WorksheetsHC S1 Exam Review Part 2
Total questions: 80
Worksheet time: 40mins
Name
Class
Date
1.
The octet rule indicates that ________.
a)
all of the noble gases have eight total electrons
b)
all of the shells in an atom hold a maximum of 8 electrons
c)
all of the Group A elements have 8 valence electrons
d)
atoms lose, gain, or share valence electrons to have 8 valence electrons
e)
the noble gases react with other compounds to get 8 valence electrons
2.
In ionic compounds, ________ lose their valence electrons to form positively charged ________.
a)
metals, anions
b)
nonmetals, cations
c)
metals, polyatomic ions
d)
nonmetals, anions
e)
metals, cations
3.
How many electrons will aluminum gain or lose when it forms an ion?
a)
lose 1
b)
gain 5
c)
lose 2
d)
lose 3
e)
gain 1
4.
An anion always ________.
a)
has a positive charge
b)
contains a group of two or more atoms with a positive charge
c)
contains a metal and a nonmetal
d)
forms covalent bonds
e)
has a negative charge
5.
The Fe2+ ion has ________.
a)
26 protons and 26 electrons
b)
56 protons and 53 electrons
c)
23 protons and 26 electrons
d)
26 protons and 24 electrons
e)
23 protons and 23 electrons
6.
Calcium chloride has the following formula.
a)
CaCl2
b)
CuCl2
c)
CaCl
d)
CuCl
e)
CaClO3
7.
Which one of the following elements forms two or more ions with different ionic charges?
a)
K
b)
F
c)
Ca
d)
O
e)
Fe
8.
The correct name for FeS is ________.
a)
iron(II) sulfate
b)
iron(II) sulfite
c)
iron(II) sulfide
d)
ferric sulfide
e)
ferrous sulfite
9.
What is the formula of a compound that contains Na+ and PO4^3- ions?
a)
Na3PO4
b)
NaPO4
c)
Na2PO3
d)
Na3PO3
e)
Na3P
10.
A group of covalently bonded atoms that has an overall electrical charge is called a(n) ________.
a)
ionic compound
b)
anion
c)
polyatomic ion
d)
cation
e)
molecule
11.
In a molecule with covalent bonding, ________.
a)
oppositely charged ions are held together by strong electrical attractions
b)
atoms of metals form bonds to atoms of nonmetals
c)
atoms of different metals form bonds
d)
atoms are held together by sharing electrons
e)
atoms of noble gases are held together by attractions between oppositely charged ions
12.
The correct name for the compound N2O3 is ________.
a)
nitrogen oxide
b)
nitrogen trioxide
c)
dinitride trioxide
d)
dinitrogen oxide
e)
dinitrogen trioxide
13.
The formula for sulfur dichloride is ________.
a)
SCl2
b)
S2Cl2
c)
S2Cl
d)
S4Cl2
e)
SCl
14.
Double and triple bonds form because ________.
a)
the atoms involved have high electronegativities
b)
single covalent bonds do not give all of the atoms in the molecule eight valence electrons
c)
one of the atoms in the molecule has more than 8 valence electrons
d)
the ions involved have charges larger than one
e)
there is at least one hydrogen atom involved in the bond
15.
Electronegativity is ______________.
a)
How large an atom is
b)
Energy required to remove one electron from an atom in the gas phase.
c)
Measure of an attraction of an atom for a shared electron.
16.
How many covalent bonds will a nitrogen atom normally make?
a)
1
b)
2
c)
3
d)
4
e)
6
17.
When two or more equivalent dot structures can be written for a given molecule it is said to have ________ structures.
a)
resonance
b)
equal
c)
identical
d)
polar
e)
electronegative
18.
The VSEPR theory allows us to determine the ________.
a)
shape of a molecule
b)
charge on an ion
c)
color of a compound
d)
bond type for a molecule
e)
formula for a compound
19.
In water, the melting point is unusually high because of ________.
a)
covalent bonds in the individual molecules
b)
ionic bonds in the individual molecules
c)
hydrogen bonding between the molecules
d)
dipole-dipole attractions between the molecules
e)
the heat content of the hydrogen-oxygen bonds
20.
The main interactions between molecules of hydrogen chloride are examples of ________.
a)
ionic bonds
b)
covalent bonds
c)
hydrogen bonds
d)
dipole-dipole attractions
e)
dispersion forces
21.
Water has a boiling point of 100 °C, and alcohol has a boiling point of 78 °C, even though water is a smaller molecule. This large difference in boiling point is due to ________.
a)
weak dipole-dipole attractions in the alcohol molecules
b)
ionic bonds between the water molecules
c)
covalent bonds in the alcohol molecules
d)
more hydrogen bonds between the water molecules
e)
more hydrogen bonds between the alcohol molecules
22.
A heating curve illustrates ________.
a)
what a substance looks like as it is heated
b)
what happens to the particles of a substance as it is heated
c)
what happens to the heat applied as the temperature is increased
d)
the changes in the temperature and physical state of a substance as it is heated
e)
the chemical changes that occur as the substance is heated
23.
Identify the physical state(s) corresponding to labeled regions on the cooling curve of water shown below. Region A
a)
gas
b)
liquid
c)
liquid and gas
d)
solid and gas
e)
solid
24.
Identify the physical state(s) corresponding to labeled regions on the cooling curve of water shown below. Region B
a)
liquid and gas
b)
liquid
c)
gas
d)
solid and gas
e)
solid
25.
Identify the physical state(s) corresponding to labeled regions on the cooling curve of water shown below. Region C
a)
liquid
b)
liquid and gas
c)
gas
d)
solid and gas
e)
solid
26.
Identify the physical state(s) corresponding to labeled regions on the cooling curve of water shown below. Region D
a)
liquid and solid
b)
liquid
c)
liquid and gas
d)
gas
e)
solid and gas
27.
Identify the physical state(s) corresponding to labeled regions on the cooling curve of water shown below. Region E
a)
solid
b)
liquid
c)
liquid and gas
d)
gas
e)
solid and gas
28.
Water, H2O, is an example of a(n) ________.
a)
chemical
b)
solid
c)
wave
d)
electric charge
e)
element
29.
Which of the following is NOT a chemical?
a)
salt
b)
water
c)
light
d)
carbon dioxide
e)
sugar
30.
Written in scientific notation, 540,000 is ________.
a)
0.54 × 10⁶
b)
54 × 10⁸
c)
5.4 × 10-⁵
d)
5.4 × 10⁵
e)
5.4
31.
Written in scientific notation, 0.00000033 is ________.
a)
3.3 × 10⁷
b)
3.3 × 10-⁷
c)
3.3 × 10-⁸
d)
3.3 × 10⁸
e)
3.3
32.
General chemistry is the study of the composition, properties, and reactions of matter.
a)
True
b)
False
33.
The first step in using the scientific method is usually the observation of some natural event.
a)
True
b)
False
34.
A theory is confirmed after one experiment is performed.
a)
True
b)
False
35.
A hypothesis can be tested by performing a(n) ________.
a)
chemical
b)
chemistry
c)
experiment
d)
hypothesis
36.
The amount of space occupied by a substance is its ________.
a)
mass
b)
density
c)
weight
d)
length
e)
volume
37.
Significant figures are important because they indicate ________.
a)
a counted number
b)
the number of digits on a calculator
c)
the number of measurements
d)
the number of digits in a measurement
e)
the accuracy of the conversion factor
38.
The cubic centimeter (cm3 or cc) has the same volume as a ________.
a)
cubic inch
b)
cubic liter
c)
milliliter
d)
centimeter
e)
cubic decimeter
39.
An alloy of iron contains 75.0% iron and 25.0% other elements. How many grams of iron are present in 150. g of the alloy?
a)
37.5 g
b)
113 g
c)
11 300 g
d)
3750 g
e)
2.00 g
40.
A solution has a density of 1.22 g/mL. What volume of the solution has a mass of 48.2 g?
a)
0.00253 mL
b)
58.8 mL
c)
39.5 mL
d)
49.4 mL
e)
1.22 mL
41.
Water (density = 1.00 g/mL) will float on hexane (density = 0.95 mL).
a)
true
b)
False
42.
A pure substance is matter that consists of matter with a composition that ________.
a)
is fixed in a definite proportion at all times
b)
varies according to the amount of water present
c)
depends on the temperature
d)
always contains two or more substances
43.
Compounds are pure substances that by definition consist of ________.
a)
a single element
b)
oxygen and hydrogen
c)
two or more elements in combination
d)
solids
e)
gases
44.
Compounds can be broken down into their elements by ________.
a)
physical processes
b)
melting
c)
evaporation
d)
cooling
e)
chemical processes
45.
Which of the following is a compound?
a)
mercury (Hg) in a gauge
b)
salt (NaCl) in a shaker
c)
aluminum (Al) in a can
d)
gold (Au) in a ring
e)
titanium (Ti) in a golf club
46.
When sugar dissolves in water, this is an example of a ________.
a)
physical change
b)
chemical change
47.
Identify the chemical change in the following list.
a)
A shoelace breaks.
b)
A log burns in the fireplace.
c)
A cat meows.
d)
A crayon melts in the sun.
e)
Water falls from the sky as hail.
48.
The energy stored in the chemical bonds of a molecule is ________.
a)
specific heat
b)
kinetic energy
c)
potential energy
d)
work
49.
In which of the following would the particles move most rapidly?
a)
ice at -20 °C
b)
water at 20 °C
c)
steam at 110 °C
d)
boiling water
e)
ice at 0 °C
50.
The specific heat of a substance is the amount of heat needed to ________.
a)
change 1 g of the substance from the solid to the liquid state
b)
raise the temperature of 1 g of the substance by 1 °C
c)
change 1 g of the substance from the liquid to the solid state
d)
convert 1 g of a liquid to gas
e)
convert 1 g of a solid to a gas
51.
The number of joules needed to raise the temperature of 32 g of water from 12 °C to 54 °C is ________. The specific heat of water is 4.184 J/g °C.
a)
1300 J
b)
1.3 J
c)
5600 J
d)
1700 J
e)
130 J
52.
This substance has a definite shape and volume.
a)
gas
b)
solid
c)
liquid
53.
This substance has a definite volume but indefinite shape.
a)
gas
b)
solid
c)
liquid
54.
This substance completely fills its container.
a)
gas
b)
solid
c)
liquid
55.
Magnesium is an element that is one example of ________.
a)
a noble gas
b)
an alkaline earth metal
c)
a transition metal
d)
a metalloid
56.
Chromium is an example of an element that is a ________.
a)
a noble gas
b)
an alkali metal
c)
a transition metal
d)
a metalloid
57.
In an atom, the nucleus contains ________.
a)
an equal number of protons and electrons
b)
all the protons and neutrons
c)
all the protons and electrons
d)
only neutrons
e)
only protons
58.
Protons, neutrons, and electrons are examples of ________.
a)
elements
b)
ions
c)
compounds
d)
subatomic particles
e)
metals
59.
The Rutherford gold foil experiment demonstrated that atoms ________.
a)
consist of an almost empty nucleus surrounded by a dense cloud of electrons
b)
are homogeneous
c)
are visible to the naked eye
d)
consist of a dense nucleus surrounded by mostly empty space
e)
consist of a single type of subatomic particle
60.
The atomic number of an atom is equal to the number of ________.
a)
nuclei
b)
neutrons
c)
neutrons plus protons
d)
electrons plus protons
e)
protons
61.
The number of neutrons in an atom is equal to the ________.
a)
atomic number
b)
mass number
c)
mass number + the atomic number
d)
mass number - the atomic number
62.
An s orbital can hold ________ electrons.
a)
6
b)
10
c)
18
d)
2
e)
8
63.
The maximum number of electrons that may occupy the third electron energy level is ________.
a)
2
b)
8
c)
10
d)
18
e)
32
64.
What electron sublevel starts to fill after completion of the 5s sublevel?
a)
5p
b)
4d
c)
4p
d)
6s
e)
4f
65.
What element has the electron configuration 1s2,2s2,2p6,3s2,3p5?
a)
Be
b)
Cl
c)
F
d)
S
e)
Ar
66.
The atomic radius of bromine is larger than the atomic radius of ________.
a)
chlorine
b)
uranium
c)
potassium
d)
iodine
e)
xenon
67.
Valence electrons are electrons located ________.
a)
in the outermost energy level of an atom
b)
in the nucleus of an atom
c)
in the first energy level of an atom
d)
throughout the atom
e)
in the first three energy levels of an atom
68.
In an electron-dot structure of an element, the dots are used to represent ________.
a)
all of the electrons in the atom
b)
the valence electrons
c)
the complete electron arrangement
d)
only the electrons that will participate in bond formation
e)
the electrons that the element will gain when it forms a compound
69.
The ionization energy of rubidium is higher than the ionization energy for ________.
a)
lithium
b)
sodium
c)
potassium
d)
cesium
e)
fluorine
70.
One mol of particles of any substance contains how many particles?
a)
10^6
b)
3 × 10^-10
c)
3 × 10^10
d)
6.022 × 10^23
e)
6.022 × 10^-23
71.
How many atoms of chlorine are in 1.00 mol of chlorine gas(Cl2)?
a)
1.20 × 10^-24
b)
1.20 × 10^24
c)
6.02 × 10^23
d)
6.02 × 10^-23
e)
3.01 × 10^23
72.
Avogadro's number is the number of ________.
a)
particles in 1 mol of a substance
b)
amu in 1 mol of a substance
c)
grams in 1 mol of a substance
d)
moles in 6.022 × 10^23 grams of an element
e)
moles in 6.022 × 10^23 amu of an element
73.
1.00 mol of neon has a mass of ________.
a)
10.0 g
b)
14.0 g
c)
1.00 g
d)
20.2 g
e)
30.2 g
74.
What is the mass, in grams, of 6.11 mol of sulfur trioxide?
a)
80.1 g
b)
48.6 g
c)
391 g
d)
489 g
e)
801 g
75.
Find the mass of 3.00 mol of acetic acid, C2H4O2.
a)
44.1 g
b)
120. g
c)
180. g
d)
60.1 g
e)
132 g
76.
What is the % (by mass) of carbon in carbon dioxide, CO2?
a)
72.7%
b)
27.3%
c)
36.4%
d)
33.3%
e)
13.6%
77.
Calculate the empirical formula of a compound that has a composition of 5.9% (by mass) hydrogen and 94.1% (by mass) oxygen.
a)
HO2
b)
H2O
c)
HO
d)
H2O4
e)
H4O2
78.
The empirical formula of a compound is NO2, and its molar mass is about 92.g. What is its molecular formula?
a)
N2O
b)
N2O4
c)
N3O6
d)
N4O2
e)
N3O3
79.
A compound with an empirical formula of CH2O has a molar mass of 150. g. The molecular formula of this compound is ________.
a)
CH2O
b)
C2H4O2
c)
C3H6O3
d)
C4H8O4
e)
C5H10O5
80.
The mass of 1.00 mol of water is 18.0 g.
a)
True
b)
False
100 %
