Unit 11 Review Activity
MM
12-13
1.
Which of the following can
exhibit dipole-dipole attractions
between its molecules?
CO2, SO2, H2, IF, HBr, CCl4
• SO2, IF, and HBr
• All are polar molecules
2.
Which of the following substances
exhibit hydrogen bonding in their
liquid and solid states?
CH3NH2, CH3F, PH3, HCOOH
•CH3NH2 and HCOOH
3.
Predict which substance will
have the higher BP.
TiO2 or TiCl4
• TiO2 has a larger BP due to
the higher charge on
Oxygen
4.
Predict which substance will
have the higher BP.
LiF or MgF2
• MgF2 has a higher BP
because of the higher
charge of magnesium
5.
List the 3 types of IMF in order
of increasing strength.
• Dispersion, dipole, and
hydrogen bonding
6.
Which type of IMFs are
common to the pair?
Xe and CH3OH
•London dispersion
7.
Which type of IMFs are
common to the pair?
NH3 and HF
•Hydrogen bonding
8.
Which of the following atoms
would you expect to be most
polarizable?
O, S, Se, Te
• Te – has the most electrons
9.
Explain what happens to the
boiling point of noble gases as
you move down the group.
• BP increases because the
atom increases in size due
to increasing number of
electrons which increases
polarizability
10.
Rationalize the difference in
boiling points between the pair.
Br2 (59C) and ICl (97C)
• ICl is polar so the most
prominent IMF is dipoledipole while the prominent
IMF in Br2 is dispersion
force.
11.
What is the relationship
between IMF and viscosity?
•As IMF becomes
stronger, viscosity
increases
12.
State the phase changes that
are exothermic.
• Freezing, condensing,
deposition and Larry
13.
Explain why the heat of fusion
for any substance is generally
lower than the heat of
vaporization.
• With heat of fusion only some
IMF are being broken, with
heat of vaporization all the
IMF are broken.
14. Identify the states of matter in
sections A, B and C.
• A = Solid
• B = Liquid
• C = Gas
15. Name the “points” on the graph. Star,
triangle, square and T
• Triangle = normal mp
• Square = normal bp
• T = triple point
• Star = critical point
16.
Covalent bonding happens in both
molecular and covalent network
solids. Why do these two kinds of
solids differ so greatly in their
hardness and melting points.
• Covalent- network solids are
extremely strong forces due to
the lattice structure of the
molecules. Comparatively the
covalent solid’s IMF bonds are
weak.
17.
A white substance melts with some
decomposition at 730C. As a solid, it
is a nonconductor of electricity, but it
dissolves in water to form a
conducting solution. Which type of
solid is it?
•Ionic
18. Suppose you have 2 colorless
molecular liquids, one boiling at -84C, the
other at 34C, and both at atmospheric
pressure.
True or False
The higher boiling liquid has
greater total IMF than the other.
•True
19. Suppose you have 2 colorless
molecular liquids, one boiling at -84C, the
other at 34C, and both at atmospheric
pressure.
True or False
The lower boiling liquid must
consist of nonpolar molecules.
•False – has less total IMF
20.
As the IMF attraction between
molecules increases in magnitude,
will vapor pressure increase or
decrease?
• IMF increases then VP
decreases
21.
As the IMF attraction between
molecules increases in magnitude,
will heat of vaporization increase
or decrease?
•IMF increases and heat
of vaporization increases
23.
A flask of water is connected to a
vacuum pump. A few moments after
the pump is turned on, the water
begins to boil. After a few minutes,
the water begins to freeze. Explain
why these processes occur.
• The pump reduces the pressure in the
flask above the water when atmospheric
pressure = vapor pressure. Water boils,
boiling is endothermic, and the
temperature drops if the system is not
able to absorb heat from the
surroundings fast enough. As the temp of
water decreases, the water freezes.