1) What volume (mL) of a concentrated solution of magnesium chloride (9.00 M) must
be diluted to 350. mL to make a 2.75 M solution of magnesium chloride?
A) 2.75
B) 50.0
C) 45.0
D) 107
E) 350
2) Consider the reaction:
FeO (s) + Fe (s) + O2(g) –> Fe2O3 (s)
Given the following table of thermodynamic data at 298 K:
The value K for the reaction at 25 oC is ________.
A) 370
B) 5.9 x 104
C) 3.8 x 10-14
D) 7.1 x 1085
E) 8.1 x 1019
3) What is the percentage of freshwater on planet Earth?
A) 97%
B) 2.1%
C) 2.8%
D) 0.6%
E) 100%
4) Elemental iodine (I2) is a solid at room temperature. What is the major attractive
force that exists among different I2 molecules in the solid?
A) London dispersion forces
B) dipole-dipole rejections
C) ionic-dipole interactions
D) covalent-ionic interactions
E) dipole-dipole attractions
5) Thermodynamic Quantities for Selected Substances at 298.15 K (25 oC)
The value of S o for the formation of POCl3 from its constituent elements,
P2 (g) + O2 (g) + 3Cl2 (g) –> 2POCl3 (g)
is ________ J/K mol.
A) -442.0
B) +771.0
C) -321.0
D) -771.0
E) +321.0
6) The N-N bond in HNNH consists of ________.
A) one σ bond and one π bond
B) one σ bond and two π bonds
C) two σ bonds and one π bond
D) two σ bonds and two π bonds
E) one σ bond and no π bonds
7) Which of the following is an ionic hydride?
A) CaH2
B) C2H4
C) HCl
D) NH3
E) CsOH
8) Which type of formula provides the most information about a compound?
A) empirical
B) molecular
C) simplest
D) structural
E) chemical
9) Oxygen forms an ion with a charge of ________.
A) 2-
B) 2+
C) 3-
D) 3+
E) 6+
10) The compound below is a(n) ________.
A) carboxylic acid
B) ketone
C) aldehyde
D) ester
E) amine
11) A sample of a gas originally at 25 °C and 1.00 atm pressure in a 2.5 L container is
subject to a pressure of 0.85 atm and a temperature of 15 °C. The final volume of the
gas is ________ L.
A) 3.0
B) 2.8
C) 2.6
D) 2.1
E) 0.38
12) Elements in Group 1A are known as the ________.
A) chalcogens
B) alkaline earth metals
C) alkali metals
D) halogens
E) noble gases
13) The specific heat of liquid bromine is 0.226 J/g-K. How much heat (J) is required to
raise the temperature of 10.0 mL of bromine from 25.00 °C to 27.30 °C? The density of
liquid bromine: 3.12 g/mL.
A) 5.20 J
B) 16.2 J
C) 300 J
D) 32.4 J
E) 10.4 J
14) According to the Arrhenius concept, an acid is a substance that ________.
A) is capable of donating one or more H+
B) causes an increase in the concentration of H+ in aqueous solutions
C) can accept a pair of electrons to form a coordinate covalent bond
D) reacts with the solvent to form the cation formed by autoionization of that solvent
E) tastes bitter
15) The molecular weight of the acetic acid (CH3CO2H), rounded to the nearest integer,
is ________ amu.
A) 60
B) 48
C) 44
D) 32
16) The correct name for the molecule CH3CH3 is ________.
A) ethane
B) propane
C) ethyl
D) propyne
E) butane
17) What is the typical percent of uranium-235 in the enriched UO2 pellets used in
nuclear reactors?
A) 0.7
B) 1
C) 3
D) 10
E) 14
18) Which one of the following is not true about transition metals?
A) They frequently have more than one common oxidation state.
B) Their compounds are frequently colored.
C) Their compounds frequently exhibit magnetic properties.
D) They are found in the d-block of the periodic table.
E) They typically have low melting points.
19) Given the equation
H2O (l) → H2O (g) ΔHrxn = 40.7 kJ at 100 °C
Calculate the heat required to convert 3.00 grams of liquid water at 100 °C to vapor.
20) What are the principal components used in making soda-lime glass?
21) All of the group VIA elements are solids except ________.
22) ________ analysis determines only the presence or absence of a particular metal
ion, whereas ________ analysis determines how much of a given substance is present.
23) What wavelengths correspond to the visible region of the electromagnetic
spectrum?
24) How many molecules are there in 4.00 L of oxygen gas at 500 °C and 50.0 torr?
25) In addition to nitrogen oxides, ________ are a major contributor to the depletion of
the ozone layer.