Name: ________________________
Hour: ____ Date: ___________
AP Chemistry: 8HW
Circle the compound in each group that has the higher lattice energy.
1A.
Group 1:
LiCl
KCl
1B.
Group 2:
MgBr2
MgS
Group 3:
NaF
NaCl
Group 4:
Ni(OH)2
Ni(OH)3
Write the shorthand electron configuration for each of the following.
2A.
Mg2+
2B.
N3–
K+
Cl–
Fe3+
Mo4+
Classify each (“ionic only,” “covalent only,” or “ionic and covalent”) according to the bonds they contain.
3A.
(NH4)2O
K2S
P4O10
3B.
RbCl
Ba3(PO4)2
Arrange the species in each set in order of increasing size.
4A.
Cu
Cu+
Cu2+
Ni2+
Pd2+
Pt2+
4B.
O
O–
O2–
La3+
Eu3+
Gd3+
Yb3+
Use the Periodic Table to predict the most polar bond in each of the following groups. Circle your prediction.
5A.
Group 1:
C–F
Si–F
Group 2:
P–Cl
S–Cl
Ge–F
5B.
Group 3:
S–F
S–Cl
S–Br
Group 4:
Ti–Cl
Si–Cl
Ge–Cl
6. Rank the following bonds in order of increasing ionic character: N–O, Mg–O, C–F, Cl–Cl, K–Br
7. Indicate the bond polarity IN TWO WAYS for each of the following.
C–O
O–P
Cl–Te
Se–S
Draw a correct Lewis structure for each of the following.
8A.
HCN
PH3
CHCl3
NH4+
8B.
CO2
O2
H2CO
SeF2
Assign formal charges to each atom in the following species.
9A.
POCl3
9B.
ClO4–
Draw Lewis structures for each of the following.
10A.
NO2–
10B.
CO32–
11B.
ICl4–
Draw Lewis structures for each of the following.
11A.
PCl5
SF4
AsF6–
Use tabulated bond energy values to estimate the reaction enthalpy for the following gas-phase reactions.
12A.
H2 + Cl2  2 HCl
13. Arrange the following species with respect to the
carbon-oxygen bond length, longest to shortest.
12B.
N2 + 3 H2  2 NH3
CO
CO2
CO32–
CH3OH