Chemistry For Today General Organic and Biochemistry 8th International Edition by Spencer L. Seager – Test Bank
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Sample Test
Chapter 3—Electronic Structure and the Periodic Law
MULTIPLE CHOICE
1. Which
of the following elements is found in the same period of the periodic table as
tin?
2. silicone
b. arsenic
c.
tellurium
d. technetium
ANS:
C
PTS: 1
2. Which
element is the first one in the group IVA(14) of the periodic table?
3. C
b.
Na
c.
Sc
d. Ti
ANS:
A
PTS: 1
3. What
is the symbol of the element that is in Period 4, and Group IIA(2) of the
periodic table?
4. Zn
b.
Ca
c.
C
d. Ti
ANS:
B
PTS: 1
4. Silver,
Ag, belongs to what period of the periodic table?
5. 1
b.
2
c.
5
d. 12
ANS:
C
PTS: 1
5. If
the formula for sulfuric acid is H2SO4, what would be the expected formula for
the compound between hydrogen and tellurium, Te?
6. H2TeO4
b.
HTe
c.
HTe2 d.
H2Te
ANS:
A
PTS: 1
6. Which
of the following statements applies to p subshells?
7. The p
subshell can contain a maximum of 14 electrons.
8. The p
subshell is subdivided into three perpendicular shapes.
9. The p
subshell fills with 2 electrons in px, then 2 in py then 2 in pz.
10.
All of these statements are correct with reference to p
subshells.
ANS:
B
PTS: 1
7. Which
of the following subshells has the higher energy?
8. 4s
b.
4p
c. 4d
d. 4f
ANS:
D
PTS: 1
8. Suppose
an electron moved from the second shell to the third shell.
9. The
move required an input of energy.
10.
The move gave off energy.
11.
Electrons can move spontaneously from shell to shell.
12.
Electrons can’t move from shell to shell, but can move into the
nucleus.
ANS:
A
PTS: 1
9. The
total number of f orbitals in an f subshell is _____ .
10.
2
b.
5
c.
7
d. 10
ANS:
C
PTS: 1
10.
The maximum number of electrons that can occupy a 3d subshell is
_____ .
11.
2
b.
4
c.
6
d. 10
ANS:
D
PTS: 1
11.
The maximum number of electrons that can occupy a 4p orbital is
_____ .
12.
2
b.
4
c.
6
d. 10
ANS:
C
PTS: 1
12.
What is the maximum number of electrons that can occupy the
third shell?
13.
2 b.
10
c.
18
d. 32
ANS:
C
PTS: 1
13.
How many electrons are in the outer shell of element 15?
14.
5
b.
3
c.
15
d. 2
ANS:
A
PTS: 1
14.
Which of the following elements should have properties similar
to those of nitrogen (element 7)?
15.
C
b.
Si
c.
P
d. O
ANS:
C
PTS: 1
15.
Which of the following has the same number of outer shell
electrons as sulfur, S?
16.
C
b.
O
c.
N
d. F
ANS:
B
PTS: 1
16.
What is the shell number for the outer shell electrons in
bromine, Br?
17.
4
b.
3
c.
5
d. 6
ANS:
A
PTS: 1
17.
Which of the following elements has the electronic configuration
shown here?
1s2 2s2 2p6 3s2 3p1
1. F b.
Al
c.
Mg
d. Ga
ANS:
B
PTS: 1
18.
The total number of unpaired electrons in silicon, Si, is _____
.
19.
0
b.
1
c.
2
d. 3
ANS:
C
PTS: 1
19.
Which of the following contains the same total number of
unpaired electrons as potassium (K)?
20.
Sc
c. Mg
21.
Cl
d. more than
one response is correct
ANS:
D
PTS: 1
20.
Which of the following will not have electrons in the 3rd
orbital?
21.
K
b.
Mg
c.
Na+ d.
Ag+
ANS:
C
PTS: 1
21.
Which of the following pairs have the same number of electrons
in the outermost shell?
22.
K and Ca
b. S4+ and
Al3+
c. Na+
and Ne d.
Ne and He
ANS:
C
PTS: 1
22.
The electronic configuration of element 17 ends with _____ .
23.
2p 3
b. 3p
5
c. 2p
5
d. 3p 3
ANS:
B
PTS: 1
23.
Which of the following elements contains a total of 10 “s”
electrons?
24.
Sr
c. Cs
25.
Sb
d. more than
one response is correct
ANS: D
PTS: 1
24.
What type of electron is the distinguishing electron in S?
25.
s
b.
p
c.
d
d. f
ANS:
B
PTS: 1
25.
Which of the following distinguishing electrons represents an
element with properties similar to an element with a 3p 3 distinguishing
electron?
26.
4p 3
b. 3p
2
c. 3d
3 d.
2p 2
ANS:
A
PTS: 1
26.
Which element is represented by the distinguishing electron
configuration 5d 9?
27.
Pd
b.
Ag
c.
Pt
d. Au
ANS:
D
PTS: 1
27.
Which of the following elements is most likely to be a
metalloid?
28.
Ge
b.
Mo
c.
S
d. Cs
ANS:
A
PTS: 1
28.
Metalloids can express the characteristics of both metals and
nonmetals. Which of the elements below is more likely to have the
characteristics of a metal than a nonmetal?
29.
As
b.
Se
c.
Si
d. Sb
ANS:
D
PTS: 1
29.
In which of the following elements does the distinguishing
electron occupy a d subshell?
30.
Cr
b. O
c.
Kr
d. Sr
ANS:
A
PTS: 1
30.
Which of the following elements is classified as a transition
element?
31.
element 76
b. element
60
c.
element 56 d.
element 17
ANS:
A
PTS: 1
31.
Which of the following elements is classified as a
representative metal?
32.
element 30
b. element
26
c.
element 38
d. element 63
ANS:
C
PTS: 1
32.
Which of the following elements is a nonmetal?
33.
Ni
b.
Cu
c.
Ba
d. I
ANS:
D
PTS: 1
33.
Which one of these elements is a gas at room temperature?
34.
antimony
b.
phosphorus
c.
nitrogen
d. arsenic
ANS:
C
PTS: 1
34.
Which element has the distinguishing electron, 5p4?
35.
Br
b.
Mn c.
Te
d. Kr
ANS:
C
PTS: 1
35.
The radius of a K atom is ____ a Ca atom.
36.
smaller than
b. larger
than
c.
equal to
d. inverted
from
ANS:
B
PTS: 1
36.
The melting point of oxygen is ____ selenium, Se.
37.
lower than
b. higher
than
c.
equal to
d. inverted
from
ANS:
A
PTS: 1
37.
Which of the following is a noble gas?
38.
gold
b.
platinum
c.
neon
d. chlorine
ANS:
C
PTS: 1
38.
One mole of an element would weigh the same as a mole of an
isotope of the same element.
39.
Mg b.
Be
c.
Al d.
B
ANS:
D
PTS: 1
39.
Which element is used for relieving the symptoms of a cold?
40.
Au
b.
K
c.
Zn
d. Fe
ANS:
C
PTS: 1
40.
Which of the following statements conforms to the trends within
the Periodic Table of the Elements?
41.
Elements become more likely to be gases at the bottom of a
group.
42.
Elements become more likely to be a solid at the bottom of a
group.
43.
Elements become more likely to be darkly colored at the bottom
of a group.
44.
Elements become more likely to be more brittle at the bottom of
a group.
ANS:
B
PTS: 1
41.
The highest-energy shell of an element that contains electrons
is know as the _____ .
42.
subshell
b. atomic
orbital
c.
valence shell d.
none of these
ANS:
C
PTS: 1
42.
____ states that, electrons will not join other electrons in an orbital
if an empty orbital of the same energy is available.
43.
Hund’s rule
c.
Periodic law
44.
Pauli exclusion principle
d. None of
these
ANS:
A
PTS: 1
43.
____ explains why orbitals can contain a maximum of two electrons.
44.
Hund’s rule
c.
Periodic law
45.
Pauli exclusion principle
d. None of
these
ANS:
B
PTS: 1
44.
Choose the correct electronic configuration for the element As.
45.
[Ar] 4s2 3d10 4p3
c. [Ar]
4s2 4d10 4p3
46.
4s2 3d10 4p3
d. 4s2 4d10
4p3
ANS:
A
PTS: 1
45.
Which element has the largest atomic radii?
46.
I
b.
F
c.
Li
d. Cs
ANS:
D PTS:
1
46.
The element chlorine is found in the same group of the periodic
table as _____ .
47.
I
b.
F
c.
Br
d. all of
these
ANS:
D
PTS: 1
47.
The family name for group VIIIA(18) of the periodic table is
48.
transition metals.
c.
representative elements.
49.
noble gases.
d. There is
no family name
ANS:
B
PTS: 1
48.
Which of the following is a reasonable explanation as to why atomic
radii become smaller as one moves to the right for the representative elements
in a period?
49.
The charge of the nucleus increases, pulling the shells closer.
50.
More densely packed shells are always smaller.
51.
Elements become less metallic.
52.
Atomic radii actually increase as you move to the right.
ANS:
A
PTS: 1
49.
Which of the following is the correct designation for an
electron occupying the orbital shown below?
1. 2p
b.
3s
c. 3d
d. 4f
ANS:
C
PTS: 1
50.
Which of the following correctly arranges the given subshells in
order of increasing energy (lowest to highest)?
51.
2s < 3d < 4s
c. 2s
< 3d < 4p
52.
4s < 3p < 3s
d. 4p
< 4f < 5s
ANS:
C
PTS: 1
51.
Which of the following violates the Pauli exclusion principle?
52.
c.
53.
d.
All of them
ANS:
C
PTS: 1
52.
Which of the following is the correct valence electron configuration
of phosphorus?
53.
c.
54.
d.
ANS:
B
PTS: 1
53.
Which pair of the following represents the same electron
configuration?
54.
[Ne] 3s2 and 1s2 2s2 2p6 3s2
c.
[Ar]3s2 and 1s2 2s2 2p6 3s2
55.
[He] 3s2 and 1s2 2s2 2p6 3s2 d.
All represent the same configuration.
ANS:
A
PTS: 1
54.
For which of the listed elements (E) would the energy required
for the following reaction be the least? E(g) ® E+(g) + e–
1. Ga
b. Na
c.
Ca
d. K
ANS:
D
PTS: 1
55.
Which of the following metals (M) would produce the fastest
reaction with ethyl alcohol (C2H5OH) as
shown? 2M + 2C2H5OH ® 2C2H5OM + H2
56.
K b.
Li
c.
Sr
d. Al
ANS:
A
PTS: 1
56.
Which of the following is a representation of a p orbital?
57.
b.
c.
d.
ANS:
B
PTS: 1
57.
What rule, principle or law is used to explain that an electrons
will not share the same orbital if there is an empty orbital of the same energy
available?
58.
Aufbau principle
c.
Pauli principle
59.
Hund’s rule d.
Avogadro’s law
ANS:
B
PTS: 1
58.
Which of the following is considered a transition element?
59.
tungsten
b.
holmium
c.
radon
d. cesium
ANS:
A
PTS: 1
59.
Unlike the original attempt by Mendeleev, the modern periodic
table arranges elements based on what elemental feature?
60.
mass number
c.
isotope composition
61.
atomic number d. relative size
ANS:
B
PTS: 1
60.
What is the basis for placing groups of elements into a family
on the periodic table?
61.
similar atomic mass numbers
62.
identical chemical and physical properties
63.
similar colors, shapes and uses
64.
similar valence electron configurations
ANS:
D
PTS: 1
61.
Calcium citrate, Ca3(C6H5O7)2, is commonly used in the
production of dietary calcium supplements. How many representative
elements are found in calcium citrate?
62.
1
b.
2
c.
3
d. 4
ANS:
D
PTS: 1
TRUE/FALSE
1. The
fifth period begins with Rb.
ANS:
T
PTS: 1
2. A 3d
orbital can hold 6 electrons.
ANS:
F
PTS: 1
3. Tin
(Sn) is a representative element.
ANS:
T
PTS: 1
4. The
electron configuration for each shell starts with an s subshell.
ANS:
T
PTS: 1
5. All
of the transition elements are metals.
ANS:
T
PTS: 1
6. Sodium,
Na, and potassium, K, are in the same period.
ANS:
F
PTS: 1
7. The
radius of a magnesium atom is larger than the radius of a sodium atom.
ANS:
F
PTS: 1
8. The
magnesium atom loses an electron easier than a calcium atom.
ANS:
F
PTS: 1
9. The
distinguishing electron in antimony, Sb, is found in a 5p subshell.
ANS:
T
PTS: 1
10.
The fourth shell contains four subshells.
ANS:
T
PTS: 1
11.
The second shell has a maximum capacity of 6 electrons.
ANS:
F
PTS: 1
12.
Element number 92, uranium, U, is a metal.
ANS:
T
PTS: 1
13.
Argon completes the fourth period of the periodic table.
ANS:
F
PTS: 1
14.
Hydrogen is a noble gas.
ANS:
F
PTS: 1
15.
A bromine atom has a larger radius than a chlorine atom.
ANS:
T
PTS: 1
16.
All non-metals are representative elements.
ANS:
T
PTS: 1
17.
An anion is smaller than the atom from which it is produced.
ANS:
T
PTS: 1
18.
The distinguishing electron for most non-metals is an s
electron.
ANS: F
PTS: 1
19.
Tin (Sn), which is found in Group IVA, has four electrons in the
outside shell.
ANS:
T
PTS: 1
20.
As one moves across the 4th period from left to right, the
valence electrons go into the same shell, and the atomic radius decreases. The
decrease in atomic radius is due to the increase in the attraction of the
nucleus for the electrons in the shells.
ANS:
T
PTS: 1
21.
Based on the physical states of the other group members, the yet
undiscovered sixth member of group VIIA(17) would be a solid.
ANS:
T
PTS: 1
22.
The distinguishing electron for any element is a valence
electron.
ANS:
T
PTS: 1
23.
The atomic size of the elements in a group increases with the
period number.
ANS:
T
PTS: 1
24.
The d and f sublevels do not fill when expected because
the energy levels for periods can overlap.
ANS:
T
PTS: 1
25.
Calcium supplements that are made from calcium carbonate should
be taken with food because stomach acid is required to dissolve them.
ANS:
T
PTS: 1
Chapter 5—Chemical Reactions
MULTIPLE CHOICE
1. Which
of the following statements is not true about the reaction?
2 CH4 + 3 O2 ® 2
CO2 + 4 H2O
1. Water
is a reactant.
2. Methane
and carbon dioxide are products.
3. Methane
is a product.
4. Water
and carbon dioxide are products.
ANS:
D
PTS: 1
2. Which
of the following reactions is correctly balanced?
3. N2 +
H ® 2NH3
c. Zn +
2HCl ® H2 +
ZnCl2
4. 2H2O
+ C ® CO +
2H2 d. CO +
O2 ® CO2
ANS:
C
PTS: 1
3. Which
set of coefficients balances the equation?
____ CH4 ® ____C3H8
+ ____ H2
1. 3,1,1
b.
3,2,1
c.
3,1,2 d.
6,2,2
ANS:
C
PTS: 1
4. When
the equation below is properly balanced, what coefficient is in front of KCl?
KClO3 ® KCl
+ O2
1. 1
b. 2
c.
3
d. 4
ANS:
B
PTS: 1
5. Propane,
C3H8, burns to produce carbon dioxide and water by the equation below. What is
the coefficient in front of the carbon dioxide in the balanced equation?
C3H8 + O2 ® CO2
+ H2O
1. 1
b.
2
c.
3
d. 6
ANS:
C
PTS: 1
6. Consider
the reactants and propose the right side of the equation.
Mg + H2SO4 ® _______
1. no reaction
b.
MgHSO4
c.
MgSO4 + H2
d. MgH2 + SO4
ANS:
C
PTS: 1
7. Consider
the reactants in the partial equation given. Which choice is a product?
H3PO4 + Sr(OH)2 ® ____
1. no
reaction b.
SrH3PO5
c.
SrH5PO6
d. Sr3(PO4)2
ANS:
D
PTS: 1
8. Which
species would be considered a spectator ion based on the following equation?
Ba2+ + 2NO3- +
2Na+ + SO42+ ®
BaSO4(s) + 2NO3- +
2Na+
1. Ba2+
b.
SO42+
c.
BaSO4
d. 2NO3-
ANS:
D
PTS: 1
9. A
REDOX reaction can also be a(n)
10.
combination reaction.
c.
decomposition reaction.
11.
single replacement reaction.
d. More than
one response is correct.
ANS:
D
PTS: 1
10.
Which of the following is an oxidizing agent?
11.
O2
b.
H2
c.
H2O d.
HCl
ANS: A
PTS: 1
11.
Single replacement reactions are always
12.
redox reactions.
c.
combination reactions.
13.
nonredox reactions.
d.
decomposition reactions.
ANS:
A
PTS: 1
12.
Which of the following equations (not balanced) represents an
oxidation-reduction process?
13.
AgNO3 + NaCl ® AgCl
+ NaNO3
c. C2H4
+ O2 ® CO2
+ H2O
14.
C + O2 ® CO2
d. more than
one response is correct
ANS:
D
PTS: 1
13.
What is the oxidation number of Cl in HClO3?
14.
+2
b.
+3
c.
+4
d. +5
ANS:
D
PTS: 1
14.
What is the oxidation number of Br in ?
15.
-1
b.
+1
c.
+2 d.
+3
ANS:
D
PTS: 1
15.
What is the oxidation number of Mn in KMnO4?
16.
+9
b.
+5
c.
+7
d. +4
ANS:
C
PTS: 1
16.
In which of the following does an element have an oxidation
number of +4?
17.
TiO2
b.
HBr
c.
SO3 d.
ANS:
A
PTS: 1
17.
Which of the following contains the metal with the highest
oxidation number?
18.
CaCl2
b.
NaCl
c.
FeCl3
d. CuCl2
ANS:
C
PTS: 1
18.
What substance is oxidized in the following reaction?
4HCl + MnO2 ® Cl2
+ 2H2O + MnCl2
1. Cl in
HCl b. Mn in
MnO2 c.
H in HCl d. O
in MnO2
ANS:
A
PTS: 1
19.
What substance is reduced in the following reaction?
4HCl + MnO2 ® Cl2
+ 2H2O + MnCl2
1. Cl in
HCl b. Mn in
MnO2
c. H in
HCl d. O in
MnO2
ANS:
B
PTS: 1
20.
What is the oxidizing agent in the following reaction?
4HCl + MnO2 ® Cl2
+ 2H2O + MnCl2
1. HCl
b.
Cl2
c.
MnO2 d.
MnCl2
ANS:
C PTS:
1
21.
What is the reducing agent in the following reaction?
4HCl + MnO2 ® Cl2
+ 2H2O + MnCl2
1. HCl
b.
Cl2
c.
MnO2 d.
MnCl2
ANS:
A
PTS: 1
22.
Which of the following is a decomposition reaction?
23.
SO2 + O2 ® 2SO3
c.
2H2O2 ® 2H2O
+ O2
24.
2C2H2 + 5O2 ® 4CO2
+ 2H2O d.
AgNO3 + NaCl ® AgCl
+ NaNO3
ANS:
C
PTS: 1
23.
Which of the following is a combination reaction?
24.
SO2 + O2 ® 2SO3
c.
2H2O2 ® 2H2O
+ O2
25.
2C2H2 + 5O2 ® 4CO2
+ 2H2O d.
AgNO3 + NaCl ® AgCl
+ NaNO3
ANS:
A
PTS: 1
24.
Which of the following is a single replacement reaction?
25.
CuO + H2 ® Cu +
H2O c.
SO2 + H2O ® H2SO3
26.
HBr + KOH ® H2O
+ KBr d. 2HI ® I2 + H2
ANS:
A
PTS: 1
25.
Which of the following is a double replacement reaction?
26.
CuO + H2 ® Cu +
H2O c.
SO2 + H2O ®
H2SO3
27.
HBr + KOH ® H2O
+ KBr d. 2HI ® I2 + H2
ANS:
B
PTS: 1
26.
Barium sulfate is often ingested to aid in the diagnosis of GI
tract disorders. The equation for its production is Ba2+ + SO ® BaSO4(s). What type
of equation is this?
27.
a total ionic equation
c. an
oxidation-reduction equation
28.
a full equation
d. a net
ionic equation
ANS:
D
PTS: 1
27.
Which ions in the following reaction would be classified as
spectator ions?
Zn + 2H+ + 2Cl ® Zn2+
+ 2Cl- + H2
1. Zn2+
c. Cl-
2. H+
d. More than
one response is correct.
ANS:
C
PTS: 1
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