practice exam

Name___________________________________________
Chem 111 Practice Exam 1
Summer 2014
(60 points) MULTIPLE CHOICE. Choose the answer that best completes the statement or answers the question.
1)
Round off 807509 to four significant figures.
a.
8076
b.
00 81
c.
8100
d.
8.075 × 105 2)
Convert 5.100 × 10-3 to ordinary notation.
a.
5100
b.
0.0005100
c.
510.0
d.
0.005100 3)
To the correct number of significant figures, an automobile traveling at 28 mi/h is traveling at ________ km/h (1 km = 0.6214 mi).
a.
45
b.
17.40
c.
45.06
d.
17 4)
The horizontal rows of the periodic table are called
a.
triads.
b.
elements.
c.
periods.
d.
groups. 5)
Gaseous elements characterized by low reactivity are found in group ________ of the periodic table.
a.
7A
b.
8A
c.
5A
d.
6A 6)
Which subatomic particle has the smallest mass?
a.
a proton
b.
a neutron
c.
an alpha particle
d.
an electron 7)
What group of elements does the shaded area in the following periodic table indicate?

a. alkali metals
b.
alkaline earth metals
c.
inner transition metals
d.
transition metals 8)
What are the possible values of l if n = 5?
a.
5
b.
-4, -3, -2, -1, 0, +1, +2, +3, or +4
c.
0, 1, 2, 3, or 4
d.
-5, -4, -3, -2, -1, 0, +1, +2, +3, +4, or +5 9)
How many electrons can a single orbital hold?
a.
8
b.
2n
c.
2l + 1
d.
2 10)
What is the ground-state valence-shell electron configuration of the group of elements indicated by the shaded portion of the periodic table?

a. ns2 (n-1) d 2
b.
ns2
c.
ns2 (n-2) f 2
d.
ns2np2 11)
The average mass of an oxygen atom is 5.3 × 10-26 kg. Calculate the kinetic energy of a mole of oxygen atoms, all moving at a speed of 400 m/s (1000 mph). K. E. = .
a.
8.2 × 10-21 J
b.
5200 J
c.
2600 J
d.
13,000 J 12)
Which of the following is the lowest temperature?
a.
313 K
b.
54°F
c.
37°C
d.
All of these temperatures are all equal. 13)
All of the following elements are nonmetals except
a.
carbon.
b.
oxygen.
c.
hydrogen.
d.
antimony. 14)
Fullerenes are molecules composed of only carbon atoms. A molecule of one fullerene has a mass of
1.516 × 10-21 g. How many carbon atoms are in a single molecule of this fullerene molecule?
a.
76
b.
84
c.
60
d.
70 15)
Which of the following represent electron configurations that violate the Pauli exclusion principle?
(A) [Ne]3s13p5(B) [Kr]4d125s25p3(C) [Ar]3d104s24p2
a.
only (A)
b.
only (B)
c.
(B) and (C)
d.
(A) and (B) 16)
The element In has how many valence electrons?
a.
1
b.
13
c.
2
d.
3 17)
Which are isotopes? An atom that has an atomic number of 34 and a mass number of 76 is an isotope of an atom that has
a.
42 protons and 34 neutrons.
b.
42 neutrons and 34 protons.
c.
an atomic number of 34 and a mass number of 80.
d.
an atomic number of 32 and a mass number of 76. 18)
How many moles and how many atoms of zinc are in a sample weighing 34.9 g?
a.
1.87 mol, 1.13 × 1024 atoms
b.
0.533 mol, 3.21 × 1023 atoms
c.
1.87 mol, 3.10 × 10-24 atoms
d.
0.533 mol, 8.85 × 10-25 atoms 19)
What is the sum of the coefficients when the following equation is balanced using the lowest, whole numbered coefficients?
___ PH3(g) + ___ O2(g) → ___ P4O10(s) + ___ H2O(g)
a.
10
b.
12
c.
22
d.
19 20)
What is the molar mass of Co(NO3)2?
a.
183 g/mol
b.
121 g/mol
c.
90 g/mol
d.
152 g/mol
(12 points) For each of the formulas, write the name of the compound:
SCl2 __________________________________________
Fe3P2 _________________________________________
Ag2SO4 _______________________________________
BF3 ___________________________________________
(12 points) For each of the names, write the chemical formula:
Copper (II) nitride _________________________________
Sodium hypochlorite________________________________
Phosphorus trihydride ______________________________
Potassium bicarbonate ___________________________________
(16 points) Propane (C3H8) burns in oxygen to produce carbon dioxide and water. Calculate the mass of CO2 that can be produced if the reaction of 45.0 g of propane and excess oxygen has a 60.0 % yield.
C3H8 (g) + 5 O2 (g) 3 CO2 (g) + 4 H2O (g)
Potentially Useful Information:
D (density) = QUOTE
TF = 1.8(TC) + 32 °
TK = oC + 273
6.022 x 1023 molecules (atoms) = 1 mole

WORKING PAGE: