Chem 101 Fall 2012 Exam 2 Section 001
1. A 91.8-g sample of Ca contains how many calcium atoms?
A) 91.8 atoms
B) 183.6 atoms
C) 2.29 100 atoms
D) 5.53 1025 atoms
E) 1.38 1024 atoms
2. 2.000 moles of aluminum contain how many grams of aluminum?
A) 53.96g
B) 26.98g
C) 13.49g
D) 13.00g
E) 1.000g
3. What is the percent (by mass) of carbon in propane, C3H8?
A) 27.3 %
B) 37.5 %
C) 74.9 %
D) 79.9 %
E) 81.7 %
4. Which of the following compounds contains one or more covalent bonds?
A) KCl
B) MgO
C) CS2
D) Cs2F
E) CaBr2
5. How many moles of Ca are in 960.5 g Ca?
A) 4.173 10–2 mol
B) 23.96 mol
C) 3.850 104 mol
D) 47.93 mol
E) 960.5 mol
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6. What is the molar mass of Al(OH)3?
A) 43.99 g/mol
B) 51.02 g/mol
C) 78.00 g/mol
D) 75.99 g/mol
E) 46.00 g/mol
7. True or false? Covalent bonding occurs when a metal reacts with a nonmetal.
A) True
B) False
8. Which of the following is not the correct chemical formula for the compound named?
A) sodium carbide Na4C
B) calcium sulfide
CaS
C) magnesium oxide MgO
D) tin(II) peroxide Sn2O
E) iron (III) oxide
Fe2O3
9. How many atoms are in 3.50 moles of lithium, Li?
A) 6.941 atoms
B) 3.500 atoms
C) 6.022 x 1023 atoms
D) 1.204 x 1024 atoms
E) 2.108 x 1024 atoms
10. How many molecules of carbon dioxide, CO2, are in 1.500 moles of CO2?
A) 1.500 molecules
B) 44.01 molecules
C) 6.022 x 1023 molecules
D) 9.033 x 1023 molecules
E) 1.204 x 1024 molecules
11. You have 45.00 grams of water, H2O in a beaker. How many moles of water do you
have?
A) 1.008 moles
B) 2.498 moles
C) 18.02 moles
D) 45.00 moles
E) 6.022 x 1023 moles
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12. Calculate the molecular formula of a compound with the empirical formula CH2O and a
molar mass of 90.078 g/mol.
A) C2H4O2
B) C3H6O3
C) C4H8O4
D) C5H10O5
E) C6H12O6
13. True or false? The atomic mass is the mass in grams of one mole of the element.
A) True
B) False
14. The nitrate ion is
A) Ni2+
B) Ni II
C) NO3D) NO2E) NO4215. Which of the following has a triple bond? (Draw the Lewis structure)
A) CH4
B) CO
C) SO2
D) NO3E) none of these
16. The chloride ion is
A) ClB) Cl2C) Cl+
D) Cl2
E) ClO4217. Which of the following contains only nonpolar covalent bonds?
A) FeO
B) HCl
C) H2O
D) Mg3N2
E) Cl2
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18. A compound is analyzed and found to contain 7.1% carbon, 9.4% oxygen, and 83.5%
chlorine (by mass). Calculate the empirical formula of this compound.
A) COCl
B) COCl2
C) CO2Cl
D) CO2Cl2
E) COCl4
19. Which one of the following species has the same electron configuration as an atom of
argon?
A) SB) Cl2C) K
D) Ca2+
E) Kr
20. Which substance has more mass, 1 mole of calcium, Ca, or 1 mole of potassium, K?
A) Calcium
B) Potassium
C) Neither, 1 mole of Ca and K have the same mass
21. Which of the following compounds has at least one ionic bond?
A) N2O4
B) SF6
C) NI3
D) SO3
E) Al2O3
22. Cl2O contains what type of bonds?
A) ionic
B) covalent
C) metallic
23. The correct electron configuration for Ca is
A) 1s22s22p63s23p33d4
B) 1s22s22p63s23p64s1
C) 1s22s22p62d9
D) 1s22s22p63s23p7
E) 1s22s22p63s23p64s2
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24. What element has the electron configuration 1s22s22p63s23p5?
A) Ar
B) Cl
C) Kr
D) S
E) none of these
25. What is the balanced equation showing the reaction between sodium metal and water to
form aqueous sodium hydroxide and hydrogen gas.
A) Na(s) +H2O(l) NaOH(aq) +H2(g)
B) Na(s) +2H2O(l) Na(OH)2(aq) +2H2(g)
C) 2Na(s) +2H2O(l) 2NaOH(aq) +H2(g)
D) Na(s) +2H2O(l) NaOH(aq) +H2(g)
26. What is the shorthand or noble gas core electron configuration for the sulfide ion, S2- ?
A) [Ne]
B) [Ne] 3p4
C) [Ar]
D) [Ne]3s23p4
E) 1s22s22p63s23p6
27. What is the element represented by 1s22s22p1
A) H
B) Be
C) B
D) He
E) Ne
28. What are the equivalencies for platinum?
A) 1 mole of Pt = 6.02 x 1023 atoms of Pt = 195.08g of Pt
B) 1 mole of Pt = 6.02 x 1023 molecules of Pt2 = 390.16g of Pt2
C) 1 mole of Pt = 195.08 molecules of Pt = 6.02 x 1023 g of Pt
D) 1 mole of Pt = 6.02 x 1023 atoms of Pt = 6.02 x 1023 g of Pt
29. What are the equivalencies for carbon dioxide?
A) 1 mole of CO2 = 6.02 x 1023 atoms of CO2 = 12.011g of CO2
B) 1 mole of CO2 = 6.02 x 1023 molecules of CO2 = 44.009g of CO2
C) 1 mole of CO2 = 44.009 x 1023 molecules of CO2 = 6.02 x 1023 g of CO2
D) 1 mole of CO2 = 18.06 x 1023 molecules of CO2 = 44.009g of CO2
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30. When the following equation is balanced using the smallest possible integers, what is
the number in front of the substance in bold type?
Pb(NO3)4 + K2CO3
A)
B)
C)
D)
E)
Pb(CO3)2 + KNO3
5
4
3
2
1
31. When the following equation is balanced using the smallest possible integers, what is
the number in front of the substance in bold type?
AlBr3 + K2SO4
A)
B)
C)
D)
E)
Al2(SO4)3 + KBr
5
4
3
2
1
32. When the following equation is balanced using the smallest possible integers, what is
the number in front of the substance in bold type?
CH4 + O2
A)
B)
C)
D)
E)
CO2 + H2O
5
4
3
2
1
33. When the following equation is balanced using the smallest possible integers, what is
the number in front of the substance in bold type?
Al + HCl
A)
B)
C)
D)
E)
5
4
3
2
1
6
AlCl3 + H2
Answer Key
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E
A
E
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E
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B
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B
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C
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