Name: ________________________ Class: ___________________ Date: __________
ID: A
Extra Practice for Midterm
Multiple Choice
Identify the choice that best completes the statement or answers the question.
Important constants
For Water
ΔHfus = 6.01 kJ/mol or 334 J/g
ΔHvap = 40.7 kJ/mol or 2260 J/g
c = 4.18 J/goC or 1.00 cal/g oC
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1.
What type of bond do all of the molecules in the table above have in common?
a. polar
c. ionic
b. metallic
d. covalent
2. What is the volume of 63.8 g of Carbon Dioxide at a pressure of 75.0 kPa and a temperature of 345
K?
a. 22.4 L
c. 8.23 L
b. 55.4 L
d. 78.4 L
3. How much energy would be required to raise the temperature of 75.0 g of water from 25.0 oC to
75.0oC?
a. 15.7 kJ
c. 1.25 x 106 J
b. 334 kJ
d. 4.85 kJ
4. What is the correct noble gas electron configuration for a Chloride ion?
c. [Ne]3s23p5
a. [Ar]3s23p5
b. [Ar]3s23p6
d. [Ne]3s23p6
5. What is the correct order of the following bonds in terms of decreasing polarity?
a. As-Cl, P-Cl, N-Cl
c. P-Cl, N-Cl, As-Cl
b. As-Cl, N-Cl, P-Cl
d. P-Cl, As-Cl, N-Cl
6. How many lone pairs of electrons are on the central atom of nitrogen trihydride?
a. 1
c. 3
b. 2
d. 4
1
Name: ________________________
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7. Which of the following covalent bonds is the most polar?
a. C---C
c. C---Cl
b. C---Br
d. C---H
32+
8. Arrange the following elements: P , S , K , Ca2+, Sc3+, in order of increasing ionic size.
a. Sc3+, Ca2+, K+, S2-, P3c. P3-, S2-, K+, Ca2+, Sc3+
+
2+
3+
23b. K , Ca , Sc , S , P
d. Sc3+, Ca2+, K+, P3-, S29. Which of the following elements has the smallest atomic size?
a. Cesium
c. Calcium
b. Oxygen
d. Chlorine
10. A syringe contains 10 ml of a gas at 120. kPa. What is the pressure if the volume is compressed to 4.2 mL.
a. 50. kPa
c. 290 kPa
b. 350 kPa
d. 101.3 kPa
11. Why is boiling a cooling process?
a. The particles with less kinetic energy
c. The particles with more potential energy
b.
____
ID: A
leave the liquid first, leaving the
remaining particles with more kinetic
energy.
The particles with more kinetic energy
leave the liquid first, leaving the
remaining particles with less kinetic
energy.
d.
leave the liquid first, leaving the
remaining particles with less potential
energy.
The particles with less potential energy
leave the liquid first, leaving the
remaining particles with more potential
energy.
12.
In the above phase diagram for carbon dioxide, carbon dioxide is a liquid at 250 C and
a very high pressure. Carbon dioxide solidifies when the temperature decreases and the
pressure remains constant.
Which letter represents the point at which all three states coexist?
a. A
b. B
c. C
d. D
2
Name: ________________________
____
____
ID: A
13. What is the specific heat of a substance if 1560 cal are required to raise the temperature of a 312-g sample
by 15°C?
cal
g°C
cal
0.33
g°C
cal
g°C
cal
1.33
g°C
a. 0.033
c. 0.99
b.
d.
14. The following equation shows the reaction that occurs when nitroglycerine explodes.
4 C3H5O9N3 --> 12CO2 + 6N2 + O2 + 10H2O + 1725 kJ
This reaction is ____________.
a. endothermic
c. a combination reaction
b. exothermic
d. a combustion reaction
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15. How much heat must you add to boil 101 g of water at 100oC?
a. 4.18 x104 J
c. 2.26 x107 J
5
b. 2.28 x 10 J
d. 3.34 x 104
16. What is the molarity of 200 mL of solution in which 2.0 moles of sodium bromide is dissolved?
a. 2.0M
c. 0.40M
b. 4.0M
d. 10M
17. How many mL of a 2.0M NaBr solution are needed to make 200.0 mL of 0.50M NaBr?
a. 25 mL
c. 50 mL
b. 150 mL
d. 100 mL
18. What is the molality of a solution containing 8.0 grams of solute in 0.50 kg of solvent? (molar mass of
solute = 24 g)
a. 0.17m
b. 0.67m
c. 4m
d. 1.67m
3
Name: ________________________
ID: A
Multiple Response
Identify one or more choices that best complete the statement or answer the question.
____
19.
a. hydrochloric acid
b. sodium nitrate
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____
c. sucrose
d. ammonium sulfate
20. Carbon disulfide is nonpolar. The molecular shape and bond angle consistent with this
observation is _____.
a. A
c. C
b. B
d. D
21. How many valence electrons does an atom of any halogen group have?
a. 4
c. 7
b. 5
d. 8
4
Name: ________________________
ID: A
____
22. Using the electron dot structure, a phosphide ion would most look like _____.
____
a. A
c. C
b. B
d. D
23. Which of the following pairs of elements is most likely to form an ionic compound?
a. magnesium and fluorine
c. nitrogen and sulfur
b. sodium and aluminum
d. oxygen and chlorine
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24. Choose the correct molecular shapter for ammonia, NH3.
a. bent
c. trigonal planar
b. linear
d. trigonal pyramidal
25. What causes water molecules to have a bent shape, according to VSPER theory?
a. the attractive forces between the two c. ionic attractions and repulsion
hydrogen’s
b. the unusual location of the free
d. repelling from the unshared pairs of
electrons
electrons
26. This force will influence the temperature at which molecules change state.
a. electrostatic
c. electromagnetic
b. intermolecular
d. intramolecular
27.
Which of the following elements has the same Lewis dot structure as Silicon?
____
a. Germanium
c. Gallium
b. Aluminum
d. Arsenic
28. Which sample is composed of particles arranged in a regular geometric pattern?
a. Cl2 (g)
c. LiCl (s)
b. CCl4 (l)
d. LiCl (aq)
5
Name: ________________________
____
ID: A
29. Which structural formula represents a nonpolar molecule?
a.
____
c.
b.
d.
30. Which structural formula represents a polar molecule?
a.
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____
____
____
____
____
____
c.
b.
d.
31. Determine the shape of SCl2:
a. bent
c. tetrahedral
b. linear
d. trigonal pyramidal
32. The reason salt crystals, such as KCl, hold together so well is because the cations are strongly
attracted to
a. neighboring cations.
c. free electrons in the crystals.
b. the protons in the neighboring
d. neighboring anions.
nucleus.
33. Determine the shape of HNO:
a. linear
c. tetrahedral
b. bent
d. trigonal planar
34. What intermolecular forces are present in CH3OH?
a. Dispersion
c. Hydrogen Bonding
b. Dipole-Dipole
d. Ionic Bonding
35. Which of the following molecules will have hydrogen bonding?
a. H2O2
c. H2O
b. CH4
d. HF
36. What intermolecular forces are present between molecules of HCN?
a. Dipole-Dipole
c. Hydrogen Bonding
b. Dispersion
d. Ionic Bonding
37. Is the following process exothermic or endothermic?
CO2(l) --> CO2(s)
a. Endothermic
b. Exothermic
6
ID: A
Extra Practice for Midterm
Answer Section
MULTIPLE CHOICE
1. ANS: D
2. ANS: B
Stt. 4h
PTS:
PTS: 1
3. ANS: A
St. 7d
STA: 4h
4.
5.
6.
7.
8.
9.
PTS:
ANS:
ANS:
ANS:
ANS:
ANS:
ANS:
1
D
A
A
C
A
B
1
STA:
PTS:
PTS:
PTS:
PTS:
PTS:
7d
1
1
1
1
1
PTS:
1
STA:
PTS:
PTS:
STA:
PTS:
PTS:
PTS:
STA:
PTS:
STA:
PTS:
STA:
7a
1
1
Ch.7.d
1
1
1
Ch.6.d
1
Ch.6.d
1
Ch.6.d
STA: 2b
St. 1c
PTS: 1
10. ANS: C
11. ANS: B
St. 7a
12.
13.
14.
15.
16.
17.
18.
PTS:
ANS:
ANS:
OBJ:
ANS:
ANS:
ANS:
OBJ:
ANS:
OBJ:
ANS:
OBJ:
1
D
B
17.1.3
B
B
D
16.2.1
C
16.2.2
B
16.4.1
1
DIF:
L1
REF: p. 509 | p. 510
DIF:
L2
REF: p. 481
DIF:
L2
REF: p. 483 | p. 484
DIF:
L2
REF: p. 491
ID: A
MULTIPLE RESPONSE
19. ANS: C
2c
PTS: 1
20. ANS: B
2f
PTS: 1
21. ANS: C
2a
PTS: 1
22. ANS: C
2e
PTS: 1
23. ANS: A
2c
PTS: 1
24. ANS: D
2f
PTS: 1
25. ANS: D
2f
PTS: 1
26. ANS: B
2c
PTS: 1
27. ANS: A
2e
PTS: 1
28. ANS: C
2c
PTS:
1
2
ID: A
29. ANS: C
2f
PTS: 1
30. ANS: D
2f
PTS: 1
31. ANS: A
2f
PTS: 1
32. ANS: D
2c
PTS: 1
33. ANS: B
2f
34.
35.
36.
37.
PTS:
ANS:
ANS:
ANS:
ANS:
1
A, B, C
A, C, D
A, B
B
PTS:
PTS:
PTS:
PTS:
1
1
1
1
3