300 Chemistry Problem Set 12 N. Martel Bonding
Do on separate paper or in your notebook
1. Predict the type of bonding that will occur between each of the following pairs of elements
(ionic, polar covalent, nonpolar covalent), using the following electronegativity values: H
2.1, Li 1.0, C 2.5, N 3.0, O 3.5, F 4.0, Mg 1.2, Cl 3.0, K 0.8, Ca 1.0, and Br 2.8. Note any
patterns since you will not always have electronegativity values readily available.
H and Br
Br and Br
C and O
F and Cl
Li and O
K and Cl
H and N
F and F
Ca and O
Li and F
Mg and F
C and H
N and O
2. Draw the Lewis structures for each of the following ionic compounds:
KF
MgF2
Li2O
AlCl3
NaI
Na2S
RbI
K2O
NaBr
AlF3
BaO
3. Draw the Lewis structures for each of the following covalently bonded compounds:
H2Se
F2
HCl
CF4
O2
NF3
H2
CO2
SiH4
N2
BH3
4. Draw Lewis structures for each of the compounds below (level 1 … straightforward):
H2
F2
O2
N2
CO2
H2O
HF
CH3OH
H2S
NH3
I2
CF4
CHCl3
SO3
CCl4
BF3
SiO2
5. Draw Lewis structures for the compounds below (level 2 … some are a little more
challenging):
PBr3
N2H2
C2H4
BSF
C2H5OH
N2F4
CO
NO2F
SiS2
C2H2
BeF2
BH3
NF3
C2H6
CS2
H2Te
C2H4Cl2
SO2
HCN
Cl2CO
H2CCl2
FNO
C4H10
OCl2
SeF2
6. Draw the Lewis structures for the following polyatomic ions:
Ammonium
Perchlorate
Sulfate
Nitrate
Thiocyanate
Hydronium (H3O+1)
7. Go back to questions 4, 5, and 6 and identify any substances that have coordinate covalent
bonds.
8. Go back to questions 4, 5, and 6 and name the three dimensional geometry of each, draw a
3D picture of it, and label the appropriate bond angle.
9. Go back to questions 4 and 5 and state whether each molecule is polar or nonpolar.
10. Go back to questions 4 and 5 and identify the most noticeable type of intermolecular
forces present in each substance.
11. For each of the following substances, determine the dominant type of intermolecular
force. You may find it useful to draw Lewis structures for some of these:
Nitrogen
Carbon tetrachloride
Water
Sulfur monoxide
Boron trihydride
N2H2
SiH2O
Ammonia (nitrogen trihydride)
Carbon dioxide
Phosphorous trichloride
Ethane (C2H6)
Acetone (CH2O)
Methanol (CH3OH)
12. Explain why ethyl alcohol (C2H5OH) has a higher boiling point than methyl alcohol
(CH3OH).
13. Rank the following in order from lowest to highest anticipated boiling point: C2H4, CH4,
Ne, H3COCH3.
14. Motor oil consists of molecules that consist of long chains of carbon atoms with hydrogen
atoms attached to them. Using your knowledge of IMFs, explain why it wouldn’t be better to
use a compound like glycerol (formula is CHOH(CH2OH)2).
15. Review problems
Identify each compound’s type of bonding: carbon dioxide, magnesium sulfate,
water, dihydrogen monosulfide, sodium fluoride, calcium oxide.
Give the Lewis structures for: CH4, NH3, O2, Li2O, NaF, and Li3N.
For each of the following compounds, draw a Lewis structure, sketch a 3D shape
showing the bond angle(s), name the geometry, identify whether or not the molecule is polar,
and identify the type of IMFs present: BeCl2, BCl3, PBr3, SiCl4, CH2, N2, CO, SO2, ClO21-,
O3, SO3, CHO21-
d. Rank each group of substances in order from lowest to highest boiling point:
. C2H4, CH4, H3COCH3
. C2H5OH, CH3OH
. HCN, CH4, H2O
. He, Ne, CO2, NH3
. HF, CH2O, SiH2O
For additional practice:
Relevant sections in book are Chapter 12 and section 14.1
Additional practice problems can be found on p. 394-397 (1-7, 9-12, 30-37, 39-42, 47-50