Download UNIT 1 WORKSHEET 1. Name three methods for the separation of

UNIT 1 WORKSHEET
1.
Name three methods for the separation of mixtures.
2.
How many significant figures are there in the number
0.0322?
A) 3 B) 5 C) 4 D) 2 E) 0
3.
Convert 974036 mm to km.
A) 9744036 km
B) 974.036 km
C) 974036000 km
D) 0.000974036 km
E) 0.974036 km
4.
Express 0.000543 in scientific notation.
A) 5.43 x 10
B) 5.43 x 10
C) 54.3 x 10
5.
–4
–6
–5
D)
54.3 x 10
E)
543 x 10
11.
Suppose that you purchased a water bed that has
dimensions 2.55 m x 2.53 dm x 230 cm. What mass of
water does this bed contain?
12.
Which of the following metric relationships is incorrect?
–3
–3
A) 1 microliter = 10
True or False: All physical changes are accompanied by
chemical changes.
7.
A metric unit for mass is
A) pound.
D)
ounce
B) kilogram.
E)
meter.
C) ton.
.
The density of a liquid is determined by successively
weighing 25, 50, 75, 100, and 125 mL of the liquid in a 250mL beaker. If volume of liquid is plotted along the
horizontal axis, and total mass of beaker plus liquid is
plotted on the vertical axis, which of the following is true?
A) The plot should be rather linear because the slope
measures the density of a liquid.
B) The plot should be curved upward because the slope
measures the density of a liquid.
C) The plot should be curved upward because the mass of
the liquid is higher in successive trials.
D) The plot should be linear because the mass of the
beaker stays constant.
E) none of these
–6
6
liters
B) 1 megagram = 10 grams
3
C) 1 millimeter = 10 meters
3
D) 1 kilogram = 10 grams
E) 100 centimeters = 1 meter
solid
liquid
gas
not enough information
At 323°F, the indium is partially solid and partially
liquid; there is an equilibrium between the two states.
6.
9.
In a recent accident, some drums of uranium hexafluoride
were lost in the English Channel, which is known for its cold
water (about 17°C). The melting point of uranium
hexafluoride is 148°F. In what physical state is the
uranium hexafluoride in these drums? (TF = TC x
(9°F/5°C) + 32°F)
A) solid
B) liquid
C) gas
D) a mixture of solid and liquid
E) not enough information
The melting point of indium is 156.2°C. At 323°F, what is
the physical state of indium?
(TF = TC x (9°F/5°C) + 32°F)
A)
B)
C)
D)
E)
8.
10.
13.
Convert: –40.0 °C = ____ °F. (TF = TC x (9°F/5°C) + 32°F)
14.
The agreement of a particular value with the true value is
called
A) accuracy.
D)
significance
B) error.
E)
certainty.
C) precision.
15.
In a recent accident some drums of uranium hexafluoride
were lost in the English Channel. The melting point of
uranium hexafluoride is 64.5°C. What is the melting point
of uranium hexafluoride on the Fahrenheit scale? (TF = TC
x (9°F/5°C) + 32°F)
A) 1.35°F
B) 82.3°F
C) 116°F
It is estimated that uranium is relatively common in the
earth's crust, occurring in amounts of 4 g/metric ton. A
metric ton is 1000 kg. At this concentration, what mass of
uranium is present in 1.0 mg of the earth's crust?
A) 4 nanograms
D)
4 x 10–5 g
B) 4 micrograms
E)
4 centigrams
C) 4 milligrams
Page 1
3
D)
E)
122°F
148°F
3
16.
Convert 0.092 ft to L. (2.54 cm = 1 in., 1 L = 1 dm )
A) 26 L
D)
1.8 L
B) 2.6 L
E)
0.40 L
C) 3.2 x 10–3 L
17.
True or False: Color changes always indicate a chemical
change.
18.
Using the rules of significant figures, calculate the
following: 4.0021 – 0.004
A) 3.998
D)
4.00
B) 4
E)
4.0
C) 3.9981
19.
What data would you need to estimate the money you would
spend on gas to drive your car from Los Angeles to
Chicago? Provide a sample calculation.
UNIT 1 WORKSHEET
20.
The state of matter for an object that has both definite
volume and definite shape is
A) solid state.
D) elemental state
B) liquid state.
E) mixed state
C) gaseous state.
21.
Convert 761 mi to km. (1 m = 1.094 yds, 1 mi = 1760 yds)
A) 832 km
B) 1470 km
C) 1.22 x 109 km
D) 696 km
E) 1220 km
22.
Explain how Archimedes might have used the concept of
density to determine whether the king's crown was pure
gold. (density of gold = 19.32 g/cm3)
23.
A method of separation that employs a system with two
phases of matter, a mobile phase and a stationary phase, is
called
A) filtration.
B) chromatography.
C) distillation.
D) vaporization.
E) homogenization.
24.
Which of the following is an example of a qualitative
observation?
A) A piece of wood is 5.3 cm long.
B) Solution 1 is much darker than solution 2.
C) The volume of liquid in beaker A is 4.3 mL
D) The temperature of the liquid is 60°C.
E) none of these
25.
Express 784000000 in exponential notation.
A) 7.84 x 106
B) 7.84 x 108
C) 78.4 x 107
D) 784 x 106
E) 784 x 107
26.
A) physical change because the water merely disappears.
B) physical change because the gaseous water is
chemically the same as the liquid.
C) chemical change because heat is needed for the
process to occur.
D) chemical change because a gas (steam) is given off.
E) chemical and physical damage.
A chemical theory that has been known for a long time
becomes a law.
28.
Convert 16.8 lb to g. (1 lb = 453.6 g)
A) 762.0 g
B) 3.70 x 104 g
C) 76.2 g
D) 7621 g
E) 7620 g
29.
The boiling of water is a
A scientist obtains the number 1250.37986 on a calculator.
If this number actually has four (4) significant figures,
how should it be written?
A) 1251
B) 1250.3799
C) 1250.4
D) 1.250 x 103
E) 1.250 x 10–3
31.
Which of the following is not a unit in the SI system?
A) ampere
B) candela
C) Kelvin
D) meter
E) calorie
32.
A piece of indium with a mass of 16.6 g is submerged in
46.3 cm3 of water in a graduated cylinder. The water level
increases to 48.6 cm3. The correct value for the density
of indium from these data is:
A) 7.217 g/cm3
B) 7.2 g/cm3
C) 0.14 g/cm3
D) 0.138 g/cm3
E) more than 0.1 g/cm3 away from any of these values.
33.
Using the rules of significant figures, calculate the
following:
A)
B)
C)
D)
E)
Convert 4301 mL to qts. (1 L = 1.06 qt)
A) 4559 qts
B) 4.058 qts
C) 4058 x 10–3 qts
D) 4058 qts
E) 4.559 qts
27.
30.
Page 2
17.5
18
17
20
17.48
6167
.
 83
510
.
34.
On a new temperature scale (°Y), water boils at 155.0 °Y
and freezes at 0.00 °Y. Calculate the normal human body
temperature using this temperature scale. On the
Fahrenheit scale, normal human body temperature is 98.6
°F, and water boils at 212.0 °F and freezes at 32.0 °F.
35.
How many significant figures are there in the number
1008500?
A) 13
B) 5
C) 7
D) 0
E) 4
UNIT 1 WORKSHEET
36.
The state of matter for an object that has a definite
volume but not a definite shape is
A) solid state.
B) liquid state.
C) gaseous state.
D) elemental state.
E) mixed state.
37.
An example of a pure substance is
A) elements.
B) compounds.
C) pure water.
D) carbon dioxide.
E) all of these
38.
A solution is also called a
A) homogeneous mixture.
B) heterogeneous mixture.
C) pure mixture.
D) compound.
E) distilled mixture.
39.
Express the volume 159 dm3 in liters.
A) 159 L
B) 159000 L
C) 0.159 L
D) 15.9 L
E) 1.59 L
40.
A freighter carrying a cargo of uranium hexafluoride sank
in the English Channel in late August 1984. The cargo of
uranium hexafluoride weighed 2.25 x 108 kg and was
contained in 30 drums, each having a volume of 1.62 x 106
L. What is the density (g/mL) of uranium hexafluoride?
A) 1.39 g/mL
B) 4.63 g/mL
C) 1.39 g/mL
D) 46.3 g/mL
E) 41.7 g/mL
41.
What are the components of the scientific method?
42.
In 1928, 1.0 g of a new element was isolated from 660 kg
of the ore molybdenite. The percent by mass of this
element in the ore was:
A) 1.5%
B) 6.6%
C) 1.0%
D) 1.5 x 10–4%
E) 3.5 x 10–3%
43.
The density of gasoline is 0.7025 g/mL at 20°C. When
gasoline is added to water:
A) it will float on top.
B) it will sink to the bottom.
C) it will mix so you can't see it.
D) the mixture will improve the running of the motor.
E) none of these things will happen.
Page 3
44.
The amount of uncertainty in a measured quantity is
determined by:
A) both the skill of the observer and the limitations of
the measuring instrument.
B) neither the skill of the observer nor the limitations of
the measuring instrument.
C) the limitations of the measuring instrument only.
D) the skill of the observer only.
45.
A quantitative observation
A) contains a number and a unit.
B) does not contain a number.
C) always makes a comparison.
D) must be obtained through experimentation.
E) none of these
46.
_________ are substances with constant composition that
can be broken down into elements by chemical processes.
A) Solutions
B) Mixtures
C) Compounds
D) Quarks
E) Heterogeneous mixtures
47.
The volume of 65 L equals
A) 65 dm3
B) 65000 cm3
C) 650 dm3
D) 650 cm3
E) 65 dm3 and 65000 cm3
48.
On a new temperature scale (°Z), water boils at 120.0 °Z
and freezes at 40.0 °Z. Calculate the normal human body
temperature using this temperature scale. On the Celsius
scale, normal human body temperature is 37 °C, and water
boils at 100.0 °C and freezes at 0.00 °C.
49.
A 20.0-mL sample of glycerol has a mass of 25.2 grams.
What is the mass of a 53-mL sample of glycerol?
50.
The calibration points for the linear Reaumur scale are the
usual melting point of ice and boiling point of water, which
are assigned the values 0°R and 80°R, respectively. The
normal body temperature of humans is 98.6°F. What is
this temperature in °R?
A) 37.0
B) 28.0
C) 29.0
D) 29.6
E) none of these
51.
The first chemist to perform truly quantitative
experiments was
A) Paracelsus.
B) Boyle.
C) Priestly.
D) Bauer.
E) Lavoisier.
UNIT 1 WORKSHEET
52.
53.
54.
55.
A species with 12 protons and 10 electrons is
A) Ne2+
B) Ti2+
C) Mg2+
D) Mg
E) Ne2–
Which among the following represent a set of isotopes?
Atomic nuclei containing:
I. 20 protons and 20 neutrons.
II. 21 protons and 19 neutrons.
III. 22 neutrons and 18 protons.
IV. 20 protons and 22 neutrons.
V. 21 protons and 20 neutrons.
A) I, II, III
B) III, IV
C) I, V
D) I, IV and II, V
E) No isotopes are indicated.
Which of the following statements from Dalton's atomic
theory is no longer true, according to modern atomic
theory?
A) Elements are made up of tiny particles called atoms.
B) Atoms are not created or destroyed in chemical
reactions.
C) All atoms of a given element are identical.
D) Atoms are indivisible in chemical reactions.
E) All of these statements are true according to modern
atomic theory.
Three samples of a solid substance composed of elements
A and Z were prepared. The first contained 4.31 g A and
7.69 g Z. The second sample was 35.9% A and 64.1% Z. It
was observed that 0.718 g A reacted with Z to form 2.00 g
of the third sample. Show that these data illustrate the
law of definite composition.
57.
Which of the following atomic symbols is incorrect?
A)
14
6
C
Page 4
37
17
Cl
C)
32
15
P
D)
39
19
K
E)
14
8
N
58.
Complete the following table.
59.
The number of neutrons in an atom is the same for all
neutral atoms of that element.
60.
The formula of water, H2O, suggests
A) there is twice as much mass of hydrogen as oxygen in
each molecule.
B) there are two hydrogen atoms and one oxygen atom per
water molecule.
C) there is twice as much mass of oxygen as hydrogen in
each molecule.
D) there are two oxygen atoms and one hydrogen atom per
water molecule.
E) none of these
61.
The scientist who discovered the law of conservation of
mass and is also called the father of modern chemistry is
A) Proust.
B) Boyle.
C) Priestly.
D) Bauer.
E) Lavoisier.
62.
All of the following are characteristics of nonmetals
except:
A) poor conductors of electricity
B) often bond to each other by forming covalent bonds
C) tend to form negative ions in chemical reactions with
metals
D) appear in the upper left-hand corner of the periodic
table
E) do not have a shiny (lustrous) appearance
63.
The correct name for Ca2+ is
A) calcium
Complete the following table.
56.
B)
UNIT 1 WORKSHEET
B)
C)
D)
E)
64.
65.
calcium (II) ion
calcium ion
calcium (I) ion
monocalcium ion
Which of the following statements are true of uranium238?
I. Its chemical properties will be exactly like those of
uranium-235.
II. Its mass will be slightly different from that of an atom
of uranium-235.
III. It will contain a different number of protons that an
atom of uranium-235.
IV. It is more plentiful in nature than uranium-235.
A) III, IV
B) I, II, III
C) I, II, IV
D) II, III, IV
E) all of these
All of the following are true except:
A) Ions are formed by adding electrons to a neutral atom.
B) Ions are formed by changing the number of protons in
an atom's nucleus.
C) Ions are formed by removing electrons from a neutral
atom.
D) An ion has a positive or negative charge.
E) Metals tend to form positive ions.
66.
What element (in trace amounts) has been shown to help in
protecting against heart disease and cancer?
A) silicon
B) oxygen
C) selenium
D) copper
E) potassium
67.
The first scientist to show that atoms emit any negative
particles was
A) J. J. Thomson.
B) Lord Kelvin.
C) Ernest Rutherford.
D) William Thomson.
E) John Dalton.
68.
Arsenopyrite is a mineral containing As, Fe, and S. Classify
each element as metal, nonmetal, or metalloid.
73.
SnI2
74.
AgCl
75.
Write the symbol for each
a)
magnesium
b)
potassium
c)
iron
d)
sodium
76.
Which statement is not correct?
A) The mass of an alpha particle is 7300 times that of the
electron.
B) An alpha particle has a 2+ charge.
C) Three types of radioactive emission are gamma rays,
beta rays, and alpha particles.
D) A gamma ray is high-energy "light."
E) There are only three types of radioactivity known to
scientists today.
77.
Which of the following are incorrectly paired?
A) Copper, Co
B) Silver, Ag
C) Iron, Fe
D) Lead, Pb
E) Sodium, Na
78.
The scientist whose alpha-particle scattering experiment
led him to conclude that the nucleus of an atom contains a
dense center of positive charge is
A) J. J. Thomson.
B) Lord Kelvin.
C) Ernest Rutherford.
D) William Thomson.
E) John Dalton.
79.
The average mass of a carbon atom is 12.011. Assuming you
were able to pick up only one carbon unit, the chances that
you would randomly get one with a mass of 12.011 is
A) 0%.
B) 0.011%.
C) about 12%.
D) 12.011%.
E) greater than 50%.
80.
How many atoms (total) are there in one formula unit of
Ca3(PO4)2?
81.
Which of the following statements is (are) true?
Use the following to answer questions 69-74:
Name the following compounds:
69.
NaH
70.
NH4NO3
71.
72.
HNO3
K2Cr2O7
Page 5
A)
18
8
O and 199 F
B)
14
6
C and 147 N
C)
18
8
O2
D)
18
8
O and 199 F
of the following elements.
_________
_________
_________
_________
have the same number of neutrons.
are isotopes of each other because
their mass numbers are the same.
20
Ne.
has the same number of electrons as 10
have the same number of neutrons and
UNIT 1 WORKSHEET
14
6
C and 147 N
18
8
O and 199 F have the same number of neutrons and
18
8
O2
D) All of the above are true.
E) Two of the above are true.
are isotopes of each other because
their mass numbers are the same.
91.
The element rhenium (Re) exists as two stable isotopes and
18 unstable isotopes. Rhenium-185 has in its nucleus
A) 75 protons, 75 neutrons.
B) 75 protons, 130 neutrons.
C) 130 protons, 75 neutrons.
D) 75 protons, 110 neutrons.
E) not enough information is given.
92.
Which of the following are incorrectly paired?
A) Mercury, Hg
B) Potassium, K
C) Tungsten, T
D) Tin, Sn
E) Antimony, Sb
93.
nitric acid
Write the names of the following compounds:
a) FeSO4
84.
dinitrogen trioxide
b)
85.
phosphoric acid
c)
86.
The formula for calcium bisulfate is
A) Ca(SO4)2
d)
E)
82.
20
Ne.
has the same number of electrons as 10
By knowing the number of protons a neutral atom has, you
should be able to determine
A) the number of neutrons in the neutral atom.
B) the number of electrons in the neutral atom.
C) the name of the atom.
D) two of the above.
E) none of the above
Use the following to answer questions 83-85:
Write the formula for:
83.
B) CaS2
C) Ca(HSO4)2
e)
95.
Rutherford's experiment was important because it showed
that:
A) radioactive elements give off alpha particles.
B) gold foil can be made to be only a few atoms thick.
C) a zinc sulfide screen scintillates when struck by a
charged particle.
D) the mass of the atom is uniformly distributed
throughout the atom.
E) an atom is mostly empty space.
96.
The correct name for LiCl is
A) lithium monochloride
B) lithium (I) chloride
C) monolithium chloride
D) lithium chloride
E) monolithium monochloride
C) H2O and C12H22O11
D) H2SO4 and H2S
E) KCl and KClO2
The first people to attempt to explain why chemical
changes occur were
A) alchemists.
B) metallurgists.
C) physicians.
D) physicists.
E) the Greeks.
The number of electrons in an atom is the same for all
neutral atoms of that element.
90.
An ion is formed
A) by either adding or subtracting protons from the atom.
B) by either adding or subtracting electrons from the
atom.
C) by either adding or subtracting neutrons from the
atom.
________________________________
NiCO3
Write the chemical formulas for the following compounds
or ions.
a)
nitrate ion
_______________________
b)
aluminum oxide
_______________________
c)
ammonium ion
_______________________
d)
perchloric acid
_______________________
e)
copper(II) bromide
_______________________
Which of the following pairs can be used to illustrate the
law of multiple proportions?
A) SO and SO2
89.
________________________________
Ca(OH)2
94.
B) CO and CaCo3
88.
________________________________
KNO2
________________________________
D) Ca2HSO4
E) Ca2S
87.
________________________________
NaC2H3O2
Page 6
UNIT 1 WORKSHEET
97.
All of the following are in aqueous solution. Which is
incorrectly named?
A) H2SO4, sulfuric acid
103.
Which of the following electron configurations are
different from those expected?
A) Ca
B) Sc
C) Ti
D) V
E) Cr
104.
Give the quantum numbers for the last electron in:
a) gold
b) magnesium
c) iodine
d) cadmium
B) H2CO3, carbonic acid
C) H3PO4, phosphoric acid
D) HCN, cyanic acid
E) HCl, hydrochloric acid
98.
99.
100.
101.
102.
127 
The numbers of protons, neutrons, and electrons in 53
I
are:
A) 52
B) 53
C) 53
D) 53
E) 53
p,
p,
p,
p,
p,
40
20
Ca 2
A)
B)
C)
D)
E)
20
22
20
22
20
128 n, 53 e
127 n, 54 e
127 n, 52 e
74 n, 54 e
74 n, 52 e
has
protons,
protons,
protons,
protons,
protons,
Use the following to answer question 105:
Consider the following portion of the energy-level diagram for
hydrogen:
n=4
–0.1361 x 10–18 J
n=3
–0.2420 x 10–18 J
n=2
–0.5445 x 10–18 J
n=1
–2.178 x 10–18 J
20 neutrons, and 18 electrons.
20 neutrons, and 20 electrons.
22 neutrons, and 18 electrons.
18 neutrons, and 18 electrons.
20 neutrons, and 22 electrons.
105.
For which of the following transitions does the light
emitted have the longest wavelength?
A) n = 4 to n = 3
B) n = 4 to n = 2
C) n = 4 to n = 1
D) n = 3 to n = 2
E) n = 2 to n = 1
106.
The number of orbitals having a given value of l is equal to
A) 2l + 1
B) 2n + 2
C) 3l
D) l + ml
Which of the following has 45 neutrons, 35 protons, and 36
electrons?
A)
80
35
B)
103
45
C)
80
35
Br 
D)
71
35
Lu
E)
81
35
Hg
Rh 
Tl 
E) the number of lobes in each orbital
A strong line in the spectrum of atomic mercury has a
wavelength of 254 nm. When mercury emits a photon of
light at this wavelength, the frequency of this light is
A) 8.46 x 10–16 s–1
B) 7.61 x 105 s–1
C) 1.18 x 1015 s–1
D) 1.31 x 10–6 s–1
E) none of these
107.
If n = 2, how many orbitals are possible?
A) 3
B) 4
C) 2
D) 8
E) 6
Use the following to answer question 108:
Which statements about hydrogen are true?
I. H has a lower ionization energy than He.
II. H– is smaller than H.
III. H bonds with the halogens to form polar covalent
compounds.
IV. H is always a metal.
V. H does not have a second ionization energy.
A) I, V
B) II, IV
C) I, III, V
D) II, IV, V
E) I, III, IV, V
Nitrogen has 5 valence electrons. Consider the following electron
arrangements.
Page 7
UNIT 1 WORKSHEET
108.
Which represents the ground state for N?
109.
What is the wavelength of light that is emitted when an
excited electron in the hydrogen atom falls from n=5 to
n=2?
A) 5.12 × 10–7 m
B) 4.34 × 10–7 m
C) 6.50 × 10–7 m
D) 5.82 × 10–7 m
E) none of these
110.
Which of the following combinations of quantum numbers
do not represent permissible solutions of the Schroedinger
equation for the electron in the hydrogen atom (i.e., which
combination of quantum numbers is not allowed)?
n
l
m
s (or ms)
A)
9
8
B)
8
2
C)
6
–5
D)
6
5
E) All are allowed.
111.
–4
2
–1
–5
1/2
1/2
1/2
1/2
116.
Sodium losing an electron is an ________ process and
fluorine losing an electron is an _______ process.
A) endothermic, exothermic
B) exothermic, endothermic
C) endothermic, endothermic
D) exothermic, exothermic
E) more information needed
117.
The Si unit for frequency is cycles per second.
118.
Order the elements S, Cl, and F in terms of increasing
atomic radii.
A) S, Cl, F
B) Cl, F, S
C) F, S, Cl
D) F, Cl, S
E) S, F, Cl
119.
Which of the following atoms has the largest ionization
energy?
A) O
B) Li
C) N
D) Be
E) K
120.
How many electrons can be contained in all of the orbitals
with n = 4?
A) 2
B) 8
C) 10
D) 18
E) 32
121.
When an electron in a 2p orbital of a lithium atom makes a
transition to the 2s orbital, a photon of wavelength 670.8
nm is emitted. The energy difference between these 2p
and 2s orbitals is
A) 2.96 x 10–10 J
B) 2.96 x 10–19 J
C) 3.38 x 1018 J
D) 2.96 x 10–17 J
E) none of these
122.
The electron configuration for the barium atom is:
A) 1s22s22p63s23p63d104s2
B) [Xe] 6s2
C) 1s22s22p63s23p64s1
D) 1s22s22p63s23p64s2
E) none of these
__________ is the energy change associated with the
addition of an electron to a gaseous atom.
Use the following to answer questions 112-114:
Given the following electronic configuration of neutral atoms,
identify the element and state the number of unpaired electrons in
its ground state:
112.
[He]2s22p3
113.
[Ne]3s23p5
Use the following to answer questions 123-124:
114.
[Ar]4s23d4
Choose the correct answer for the atom using the periodic chart.
115.
In general the ionization energy and electron affinity
increase from __________ (left to right or right to left)
in a period of the periodic table. Why?
Page 8
123.
Larger first ionization energy, Na Rb
124.
Larger atomic or ionic radius, Mg Mg2+
UNIT 1 WORKSHEET
125.
All halogens have the following number of valence
electrons:
A) 2
B) 3
C) 5
D) 7
E) none of these
126.
Which of the following electron configurations is correct?
A) Ga:
[Kr]3d104s24p1
B) Mo: [Kr]5s24d5
C) Ca:
[Ar]4s13d10
D) Br:
[Kr]3d104s24p7
E) Bi:
[Xe]6s24f145d106p3
127.
List the following atoms in order of increasing ionization
energy: Li, Na, C, O, F.
A) Li < Na < C < O < F
B) Na < Li < C < O < F
C) F < O < C < Li < Na
D) Na < Li < F < O < C
E) Na < Li < C < F < O
128.
129.
How many f orbitals have the value n = 3?
A) 0
B) 3
C) 5
D) 7
E) 1
135.
How many electrons in an atom can have the quantum
numbers n = 3, l = 2?
A) 2
B) 5
C) 10
D) 18
E) 6
136.
Which of the following is an incorrect designation for an
atomic orbital?
A) 1s
B) 3d
C) 1p
D) 4f
E) 6s
137.
When ignited, a uranium compound burns with a green
flame. The wavelength of the light given off by this flame
is greater than that of
A) red light.
B) infrared light.
C) radio waves.
D) ultraviolet light.
E) none of these
138.
Which of the following is a reasonable criticism of the
Bohr model of the atom?
A) It makes no attempt to explain why the negative
electron does not eventually fall into the positive
nucleus.
B) It does not adequately predict the line spectrum of
hydrogen.
C) It does not adequately predict the ionization energy of
the valence electron(s) for elements other than
hydrogen.
D) It does not adequately predict the ionization energy of
the 1st energy level electrons for one-electron species
for elements other than hydrogen.
E) It shows the electrons to exist outside of the nucleus.
139.
The magnetic quantum number tells the polarity of the
atom.
140.
If l = 3, how many electrons can be contained in all the
possible orbitals?
A) 7
B) 6
C) 14
D) 10
E) 5
141.
The calcium atom is much larger than the calcium ion, while
the fluorine atom is much smaller than the fluorine ion.
Explain this natural occurrence.
142.
When a strontium salt is ignited, it burns with a red flame.
The frequency of the light given off by this flame is
greater than
A) yellow light
How many unpaired electrons are there in an atom of sulfur
in its ground state?
A) 0
B) 1
C) 2
D) 3
E) 4
Use the following to answer questions 130-132:
Write the electron configuration for the following:
130.
Fe3+
131.
I
132.
P
133.
__________ is the distance between two consecutive
peaks or troughs in a wave.
134.
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
Page 9
UNIT 1 WORKSHEET
B)
C)
D)
E)
infrared light
ultraviolet light
radio waves
x-rays
B)
C)
D)
E)
Use the following to answer questions 143-144:
From the following list of observations, choose the one that most
clearly supports the following conclusion:
a) emission spectrum of hydrogen
b) the photoelectric effect
c) scattering of alpha particles by metal foil
d) diffraction
e) cathode "rays"
143.
Electromagnetic radiation has wave characteristics.
144.
Electrons have wave properties.
145.
The first ionization energy of Mg is 735 kJ/mol. The
second ionization energy is
A) 735 kJ/mol
B) less than 735 kJ/mol
C) greater than 735 kJ/mol
D) More information is needed to answer this question.
146.
The statement that "the lowest energy configuration for
an atom is the one having the maximum number of unpaired
electrons allowed by the Pauli principle in a particular set
of degenerate orbitals" is known as
A) the aufbau principle.
B) Hund's rule.
C) Heisenberg uncertainty principle.
D) the Pauli exclusion principle.
E) the quantum model.
147.
148.
149.
Which of the following statements is true about the
ionization energy of Mg+?
A) It will be equal to the ionization energy of Li.
B) It will be equal to and opposite in sign to the electron
affinity of Mg.
C) It will be equal to and opposite in sign to the electron
affinity of Mg+.
D) It will be equal to and opposite in sign to the electron
affinity of Mg2+.
E) none of these
An element with the electron configuration
[Xe]4f145d76s2 would belong to which class on the
periodic table?
A) transition elements
B) alkaline earth elements
C) halogens
D) rare earth elements
E) none of these
Who was the first chemist to recognize patterns in
chemical properties of the elements?
A) Medeleev
Page 10
Newlands
Meyer
Dobereiner
Bohr
150.
In general, the ionization energy and electron affinity
increase from _________ (top to bottom or bottom to
top) in a family of the periodic table. Why?
151.
Which of the following statements is (are) true?
I. An excited atom can return to its ground state by
absorbing
electromagnetic radiation.
II. The energy of an atom is increased when
electromagnetic radiation is
emitted from it.
III. The energy of electromagnetic radiation increases as
its frequency
increases.
IV. An electron in the n = 4 state in the hydrogen atom
can go to the
n = 2 state by emitting electromagnetic radiation at
the appropriate
frequency.
V. The frequency and wavelength of electromagnetic
radiation are inversely
proportional to each other.
A) II, III, IV
B) III, V
C) I, II, III
D) III, IV, V
E) I, II, IV
152.
The electron configuration for Cr2+ is
A) [Ar]4s23d4
B) [Ar]4s13d5
C) [Ar]3d4
D) [Ar]4s23d2
E) none of these
153.
Which of the following is incorrect?
A) The continuous spectrum of hydrogen contains only
four discrete colors.
B) Diffraction produces both constructive and
destructive interference.
C) All matter displays both particle and wavelike
characteristics.
D) Niels Bohr developed a quantum model for the
hydrogen atom.
E) The lowest possible energy state of a molecule or atom
is called its ground state.
154.
The number of unpaired electrons in the outer subshell of
a Cl atom is
A) 0.
B) 1.
C) 2.
D) 3.
E) none of these
UNIT 1 WORKSHEET
155.
156.
157.
158.
159.
160.
Which of the following atoms has three electrons in p
orbitals in its valence shell?
A) Ba
B) Ga
C) V
D) Bi
E) none of these
An atom of fluorine contains 9 electrons. How many of
these electrons are in s orbitals?
A) 2
B) 4
C) 6
D) 8
E) none
Which of the following combinations of quantum numbers is
not allowed?
n
l
m(l)
m(s)
A)
1
1
0
1/2
B)
3
0
0
–1/2
C)
2
1
–1
1/2
D)
4
3
–2
–1/2
E)
4
2
0
1/2
Which of the following concerning second IE's is true?
A) That of Al is higher than that of Mg because Mg wants
to lose the second electron, so it is easier to take the
second electron away.
B) That of Al is higher than that of Mg because the
electrons are taken from the same energy level, but
the Al atom has one more proton.
C) That of Al is lower than that of Mg because Mg wants
to lose the second electron, thus the energy change is
greater.
D) That of Al is lower than that of Mg because the second
electron taken from Al is in a p orbital, thus it is easier
to take.
E) The second ionization energies are equal for Al and Mg.
4
He2+
Alpha particles 2
beamed at thin metal foil may
A) pass directly through without changing direction.
B) be slightly diverted by attraction to electrons.
C) be reflected by direct contact with nuclei.
D) pass directly through without changing direction and
be reflected by direct contact with nuclei.
E) pass directly through without changing direction, be
slightly diverted by attraction to electrons, and be
reflected by direct contact with nuclei.
The electron configuration of Ti2+ is
A) [Ar]4s2
B) [Ar]4s13d1
C) [Ar]3d2
D) [Ar]4s23d2
E) none of these
Page 11
161.
When electron configurations differ from expected, it is
because orbitals want to be half-filled.
162.
Which of the following is not determined by the principal
quantum number, n, of the electron in a hydrogen atom?
A) the energy of the electron
B) the minimum wavelength of the light needed to remove
the electron from the atom.
C) the size of the corresponding atomic orbital(s)
D) the shape of the corresponding atomic orbital(s)
E) All of these are determined by n.
163.
The ionization energies in kcal for Mg and Ca are
Mg
Ca
1st
176
141
2nd
346
247
3rd
1847
a) Indicate the reasons for the relatively high 3rd
ionization energy for magnesium.
b) Indicate the reasons for the differences in 1st
ionization energies for Mg and Ca.
c) Predict the 3rd ionization energy for calcium.
164.
Which of the following statements is false?
A) A sodium atom has a smaller radius than a potassium
atom.
B) A neon atom has a smaller radius than an oxygen atom.
C) A fluorine atom has a smaller first ionization energy
than an oxygen atom.
D) A cesium atom has a smaller first ionization energy
than a lithium atom.
E) All are true.
165.
Order the elements S, Cl, and F in terms of increasing
ionization energy.
A) S, Cl, F
B) Cl, F, S
C) F, S, Cl
D) F, Cl, S
E) S, F, Cl
166.
The modern periodic table was developed independently by
Dimitri Mendeleev and John Newlands.
167.
The electron configuration of indium is
A) 1s22s22p63s23p63d104s24p64d105s25p15d10
B) 1s22s22p63s23p63d104s24d104p1
C) 1s23s22p63s23p64s24p64d105s25d105p1
D) 1s22s22p63s23p63d104s24p64d105s25p1
E) none of these
168.
An element has the electron configuration [Kr]4d105s25p2.
The element is a(n)
A) nonmetal.
B) transition element.
C) metal.
D) lanthanide.
E) actinide.
UNIT 1 WORKSHEET
169.
Diffraction results when light is scattered from a regular
array of points or lines.
170.
The energy of the light emitted when a hydrogen electron
goes from n = 2 to n = 1 is what fraction of its groundstate ionization energy?
A) 3/4
B) 1/2
C) 1/4
D) 1/8
E) 1/9
171.
Fe has __________ that is (are) unpaired in its d orbitals.
A) 1 electron
B) 2 electrons
C) 3 electrons
D) 4 electrons
E) none of these
172.
__________ states that the lowest energy configuration
for an atom has the maximum number of unpaired electrons
in degenerate orbital.
173.
Germanium has __________ in its 4p orbitals.
A) 1 electron
B) 2 electrons
C) 3 electrons
D) 4 electrons
E) none of these
174.
Consider the following orderings.
I. Al < Si < P < Cl
II. Be < Mg < Ca < Sr
III. I < Br < Cl < F
IV. Na+ < Mg2+ < Al3+ < Si4+
Which of these give(s) a correct trend in ionization
energy?
A) III
B) I, II
C) I, IV
D) I, III, IV
E) none of them
175.
A given set of p orbitals consists of ______ orbitals.
A) 1
B) 2
C) 3
D) 4
E) 5
Page 12
UNIT 1 WORKSHEET
Answer Key -- Unit 1 Worksheet
1.
2.
3.
4.
5.
6.
7.
8.
9.
10.
11.
12.
13.
14.
15.
16.
17.
18.
19.
20.
21.
22.
23.
24.
25.
26.
27.
28.
29.
30.
31.
32.
33.
34.
35.
36.
37.
38.
39.
40.
41.
42.
43.
44.
45.
46.
47.
48.
49.
50.
51.
52.
53.
54.
55.
See Sec. 1.9 of Zumdahl, Chemistry.
A
E
A
D
False
B
A
A
A
1.48 x 106 g
C
–40.0 °F
A
E
B
False
A
average price per gallon of gasoline, average MPG of the
car, mileage of trip
A
E
See Sec. 1.8 of Zumdahl, Chemistry.
B
B
B
E
False
E
B
D
E
B
C
57.3 °Y
B
B
E
A
A
B
See Sec. 1.2 of Zumdahl, Chemistry.
D
A
A
A
C
E
69.6 °Z
(25.2 g/20.0 mL) (53 mL) = 66.8 g = 67 g to 2 sig. figs.
D
B
C
D
C
56.
57.
58.
See Sec. 2.2 of Zumdahl, Chemistry.
E
59.
60.
61.
62.
63.
64.
65.
66.
67.
68.
69.
70.
71.
72.
73.
74.
75.
76.
77.
78.
79.
80.
81.
82.
83.
False
B
E
D
C
C
B
C
A
As = metalloid, Fe = metal, S = nonmetal
sodium hydride
ammonium nitrate
nitric acid
potassium dichromate
tin(II) iodide
silver chloride
a) Mg b) K c) Fe d) Na
E
A
C
A
13
E
D
HNO3
84.
85.
86.
87.
88.
89.
90.
91.
Page 13
N2O3
H3PO4
C
A
E
True
B
D
UNIT 1 WORKSHEET
92.
93.
94.
95.
96.
97.
98.
99.
100.
101.
102.
103.
104.
105.
106.
107.
108.
109.
110.
111.
112.
113.
114.
115.
116.
117.
118.
119.
120.
121.
122.
123.
124.
125.
126.
127.
128.
129.
130.
131.
132.
133.
134.
135.
136.
137.
C
a) iron(II) sulfate
b) sodium acetate
c) potassium nitrite
d) calcium hydroxide
e) nickel(II) carbonate
a) NO3– b) Al2O3 c) NH4+ d) HClO4 e) CuBr2
E
D
D
D
A
C
C
C
E
a) gold-5, 2, 2, 1/2
b) magnesium-3, 0, 0, 1/2
c) iodine-5, 1, 1, 1/2
d) cadmium-4, 2, 2, 1/2
A
A
B
138.
139.
140.
141.
142.
143.
144.
145.
146.
147.
148.
149.
150.
151.
152.
153.
154.
155.
156.
157.
158.
159.
160.
161.
162.
163.
164.
165.
166.
167.
168.
169.
170.
171.
172.
173.
174.
175.
B
C
Electron affinity
The element is N with three unpaired electrons in its
ground state.
The element is Cl with one unpaired electron in its ground
state.
The element is Cr with four unpaired electrons in its
ground state.
The increase is from left to right because of the increase
in nuclear charge.
C
False
D
C
E
B
B
Na
Mg
D
E
B
A
C
1s22s22p63s23p64s23d3 or [Ar]4s23d3
1s22s22p63s23p64s23d104p65s24d105p5 or [Kr]5s25p5
1s22s22p63s23p3 or [Ne]3s23p3
Wavelength
B
C
C
D
Page 14
C
False
C
See Sec. 7.13 of Zumdahl, Chemistry.
B
d) diffraction
d) diffraction
C
B
D
A
D
The increase is from bottom to top because the electrons
being removed are closer to the nucleus.
D
C
A
D
D
B
A
B
E
C
False
D
c) 1173
C
A
False
D
C
True
A
D
Hund's rule
B
D
C