1510 Ch 7-10 Review for Finals Exam
Name:_______________________
What is the frequency of a photon having a wavelength of 602.5 nm? ( c  3.00 10 m/s , h  6.63 10
8
34
J s )
What is the energy of a photon of electromagnetic radiation with a wavelength of 689.8 nm? (c = 3.00 × 108 m/s, h = 6.63 × 10-34 J • s)
What is the frequency of a photon having an energy of 9.08 × 10 –16 J? (c = 3.00 × 108 m/s, h = 6.63 × 10-34 J • s)
____In Bohr's atomic theory, when an electron moves from one energy level to another energy level more distant from the nucleus,
a)
energy is emitted.
b)
energy is absorbed.
c)
no change in energy occurs.
d)
light is emitted.
e)
none of these
_____When a hydrogen electron makes a transition from n = 3 to n = 1, which of the following statements is(are) true?
I.
Energy is emitted.
II.
Energy is absorbed.
III.
The electron loses energy.
IV.
The electron gains energy.
V.
The electron cannot make this transition.
a)
b)
c)
d)
e)
I, IV
I, III
II, III
II, IV
V
_____What is the frequency of light emitted when the electron in a hydrogen atom undergoes a transition from level n = 6 to level n =
3? (c = 3.00 × 108 m/s, h = 6.63 × 10-34 J • s), RH = 2.179 × 10-18 J)
a)
2.74 × 1014 Hz
b)
1.82 × 10–19 Hz
c)
1.65 × 1027 Hz
d)
9.13 × 105 Hz
e)
1.10 × 10–6 Hz
_____Which quantum number distinguishes the different shapes of the orbitals?
a)
n
b)
l
c)
ms
d)
ml
e)
any of these
_____Which of the following sets of quantum numbers (n, l, ml, ms) refers to a 3d orbital?
a)
2 1 0 +½
b)
3 2 2 +½
c)
4 2 -2 +½
d)
4 3 2 +½
e)
5 4 3 +½
_____An orbital with the quantum numbers n = 5, l = 2, ml = 2 may be found in which subshell?
a)
5s
b)
5p
c)
5d
d)
5f
e)
5g
_____Which of the following combinations of quantum numbers is permissible?
a)
n = 3, l = 3, ml = 1, ms = –½
b)
n = 4, l = 3, ml = 4, ms = –½
c)
n = 3, l = 2, ml = 1, ms = +½
d)
n = 1, l = 2, ml = 0, ms = –½
e)
n = 2, l = 1, ml = –1, ms = 0
_____What is the maximum number of electrons that can occupy one p orbital?
a)
1
b)
2
c)
6
d)
10
e)
14
_____Which of the following orbital diagrams violates the Pauli exclusion principle?
1s
2s
2p
a)
b)
c)
d)
e)








 









_____Which of the following electron configurations corresponds to the ground state of an atom of a transition element?
a)
1s22s22p2
b)
1s22s22p63s23p5
c)
1s22s22p63s23p64s2
d)
1s22s22p63s23p63d54s2
e)
1s22s22p63s23p63d104s24p3
_____The ground-state valence-shell configuration of a particular atom is 4f146s2. The element to which this atom belongs is a
a)
noble gas.
b)
s-block main-group element.
c)
transition element.
d)
inner transition element.
e)
p-block main-group element.
_____Which of the following may represent an excited-state electron configuration for a cobalt atom?
a)
[Ar]3d64s1
b)
[Ar]3d84s1
c)
[Ar]3d74s2
d)
[Ar]3d64s2
e)
[Ar]3d54s1
_____How many valence electrons does an arsenic atom have?
a)
2
b)
5
c)
6
d)
33
e)
7
_____What is the ground-state electron configuration of terbium (Tb)?
a)
1s22s22p63s23p63d104s24p64d104f145s25p3
b)
1s22s22p63s23p63d104s24p64d105s25p65d96s2
c)
1s22s22p63s23p63d104s24p64d105s25p65d106s1
d)
1s22s22p63s23p63d104s24p64d104f95s25p66s2
e)
1s22s22p63s23p63d104s24p64d94f105s25p66s2
_____The phosphorus atom would be expected to have ____ unpaired electrons in its ground state.
a)
0
b)
1
c)
2
d)
3
e)
4
_____An atom of which of the following elements is not diamagnetic in the ground state?
a)
Ba
b)
Kr
c)
Hg
d)
Pt
e)
All are diamagnetic.
_____The ground-state electron configuration of a Cr2+ ion is 1s22s22p63s23p63d4. Therefore, Cr2+ is
a)
diamagnetic.
b)
paramagnetic with one unpaired electron.
c)
paramagnetic with five unpaired electrons.
d)
paramagnetic with four unpaired electrons.
e)
paramagnetic with three unpaired electrons
_____Which of the following orbital diagrams represents a paramagnetic atom?
1s
2s
2p
a)
b)
c)
d)
e)



















_____In general, atomic radii
a)
decrease from left to right in a period and increase down a group.
b)
increase from left to right in a period and decrease down a group.
c)
increase from left to right in a period and increase down a group.
d)
decrease from left to right and decrease down a group.
e)
do not change across a period or a group.
_____An atom of which of the following elements has the largest atomic radius?
a)
Pb
b)
Po
c)
At
d)
Bi
e)
Cs
_____An atom of which of the following elements has the largest ionization energy?
a)
At
b)
Po
c)
Bi
d)
Pb
e)
Cs
_____The electron affinity value expected for the process
Cl(g) + e– → Cl–(g)
would be
a)
b)
c)
d)
e)
a large negative number.
a small negative number.
zero.
a small positive number.
a large positive number.
_____Which of the following ground-state electron configurations corresponds to an atom that has the most negative value of the
electron affinity?
a)
1s22s22p63s1
b)
1s22s22p63s23p5
c)
1s22s22p63s23p2
d)
1s22s22p63s23p63d54s2
e)
1s22s22p6
_____In which pair do both compounds exhibit predominantly ionic bonding?
a)
PCl5 and HF
b)
Na2SO3 and BH3
c)
KI and O3
d)
NaF and H2O
e)
RbCl and CaO
_____Which of the following compounds has the most ionic bonding (has the highest percentage of ionic character)?
a)
LiI
b)
CaF2
c)
CsF
d)
LiF
e)
OF2
Draw the Lewis dot structure for one formula unit of magensium sulfide?
The ground-state electron configuration of the Mg 2+ ion is________________________________________
The Cr2+ ion would be expected to have ____ unpaired electrons.
a)
0
b)
1
c)
2
d)
3
e)
4
What is the ground-state electron configuration of Co3+?________________________________________
_____All of the following species are isoelectronic except
a)
N3–.
b)
F–.
c)
Ne.
d)
O –.
e)
Mg2+.
_____The following species,
a)
b)
c)
d)
e)
31
15
P 3 ,
37
17
Cl , and
40
20
Ca 2+ , all have the same number of
protons.
electrons.
neutrons.
isotopes.
nucleons.
____Which of the following is the best explanation for a covalent bond?
a)
electrons simultaneously attracted by more than one nucleus
b)
the overlapping of two electron-filled orbitals having different energies
c)
the overlapping of unoccupied orbitals of two or more atoms
d)
a positive ion attracting negative ions
e)
an interaction between outer electrons
_____The measure of the attraction that an atom has for the electrons in a chemical bond is called
a)
electron affinity.
b)
ionization energy.
c)
electronegativity.
d)
resonance energy.
e)
lattice energy.
_____The larger the difference in electronegativity between two bonded atoms,
1. the more ionic the bond.
2. the more covalent the bond.
3. the more polar the bond.
a)
b)
c)
d)
e)
1 only
2 only
3 only
1 and 3 only
2 and 3 only
_____ Which pair of elements would form a covalent bond that is the least polar?
a)
O and H
b)
O and F
c)
S and Cs
d)
S and Li
e)
Al and N
_____In the Lewis formula for difluorodiazine, N2F2, the total number of lone electron pairs around the two nitrogen atoms is
a)
0.
b)
1.
c)
2.
d)
3.
e)
4.
_____Which of the following Lewis formulas is incorrect?
a)
b)
c)
d)
e)
_____How many valence electrons does a nitrate ion have?
a)
22
b)
24
c)
28
d)
30
e)
32
____In which of the following species is resonance most likely to take place?
a)
b)
c)
d)
e)
_____Which of the following molecules has an incorrect Lewis formula?
a)
b)
c)
F
Xe
F
d)
e)
_____Which molecule or ion does not have a trigonal pyramidal molecular geometry?
a)
NI3
b)
PO33–
c)
SO32–
d)
BF3
e)
XeO3
____Which molecule or ion is nonlinear?
a)
CO2
b)
HCCH
c)
NF2–
d)
NO2+
e)
OCN–
_____What is the predicted H—N—H bond angle in the ammonium ion?
a)
180°
b)
120°
c)
90°
d)
109.5°
e)
45°
_____The molecular geometry of the CH3– ion is
a)
square pyramidal.
b)
tetrahedral.
c)
trigonal planar.
d)
trigonal pyramidal.
e)
square planar.
_____What is the H—O—H bond angle in water?
a)
180°
b)
120°
c)
90°
d)
109°
e)
slightly less than 109°