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1. Matter in which physical state has no specific shape but does have a specific volume?
a. gas
b. solid
c. liquid
d. salts
e. ice
2. A combination of sand, salt, and water is an example of a __________.
a. homogeneous mixture
b. heterogeneous mixture
c. compound
d. pure substance
e. solid
3. If matter is uniform throughout, cannot be separated into other substances by physical
processes, but can
be decomposed into other substances by chemical processes, it is ________.
a. a heterogeneous mixture
b. an element
c. a homogeneous mixture
d. a compound
e. a mixture of elements
4. Which of the following are chemical processes?
1. rusting of a nail
2. freezing of water
3. decomposition of water into hydrogen and oxygen gases
4. compression of oxygen gas
a.
b.
c.
d.
e.
2, 3, & 4
1, 3, & 4
1&3
1&2
1&4
5. Which of the following is not a physical property of water?
a. It is a liquid at room temperature.
b. It can be decomposed into oxygen and hydrogen gases.
c. It boils at 100oC.
d. It melts at 0oC.
e. These are all physical properties of water.
6. What is the volume of a 12.2 g piece of metal with a density of 9.43 g/cm3?
a. 12.2 cm3
b. 1.29 cm3
c. 0.773 cm3
d. 115 cm3
e. none of these
7. "Absolute zero" refers to _______.
a. 0 Kelvin
b. 0o Fahrenheit
c. 0o Celsius
d. oC + 9/5(oF - 32)
e. 273.15 oC
8. 1.035 x 10-4L = _____ mL
a. 1.035 x 107
b. 1.035 x 10-7
c. 0.1035
d. 1.035
e. 0.01035
9. Precision refers to _______.
a. how close a measured number is to other measured numbers
b. how close a measured number is to the true value
c. how close a measured number is to the calculated value
d. how close a measured number is to zero
e. how close a measured number is to infinity
10.
Accuracy refers to _______.
a. how close a measured number is to zero
b. how close a measured number is to the calculated value
c. how close a measured number is to other measured numbers
d. how close a measured number is to the true value
e. how close a measured number is to infinity
11.
A certain liquid has a density of 2.67 g/cm3. What would the mass be (in kg) of
30.5 mL of this liquid?
a. 81.4
b. 11.4
c. 0.0875
d. 0.0814
e. 0.0114
12.
Isotopes are atoms that have the same number of _________ but differing number
of _________.
a. protons, electrons
b. neutrons, protons
c. protons, neutrons
d. electrons, protons
e. neutrons, electrons
13.
In the periodic table, the elements are arranged in __________.
a.
b.
c.
d.
e.
14.
alphabetical order
order of increasing atomic number
order of increasing metallic properties
order of increasing neutron content
reverse alphabetical order
In the periodic table, the rows are called _____ and the columns are called _____.
a.
b.
c.
d.
e.
octaves, groups
staffs, families
periods, groups
congeners, families
rows, groups
15.
The element __________ is the most similar to strontium in chemical and physical
properties.
a. Li
b. At
c. Rb
d. Ba
e. Cs
16.
Which one of the following molecular formulas is also an empirical formula?
a. C6H6O2
b. C2H6SO
c. H2O2
d. H2P4O6
e. C6H6
17.
When the reaction below is balanced, the coefficients are __________.
NH3 + O2 → NO2 + H2O
a.
b.
c.
d.
e.
1,1,1,1
4,7,4,6
2,3,2,3
1,3,1,2
none of these
18.
What is the coefficient of Fe3O4 when the following equation is balanced?
Al + Fe3O4 → Al2O3 + Fe
a. 2
b. 3
c. 4
d. 5
e. 1
19.
Of the following compounds, which one will form something other than carbon
dioxide and water when combusted?
a.
b.
c.
d.
e.
C2H6
CH4
C32H44O9
CH3OCH3
C5H5N
20.
What is the coefficient of O2 when the following equation is balanced?
C4H8O2 + O2 → __________
a. 2
b. 3
c. 5
d. 6
e. 1
21.
Of the reactions below, which one is not a combination reaction?
a.
b.
c.
d.
e.
C + O2 → CO2
2Mg + O2 → 2MgO
2N2 + 3H2 → 2NH3
CaO + H2O → Ca(OH)2
Cd(NO3) + Na2S → CdS + 2NaNO3
22.
Of the reactions below, which one is a decomposition reaction?
a.
b.
c.
d.
e.
23.
The balanced equation for the decomposition of sodium azide is ____________.
a.
b.
c.
d.
e.
24.
NH4Cl → NH3 + HCl
2Mg + O2 → 2MgO
2N2 + 3H2 → 2NH3
Zn + Cu(NO3)2 → Cu + Zn(NO3)2
Cd(NO3)2 + Na2S → CdS + 2NaNO3
2NaN3(s) → 2Na(s) + 3N2(g)
2NaN3(s) → Na2(s) + 3N2(g)
NaN3(s) → Na(s) + N2(g)
NaN3(s) → Na(s) + N2(g) + N(g)
2NaN3(s) → 2Na(s) + 2N2(g)
Which of the following are combination reactions?
1) CH4(g) + O2(g) → CO2(g) + H2O(l)
2) CaO(s) + CO2(g) → CaCO3(s)
3) Mg(s) + O2(g) → MgO(s)
4) PbCO3(s) → PbO(s) + CO2(g)
a.
b.
c.
d.
e.
25.
1, 2, and 3
2 and 3
1, 2, 3, and 4
4 only
2, 3, and 4
Which of the following are combustion reactions?
1) CH4(g) + O2(g) → CO2(g) + H2O(l)
2) CaO(s) + Co2(g) → CaCO3(s)
3) PbCO3(s) → PbO(s) + CO2(g)
4) CH3OH(l) + O2(g) → CO2(g) + H2O(l)
a. 1 and 4
b. 1, 2, 3, and 4
c. 1, 3, and 4
d. 2, 3, and 4
e. 3 and 4
26.
Knowing that sodium reacts with water to form sodium hydroxide and hydrogen
gas, you may reasonably predict that ____________.
a.
b.
c.
d.
e.
27.
sodium will react with hydrogen gas to form sodium hydride
potassium will react with water to form potassium hydroxide and hydrogen gas
potassium will react with sodium
sodium will react with water to form sodium hydride
sodium hydroxide will react with water to form sodium oxide
The formula weight (amu) of silver chromate is __________.
a.
b.
c.
d.
e.
159.87
223.87
331.73
339.86
175.87
28.
What is the mass % of carbon in dimethylsulfoxide, C2H6SO?
a. 60.0
b. 20.6
c. 30.7
d. 7.74
e. 79.8
29.
There are __________ mol of carbon atoms in 4 mol of dimethylsulfoxide
(C2H6SO).
a. 2
b. 6
c. 8
d. 4
e. 3
30.
How many sulfur atoms are there in 25 molecules of C4H4S2?
a. 1.5 x 1025
b. 4.8 x 1025
c. 3.0 x 1025
d. 50
e. 6.02 x 1023
31.
A sample of CH4O with a mass of 32.0 g contains __________ molecules of
CH4O.
a. 5.32 x 10-23
b. 1.00
c. 1.88 x 1022
d. 6.02 x 1023
e. 32.0
32.
What is the empirical formula of a compound that contains 27.0% S, 13.4% O, and
59.6% Cl?
a.
b.
c.
d.
e.
33.
The empirical formula of a compound with the molecular formula C8H16 and a
molecular weight of 112.21 amu is __________.
a.
b.
c.
d.
e.
34.
SOCl
SOCl2
S2OCl
SO2Cl
ClSO4
C8H16
CH3
C2H8
C3H
CH2
A compound contains 40.0% C, 6.71% H, and 53.29% O by mass. The molecular
mass of the compound is 60.05 amu. The molecular formula of this compound is
__________.
a. C2H4O2
b. CH2O
c. C2H3O4
d. C2H2O4
e. CHO2
35.
A sample of nitrogen (9.27 g) reacts completely with magnesium, according to the
equation:
3 Mg + N2 → Mg3N2
The mass of Mg consumed is _____ g.
a. 8.04
b. 24.1
c. 16.1
d. 0.92
e. 13.9
36.
What mass (g) of carbon dioxide will be produced by the complete combustion of
0.4560 g of C5H19O?
a. 1.054
b. 0.02395
c. 0.004790
d. 2.108
e. 0.5270
37.
How many quantum numbers are necessary to designate a particular orbital in an
atom?
a. 4
b. 2
c. 1
d. 3
e. 5
38.
How many p-orbitals are there in a Ne atom?
a. 0
b. 1
c. 6
d. 3
e. 2
39.
How many quantum numbers are necessary to designate a particular electron in an
atom?
a. 3
b. 4
c. 2
d. 1
e. 5
40.
[Ar]4s23d104p3 is the electron configuration of an _____ atom.
a. As
b. V
c. P
d. Sb
e. Sn
41.
The electron configuration of a ground-state Ag atom is _____.
a. [Ar]4s24d9
b. [Kr]5s14d10
c. [Kr]5s23d9
d. [Ar]4s14d10
e. [Kr]5s24d10
42.
In which group of elements would all members be expected to have very similar
chemical properties?
a. O, S, Se
b. N, O, F
c. Na, Mg, K
d. S, Se, Si
e. Ne, Na, Mg
43.
Atomic radius generally increases as we move __________.
a. down a group and from right to left across a period
b. up a group and from left to right across a period
c. down a group and from left to right across a period
d. up a group and from right to left across a period
e. down a group. The period position has no effect.
44.
Which one of the following elements has the largest atomic radius?
a. O
b. F
c. Al
d. P
e. B
45.
The first ionization energies of the elements _______ as you go from left to right
across a period of the periodic table, and ________ as you go from the bottom to
the top of a group in the table.
a. increase, increase
b. increase, decrease
c. decrease, increase
d. decrease, decrease
e. are completely unpredictable
46.
Which of the following has the largest second ionization energy?
a. Ca
b. K
c. Ga
d. Ge
e. Se
47.
Which of the following correctly represents the second ionization of phosphorus?
a. P+(g) + e- → P2+(g)
b. P(g) → P+(g) + ec. P-(g) + e- → P2-(g)
d. P+(g) → P2+(g) + ee. P+(g) + e- → P(g)
48.
The ___ have the most negative electron affinities.
a. alkaline earth metals
b. alkali metals
c. halogens
d. transition metals
e. chalcogens
49.
In general, as you go across a period in the periodic table from left to right: (1) the
atomic radius __________; (2) the electron affinity becomes __________ negative;
and (3) the first ionization energy ___________.
a. decreases, decreasingly, increases
b. increases, increasingly, decreases
c. increases, increasingly, increases
d. decreases, increasingly, increases
e. decreases, decreasingly, decreases
50.
Sodium is much more apt to exist as a cation than is chlorine. This is because
____________.
a. chlorine is a gas and sodium is a solid
b. chlorine has a greater electron affinity than sodium does
c. chlorine is bigger than sodium
d. chlorine has a greater ionization energy than sodium does
e. chlorine is more metallic than sodium
51.
Of the elements below, __________ is the most metallic.
a. sodium
b. barium
c. magnesium
d. calcium
e. cesium
52.
In the Lewis symbol for a fluorine atom, there are _____ paired and _____
unpaired electrons.
a. 4, 2
b. 4, 3
c. 2, 5
d. 6, 1
e. 0, 5
53.
Based on the octet rule, phosphorus most likely forms a ______ ion.
a. P3+
b. P3c. P5+
d. P5e. P+
54.
How many unpaired electrons are there in the Lewis structures of a N3- ion?
a. 0
b. 1
c. 2
d. 3
e. This cannot be predicted.
55.
Which ion below has a noble gas electron configuration?
a. Li2+
b. Be2+
c. B2+
d. C2+
e. N2-
56.
According to VSEPR theory, if there are 4 pairs of electrons in the valence shell of
an atom, they will be arranged in a(n) _________ geometry.
a. octahedron
b. straight line
c. tetrahedron
d. trigonal plane
e. trigonal bipyramid
57.
A sample of a gas (5.0 mol) at 1.0 atm is expanded at constant temperature from 10
L to 15 L. The final pressure is _____ atm.
a. 1.5
b. 7.5
c. 0.67
d. 3.3
e. 15
58.
A sample of He gas (2.35 mol) occupies 57.9 L at 300.0 K and 1.00 atm. The
volume of this sample is _____ L at 423 K and 1.00 atm.
a. 0.709
b. 41.1
c. 81.6
d. 1.41
e. 57.9
59.
The strength of London dispersion forces between like-molecules depends on
__________ and __________.
a. molecular mass, polarizability
b. polarizability, size
c. molecular mass, volatility
d. size, shape
e. vapor pressure, size
60.
Of the following substances, _____ has the highest boiling point.
a. H2O
b. CO2
c. CH4
d. Kr
e. NH3
61.
Of the following, __________ is an exothermic process.
a. melting
b. subliming
c. freezing
d. boiling
e. All of these are exothermic.
62.
Volatility and vapor pressure are ____________.
a. inversely proportional to one another
b. directly proportional to one another
c. not related
d. the same thing
e. both independent of temperature