1) The value of ΔH° for the reaction below is -6535 kJ. ________ kJ of heat are
released in the combustion of 16.0 g of C6H6 (l)?
2C6H6 (l) + 15O2 (g) → 12CO2 (g) + 6 H2O (l)
A) 1.34 x 103
B) 5.23 x 104
C) 669
D) 2.68 x 103
E) -6535
2) Consider the general valence electron configuration of ns2np5 and the following
statements:
(i)Elements with this electron configuration are expected to form -1 anions.
(ii)Elements with this electron configuration are expected to have large
positive electron affinities.
(iii)Elements with this electron configuration are nonmetals.
(iv)Elements with this electron configuration form acidic oxides.
Which statements are true?
A) (i) and (ii)
B) (i), (ii), and (iii)
C) (ii) and (iii)
D) (i), (iii,) and (iv)
E) All statements are true.
3) The mass of a proton is 1.673 x 10-24 g. The mass of a neutron is 1.675 x 10-24g. The
mass of the nucleus of an 56Fe atom is 9.289 x 10-23 g. What is the nuclear binding
energy (in J) for a 56Fe nucleus?
(c = 3.00 x 108 m/s)
A) 2.57 x 10-16
B) 7.72 x 10-8
C) 8.36 x 10-9
D) 7.65 x 10-11
E) 6.07 x 106
4) The curie is a measure of the ________.
A) number of disintegrations per second of a radioactive substance
B) total energy absorbed by an object e x posed to a radioactive source
C) lethal threshold for radiation e x posure
D) number of alpha particles emitted by e x actly one gram of a radioactive substance
E) None of the above is correct.
5) A typical double bond ________.
A) is stronger and shorter than a single bond
B) consists of one bond and one € bond
C) imparts rigidity to a molecule
D) consists of two shared electron pairs
E) All of the above answers are correct.
6) The lowest orbital energy is reached when the number of electrons with the same
spin is maximized. This statement describes ________.
A) Pauli Exclusion Principle
B) Planck’s constant
C) deBroglie hypothesis
D) Heisenberg Uncertainty Principle
E) Hund’s rule
7) Which electron configuration represents a violation of Hund’s rule for an atom in its
ground state?
A)
B)
C)
D)
E)
8) Which mineral contains mercury?
A) cinnabar
B) sphalerite
C) rutile
D) chromite
E) cassiterite
9) In the periodic table, the elements are arranged in ________.
A) alphabetical order
B) order of increasing atomic number
C) order of increasing metallic properties
D) order of increasing neutron content
E) reverse alphabetical order
10) The charge of the complex ion in [Zn(H2O)3Cl]Cl ________.
A) 0
B) 1-
C) 2+
D) 1+
E) 2-
11) How many moles of Na+ are present in 343 mL of a 1.27 M solution of Na2SO4?
A) 0.436
B) 0.871
C) 1.31
D) 3.70
E) 11.1
12) How many grams of NaOH (MW = 40.0) are there in 375.0 mL of a 0.325 M NaOH
solution?
13) Radioactive seeds that are implanted into a tumor are coated with ________ to stop
alpha and beta ray penetration.
14) The minimum energy to initiate a chemical reaction is the ________.
15) The two more common oxidation states of chromium are ________ and ________.
16) In a discussion of oxygen compounds, a disproportionation reaction is ________.
17) Polyatomic ions with an odd number of electrons will ________ the octet rule.
18) Describe the major difference in the charge distribution in CH4 and SiH4.
19) Explain why HF (aq) is a relatively weak acid compared to other hydrohalic acids.