3.12: End of Chapter Problems
Ions
1. Identify each as a cation, an anion, or molecule.
a. H +
b. Cl −
c. O 2
d. Ba 2 +
e. CH 4
f. CS 2
g. NH 3
h. Br −
i. H −
j. Hg 2 +
k. CCl 4
l. SO 3
2. What are ionophores? Explain how ionophores act as antibiotics.
Main Group Elements
1. Which of these ions is not likely to form?
a. Mg +
b. K +
c. S 3 −
d. N 3 −
2. When the following atoms become ions, what charges do they acquire?
a. Li
b. S
c. Ca
d. F
3. What characteristic charge do atoms in the first column of the periodic table have when they become ions?
4. What characteristic charge do atoms in the second column of the periodic table have when they become ions?
5. What characteristic charge do atoms in the third-to-last column of the periodic table have when they become ions?
6. What characteristic charge do atoms in the next-to-last column of the periodic table have when they become ions?
7. Starting with lithium and bromine atoms, use Lewis diagrams to show the formation of the ionic compound.
a. LiBr
b. MgO
Nomenclature of Ions
1. Name each ion.
a. Ca 2 +
b. S 2−
c. SO 4 2 −
d. NH 4 +
e. Ba 2 +
f. HCO 3 −
g. Ca 2 +
h. P 3−
i. H 2 PO 4 −
j. Sn 4 +
k. K +
l. Fe 3 +
m. HSO 4 −
n. Sn 2 +
o. Ca 2 +
p. S 2−
q. SO 3 2 −
r. NH 4 +
s. Cu +
t. Fe 2 +
2. Write the formula for each ion.
a. the bromide ion
b. the phosphate ion
c. the cupric ion
d. the magnesium ion
e. the fluoride ion
f. the carbonate ion
g. the ferrous ion
h. the potassium ion
i. the bromide ion
j. the phosphate ion
k. the cupric ion
l. the magnesium ion
m. the fluoride ion
n. the carbonate ion
o. the potassium ion
Formula of Ionic Compounds
1. Starting with lithium and bromine atoms, use Lewis diagrams to show the formation of the ionic compounds.
LiBr
MgO
2. Write the chemical formula for an ionic compound composed of each pair of ions.
a. the 3+ iron ion and the oxide ion
b. the calcium ion and the oxide ion
c. the 2+ copper ion and the sulfide ion
d. the 1+ copper ion and the sulfide ion
e. the potassium ion and the sulfate ion
f. the calcium ion and the nitrate ion
g. the magnesium ion and the carbonate ion
h. the aluminum ion and the acetate ion
i. the sodium ion and the sulfide ion
j. the aluminum ion and the fluoride ion
Nomenclature of Ionic Compounds
1. Name each ionic compound using both Stock and common systems if necessary.
Ca 3 (PO 4 ) 2
(NH 4 ) 2 Cr 2 O 7
KCl
CuCl
SnF 2
ZnBr 2
Fe(NO 3 ) 3
Al 2 O 3
CuF 2
AgF
Ca 3 (PO 4 ) 2
(NH 4 ) 2 Cr 2 O 7
KCl
CuCl
SnF 2
ZnBr 2
Fe(NO 3 ) 3
Al 2 O 3
CuF 2
AgF
2. Give two names for each compound
a. Al(HSO 4 ) 3
b. Mg(HSO 4 ) 2
c. Co(HCO 3 ) 2
d. LiHCO 3
Formula and Nomenclature of Ionic Compounds
Give the formula and the name of the ionic compound formed by each pair of ions. Use both the Stock and common systems, where appropriate.
a. Na + and Br −
b. Mg 2 + and Br −
c. Mg 2 + and S 2−
d. K + and Cl −
e. Mg 2 + and Cl −
f. Mg 2 + and F −
g. Na + and N 3−
h. Mg 2 + and N 3−
i. Al 3 + and S 2−
j. Li + and N 3−
k. Mg 2 + and P 3−
l. Li + and P 3−
m. Fe 3 + and Br −
n. Fe 2 + and Br −
o. Fe 3 + and S 2−
p. Cu + and S 2−
q. Cr 3 + and O 2−
r. Cr 2 + and O 2−
s. Pb 2 + and Cl −
t. Pb 4 + and Cl −
u. Cr 3 + and NO 3 −
v. Fe 2 + and PO 4 3 −
w. Ca 2 + and SO 4 2 −
x. Al 3 + and OH −
y. NH 4 + and NO 3 −
z. K + and SO 4 2 −
Covalent Bonds
Predict the number of covalent bonds formed by each nonmetal atom.
N
Cl
C
O
Br
H
Ionic vs. Molecular Compounds
1. Which compounds would you predict to be ionic? Circle.
a. Li 2 O
b. (NH 4 ) 2 S
c. CO 2
d. FeSO 3
e. C 6 H 6
f. C 2 H 6 O
g. Ba(OH) 2
h. CH 2 O
i. NH 2 CONH 2
j. (NH 4 ) 2 CrO 4
k. C 8 H 18
l. NH 3
2. Identify each compound as ionic or molecular.
a. Na 2 O
b. PCl 3
c. NH 4 Cl
d. OF 2
e. N 2 O
f. FeCl 3
g. (NH 4 ) 3 PO 4
h. SOCl 2
3. Is each compound formed from ionic bonds, covalent bonds, or both?
a. Na 2 O
b. Na 3 PO 4
c. N 2 O 4
d. Ba(OH) 2
e. F 2
f. PCl 3
4. Write the molecular formula for each compound.
- chlorine trifluoride
- phosphorus pentachloride
- sulfur dioxide
d. nitrogen dioxide
e. dioxygen difluoride
f. dinitrogen pentoxide
g. sulfur hexafluoride
h. nitrogen monoxide
5. Write the name for each compound.
- BrF 5
- S 2 F 2
- CO
d. CF 4
e. SeCl 2
f. SO 3
Formula Weight and Molecular Weight
1. Use the atomic weights rounded to two decimal places to determine the formula weight for each ionic compound.
- TiO 2
- AgBr
- Au(NO 3 ) 3
- Fe 3 (PO 4 ) 2
2. Calculate the molecular weight of each covalent compound? Use the atomic weights rounded to two decimal places.
a. C 2 H 2
b. CO
c. CO 2
d. BF 3
Mass-Mole Conversions
1. A biochemist needs 0.00655 mol of bilirubin (C 33 H 36 N 4 O 6 ) for an experiment. How many grams of bilirubin will that be?
2. A chemist needs 457.8 g of KMnO 4 to make a solution. How many moles of KMnO 4 is that?
3. What is the mass of 62.5 moles of carbon tetrachloride?
4. How many moles of ammonium hydroxide are present in 0.475 g?