Chapter 10 WS
SI Leader: Kristen Kelly
Summer 2013 CHM 112
1. Why don't some molecules with polar covalent bonds have dipole moments?
2. Identify the type of intermolecular forces present in the following substances:
a. HCl
b. CH3CH3
c. CH3NH2
d. Kr
e. CHCl3
f.
CnH2n +2
g. O2
h. CH3OH
i.
3.
HF
For the following molecule identify if the bond is non-polar covalent, polar covalent, or ionic. Draw out dipole forces in
order to assess the polarity.
===
4. Methanol (CH3OH) boils nearly 230 °C higher than methane (CH4 B.P. -164 °C) but 1-decanol (C10H21OH, bp = 231
°C) boils only 57 °C higher than decane (C10H22 bp= 172 °C).
4. Why is the dipole moment for SO2 1.63 D but the dipole moment for CO2 is zero? Draw lewis structures to help you
explain.