1) If chloride is a ligand to a transition metal, it will not be precipitated by silver nitrate.
2) The principal source of the difference in the normal boiling points of ICl (97 oC;
molecular mass
162 amu) and Br2 (59 oC; molecular mass 160 amu) is both dipole-dipole interactions
and London dispersion forces.
3) Cyclobutane is more reactive than butane.
4) If the temperature is lowered from 60 °C to 30 °C, the volume of a fixed amount of
gas will be one half the original volume.
5) Hybridization is the process of mixing atomic orbitals as atoms approach each other
to form a bond.
6) A group of ions all containing the same number of electrons constitutes an
isoelectronic series.
7) The greenhouse effect of a methane molecule far exceeds the effect of a carbon
dioxide molecule.
8) Nitrogen oxides catalytically destroy ozone.
9) In an exothermic equilibrium reaction, increasing the reaction temperature favors the
formation of reactants.
10) The possible oxidation numbers for iron are +1 and +2.
11) The equilibrium constant for the following reaction is 3.0 x 108 at 25 oC.
N2 (g) + 3H2 (g) 2NH3 (g)
The value of G o for this reaction is ________ kJ/mol.
A) 22
B) -4.1
C) 4.1
D) -48
E) -22
12) In general, as temperature goes up, reaction rate ________.
A) goes up if the reaction is exothermic
B) goes up if the reaction is endothermic
C) goes up regardless of whether the reaction is exothermic or endothermic
D) stays the same regardless of whether the reaction is exothermic or endothermic
E) stays the same if the reaction is first order
13) The Cl-Si-Cl bond angle in the SiCl2F2 molecule is approximately ________.
A) 90°
B) 109.5°
C) 120°
D) 180°
E) 60°
14) A 0.1 M solution of ________ has a pH of 7.0.
A) Na2S
B) KF
C) NaNO3
D) NH4Cl
E) NaF
15) There are ________ σ and ________ π bond(s) in the molecule.
A) 3 and 2
B) 3 and 4
C) 4 and 3
D) 2 and 3
E) 5 and 1
16) Thermodynamic Quantities for Selected Substances at 298.15 K (25 oC)
The value of H o for the decomposition of phosphorous trichloride into its constituent
elements,
2PCl3 (g) –> P2 (g) + 3Cl2 (g)
is ________ kJ/mol.
A) +576.2
B) -288.1
C) +720.5
D) +288.1
E) -720.5
17) Most mined phosphate rock is ________.
A) used as a strong acid
B) used as a reducing agent
C) used as a detergent
D) converted to fertilizer
E) discarded as a by-product
18) An empirical formula always indicates ________.
A) which atoms are attached to which in a molecule
B) how many of each atom are in a molecule
C) the simplest whole-number ratio of different atoms in a compound
D) the isotope of each element in a compound
E) the geometry of a molecule
19) A tenfold dilution of a sample solution can be obtained by taking ________.
A) 1 part sample and 9 parts solvent
B) 1 part sample and 10 parts solvent
C) 9 parts sample and 1 part solvent
D) 10 parts sample and 1 part solvent
E) 99 parts sample and 1 part solvent
20) The double helix of DNA is stabilized mainly by ________.
A) ionic bonds
B) covalent bonds
C) ion-dipole bonds
D) ester bonds
E) hydrogen bonds
21) The mass of a proton is 1.00728 amu and that of a neutron is 1.00867 amu. What is
the mass defect (in amu) of a Co nucleus? (The mass of a cobalt-60 nucleus is
59.9338 amu.)
A) 27.7830
B) 0.5489
C) 0.5405
D) 0.0662
E) 0.4827
22) Using the VSEPR model, the molecular geometry of the central atom in CH4 is
________.
A) linear
B) trigonal planar
C) tetrahedral
D) bent
E) trigonal pyramidal
23) How is the reaction quotient used to determine whether a system is at equilibrium?
A) The reaction quotient must be satisfied for equilibrium to be achieved.
B) At equilibrium, the reaction quotient is undefined.
C) The reaction is at equilibrium when Q < Keq.
D) The reaction is at equilibrium when Q > Keq.
E) The reaction is at equilibrium when Q = Keq.
24) The frequency of electromagnetic radiation required to promote an electron from n
= 2 to n = 4 in a Bohr hydrogen atom is ________ Hz.
A) 4.13 X 10-19
B) 6.17 X 1014
C) 5.46 X 10-19
D) 8.22 X 1014
E) 4.13 X 1019
25) Which metal is a liquid at room temperature?
26) Write the balanced equation for the reaction of elemental chlorine with liquid water.
27) In the purification of drinking water, the filtered water is made basic by adding
________, then particles and bacteria are captured by adding ________.
28) For a dilute aqueous solution, a concentration of 1 ppm also corresponds to a
concentration of 1 ________ per liter of solution.
29) Alternative but equivalent Lewis structures are called ________.
30) The phenomenon used to differentiate colloids and true solutions is called the
________ effect.
31) Define the chelate effect.
32) In general, intramolecular forces determine the ________ properties of a substance
and intermolecular forces determine its ________ properties.