CHEMISTRY HONORS QUARTER 2 REVIEW
(chapter numbers correspond with textbook chapters order)
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CHAPTER 8
Define 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
various ions
Define and give examples for:
o Ionic bonds
o Metallic bonds
Name compounds containing ions and
polyatomic ions
Construct chemical formulas based on
chemical name
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CHAPTER 9
Name covalent compounds using numeric
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:
o Shape
o Bond angle
o Polarity
o Hybrid orbital
Define covalent bond and explain how one
works
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
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List the characteristics of covalently bonded
molecules
Explain resonance. Draw resonance
structures for molecules.
CHATPER 11
Convert the number of:
o Moles to grams
o Grams to moles
o Molecules to moles
o Moles to molecules
o Grams to molecules
o Molecules to grams
Determine the:
o Molar mass of compounds
o Percent composition
o Molecular formula
o Hydrates
o Empirical formula
CHEMISTRY HONORS QUARTER 2 REVIEW
(chapter numbers correspond with textbook chapters order)
CHAPTER 13
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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
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Boyle’s law
Charles’s law
Gay- Lussac's law
Combined gas law
CHAPTER 14
CHAPTER 16
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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?
17. Name the following:
a. P2O5
b. Ca(ClO3)2
c. NH4F
d. AlN
e. Fe(NO2)3
f. SnO2
g. H2SO3
h. H3P
Write formulas for the following:
a. lead (IV) sulfide
b. hydrosulfuric acid
c. dinitrogen trioxide
d. chromium (III) hydroxide
e. chromic acid
f. sodium carbonate
g. zinc oxalate
h. sulfur hexafluoride
18. Fill in the following chart
Formula
Lewis
Structure
Geometry
Bond Angles
Hybridization
Molecular
Polarity
PH3
H2S
CCl4
CS2
CH2O
AsI5
SeBr6
19. Find the mass of 2.25 x 1021 formula units of magnesium iodate.
20. Find the mass percent of water in nickel(II) cyanide tetrahydrate.
21. A 5.0g sample of nickel(II) cyanide is heated until all water is removed. What mass of
anhydrous nickel(II) cyanide will remain?
22. Identify all types of intermolecular forces in a-d:
a. Attraction between any two polar molecules _____________________
b. Very weak force that increases with molar mass ___________________
c. Attraction between two induced dipoles _________________________
d. Very strong attractive force between molecules with N-H, O-H, or F-H bonds_________
23. Compare and contrast solids and liquids
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24. Identify the type of solid in a-e:
a. Every atom is covalently bonded to another atom ____________________
b. Atoms are surrounded by a sea of electrons _________________________
c. Particles are connected only by IMF ______________________________
d. There is no geometric pattern in the structure _______________________
e. Charged particles in a geometric pattern ___________________________
25. Explain the relationship between strong intermolecular forces and the following
properties – volatility, vapor pressure and boiling point:
___________________________________________________________________________
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26. Refer to the phase diagram below when answering the questions:
a. What is the normal freezing point of this substance? ________
b. What is the physical state of this substance at 300°C and 0.50 atm ? ____________
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? _________
27. Indicate whether a heating curve would be flat or rising in a-e.
a. Liquid is boiling ___________
b. Potential energy is increasing ____________
c. Solid is warming ___________
d. Kinetic energy is increasing ______________
e. Solid is melting ______________
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).
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)
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)
31. 50.0 L of gas has a temperature of 75°C. What is the temp in Celsius when the volume
changes to 110. L?
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.)
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?
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.
35. Pressure and volume of a gas at constant temperature are __________________
proportional. Why? __________________________________________________
36. Volume and temperature of a gas at constant pressure are __________________
proportional. Why? ______________________________________________________
37. Which travels faster CO2 or O2? How much 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.
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).