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Worksheets2018-19 Chemistry Final Exam
Total questions: 113
Worksheet time: 2hrs 30mins
Name
Class
Date
1.
vaporization at the surface of a liquid that is not boiling
a)
melting point
b)
evaporation
c)
boiling point
d)
vaporization
e)
sublimation
2.
the conversion of a liquid to a gas below the boiling point
a)
melting point
b)
evaporation
c)
boiling point
d)
vaporization
e)
sublimation
3.
the temperature at which the vapor pressure of a liquid is equal to the external pressure
a)
melting point
b)
evaporation
c)
boiling point
d)
vaporization
e)
sublimation
4.
the change of a solid directly to a vapor
a)
melting point
b)
evaporation
c)
boiling point
d)
vaporization
e)
sublimation
5.
the temperature at which a solid changes into a liquid
a)
melting point
b)
evaporation
c)
boiling point
d)
vaporization
e)
sublimation
6.
What is another name for the transition metals?
a)
noble gases
b)
Group B elements
c)
Group A elements
d)
Group C elements
7.
Which of the following elements is in the same period as phosphorus?
a)
carbon
b)
nitrogen
c)
magnesium
d)
oxygen
8.
Each period in the periodic table corresponds to ____.
a)
a principal energy level
b)
an energy sublevel
c)
an orbital
d)
a suborbital
9.
The modern periodic table is arranged in order of increasing atomic ____.
a)
mass
b)
charge
c)
number
d)
radius
10.
Who arranged the elements according to atomic mass and used the arrangement to predict the properties of missing elements?
a)
Henry Moseley
b)
Antoine Lavoisier
c)
John Dalton
d)
Dmitri Mendeleev
11.
Which of the following categories includes the majority of the elements?
a)
metalloids
b)
liquids
c)
metals
d)
nonmetals
12.
Of the elements Pt, V, Li, and Kr, which is a nonmetal?
a)
Pt
b)
V
c)
Li
d)
Kr
13.
To what category of elements does an element belong if it is a poor conductor of electricity?
a)
transition elements
b)
metalloids
c)
nonmetals
d)
metals
14.
In which of the following sets is the symbol of the element, the number of protons, and the number of electrons given correctly?
a)
In, 49 protons, 49 electrons
b)
Zn, 30 protons, 60 electrons
c)
Cs, 55 protons, 132.9 electrons
d)
F, 19 protons, 19 electrons
15.
What element has the electron configuration 1s22s22p63s23p2?
a)
nitrogen
b)
selenium
c)
silicon
d)
silver
16.
Which of the following is true about the electron configurations of the noble gases?
a)
The highest occupied s and p sublevels are completely filled.
b)
The highest occupied s and p sublevels are partially filled.
c)
The electrons with the highest energy are in a d sublevel.
d)
The electrons with the highest energy are in an f sublevel.
17.
Which subatomic particle plays the greatest part in determining the properties of an element?
a)
proton
b)
electron
c)
neutron
d)
none of the above
18.
Which of the following groupings contains only representative elements?
a)
Cu, Co, Cd
b)
Ni, Fe, Zn
c)
Al, Mg, Li
d)
Hg, Cr, Ag
19.
How does atomic radius change from top to bottom in a group in the periodic table?
a)
It tends to decrease.
b)
It tends to increase.
c)
It first increases, then decreases.
d)
It first decreases, then increases.
20.
How does atomic radius change from left to right across a period in the periodic table?
a)
It tends to decrease.
b)
It tends to increase.
c)
It first increases, then decreases.
d)
It first decreases, then increases.
21.
What is the charge of a cation?
a)
a positive charge
b)
no charge
c)
a negative charge
d)
The charge depends on the size of the nucleus.
22.
Which of the following statements is true about ions?
a)
Cations form when an atom gains electrons.
b)
Cations form when an atom loses electrons.
c)
Anions form when an atom gains protons.
d)
Anions form when an atom loses protons.
23.
The metals in Groups 1A, 2A, and 3A ____.
a)
gain electrons when they form ions
b)
all form ions with a negative charge
c)
all have ions with a 1 charge
d)
lose electrons when they form ions
24.
Why is the second ionization energy greater than the first ionization energy?
a)
It is more difficult to remove a second electron from an atom.
b)
The size of atoms increases down a group.
c)
The size of anions decreases across a period.
d)
The nuclear attraction from protons in the nucleus decreases.
25.
In which of the following sets are the charges given correctly for all the ions?
a)
Na+, Mg+, Al+
b)
K+, Sr2+, O2-
c)
Rb-, Ba2-, P3+
d)
N-, O2-, F3-
26.
What is the energy required to remove an electron from an atom in the gaseous state called?
a)
nuclear energy
b)
ionization energy
c)
shielding energy
d)
electronegative energy
27.
How many valence electrons are in an atom of phosphorus?
a)
2
b)
3
c)
4
d)
5
28.
How many valence electrons does a helium atom have?
a)
2
b)
3
c)
4
d)
5
29.
What is the name given to the electrons in the highest occupied energy level of an atom?
a)
orbital electrons
b)
valence electrons
c)
anions
d)
cations
30.
How does calcium obey the octet rule when reacting to form compounds?
a)
It gains electrons.
b)
It gives up electrons.
c)
It does not change its number of electrons.
d)
Calcium does not obey the octet rule.
31.
What is the charge on the strontium ion?
a)
2-
b)
1-
c)
1+
d)
2+
32.
What is the formula of the ion formed when potassium achieves noble-gas electron configuration?
a)
K2+
b)
K+
c)
K1-
d)
K2-
33.
Which of the following elements does NOT form an ion with a charge of 1+?
a)
fluorine
b)
hydrogen
c)
potassium
d)
sodium
34.
What is the formula of the ion formed when phosphorus achieves a noble-gas electron configuration?
a)
P3+
b)
P2+
c)
P2-
d)
P3-
35.
How does oxygen obey the octet rule when reacting to form compounds?
a)
It gains electrons.
b)
It gives up electrons.
c)
It does not change its number of electrons.
d)
Oxygen does not obey the octet rule.
36.
The electron configuration of a fluoride ion, F-, is ____.
a)
1s22s22p5
b)
the same as that of a neon atom
c)
1s22s22p63s1
d)
the same as that of a potassium ion
37.
Which of the following occurs in an ionic bond?
a)
Oppositely charged ions attract.
b)
Two atoms share two electrons.
c)
Two atoms share more than two electrons.
d)
Like-charged ions attract.
38.
Which of the following is true about an ionic compound?
a)
It is a salt.
b)
It is held together by ionic bonds.
c)
It is composed of anions and cations.
d)
all of the above
39.
How many valence electrons are transferred from the calcium atom to iodine in the formation of the compound calcium iodide?
a)
0
b)
1
c)
2
d)
3
40.
What is the formula unit of sodium nitride?
a)
NaN
b)
Na2N
c)
Na3N
d)
NaN3
41.
What is the formula unit of aluminum oxide?
a)
AlO
b)
Al3O
c)
AlO3
d)
Al2O3
42.
What is the name of the ionic compound formed from lithium and bromine?
a)
lithium bromine
b)
lithium bromide
c)
lithium bromium
d)
lithium bromate
43.
Alloys are commonly used in manufacturing. Which of the following is NOT a reason to use an alloy instead of a pure metal?
a)
Bronze is tougher than pure copper.
b)
Sterling silver is stronger than pure silver.
c)
Brass is more malleable than pure copper.
d)
Cast iron is more brittle than pure iron.
44.
Which of the following pairs of elements is most likely to form an ionic compound?
a)
magnesium and fluorine
b)
nitrogen and sulfur
c)
oxygen and chlorine
d)
sodium and aluminum
45.
Ionic compounds are normally in which physical state at room temperature?
a)
solid
b)
liquid
c)
gas
d)
plasma
46.
Under what conditions can potassium bromide conduct electricity?
a)
only when melted
b)
only when dissolved
c)
only when it is in crystal form
d)
only when melted or dissolved in water
47.
Which of the following particles are free to drift in metals?
a)
protons
b)
electrons
c)
neutrons
d)
cations
48.
What is the basis of a metallic bond?
a)
the attraction of metal ions to mobile electrons
b)
the attraction between neutral metal atoms
c)
the neutralization of protons by electrons
d)
the attraction of oppositely charged ions
49.
What characteristic of metals makes them good electrical conductors?
a)
They have mobile valence electrons.
b)
They have mobile protons.
c)
They have mobile cations.
d)
Their crystal structures can be rearranged easily.
50.
An ionic bond is a bond between ____.
a)
a cation and an anion
b)
valence electrons and cations
c)
the ions of two different metals
d)
the ions of two different nonmetals
51.
How do atoms achieve noble-gas electron configurations in single covalent bonds?
a)
One atom completely loses two electrons to the other atom in the bond.
b)
Two atoms share two pairs of electrons.
c)
Two atoms share two electrons.
d)
Two atoms share one electron.
52.
Why do atoms share electrons in covalent bonds?
a)
to become ions and attract each other
b)
to attain a noble-gas electron configuration
c)
to become more polar
d)
to increase their atomic numbers
53.
Which of the following is the name given to the pairs of valence electrons that do not participate in bonding in diatomic oxygen molecules?
a)
unvalenced pair
b)
outer pair
c)
inner pair
d)
unshared pair
54.
A molecule with a single covalent bond is ____.
a)
CO2
b)
Cl2
c)
CO
d)
N2
55.
How many electrons can occupy a single molecular orbital?
a)
0
b)
1
c)
2
d)
4
56.
According to VSEPR theory, molecules adjust their shapes to keep which of the following as far apart as possible?
a)
pairs of valence electrons
b)
inner shell electrons
c)
mobile electrons
d)
the electrons closest to the nuclei
57.
A bond formed between a silicon atom and an oxygen atom is likely to be ____.
a)
ionic
b)
coordinate covalent
c)
polar covalent
d)
nonpolar covalent
58.
What is thought to cause the dispersion forces?
a)
attraction between ions
b)
motion of electrons
c)
sharing of electron pairs
d)
differences in electronegativity
59.
Which of the forces of molecular attraction is the weakest?
a)
dipole interaction
b)
dispersion
c)
hydrogen bond
d)
single covalent bond
60.
What causes dipole interactions?
a)
sharing of electron pairs
b)
attraction between polar molecules
c)
bonding of a covalently bonded hydrogen to an unshared electron pair
d)
attraction between ions
61.
What causes hydrogen bonding?
a)
attraction between ions
b)
motion of electrons
c)
sharing of electron pairs
d)
bonding of a covalently bonded hydrogen atom with an unshared electron pair
62.
What type of ions have names ending in -ide?
a)
only cations
b)
only anions
c)
only metal ions
d)
only gaseous ions
63.
When naming a transition metal ion that can have more than one common ionic charge, the numerical value of the charge is indicated by a ____.
a)
prefix
b)
suffix
c)
Roman numeral following the name
d)
superscript after the name
64.
Aluminum is a group 3A metal. Which ion does A1 typically form?
a)
Al3-
b)
Al3+
c)
Al5-
d)
Al5+
65.
The nonmetals in Groups 6A and 7A ____.
a)
lose electrons when they form ions
b)
have a numerical charge that is found by subtracting 8 from the group number
c)
all have ions with a –1 charge
d)
end in -ate
66.
What determines that an element is a metal?
a)
the magnitude of its charge
b)
the molecules that it forms
c)
when it is a Group A element
d)
its position in the periodic table
67.
An -ate or -ite at the end of a compound name usually indicates that the compound contains ____.
a)
fewer electrons than protons
b)
neutral molecules
c)
only two elements
d)
a polyatomic anion
68.
Which of the following compounds contains the Mn3+ ion?
a)
MnS
b)
MnBr2
c)
Mn2O3
d)
MnO
69.
How are chemical formulas of binary ionic compounds generally written?
a)
cation on left, anion on right
b)
anion on left, cation on right
c)
Roman numeral first, then anion, then cation
d)
subscripts first, then ions
70.
Which of the following formulas represents an ionic compound?
a)
CS2
b)
BaI2
c)
N2O4
d)
PCl3
71.
Which of the following compounds contains the lead(II) ion?
a)
PbO
b)
PbCl4
c)
Pb2O
d)
Pb2S
72.
Binary molecular compounds are made of two ____.
a)
metallic elements
b)
nonmetallic elements
c)
polyatomic ions
d)
cations
73.
In naming a binary molecular compound, the number of atoms of each element present in the molecule is indicated by ____.
a)
Roman numerals
b)
superscripts
c)
prefixes
d)
suffixes
74.
Which of the following is a binary molecular compound?
a)
BeHCO3
b)
PCl5
c)
AgI
d)
MgS
75.
Select the correct formula for sulfur hexafluoride.
a)
S2F6
b)
F6SO3
c)
F6S2
d)
SF6
76.
What is the correct name for the compound CoCl2?
a)
cobalt(I) chlorate
b)
cobalt(I) chloride
c)
cobalt(II) chlorate
d)
cobalt(II) chloride
77.
When an acid reacts with a base, what compounds are formed?
a)
a salt only
b)
water only
c)
metal oxides only
d)
a salt and water
78.
Which of the following is a property of an acid?
a)
sour taste
b)
nonelectrolyte
c)
strong color
d)
unreactive
79.
What is a property of a base?
a)
bitter taste
b)
watery feel
c)
strong color
d)
unreactive
80.
The formula of the hydrogen ion is often written as ____.
a)
H2O+
b)
OH+
c)
H+
d)
H4N+
81.
In a neutral solution, the [H+] is ____.
a)
10-14 M
b)
zero
c)
1 x 107 M
d)
equal to [OH-]
82.
Which type of solution is one with a pH of 8?
a)
acidic
b)
basic
c)
neutral
d)
The type varies, depending on the solution.
83.
What SI unit is used to measure the number of representative particles in a substance?
a)
kilogram
b)
ampere
c)
kelvin
d)
mole
84.
Which of the following is NOT a representative particle?
a)
atom
b)
cation
c)
anion
d)
all of the above
85.
Avogadro's number of representative particles is equal to one ____.
a)
kilogram
b)
ampere
c)
kelvin
d)
mole
86.
How many moles of tungsten atoms are in 4.8 x 1025 atoms of tungsten?
a)
8.0 x 102 moles
b)
8.0 x 101 moles
c)
1.3 x 10-1 moles
d)
1.3 x 10-2 moles
87.
How many atoms are in 0.075 mol of titanium?
a)
1.2 x 10-25
b)
2.2 x 1024
c)
6.4 x 102
d)
4.5 x 1022
88.
How many molecules are in 2.10 mol CO2?
a)
2.53 x 1024 molecules
b)
3.79 x 1024 molecules
c)
3.49 x 10-24 molecules
d)
1.26 x 1024 molecules
89.
Which of the following is NOT a true about atomic mass?
a)
The atomic mass is 12 g for magnesium.
b)
The atomic mass is the mass of one mole of atoms.
c)
The atomic mass is found by checking the periodic table.
d)
The atomic mass is the number of grams of an element that is numerically equal to the mass in amu.
90.
What is true about the molar mass of chlorine gas?
a)
The molar mass is 35.5 g.
b)
The molar mass is 71.0 g.
c)
The molar mass is equal to the mass of one mole of chlorine atoms.
d)
none of the above
91.
What is the molar mass of AuCl3?
a)
96 g
b)
130 g
c)
232.5 g
d)
303.6 g
92.
What is the mass in grams of 5.90 mol C8H18?
a)
0.0512 g
b)
19.4 g
c)
389 g
d)
673 g
93.
What is the number of moles in 432 g Ba(NO3)2?
a)
0.237 mol
b)
0.605 mol
c)
1.65 mol
d)
3.66 mol
94.
What is the number of moles of beryllium atoms in 36 g of Be?
a)
0.25 mol
b)
4.0 mol
c)
45.0 mol
d)
320 mol
95.
The molar volume of a gas at STP occupies ____.
a)
22.4 L
b)
0° C
c)
1 kilopascal
d)
12 grams
96.
Which combination of temperature and pressure correctly describes standard temperature and pressure, STP?
a)
0° C and 101 kPa
b)
1° C and 0 kPa
c)
0° C and 22.4 kPa
d)
100° C and 100 kPa
97.
What is the volume, in liters, of 0.500 mol of C3H8 gas at STP?
a)
0.0335 L
b)
11.2 L
c)
16.8 L
d)
22.4 L
98.
What is the density at STP of the gas sulfur hexafluoride, SF6?
a)
0.153 g/L
b)
6.52 g/L
c)
3270 g/L
d)
3.93 10 g/L
99.
What information is needed to calculate the percent composition of a compound?
a)
the weight of the sample to be analyzed and its density
b)
the weight of the sample to be analyzed and its molar volume
c)
the formula of the compound and the atomic mass of its elements
d)
the formula of the compound and its density
100.
If 60.2 grams of Hg combines completely with 24.0 grams of Br to form a compound, what is the percent composition of Hg in the compound?
a)
0.285
b)
0.399
c)
0.715
d)
0.601
101.
What is the percent by mass of carbon in acetone, C3H6O?
a)
0.207
b)
0.621
c)
0.0161
d)
0.3
102.
Chemical equations ____.
a)
describe chemical reactions
b)
show how to write chemical formulas
c)
give directions for naming chemical compounds
d)
describe only biological changes
103.
In the chemical equation H2O2 → H2O + O2, the O2 is a ____.
a)
catalyst
b)
solid
c)
product
d)
reactant
104.
A catalyst is ____.
a)
the product of a combustion reaction
b)
not used up in a reaction
c)
one of the reactants in single-replacement reactions
d)
a solid product of a reaction
105.
When the equation Fe + Cl2 → FeCl3 is balanced, what is the coefficient for Cl2?
a)
1
b)
2
c)
3
d)
4
106.
When the following equation is balanced, what is the coefficient for HCl? Mg + HCl → MgCl2 + H2
a)
6
b)
3
c)
1
d)
2
107.
Chemical equations must be balanced to satisfy ____.
a)
the law of definite proportions
b)
the law of multiple proportions
c)
the law of conservation of mass
d)
Avogadro’s principle
108.
What are the missing coefficients for the skeleton equation below? Cr + Fe(NO3)2 → Fe + Cr(NO3)3
a)
4, 6, 6, 2
b)
2, 3, 2, 3
c)
2, 3, 3, 2
d)
1, 3, 3, 1
109.
The type of reaction that takes place when one element reacts with a compound to form a new compound and a different element is a ____.
a)
combination reaction
b)
decomposition reaction
c)
single-replacement reaction
d)
double-replacement reaction
110.
In a double-replacement reaction, the ____.
a)
products are always molecular
b)
reactants are two ionic compounds
c)
reactants are two elements
d)
products are a new element and a new compound
111.
The equation Mg + 2HCl → MgCl2 + H2 is an example of which type of reaction?
a)
combination reaction
b)
single-replacement reaction
c)
decomposition reaction
d)
double-replacement reaction
112.
The equation H3PO4 + 3KOH → K3PO3 + 3H2O is an example of which type of reaction?
a)
double-replacement reaction
b)
combination reaction
c)
decomposition reaction
d)
single-replacement reaction
113.
The equation 2C3H7OH + 9O2 → 6CO2 + 8H2O is an example of which type of reaction?
a)
combustion reaction
b)
single-replacement reaction
c)
double-replacement reaction
d)
decomposition reaction
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