1. To the correct number of significant figures, (5.0 x
10-5)÷(2.00 x 10-2) is
2.50 x
10
4
2.5 x
10
-7
2.5 x
10
-4
2.5 x
10
-3
2.50 x
10
-3
none of
these
2. The density of mercury is 13.6 g/mL. How many pounds does one
quart of mercury weigh? (1 pound is 454 g, 4 quarts are 3.7854
liters.)
(13.6 x 454 x 1000 x 3.7854)/4
(13.6 x 1000 x 4)/(454 x 3.7854)
(13.6 x 1000 x 3.7854)/(454 x 4)
(13.6 x 454 x 3.7854)/(1000 x 4)
(13.6 x 3.7854)/(454 x 1000 x 4)
none of these
3. The fuel tank of a Toyota Tercel holds 11.4 gallons of gasoline.
What is the equivalent volume in cubic centimeters? (1 gallon is
3.7854 liters).
(11.4 x
11.4 x 3.7854 x 1000
11.4 x 3.7854 x 100
11.4/(3.7854 x
none of these
1000)/3.7854
(11.4 x
1000)
3.7854)/1000
4. Which of the following measurements are equivalent?
10 micrograms and
40 km and 40000 cm
all of these
0.01 mm and 1 x
none of these
0.1 milligrams
10 nL and 1000 pL
10
-3
cm
5. A crime lab analyzes two samples of a drug, sample A and sample
B. Sample A is crystalline. Several microscopic samples taken from
different points in Sample A are indistinguishable; all
properties of the material seem uniform. Sample B has a slightly
different color than sample A. Chromatographic techniques resolve
sample B into separate components. Which of the following
conclusions are valid?
1. Sample A is a pure substance.
2. Sample B is a mixture.
3. Sample A is not a heterogeneous mixture.
2 and 3
1 and 2
1 and 3
all are valid
none are valid
6. Which of the following lists of elements contains an alkaline
earth metal, a transition metal, and a halogen, respectively?
Rb, Y,
I
Ba, Fe,
Br
Sr, Zr,
Xe
K, Ni,
O
none of
these
all of
these
7. A beam of particles is passed between a positively charged
and a negatively charged plate. The beam splits into three parts
while passing between the plates. Beam A is slightly deflected
towards the negatively charged plate; Beam B is strongly deflected
towards the positively charged plate, and beam C is undeflected.
Which of the following conclusions is correct?
1. Particles in beam A are positively charged.
2. B particles are more massive than A particles.
3. C particles are negatively charged.
1 and 3
2 only
3 only
1 and 2
1 only
2 and 3
8. Rutherford's alpha particle scattering experiments showed
that while most alpha particles fired at a metal foil sample passed
straight through, about 1 in 104 were scattered backwards.
Rutherford realized that this phenomenon could be accounted for
by assuming that
alpha particles must be ricocheting off the electrons
all of the positive charge and most of the mass of the atom
is concentrated in a tiny kernel
atoms were indestructible and reflected alpha particles
alpha particles were annhilating the metal atoms
Thomson's plum pudding model was valid
none of the above
9. Bromine has two common isotopes,
Br and
79
Br. Which is the
81
following statements is true?
81
Br has two more electrons
79
Br has 79 neutrons.
79
than
Br.
79
Br has 35 electrons and 44
81
Br has two more protons
protons.
79
than
Br.
none of these
81
than
Br has two more neutrons
79
Br.
10. The average atomic mass of Cl is 35.453. About 75% of all
Cl atoms are
Cl. If there is only one other common isotope, it
35
is most likely to be
36
Cl
37
38
Cl
34
Cl
35.453
Cl
Cl
none of these
11. Which of the following compounds are correctly named?
Cu(HCO3)2, copper (II)
SrSO3, strontium sulfate
bicarbonate
FeCO3, iron (III) carbonate
Ba3(PO4)2, tribarium diphosphate
none of these
AgNO3, argentum nitrate
12. Cadmium (II) selenide can be used to prepare solutions which
have almost any color in the spectrum. If the selenide ion is Se2-,
the formula for this compound is
CdSe2
Cd2Se
CdSe
Cd2Se2
Cd-II-Se
none of these
13. Which of the following is the formula for hydrosulfuric acid?
HS
H2S
H2SO2
H2SO3
H2SO4
HSO4
14. The following equation for the combustion of glucose is NOT
balanced:
C6H12O6(s) + O2(g) = CO2(g) + H2O(l)
If the equation is balanced with smallest integer coefficients,
the coefficient of O2(g) is
18
9
6
12
15
none of these
15. Mixing which of the following will produce a precipitation
reaction?
none of these
NaOH and KBr
AgNO3
HNO3(aq) and
Zn and HCl
Na2SO4(aq) and
Sr(OH)2(aq)
and NaClO4
Ba(OH)2(aq)
16. Which of the following species are present in an aqueous
acetic acid solution?
all of these
+
H3O (aq)
-
HC2H3O2(aq)
-
C2H3O2 (aq)
OH (aq)
H2O(l)
17. Which of the following is the net ionic equation for the
reaction between hydrochloric acid and potassium hydroxide?
HCl(aq) + KOH(aq) = H2O(l) + KCl(aq)
+
-
K (aq) + Cl (aq) = KCl(aq)
+
-
K (aq) + Cl (aq) = KCl(s)
+
-
+
-
+
-
K (aq) + Cl (aq) + H (aq) + OH (aq) = H2O(l) + K (aq) + Cl (aq)
+
-
H3O (aq) + OH (aq) = 2 H2O(l)
HClO4(aq) + KOH(aq) = H2O(l) + KClO4(aq)
18. A well near the beach is suspected to be contaminated with
chloride ions from sea water. If chloride is present, which of
the following will produce a cloudy suspension when mixed with
the water?
acetic
LiBr
NaNO3(aq)
KC2H3O2(aq)
AgNO3(aq)
acid
none of
these
19. Ammonium nitrate is used as a nitrogen fertilizer. What is
the percentage of nitrogen by mass in ammonium nitrate? (The
atomic weights of N, H, and O are 14.0, 1.0, and 16.0,
respectively.)
43.8%
35.4%
17.5%
42.9%
35.0%
none of these
20. A compound of sulfur and oxygen is 40.1% sulfur by mass. What
is the empirical formula for the compound? The atomic weights of
S and O are 32.07 and 16.00, respectively.
SO
SO4
SO2
S2O3
SO3
none of these
21. The first step in an analysis of water for dissolved oxygen
involves the reaction
4 Mn(OH)2(aq) + O2(aq) + 2 H2O(aq) = 4 Mn(OH)3(s)
.If treatment of 1.000 L of water from a creek with excess
Mn(OH)2(aq) produces 0.103 g of Mn(OH)3, how many grams of O2(aq)
does one liter of the water contain? The molecular weights of
Mn(OH)2 and Mn(OH)3 are 88.94 and 105.94, respectively.
(0.103 x 32)/(88.94 x 4)
(0.103 x 16)/(105.94 x 4)
(0.103 x 105.94 x 32)/4
(0.103 x 32)/(105.94 x 4)
(0.103 x 4 x 32)/105.94
(0.103 x 16)/(88.94 x 4)
22. Sucrose (table sugar) has empirical formula CH2O and
molecular weight 360. The atomic weights of C, H, and O are 12,
1, and 16, respectively. The molecular formula of sucrose is
C6H12O6
C12H24O12
C360H720O360
CH2O
C12H12O12
none of these
23. Oxygen gas is converted to ozone gas by exposure to intense
ultraviolet light:
3 O2(g) = 2 O3(g)
If an ultraviolet source converts oxygen to ozone with a 4% yield,
how many grams of oxygen are required to produce 1 gram of ozone?
The atomic weight of O is 16.
1.5 g
25 g
0.04 g
0.06 g
1 g
none of these