula unit.
Name ionic compounds and binary molecular compounds.
Write formulas for ionic and molecular chemical compounds.
Differentiate between molecular, structural, and empirical (simplest) formulas.
Name the common acids.
Name hydrates.
READING ASSIGNMENT
SECTION
PAGES
TOPIC
#
#
2.1
29-30
Atoms and Atomic Theory: combination laws
2.2
31-34
Components of the atom; isotopes
Introduction to the Periodic Table: Periods and Groups; Metals and
2.3
35-38
Nonmetals
2.4
38-42
Molecules and Ions
2.5
42-44
Formulas of Ionic Compounds
2.6
44-47
Names of Compounds: ions, molecular compounds, acids
WRITTEN ASSIGNMENTS:
TOPIC
PAGE #
QUESTION(S) #
Atomic Theory and Laws
51
1 through 6; 8-18 even
Elements and Periodic Table
Names of Compounds
Packet
52
52
20-26 even
28-54 even
As assigned
CHAPTER 2: ATOMS, MOLECULES AND IONS
Development of Atomic Theory
Choose words from the list to fill in the blanks in the paragraphs.
Atom
Atomic number
Chadwick
Conservation of
matter
Dalton
Definite
proportions
Electron
Isotope
Lavoisier
Mass number
Multiple
proportions
Neutron
Proton
Proust
Quantum
Rutherford
Subatomic
number
Thomson
More than 2000 years ago, Greek philosophers proposed the existence
of very small, indivisible particles, each of which is called a(n) (1). The
theory that such particles existed was supported, much later, by _ (2),
who proposed, in his law of __ (3), that matter
cannot be created or destroyed. Then
(4) proposed, in his law of
_____(5), that the ratio of the masses of
elements in any given compound is always the same. The law of
____(6), proposed soon after, states that the masses of one element that
combine with fixed mass of another element in different compounds are in
simple whole-number ratios. An atomic theory based on these laws was
developed by ____ (7).
1. __________________
2. __________________
3. __________________
4. __________________
5. __________________
6. __________________
7. __________________
8. __________________
It was later proposed that the atom is not indivisible, but is made up of
smaller particles, each of which is called ____ (8). These particles
include the negatively charge ____ (9), discovered by ___ (10); the
positively charged ____ (11); and the uncharged _____ (12);
discovered by ____(13). The latter two particles were present in the _
(14), or center of the atom, which is discovered by __(15) in his goldfoil experiment.
9. __________________
The number of positively charged particles in an atom is called its
____(16). The total number of the positively charged and the
uncharged particles is called the _ (17) of the atom. An atom that has
the same number of positively charged particles as another atom, but a
different number of uncharged particles, is called a(n) __(18)
14. _________________
10. _________________
11. _________________
12. _________________
13. _________________
15. _________________
16. _________________
17. _________________
18. _________________
H O N O R S C H E M I S T RY - C H A PT E R 2 : ATO M I C T H E O RY
Historical Development
Match the concept, theory, or discovery in Column I with the scientist most closely associated with it. Some
scientists may be used more than once and some not at all.
Column I
Column II
______ 1.
Determined that most of the atom is empty
(a) Rutherford
______ 2.
(b) Becquerel
______ 3.
Worked extensively with cathode ray tubes
to decipher the structure of the atom
Planetary model of the atom
______ 4.
Gold-foil experiment
(d) Crooks
______ 5.
Tried to explain the nature of cathode ray tubes (e) Chadwick
______ 6.
Discovered Radium and Polonium
(f)
______ 7.
Discovered neutron
(g) Democritus
______ 8.
Charge to mass ratio of electron
(h) Einstein
______ 9.
Charge on the electron
(i)
Millikan
______ 10.
Discovered radioactivity
(j)
Moseley
______ 11.
First modern atomic theory
(k) Planck
______ 12.
Coined the word “atom”
(l) Aristotle
______13.
Law of definite composition
(m) J. J. Thomson
______ 14.
Law of conservation of mass
(n) Lavoisier
______ 15.
Plum pudding model of the atom
(o) Gay Lussac
______ 16.
Law of multiple proportions
(p) Madam Curie
______ 17.
Discovered electron
(q)
______ 18.
Claimed that there are only four elements
(c) Bohr
Dalton
Proust
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H O N O R S C H E M I S T RY - C H A PT E R 2 : ATO M I C T H E O RY
Atomic Structure
Part I. Atomic Structure
1.
Compute the number of electrons, protons, and neutrons in the following nuclides, and write the
nuclear symbol for each.
a. Cr A = 50
d. Ir A = 193
b. Cl A = 37
e. Si A = 29
c. Mg A = 26
2.
3.
f. Ne
A = 22
Moseley used X rays to determine the atomic numbers of the elements. Identify each of the following
elements by name.
a. 1 proton
d. 12 protons
b. 4 protons
e. 20 protons
c. 8 protons
f. 30 protons
Give the number of neutrons in each of the following isotopes.
a. titanium - 46
c.
b. nitrogen - 15
d.
24
16
S
65
29
Cu
4
H O N O R S C H E M I S T RY - C H A PT E R 2 : ATO M I C T H E O RY
Chemical Formulas – Ions
1.
Identify the following elements as metals, nonmetals, or semimetals.
a. potassium _______ b. boron _______
e. uranium _______
c. molybdenum _______
f. strontium _______ g. sulfur _______
d. iodine _______
h. cobalt _______
2.
Which of the above elements are part of the representative (main group) elements? _____________
3.
In which group are the elements in question 1 found?
a. potassium _______ b. boron _______
e. uranium _______
4.
c. molybdenum _______
f. strontium _______ g. sulfur _______
d. iodine _______
h. cobalt _______
Write the symbol and the name of the ion formed.
a. A strontium atom loses two electrons. _________________________________
b. An iodine atom gains one electron. ___________________________________
c. A nitrogen atom gains three electrons. _________________________________
d. A hydrogen atom loses one electron. ___________________________________
5.
Complete this table:
Symbol of the Element
Change in Electrons
a.
Ca
2 electrons lost
b.
F
Al+3
Na+1
Na
P-3
e.
f.
Name of Ion
F-
c.
d.
Formula of Ion
Se
2 electrons gained
6.
State the number of electrons either lost or gained in forming each ion.
a. S-2
_____________
7.
Write the formula and charge of each of the following ions.
a. magnesium ion __________________
e. hydroxide __________________
b. lead(IV) ion
__________________
f. iron(II) ion __________________
c. chromate ion
__________________
g. ammonium ion __________________
d. nitrite ion
__________________
h. copper(I) ion __________________
5
H O N O R S C H E M I S T RY - C H A PT E R 2 : ATO M I C T H E O RY
8.
9.
10.
Would you expect the following compounds to be ionic or molecular?
a. CO __________________
b. KBr __________________
c. C3H8 __________________
d SO3 __________________
e. NaF __________________
f. NH3 __________________
State whether each formula represents a molecule or a formula unit?
a. CO __________________
b. KBr __________________
c. C3H8 __________________
d SO3 __________________
e. NaF __________________
f. NH3 __________________
Using only the periodic table, name and write the formulas of the ions of these representative elements:
a. lithium
____________________
d. oxygen ____________________
b. barium
____________________
e. fluorine ____________________
c. potassium ____________________ f. lead(II)
11.
Without consulting any tables, name the following ions:
a. H+1
____________________
e. Mg+2 ____________________
b. N-3
____________________
f. Sn+4
c. Cr+3
____________________
g. SO4-2 ____________________
d. Zn+2 ____________________
12.
____________________
h. Se-2
____________________
____________________
Write the formula and charge of each of the following ions.
a. barium ion
____________________
e. cyanide
____________________
b. lead(II) ion
____________________
f. vanadium(V) ion ____________________
c. dichromate ion ____________________
g. chlorite ion ____________________
d. nitride ion
h. cesium ion ____________________
____________________
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H O N O R S C H E M I S T RY - C H A PT E R 2 : ATO M I C T H E O RY
Empirical and Molecular Formula - Identification
Identify the following elements as metals, nonmetals, or metalloids. Write the symbol of the element.
1. cesium
_____________5. zirconium _____________ 9. sodium
_____________
2. vanadium
_____________6. aluminum
_____________ 10. nickel
_____________
3. chromium
_____________7. silicon
_____________ 11. germanium _____________
4. fluorine
_____________8. helium
_____________ 12. tellurium _____________
State the number of electrons either lost or gained in forming each of the following ions:
13. S2- _____________ 15. Al+3
17. Cl-1 _____________
_____________
14. K+1 _____________ 16. OH-1_____________
18. Ba+2
_____________
Would you expect the following compounds to be ionic or molecular?
19. CO2 _____________
21. RbI_____________23. C6H12O6
20. TeO3 _____________
22. AlI3
_____________
_____________24. Zn(NO3)2 _____________
Write the empirical formula for each of the following compounds:
25. N2O4
_____________28. CH4
_____________
26. C6H18O6
_____________29. Hg2I2
_____________
27. C2H6
_____________30. C10H22
_____________
State the number of formula units that is represented by each of the following:
31. Ag2CO3
_____________33. 4AlBr3
_____________35. HCl _____________
32. 3HBr
_____________34. 6Ba3(PO4)2_____________ 36. 3CH3COOH ____
37.
How many atoms of chlorine are in 7Al(ClO3)3? _____________
38.
How many atoms of all elements are in 4Al2(SO4)3? _____________
39.
The earliest cosmetics were made from natural compounds. Green eye shadow was made from
malachite, Cu2CO3(OH)2, a copper ore. How many hydrogen atoms are there in 17 Cu2CO3(OH)2?
7
H O N O R S C H E M I S T RY - C H A PT E R 2 : ATO M I C T H E O RY
Formulas for Ionic Compounds
I.
Writing Formulas for Binary Ionic Compound.
Write the correct formula for the compound formed by each of the following pairs of ions.
1.
Na+1, F-1
__________________
5. Li+1, S-2
__________________
2.
K+1, S-2
__________________
6. Sn+4, O-2
__________________
3.
+3
-2
Al , O
__________________
+1,
7. H
__________________
4.
Ca+2, N-3
__________________
8. Cs+1, O-2
__________________
II.
Naming Binary Ionic Compounds
Cl
-1
Name these binary ionic compounds.
9.
CoI3
__________________
13.
Cu2S
__________________
10.
Cs2O
__________________
14.
K2O
__________________
11.
AlI3
__________________
15.
PbO
__________________
12.
FeO
__________________
16.
PbO2
__________________
III.
Writing Formulas for Ternary Ionic Compounds.
Write formulas for these compounds.
17.
barium hydroxide
__________________ 21. sodium chlorite __________________
18.
aluminum sulfate
__________________ 22. lead(IV) dichromate
19.
magnesium cyanide
__________________ 23. iron(III) carbonate
20.
ammonium sulfite
__________________ 24. aluminum hydroxide __________________
__________________
__________________
IV. Naming Ternary Ionic Compounds.
Write the name for these compounds.
25.
NaCN
________________________
29. Cu(NO3)2 ________________________
26.
CaSO4
________________________
30. Mg3P2 ________________________
27.
Sn(HPO4)2
________________________
31. HgHPO4
28.
Fe(ClO4)3
________________________
32. Na2Cr2O7 ________________________
________________________
8
H O N O R S C H E M I S T RY - C H A PT E R 2 : ATO M I C T H E O RY
Formulas for Ionic Compounds
V.
Writing Formulas for Binary Ionic Compounds ( Cations with Multiple Charges).
Write formulas for the following compounds.
39.
tin(II) oxide
40.
_____________________
44.
Iron(II) chloride _____________________
nickel(III) chloride _____________________
45.
Copper(II) oxide _____________________
41.
copper(I) nitride _____________________ 46.
Chromium(III) oxide _____________________
42.
lead(IV) chloride _____________________
47.
Manganeese(IV) oxide _____________________
43.
iron(III) nitride _____________________
48.
Mercury(I) sulfide _____________________
VI. Writing Formulas for Ternary Ionic Compounds (Ions Given).
Write formulas for the following compounds.
49.
K+1, OH-1
_____________________
55.
Al+3, Cl-1
_____________________
50.
Na+1, CN-1
_____________________
56.
Al+3, SO4-2
_____________________
51.
Ca+2, OH-1
_____________________
57.
Al+3, N-3
_____________________
52.
Ca+2, SO4-2
_____________________
58.
Ba+2, C2H3O2-1
_____________________
53.
NH4+1, Cl-1
_____________________
59.
Ca+2, NO3-1
_____________________
54.
NH4+1, CO3-2
_____________________
60.
Zn+2, ClO4-1
_____________________
VII.
Writing Formulas for Ternary Compounds ( Names Given).
61.
magnesium hydroxide
_________________
65.
Sodium hypochlorite
_________________
62.
potassium sulfate
_________________
66.
Lead(IV) chromate
_________________
63.
magnesium dichromate
_________________
67.
Iron(II) sulfate
_________________
64.
ammonium sulfide
_________________
68.
Aluminum nitrate _________________
VIII. Naming Ternary Ionic Compounds (Formulas Given).
69.
LiCN
70.
________________________
74.
Cr(NO3)2
________________________
(NH4)2SO4 ________________________
75.
Mg3(PO4)2
________________________
71.
Sr(H2PO4)2 ________________________
76.
Sr3(PO4)2
________________________
72.
Fe(ClO3)3 ________________________
77.
Cu2HPO4
________________________
73.
(NH4)2CO3 ________________________
78.
KClO3
________________________
9
H O N O R S C H E M I S T RY - C H A PT E R 2 : ATO M I C T H E O RY
Ionic Formulas
IX. Naming and Writing Formulas for all Ionic Compounds.
Write the name or formula, as appropriate.
1.
aluminum hydroxide
___________________________________________
2.
K2SO3
___________________________________________
3.
LiF
___________________________________________
4.
potassium chlorite
___________________________________________
5.
Sn3(PO4)2
___________________________________________
6.
zinc hydrogen sulfate
___________________________________________
7.
calcium sulfate
___________________________________________
8.
Pb3(PO4)4
___________________________________________
9.
Al2S3
___________________________________________
10.
barium hydroxide
___________________________________________
11.
silver chloride
___________________________________________
12.
FeS
___________________________________________
13.
Hg2S
___________________________________________
14.
SnI4
___________________________________________
15.
CoF3
___________________________________________
16.
CuO
___________________________________________
17.
sodium iodide
___________________________________________
18.
calcium chloride
___________________________________________
19.
potassium sulfide
___________________________________________
20.
lithium nitrate
___________________________________________
21.
copper(II) sulfate
___________________________________________
22.
sodium carbonate
___________________________________________
23.
barium phosphate
___________________________________________
24.
Ag2O
___________________________________________
25.
Ca(OH)2
___________________________________________
26.
Zn(NO3)2
___________________________________________
27.
KClO3
___________________________________________
28.
NH4OH
29.
FeCr2O7
___________________________________________
30.
Pb3(PO4)2
___________________________________________
___________________________________________
10
H O N O R S C H E M I S T RY - C H A PT E R 2 : ATO M I C T H E O RY
Naming and Writing Formulas for Molecular Compounds(1)
Write formulas for the following molecular compounds:
1.
carbon monoxide
________________________________
2.
nitrogen monoxide
________________________________
3.
sulfur dioxide
________________________________
4.
phosphorus trichloride ________________________________
5.
carbon dioxide
________________________________
6.
dinitrogen pentoxide
________________________________
7.
dihydrogen monosulfide
8.
dihydrogen monoxide
9.
diphophorus pentoxide ________________________________
10.
carbon tetraiodide
________________________________
________________________________
________________________________
Name the following molecular compounds:
11.
PCl5
________________________________ 18.
N2O3 _____________________________
12.
NO
________________________________ 19.
Cl2O7 ___________________________
13.
P2O5
________________________________ 20.
OF2
14.
CO2
________________________________ 21.
SO2
____________________________
15.
NO2
________________________________ 22.
BrI5
____________________________
16.
SO3
________________________________ 23.
CF4
____________________________
17.
SiF6
________________________________ 24.
SiCl4
____________________________
______________________________
Name each of the following substances. Specify if the compound is ionic or molecular.
Molecular or Ionic
Name
21.
CO
_____________________
________________________________
22.
MgI2
_____________________
________________________________
23.
Cu2O
_____________________
_________________________________
24.
Al2O3
_____________________
_________________________________
25.
SO2
_____________________
_________________________________
26.
Li2CO3
_____________________
_________________________________
27.
PI3
_____________________
_________________________________
28.
Ba3(PO4)2
_____________________
_________________________________
11
H O N O R S C H E M I S T RY - C H A PT E R 2 : ATO M I C T H E O RY
Naming Molecular Compounds (2)
Determine the oxidation number of the underlined element in each of the following compound or ions:
1.
N2O
_________
5.
SO3
_________
9.
H2S
_________
2.
H2SO4 _________
6.
KClO
_________
10.
P4O10
_________
3.
N2O5
_________
7.
IO3-1
_________
11.
MnO4-1 _________
4.
PO4-3
_________
8.
ClO4-1 _________
12.
NO3-1
_________
Write formulas for the following compounds:
13.
dichlorine monoxide
_____________________________________________________
14.
dinitrogen tetroxide
_____________________________________________________
15.
mono-nitrogen dioxide _____________________________________________________
16.
iodine tri-chloride
_____________________________________________________
17.
carbon disulfide
_____________________________________________________
18.
sulfur hexafluoride
_____________________________________________________
19.
carbon tetrafluoride
_____________________________________________________
20.
dinitrogen pentoxide
_____________________________________________________
Name the following molecular compounds:
21.
ICl3
_________________________
28.
N2O4
_________________________
22.
NO2
_________________________
29.
I2O7
_________________________
23.
P2O3
_________________________
30.
XeF4
_________________________
24.
CO
_________________________
31.
CH4
_________________________
25.
N 2O 5
_________________________
32.
BrI5
_________________________
26.
SiO3
_________________________
33.
H2O
_________________________
27.
PCl3
_________________________
34.
C2H6
_________________________
Name each of the following substances. Specify if the compound is ionic or molecular.
Molecular or Ionic
Name
35.
SiF6
____________________
____________________
36.
Ca(OH)2
____________________
____________________
37.
Hg2Cr2O7
____________________
____________________
38.
N 2O 3
____________________
____________________
39.
Al(MnO4)3
____________________
____________________
40.
Cl2O
____________________
____________________
41.
XeF6
____________________
____________________
12
H O N O R S C H E M I S T RY - C H A PT E R 2 : ATO M I C T H E O RY
Nomenclature/Formula Writing - Review (GR)
Write formulas for the following compounds:
1. Lead(II) sulfate ______________________
9.
Chloric acid _______________________
2. Sodium bicarbonate ___________________
10.
Mercury(II) peroxide ________________
3. Dinitrogen tetroxide __________________
11.
Calcium phosphate __________________
4. Potassium permanganate _______________
12.
Iron(III) oxide ______________________
5.
Sulfuric acid _________________________
13.
Barium nitrate ______________________
6.
Copper(II) fluoride ____________________
14.
Cuprous sulfite _____________________
7.
Stannic carbonate _____________________
15.
Bismuth(V) selenide _________________
8.
Potassium dichromate __________________
16.
Nitric acid _________________________
Name the following compounds. Use as many names as possible for each compound ( old and new names if appropiate).
17. NaOH
___________________________
25.
HCl
___________________________
18. N2O5
___________________________
26.
HNO3
___________________________
19. CuSO3
___________________________
27.
MnCl2 ___________________________
20. K2O2
___________________________
28.
HClO
21. FeCl3
___________________________
29.
MnCl4 ___________________________
22. Ca(CN)2
___________________________
30.
SF6
23. NH4NO2
___________________________
31.
Ni(OH)2 ___________________________
24. Al2(SO4)3
___________________________
32.
H2SO4 ___________________________
___________________________
___________________________
Look at the following formulas. SOME are correct as written, while others are not. If the formula is NOT CORRECT,
write the correct formula, and give it a name. If the formula is correct as written, you only have to name the compound.
33. LiCrO4
_________________________
41.
CaSO4 ___________________________
34. BaN
_________________________
42.
NH4PO4 _____________________ ______
35. KF
_________________________
43.
BI
____________________________
36. CaCl
_____________________ ____
44.
KCO3
____________________________
37. HClO4
_____________________ ____
45.
AlO
____________________________
38. SiCl4
_________________________
46.
TiCl4
____________________________
39. PbO
_____________________ ____
47.
K2C2H3O2 ___________________________
40. LiN
_____________________ ____
48.
HSO4
_____________________________
49.
Potassium Oxalate_______
50. HCN ________________ 51. HBrO3________________
52.
KSCN _________________
53. NiHPO3 _______________ 54. Bismuth(V) sulfite _______
55.
Ag2Cr2O7__________________56. Pb(C2H3O2)2 ___________________________
13
H O N O R S C H E M I S T RY - C H A PT E R 2 : ATO M I C T H E O RY
ANSWER KEY
Page 2.
1. atoms
2. Lavoisier
5. law of Definite Composition
8. Subatomic particle
12. neutron
16. atomic number
20. energy level
Page 3.
1.a
2.d
3.a
4.a
5.m
3. Law of conservation os matter
4. Proust
6. Law of multiple proportions
7. Dalton
9. electrons
10. Thomson 11. proton
13. Chadwick
14. nucleus
15. Rutherford
17. mass number
18. isotope
19. Bohr
21. Planck
22. quantum
6.j
7.e
8.m
9.i
10.b
Page 4/5
1a. metal
g. nonmetal
11.f
12.g
13.q
14.n
15.m
b. semi metal
h. metal
c. metal
2. a, b, g, d, f
f. 2
g. 16
3. a. 1
b. 13
4. a. Sr+2
5. a. Ca+2 calcium
d. 1 lost, sodium
b. I-1
c. N-3
b. 1 electron gained, fluoride
e. P, 3 gained, phosphide
6. 2 gained
7. a. Mg+2
e. OH-1
b. Pb+4
f. Fe+2
8. a. molecular
9. see 8
10. a. Li+1
11. hydrogen
f. tin(IV)
12. a. Ba+2
g. ClO2-1
Page 6
1. m
7. non
13. 2 gained
19.
24.
25.
30.
31.
37.
16.f
17.m
18.l
d. nonmetal
c. 6
e. metal
d. 17
f. metal
e. 3
h. 9
c. CrO4-2
g. NH4+1
b. ionic
c. molecular
b. Ba+2
b. nitride
g. sulfate
b. Pb+2
h. Cs+1
c. O-2
2. m
8. noble gas
14. 1 lost
d. H+1
c. Al, 3 lost, aluminum
f. Se-2, selenide
3. m
9. m
15. 3 lost
molecular
20. molecular
ionic
NO2
26. CH3O
C5H11
1
32. 3
33. 4
21
38. 68
39. 34
d. NO3-1
h. Cu+1
d. molecular
e. ionic
f. molecular
d. F-1
f. Pb+2
c. chromium(III)
d. zinc
e. magnesium
h. selenide
c. Cr2O7-2
d. N-3
e. CN-1
f. V+5
4. non
10. m
16. 1 gained
5. m
11. metalloid
17. 1 gained
6. metalloid
12. metalloid
18. 2 lost
21. ionic
22. ionic
23. molecular
27. CH3
28. CH4
29. HgI
34. 6
40. a. Al, Cr
35. 1
36. 3
b. Cr2O3, Al2O3
14
H O N O R S C H E M I S T RY - C H A PT E R 2 : ATO M I C T H E O RY
Honors Chemistry: Chapter 2: Atomic Theory... Answer Sheet page 7, 8, 9
I. Writing formulas for Binary Ionic Compounds
1. NaF
2. K2S
3. Al2O3
4. Ca3N2
II. Naming Binary Ionic Compounds
9. Cobalt (III) iodide
10. Cesium oxide
11. Aluminum iodide
12. Iron (II) oxide
5.
6.
7.
8.
Li2S
SnO2
HCl
Cs2O
13. Copper (I) sulfide
14. potassium oxide
15. Lead (II) oxide
16. Lead (IV) oxide
III. Writing Formulas for Ternary Ionic Compounds
17. Ba(OH)2
21. NaClO2
18. Al2(SO4)3
22. Pb(Cr2O7)2
19. Mg(CN)2
23. Fe2(CO3)3
20. (NH4)2SO3
24. Al(OH)3
IV. Naming Ternary Ionic Compounds
25. sodium cyanide
26. calcium sulfate
27. Tin (IV) hydrogen phosphate
28. Iron (III) perchlorate
29. copper (II) nitrate
30. magnesium phosphide
31. Mercury (II) hydrogen phosphate
32. sodium dichromate
V. Writing Formulas for Binary Ionic Compounds
39. SnO
44.
40. NiCl3
45.
41. Cu3N
46.
42. PbCl4
47.
43. FeN
48.
FeCl2
CuO
Cr2O3
MnO2
Hg2S
VI. Writing Formulas for Ternary Ionic Compounds
49. KOH
55. AlCl3
50. NaCN
56. Al2(SO4)3
51. Ca(OH)2
57. AlN
52. CaSO4
58. Ba(C2H3O2)2
53. NH4Cl
59. Ca(NO3)2
54. (NH4)2CO3
60. Zn(ClO4)2
VII. Writing Formulas for Ternary Compounds
61. Mg(OH)2
62. K2SO4
63. MgCr2O7
64. (NH4)2S
65.
66.
67.
68.
NaClO
Pb(CrO4)2
FeSO4
Al(NO3)3
VIII. Naming Ternary Ionic Compounds
69. lithium cyanide
74. chromium (II) nitrate
70. ammonium sulfate
75. magnesium phosphate
71. strontium dihydrogen phosphate
76. Strontium phosphate
72. Iron (III) chlorate
77. Copper (I) hydrogen phosphate
73. ammonium carbonate
78. potassium chlorate
IX. Naming and Writing Formulas for All Ionic Compounds
1. Al(OH)3
2. potassium sulfite
15
H O N O R S C H E M I S T RY - C H A PT E R 2 : ATO M I C T H E O RY
3. lithium fluoride
4. KClO2
5. Tin (II) phosphate
6. Zn(HSO4)2
7. CaSO4
8. Lead (IV) phosphate
9. aluminum sulfide
10. Ba(OH)2
11. AgCl
12. Iron (II) sulfide
13. Mercury (I) sulfide
14. Tin (IV) iodide
15. Cobalt (III) fluoride
16. Copper (II) oxide
Page 10
1. CO
2. NO
7. H2S
8. H2O
11. phosphorus pentoxide
14. carbon dioxide
17. silicon hexafluoride
20. oxygen difluoride
23. carbon tetrafluoride
17.
18.
19.
20.
21.
22.
23.
24.
25.
26.
27.
28.
29.
30.
3. SO2
9. P2O5
15.
18.
21.
24.
4. PCl3
10. CI4
12. nitrogen monoxide
nitrogen dioxide
dinitrogen trioxide
sulfur dioxide
silicon tetrachloride
NaI
CaCl2
K2S
LiNO3
CuSO4
Na2CO3
Ba3(PO4)2
silver oxide
calcium hydroxide
zinc nitrate
potassium chlorate
ammonium hydroxide
Iron (II) dichromate
Lead (II) phosphate
5. CO2
6. N2O5
13. diphosphorus pentoxide
16. sulfur trioxide
19. dichloro heptoxide
22. bromine pentaiodide
21. molecular, carbon monoxide
22. magnesium iodide, ionic 23. coper(I) oxide, ionic
24. aluminum oxide, ionic
25. sulfur dioxide, molecular 26. lithium carbonate, ionic
27. phosphorus tri-iodide, molecular
28. barium phosphate, ionic
Page 11
1. +1
2. +6
3. +5
4. +5
5. +6
6. +1
7. +5
8. +7
9. -2
10. +5
11. +7
12. +5
13. Cl2O
14. N2O4
15. NO2
16. ICl3
17. CS2
18. SF6
19. CF4
20. N2O5
21. iodine trichloride
22. nitrogen dioxide
23. diphoshorus trioxide
24. carbon monoxide
25. dinitrogen pentoxide
26. silicon trioxide
27. phosphorus trichloride
28. dinitrogen tetroxide
29. diiodine heptoxide
30. xenon tetrafluoride
31. carbon tetrahydride
32. bromine pentaiodide
33. dihydrogen monoxide
34. dicarbon hexahydride (ethane)
35. molecular, silicon hexafluoride
36 ionic, calcium hydroxide
37. ionic, mercury(I) dichromate
38. molecular, dinitrogen trioxide
39. ionic, aluminum permanganate
40. molecular, dichlorine monoxide
41. molecular, xenon hexafluoride
16