CHEMISTRY HONORS QUARTER 2 REVIEW
(chapter numbers correspond with textbook chapters order)
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CHAPTER 8
Define the term ion
Differentiate between a cation and anion
Describe the composition of ionic
compounds and list their characteristics
Determine the probable charge of an
element based on its periodic placement
Construct the electron configuration for ions
Define and give examples for ionic and
metallic bonds
Name compounds containing ions and
polyatomic ions
Construct chemical formulas based on
chemical name
CHAPTER 13
Define/ describe following terms:
 surface tension
 crystalline vs. amorphous
 capillary action
 sublimation
 volatility
 diffusion
 vapor pressure
 effusion
 boiling point
 hydrogen bond
 London-dispersion forces
 dipole-dipole forces
 viscosity
 phase diagram
 Kinetic molecular theory
 Graham’s law of effusion
 Dalton’s law of partial pressures
 Manometer
 Barometer
CHAPTER 9
Name covalent compounds using prefixes
Name acids (binary and oxyacid)
Write the formula for a covalent compound
from its name
Write the formula for a binary and oxyacid
from its name
Construct Lewis structures for compounds
Determine shape, bond angle, polarity &
hybridization
Define and explain covalent bonding Use
electronegativity to predict bond polarity
Compare the relative bond energy and
length of single, double and triple bonds
Define coordinate covalent bond and
explain how one works
VSEPR theory
Define hybrid orbitals
Describe the polarity of molecules and the
formation of bonds between them
List the characteristics of covalently bonded
molecules
Explain resonance. Draw resonance
structures for molecules.
CHAPTER 14
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Convert the number of moles to grams,
grams to moles, molecules to moles, moles
to molecules, grams to molecules and
molecules to grams.
Boyle’s law
Charles’s law
Gay- Lussac's law
Combined gas law
CHAPTER 16
CHATPER 11
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Determine the:
o Molar mass of compounds
o Percent composition
o Molecular formula
o Hydrates
o Empirical formula
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 Heating curves
 Specific heat capacity
 Heat of fusion
 Heat of vaporization
 Calorimetry
endothermic / exothermic
MULTIPLE CHOICE: Choose the best answer for each question.
1. Calculate the molecular weight of CrSO4?
A. 100 g/mol
B. 244 g/mol
Cr = 52; S = 32; O =16
C. 400 g/mol
D. 148 g/mol
2. What is the number of total atoms in a molecule of Fe3(PO4)2?
A. 3
B. 5
C. 13
D. 12
3. The mass of 0.10 mol of H2O
A. 18 g
B. 180 g
D. none of the above
H = 1; O = 16
C. 1.8 g
4. How many mole(s) are in 300 g of CaCO3?
A. 3
B. 300
Ca = 40; C = 12; O = 16.
C. 9
D. 900
5. The mole is
A. 1,000 grams.
B. The number of C-atoms in 12.0 g of Carbon
C. The SI unit for the amount of substance in Chemistry
D. B and C
6. Which of the following element is diatomic?
A. Iodine
B. Copper
C. Silicon
D. Potassium
7. What is the electron configuration of Al3+?
A. 1s2 2s2 2p6 3s2 3p6
B. 1s2 2s2 2p6 3s2 3p6 4d2
C. 1s2 2s2 2p6 3s2
D. 1s2 2s2 2p6
8. Which of the following has a linear shape?
A. CH4
B. BCl4-
C. CO2
D. All of these
9. If chlorine has an electronegativity of 3.0, what type of bond is formed in Cl2?
A. ionic B. polar covalent
C. nonpolar covalent
D. Metallic
10. The concept used in writing the electron-dot structures of certain molecules that oscillate between two or more
possible structures is called:
A. hybridization
B. electrostatic repulsion
C. resonance
D. electronegativity
11. Which of the following compounds violates the octet rule?
A. NF3
B. CCl4
C. SbCl5
D. Cl2
12. Which of the following is the most polar bond? EB = 2.0; EC = 2.5; EO = 3.5; ES = 2.5
A. B-C
B. S-O
C. C-O
D. B-O
13. Which substance below is composed of cations surrounded by a “sea of mobile electrons”?
A. Mn
B. Si
C. NaCl
D. CH4
14. The VSEPR Theory basically:
A. explains why bonds form
B. helps predict the shape of the molecules
C. has to do with why hybrid orbitals form
D. allows scientist to calculate the bond energies
15. A triple bond is made of sharing of _____ electrons between two atoms.
A. 2
B. 4
C. 6
D. 3
FREE RESPONSE:
16. A compound is found to be 40.00% carbon, 6.67% hydrogen, and 53.33% oxygen. Its molar mass is 210.0
g/mol. What is the molecular formula of this compound?
C7H14O7
17. Name the following:
a.
b.
c.
d.
e.
f.
g.
h.
P2O5
Ca(ClO3)2
NH4F
AlN
Fe(NO2)3
SnO2
H2SO3
H3P
Write formulas for the following:
diphosphorus pentoxide
calcium chlorate
ammonium fluoride
aluminum nitride
iron(III) nitrite
tin(IV) oxide or tin(II) peroxide
sulfurous acid
hydrophosphoric acid
a.
b.
c.
d.
e.
f.
g.
h.
lead (IV) sulfide
hydrosulfuric acid
dinitrogen trioxide
chromium (III) hydroxide
chromic acid
sodium carbonate
zinc oxalate
sulfur hexafluoride
PbS2
H2 S
N2O3
Cr(OH)3
H2CrO4
Na2CO3
ZnC2O4
SF6
18. Fill in the following chart
Formula
Lewis Structure
Geometry
Bond Angles
107°
Hybridizati
on
sp3
Molecular
Polarity
polar
pyramidal
104°
sp3
polar
H2S
bent or
angular
109.5°
sp3
nonpolar
CCl4
tetrahedra
l
linear
180°
sp
nonpolar
trigonal
planar
120°
sp2
polar
trigonal
bipyramid
al
90°, 120°
sp3d
nonpolar
octahedral
90°
sp3d2
nonpolar
PH3
6 lone pr on each Cl
CS2
CH2O
AsI5
(substitute I for F)
SeBr6
(substitute Br for F)
19. Find the mass of 2.25 x 1021 formula units of magnesium iodate.
Answer: 1.40g
20. Find the mass percent of water in nickel(II) cyanide tetrahydrate.
Answer: 39.43% H2O
21. A 5.0g sample of nickel(II) cyanide hydrate is heated until all water is removed. What mass of anhydrous
nickel(II) cyanide will remain? (REFER BACK TO #20 ON PREVIOUS PAGE!)
Answer: 3.0g Ni(CN)2
22. Identify all types of intermolecular forces in a-d:
a. Attraction between any two polar molecules ___dipole- dipole__________________
b. Very weak force that increases with molar mass ___London dispersion________________
c. Attraction between two induced dipoles _____ London dispersion ____________________
d. Very strong attractive force between molecules with N-H, O-H, or F-H bonds___H- bond______
23. Compare and contrast solids and liquids
24. Identify the type of solid in a-e:
a. Every atom is covalently bonded to another atom ___network covalent_________________
b. Atoms are surrounded by a sea of electrons _metallic________________________
c. Particles are connected only by IMF ___Molecular___________________________
d. There is no geometric pattern in the structure ______amorphous_________________
e. Charged particles in a geometric pattern _____ionic______________________
25. Explain the relationship between strong intermolecular forces and the following properties – volatility,
vapor pressure and boiling point: __The stronger IMFs , the lower the vapor pressure, the higher the boiling
point. Volatility is the tendency of a substance to vaporize. Volatility is directly related to a substance's
vapor pressure. At a given temperature, a substance with higher vapor pressure vaporizes more readily than
a substance with a lower vapor pressure.
26. Refer to the phase diagram below when answering the questions:
a. What is the normal freezing point of this substance? __100°C______
b. What is the physical state of this substance at 300°C and 0.50 atm ? __gas __________
c. If I had a quantity of this substance at a pressure of 1.25 atm and a temperature of 3000 C and lowered
the pressure to 0.25 atm, what phase transition(s) would occur? _vaporization________
27. Indicate whether a heating curve would be flat or rising in a-e.
a. Liquid is boiling _flat__________
b. Potential energy is increasing __flat__________
c. Solid is warming __rising_________
d. Kinetic energy is increasing ___rising___________
e. Solid is melting ____flat__________
28. How much heat does a 23.0 g ice cube absorb as its temperature increases from -17.4°C to 0.0°C? (use
constants from homework sheets).
836 J
29. A 50.6 g sample of silver at 97.4°C is placed into 104 g of water at 19.7°C. What is the final
temperature of the system? (CAg= 0.235J/g°C)
21.8°C
30. How much heat is required to change 20.0 g of ice at -13.0°C to steam at 125.0°C? (use constants from
homework sheets)
61.7 kJ
31. 50.0 L of gas has a temperature of 75°C. What is the Celsius temp when the volume changes to 110. L?
493°C
32. A balloon is filled with 3.0 L of helium at 1 atm. What is the volume when the balloon rises to an
altitude where the pressure is only 0.25 atm? (assume temperature remains constant.)
10L
33. The gas left in a used aerosol can is at a pressure of 1 atm at 27°C. If this can is thrown into a fire, what
is the internal pressure of the gas when its temperature reaches 927°C?
4 atm
34. 5.2 L of a gas is at STP. Find the new volume when the temperature rises to 38°C and the pressure
drops to 600 mmHg.
8L
35. Pressure and volume of a gas at constant temperature are ____ inversely ___ proportional. Why?
Particles collide more often in the smaller amount of space.
36. Volume and temperature of a gas at constant pressure are ___directly_______________ proportional.
Why? Faster moving particles need more space in order to keep pressure constant.
37. Which travels faster CO2 or O2? How much faster?
O2, it travels 1.17x faster
38. Gas A travels 4 times faster than Gas B. If the molar mass of Gas B is 80 g/mole, find the molar mass of
Gas A.
5 g/mol
39. A 250. ml sample of oxygen is collected over water at 25 ° C and 760.0 mmHg pressure. What is the
pressure of the dry oxygen alone? (Vapor pressure of water at 25°C = 23.8 mmHg).
736. 2 mmHg