Honors Chemistry
Name: ____________________________________ Date: __________________ Mods: __________
Chapter 11 Review
A.
Directions: On the line at the left, write the term that best matches each description below:
vaporization
condensation
melting point
melting/fusion
phase change
sublimation
equilibrium vapor pressure
volatile
deposition
________________________________ 1) conversion of solid directly into a gas
________________________________ 2) opposite of vaporization
________________________________ 3) temperature at which solid and liquid phases exist in equilibrium.
________________________________ 4) conversion of a substance from one of the three states of matter to
another
________________________________ 5) change from a liquid to gas
________________________________ 6) pressure exerted by a constant number of gas molecules in
equilibrium with their liquid phase
________________________________ 7) description of a liquid that evaporates easily, with a low boiling point
and high vapor pressure
________________________________ 8) transformation of a gas directly into a solid
________________________________ 9) phase change from a solid to a liquid
B.
Directions: On the line at the left, write the term that best matches each description below:
hydrogen bonding
ion-dipole forces
intermolecular forces
london dispersion forces
ionic bonding
metallic bonding
dipole-dipole forces
intramolecular forces
covalent bonding
________________________________ 9) attractive forces between a polar molecule and an ion
________________________________ 10) attractive forces between molecules near one another
________________________________ 11) attractive forces between nonpolar molecules resulting due to an
instantaneous dipole
________________________________ 12) forces within a molecule, responsible for bonding atoms together
________________________________ 13) forces responsible for holding aluminum and chloride ions bound
together
________________________________ 14) attractive forces between polar molecules
________________________________ 15) attractive forces between polar molecules when H is attracted to N,
O, or F.
________________________________ 16) forces responsible for holding atoms of magnesium bound together
C.
Directions: Indicate the predominant intermolecular force of attraction between the 2 molecules
listed.
List of IMFs:
ionic bonding
metallic bonding
ion-dipole forces (IDFs)
dipole-dipole forces (DDFs)
hydrogen bonding (H-bond)
London dispersion forces (LDFs)
__________________________________ 1) NaCl and NaCl
__________________________________ 2) N2 and N2
__________________________________ 3) H2O and K2O
__________________________________ 4) XeF4 and H2
__________________________________ 5) NH3 and NH3
__________________________________ 6) CO2 and O2
__________________________________ 7) Sn and Ni
__________________________________ 8) SrCl2 and HBr
__________________________________ 9) C5H12 and CH4
__________________________________ 10) PCl3 and CH3Cl
__________________________________ 11) Cu and Cu
__________________________________ 12) CH3-OH and H2O
Use the space below to draw Lewis structures (as needed):
D.
E.
Directions: Rank the following IMFs and intramolecular bonds in order of decreasing strength
(with #1 being the strongest, and #6 being the weakest)
________ dipole-dipole forces
________ ionic bonding
________ metallic bonding
________ ion-dipole forces
________ hydrogen bonding
________ London dispersion forces
Directions: Each of the following questions consists of two statements, I in the left-hand column
and II in the right-hand column. For each question, determine whether statement I is true or
false and whether statement II is true or false. Then, fill in the CE oval only if statement II is a
correct explanation of the true statement I.
Example - True/False: Relationship Analysis
Ex (A)
I
Hydroxide, OH–, is a
polyatomic ion
Ex (B)
Xe is a nonreactive gas
BECAUSE
II
Hydroxide has a net charge and is made up
of more than one element
Xe has 54 protons in its nucleus.
BECAUSE
Ex (A)
Ex (B)
Ex (A):
CE is bubbled in because both
statements I and II are TRUE and
statement I is true BECAUSE of
statement II.
Ex (B):
Even though both statements I and II are
TRUE, statement I is not true BECAUSE of
statement II (Xe is a nonreactive gas
because it has 8 valence electrons, not
because it has 54 protons) therefore CE is
not bubbled in.
*Note: If either statement I or II are false, CE cannot be bubbled in!!!*
I
II
Freezing is an exothermic phase
change.
BECAUSE
2
London dispersion forces are the
strongest of the intermolecular forces.
BECAUSE
3
The stronger the IMFs in a substance,
the lower the vapor pressure.
BECAUSE
4
Water in a glass tube exhibits capillary
action.
BECAUSE
5
At higher temperatures, a substance
has weaker intermolecular attractive
forces.
1
BECAUSE
6
The more viscose the substance, the
weaker its IMFs.
BECAUSE
7
Water has a high surface tension.
BECAUSE
1)
5)
2)
6)
3)
7)
4)
Heat is released when a gas becomes a
liquid
London dispersion forces exist due to a
brief, instantaneous dipole within a
molecule
In substances with stronger IMFs, fewer
molecules are able to escape to the gas
phase, thus reducing the vapor pressure.
The cohesive forces between water
molecules are stronger than the adhesive
forces between water and glass.
The greater the kinetic energy of a
substance, the further apart and less
attracted the molecules are to one
another
Viscosity is the ease with which a
substance evaporates.
When interacting with itself, water
molecules have very strong cohesive
forces.
F.
Directions: If the statement is true, write “true”. If it is false, change the underlined word or words
to make the statement true. Write your answer on the line provided.
_________________________________ 1) The average kinetic energy of the particles in a
liquid depends upon the temperature.
_________________________________ 2) Solids do not flow because the attractive forces
between their particles are weaker than those in
liquids or gases
_________________________________ 3) Dynamic equilibrium is reached when the rate of
vaporization exceeds the rate of condensation.
_________________________________ 4) Subliming ice is the opposite of freezing water
_________________________________ 5) All three states of matter can exist in equilibrium at
the triple point
G. Directions: Fill in the diagram (with high or low) to show how intermolecular forces influence the
volatility, vapor pressure, and boiling point of a substance.
weak
When IMFs are…
strong
volatility is ____________
volatility is ____________
vapor pressure is ___________
vapor pressure is ___________
boiling point is ___________
boiling point is ___________
_________________________________________________________________________________
H.
Directions: Use the vapor pressure curves
below to answer the following questions.
1) What is the vapor pressure of H2O at 50C?
______________________________
2) What is the boiling point of CCl4 when the
external pressure is 30 kPa?
______________________________
3) What is the normal boiling point of CHCl3?
______________________________
4) Which substance has the strongest IMFs?
______________________________
I)
Directions: Use the heating curve below to answer the following questions.
1) What is the melting point of the substance? __
2) What is the boiling point of the substance?
3) Which letter represents heating of the solid?
4) Which letter represents heating of the vapor?
5) Which letter represents melting of the solid?
6) Which letter represents boiling of the liquid?
J)
Directions: Use the phase diagram for water below to answer the following questions.
1) What state of matter is water at 2 atm and 50C ________________________________
2) What phase change will occur if the temperature is lowered from 80C to -5C at 1 atm?
_______________
3) You have ice at –10C and 1 atm. What could you do in order cause the ice to sublime?
_________________________________________________________________________
K)
Phase Change Calculations:
For problem below involving water, use the following ∆H and Cp values to solve:
Melting Point = 0ºC
∆Hfus = 6.00 kJ/mol
Cp ice = 2.06 J/g•ºC
Boiling Point = 100ºC
∆Hvap = 40.7 kJ/mol
Cp water = 4.184 J/g•ºC
Cp steam = 1.86 J/g•ºC
1) Given a sample of 145 grams of steam starting at 102.9ºC, determine the quantity of heat (in
kJ) released as the sample is cooled down to – 3.7ºC.
2) Calculate the total heat energy, in kJ, needed to convert 100 grams of ice at –13ºC into steam
at 105ºC. Is this change endothermic or exothermic?
3) The conversion of 72 grams of steam at 116ºC to liquid at 37ºC releases how many kJ of
heat? Is this change endothermic or exothermic?
For problem #5 (involving methanol) use the following ∆H and Cp values to solve:
Melting Point = –97.6ºC
∆Hfus = 3.18 kJ/mol
Cp solid = 84.4 J/g•ºC
Boiling Point = 64.7ºC
∆Hvap = 35.28 kJ/mol
Cp liquid = 79.5 J/g•ºC
Cp gas = 52.3 J/g•ºC
4) How much heat, in kJ, is needed to get 65 grams of solid methanol, CH4O, at –112.6ºC into
liquid methanol at 50ºC? Is this change endothermic or exothermic?