Semester I Review
Students are using heat, chemicals and
glassware in a laboratory experiment.
Which of these is the best method of
eye protection?
 A. safety goggles
 B. contact lenses
 C. prescription eye glasses
 D. eye protection is not needed
Where should a student discard solid
chemical
waste?
 A. sink
 B. trash can
 C. disposable box
 D. container identified by the chemistry
teacher
What should be used to put out a
fire in
person’s hair or clothing?
 A. your hands
 B. a fire blanket
 C. a fire extinguisher
 D. water from the sink faucet
Eating in the laboratory
 A. is not permitted.
 B. is permitted if it was purchased in the
cafeteria.
 C. is permitted if the lab experiment
does
not involve chemicals.
 D. is permitted as soon as the lab
experiment is finished.
Safety goggles and a lab apron must be
worn when handling chemicals labeled
corrosive because they
 A. may stain clothes
 B. react with the skin
 C. are difficult to pour
 D. are highly flammable
This hazardous materials symbol indicates that the
chemicals stored in that container are highly
reactive.
Which of the following procedures should be taken
when dealing with the chemical?
 A. Always use safety goggles when
working with this chemical.
 B. Always leave the container sealed,
never open it.
 C. Always keep water nearby in case of spills.
 D. Always keep this chemical away from open
flame.
This hazardous materials symbol indicates that
the chemical in the container with this symbol
 A. is flammable and combustible.
 B. is poisonous and infectious.
 C. is biohazardous and can produce body
infections.
 D. is highly corrosive and able to burn organic
material.
Which of the following is NOT
considered a type of matter?
 A. rock
 B. light
 C. air
 D. steam
Which of the following is NOT considered a
chemical property of matter?
 A. reactivity
 B. pH
 C. solubility
 D. heat of combustion
Which two features are used to describe
matter?
 A. mass and speed of particles
 B. weight and color of particles
 C. weight and volume
 D. mass and volume
Which of the following is NOT a
physical property of matter?
 A. viscosity
 B. reactivity
 C. texture
 D. density
Which state of matter is most resistant
to compression?
 A. solid state
 B. gaseous state
 C. liquid state
 D. plasma state
Definite shape and definite volume
describe which state of matter?
 A. liquid state
 B. solid state
 C. plasma state
 D. gaseous state
Material that has neither a definite
shape nor a definite volume is in
which state of matter?
 A. gaseous state
 B. liquid state
 C. plasma state
 D. solid state
Which of the following is NOT a method
of separating a mixture?
 A. filtration
 B. evaporation
 C. melting
 D. chromatography
Which of the following methods
involves heating or boiling a mixture
to recover the solid elements?
 A. evaporation
 B. distillation
 C. chromatography
 D. filtration
An increase in which of the following
would increase the boiling point of a
liquid?
 A. volume
 B. the mass of the liquid
 C. pressure
 D. temperature
Which of the following is correct
statement regarding mixtures?
 A. mixtures are composed of a single
substance
 B. mixtures are composed of more than
one substance
 C. mixtures have a fixed composition
 D. all substances in a mixture are visible
at all times
Solid sodium chloride has a crystal structure.
Which of the following best explains why some
solids can form crystals?
 A. Particles experience strong intermolecular
forces, causing them to be held in very orderly
positions.
 B. Particles spread out and mix with each other,
even if they are not stirred, making crystal
formation more likely.
 C. Particles experience strong intermolecular
forces, but can still move about freely and are
not bound to fixed positions.
 D. Particles are very closed together and,
therefore, barely compress at all, making them
predisposed to form crystals
Breakfast Cereal A costs $4.99 for 793 g,
Cereal B costs $3.79 for 400 g, Cereal C
costs $4.19 for 1.19 kg, and Cereal D
costs $3.99 for 567 g. Which cereal has
the lowest price per gram?
 A. Cereal A
 B. Cereal B
 C. Cereal C
 D. Cereal D
A student measures the mass of an object
as 32.4g. The actual mass of the object is
31.8 g. What is the percent error of the
student's measurement?
 A. 0.060%
 B. 1.01%
 C. 1.85 %
 D. 60.0%
If you wanted to separate a mixture of
isopropyl alcohol and water, what
example below would help you select
the technique you should use?
 A. The boiling point is 82ºC.
 B. The mixture is clear.
 C. The water was tap water.
 D. 8 oz of alcohol was added to 8 oz of
water.
A student is trying to identify an unknown
white crystalline solid made of small grains.
The student believes these are sugar
crystals. How should the student test this
hypothesis?
 A. Identify the particle pattern in the crystal
 B. See if the crystals will dissolve in water
 C. Find the crystal's melting point
 D. Use a ruler and balance to measure the
crystals
Which of the following statements is
most accurate regarding atoms?
 A. Most atoms cannot combine with
other atoms.
 B. Chemical reactions divide atoms into
smaller units.
 C. Atoms of the same element may have
different mass numbers.
 D. Atoms only contain protons.

The cathode ray experiments lead to which
particle being discovered?
 A. nucleus
 B. proton
 C. neutron
 D. electron
The proton, in Rutherford’s experiments, were
used to —
 A. identify chemical properties
 B. identify the melting point
 C. determine molecular mass
 D. bombard sheets of gold
Which nuclear particle has the same relative
mass as the proton, but has no electrical charge?
 A. electron
 B. neutron
 C. isotope
 D. quark
Why is an atom considered electrically neutral?
 A. neutrons equal the number of protons
 B. proton forces pull on the neutrons
 C. electrons equal the number of protons
 D. electrons equal the number of neutrons
Which of the following statements describes
isotopes of an atom?
 A. different chemical properties
 B. different numbers of protons
 C. different masses
 D. different numbers of electrons
What happens to the number of electrons in an
atom as the atomic number on the periodic
table increases?
 A. increases
 B. decreases
 C. remains the same
 D. depends on the atom
Which of the following is used to calculate the
average atomic mass of an element?
 A. the naturally occurring isotopes
 B. the five most abundant isotopes
 C. the isotopes that are man made
 D. the least most common isotopes
What is the mass number of a carbon isotope
that consists of 6 protons, 6 electrons, and 8
neutrons?
 A. 13
 B. 14
 C. 20
 D. 28
Which of the following showed electrons in
specific, fixed orbits?
 A. Rutherford Model
 B. Planck Model
 C. Bohr Model
 D. Quantum Model
Which orbitals are dumbbell-shaped and are
arranged along the x, y, and z axes?
 A. s orbitals
 B. d orbitals
 C. p orbitals
 D. f orbitals
Which of the following orbitals contains
quantum number combinations that are NOT
possible?
 A. 4d
 B. 3s
 C. 4p
 D. 3f
How many electrons are required to completely
fill the 3rd energy level?
 A. 0
 B. 8
 C. 18
 D. 32
An electron must occupy the lowest available
energy orbital is stated by —
 A. the Aufbrau Principle
 B. Hund's Rule
 C. the Pauli Exclusion Principle
 D. Bohr's Law
What is the electron configuration for manganese,
atomic number 25?
 A. 1s2 2s2 2p6 3s2 3p6 4s2 3d5
 B. 1s2 2s2 2p6 3s2 3p6 4s2 3d10
 C. 1s2 2s2 2p6 3s2 3p6 4s2
 D. 1s2 2s2 2p6 3s2 3p6
The properties of elements, according to
periodic law, can be predicted by —
 A. the number of isotopes
 B. the solubility of the element
 C. the position on the periodic table
 D. the color of the element
Which family correctly labels the elements in
Group 1 on the periodic table?
 A. transition metals
 B. alkali series
 C. lanthanide elements
 D. actinide series
As the atomic number increases, within a
group of elements, the atomic radius usually —
 A. decreases
 B. remains the same as the one above it
 C. increases
 D. decreases, then increases
What happens to the ionization energy of an
element as electrons are removed?
 A. increases
 B. decreases
 C. remains constant
 D. decreases, then increases
Which of the following best explains why Mendeleev's
periodic table was organized according to atomic
mass rather than atomic number?
 A. Atomic number had not yet been
 discovered.
 B. Atomic mass is unaffected by
 chemical reactions.
 C. Atomic number is more closely related
 to reactivity.
 D. Atomic mass varies among the
 isotopes of an element.
Which of the following groups, with a few
exceptions, has the d-orbitals unfilled?
 A. transition metals
 B. nonmetals
 C. gases
 D. metalloids
Which of the following describes the properties
of noble gases?
 A. They have high boiling points.
 B. They are highly reactive.
 C. They are generally unreactive.
 D. They are solid at room temperature.
The number of valence electrons in Group 2
elements is —
 A. 0
 B. 1
 C. 2
 D. 3
Which of the following are involved in forming
a chemical bond?
 A. electrons and protons
 B. protons and neutrons
 C. neutrons and electrons
 D. dipoles and electrons
What happens to the potential energy of atoms
when they form a chemical bond?
 A. increase their potential energy
 B. decrease their potential energy
 C. their potential energy remains the same
 D. their potential energy fluctuates over time
When 2 atoms share a pair of electrons, which
type of bond is formed?
 A. ionic
 B. sublevel
 C. static
 D. covalent
The unequal attraction for the electrons in a
chemical bond is called —
 A. nonpolar
 B. polar
 C. triplanar
 D. ionic
Which of the following increases as the
electronegativity difference between 2 atoms
increases?
 A. ionic nature of the bond
 B. covalent nature of the bond
 C. metallic nature of the bond
 D. electron sharing between the 2 atoms
Which of the the 2 outermost orbitals must be
filled to satisfy the octet rule?
 A. d and f orbitals
 B. d and p orbitals
 C. s and d orbitals
 D. s and p orbitals
Which of the following is used to draw a Lewis
structure of either a molecule or atom?
 A. bond length between 2 atoms
 B. electronegativity of an atom
 C. number of valence electrons
 D. atomic mass or masses
How many double bonds are in the Lewis
structure for carbon dioxide, CO2?
 A. none
 B. one
 C. two
 D. three

O C O
for carbon to have 8
valence electrons it will have to have two
pairs on each side sharing with oxygen
Which of the following is a property of a
molecular compound?
 A. low boiling point
 B. tend to be brittle
 C. conducts electricity well when
 dissolved
 D. hardness
The attraction between positive ions and
surrounding mobile electrons forms which type
of bond?
 A. polar covalent bond
 B. nonpolar covalent bond
 C. ionic bond
 D. metallic bond
What happens to electron pairs, according to
VSEPR, when a molecule is formed?
 A. Electron pairs form negative ions.
 B. Electron pairs form positive ions.
 C. Electron pairs cause molecules to attract
each other to form electrostatic positions.
 D. Electrons pairs move away from each other
to electrostatic balanced positions.
According to the VSEPR theory, which shape
represents a carbon tetrafluoride molecule, CF4?
 A. tetrahedral
 B. trigonal planar
 C. bent
 D. linear
Which of the following has the greatest affect
on the strength of London dispersion forces
between molecules?
 A. the number of electrons
 B. the number of protons and neutrons in
 the molecule
 C. the number of electrons and the number of
neutrons in the molecule
 D. the number of electrons in the molecule
and the mass of the molecule
Which statement is true regarding the strength
of molecular bonds compared to the strength
of intermolecular forces?
 A. Molecular bonds tend to be weaker.
 B. Molecular bonds tend to be stronger.
 C. Intermolecular bonds tend to be stronger.
 D. The bond strengths are about the same.
Oxygen forms covalent bonds with carbon and
sulfur, but forms ionic bonds with sodium and
magnesium. What is the best inference for this
difference in how oxygen behaves?
 A. Oxygen bonds randomly with elements in
unpredictable ways.
 B. The difference in atomic radii between the
groups accounts for the difference in behavior.
 C. Oxygen only bonds with elements that have a
smaller atomic mass.
 D. Electronegativity differences between the
bonding elements allow electrons to be either
shared or donated.
Assuming an element has 8 electrons in the
valence shell, what conclusions can be drawn
regarding the type of bonding behavior?
A. The element will form polar covalent bonds.
B. The element will form non-polar covalent
bonds.
C. The element will form ionic bonds.
D. The element will form no bonds.
Which statement is true comparing the research
of Bohr, Rutherford, and Dalton?
 A. Dalton and Bohr modeled their experiments
and their theories after Rutherford.
 B. Rutherford and Bohr modeled their
experiments and their theories after Dalton.
 C. Dalton and Rutherford modeled their
experiments and their theories after Bohr.
 D. All three scientists developed their theories at
the same time.
How many atoms of carbon are present in a
molecule of carbon tetrachloride, CCl4?
 A. 1
 B. 2
 C. 4
 D. 5
Changing the subscript on an element within a
correctly written chemical formula —
 A. changes the charges of all the other ions in
the compound
 B. changes the number of ions represented by
the formula
 C. changes the oxidation number of each
element in the formula
 D. changes the formula so that it no longer
represents that compound
What is the formula for potassium fluoride?
 A. KF
 B. KF2
 C. K2F
 D. K2F2
What is the formula for the compound formed
by iron (II) ions and chromate ions?
 A. FeCrO4
 B. Fe2CrO4
 C. Fe2(CrO4)3
 D. Fe(CrO4)2
What is the formula for aluminum hydroxide?
 A. AlOH
 B. Al(OH)3
 C. Al2(OH)3
 D. Al3OH
What is the formula for tin (IV) oxide?
 A. Tn4O2
 B. SnO
 C. TnO2
 D. SnO2
What is the formula for barium nitrate?
 A. Ba(NO3)2
 B. BaNO2
 C. Ba2NO3
 D. Ba(NO4)2
What is the name of the compound NiSO4 ?
 A. nickel (II) sulfite
 B. nickel (II) sulfide
 C. nickel (II) sulfate
 D. nickel (II) sulfuroxide
What is the name of the compound AlPO4?
 A. aluminum phosphide
 B. aluminum phosphate
 C. aluminum phosphite
 D. aluminum phosphoroxide
Which of the following is the metallic ion in
scandium (II) chloride?
 A. Sd 2+
 B. Cl 2 C. Sc 2+
 D. Cl 1-
What is the name of the compound N2O3?
 A. sodium dioxide
 B. dinitrogen oxide
 C. nitrous oxide
 D. dinitrogen trioxide
What is the formula for sulfur trioxide?
 A. SO
 B. SO2
 C. SO3
 D. SrO3
What is the oxidation number of nitrogen in
most compounds?
 A. -3
 B. -2
 C. -1
 D. +1
What is the oxidation number of hydrogen in
HCl?
 A. 0
 B. +1
 C. +2
 D. +3
Which law states that "when two or more
compounds are composed of the same two
elements, the ratio of the masses of one
element that combine with a fixed mass of the
other element is a simple whole number"?
 A. Conservation of Mass
 B. Atomic Law
 C. Multiple Proportions
 D. Definite Composition
Which of the following is a possible compound
formed from Calcium (2+) and the polyatomic
ion Nitrate, NO3 (1-)?
 A. Ca2NO3
 B. Ca3NO2
 C. CaNO
 D. Ca(NO3)2
How many grams of NaCl are present in 11.00
moles?
 A. 0.45 g
 B. 156.60 g
 C. 331.00 g
 D. 642.93 g

11.0 moles x 58.5g/mole =
How many Mg 2+ ions are present in
3.00 moles of MgCl2?
 A. 1.806 x 1024
 B. 3.02 x 1024
 C. 12.00 x 1025
 D. 16.00 x 1023

3.00 moles x 6.02 x 1023 molecules/mole x 1Mg/molecule
Which of the following is the scientific name
for NH3 ?
 A. Water
 B. Ammonia
 C. Nitric acid
 D. Methane
What is the formula mass of MgSO4?
 A. 116.13 amu
 B. 272.83 amu
 C. 111.21 amu
 D. 120.36 amu

Mg = 1 x 24.31= 24.31
S = 1 x 32.06 = 32.06
O = 4 x 15.999= 63.99
The mass of one _________ is the molar mass of
the element.
 A. mole of the element
 B. picogram of the element
 C. milliliter of the element
 D. representative particle of the element
The sum of the atomic masses of all the atoms
in a formula for a compound is the—
 A. real mass
 B. formula mass
 C. Avogadro mass
 D. molecule mass
What is the formula mass of sodium chloride,
NaCl?
 A. 53.023 amu
 B. 58.439 amu
 C. 102.771 amu
 D. 112.539 amu
Na = 1 x 22.99 amu
Cl = 1 x 35.45 amu
What is the formula mass of glucose,
C6H12O6?
 A. 58.347 amu
 B. 137.490 amu
 C. 180.017 amu
 D. 231.369 amu
Describe the process of calculating the molar
mass of Li2S.
 A. Add the masses of 1 mole of lithium and 2
moles of sulfur.
 B. Add the masses of 1 mole of lithium and 1
mole of sulfur.
 C. Add the masses of 2 moles of lithium and
1 mole of sulfur.
 D. Add the masses of 2 moles of lithium and
2 moles of sulfur.
How many moles of CO2 are present in 200.00 g?
 A. .22 mol
 B. 4.54 mol
 C. 9.08 mol
 D. 88.02 mol
200g CO2 x 1 mole CO2/44g CO2
Calculate the number of representative particles
that are present in .20 moles of H2O without
regards to significant figures.
 A. 3.612x 1023 atoms
 B. 1.204 x 1024 atoms
 C. 2.408 x 1024 atoms
 D. 2.944 x 1025 atoms
.20 moles x 6.02 x 1023 H20/1mole x 3rp/1H20
You are performing an experiment to determine
whether the "S" on Skittles dissolves faster in
cold water, warm water or hot water. In 9 out
10 trials the data indicates that the "S" dissolves
faster in hot water. "S“ dissolves in warm water
faster than hot water. What should you do?
 A. Report this data
 B. Throw out this data
 C. Redo the experiment
 D. Change your hypothesis
If the average mass of a one pound bag of
Skittles is 453.6 g and there are 927 Skittles in
a bag, determine which best represents the
mass of one Skittle.
 A. 489.3 mg
 B. 4893 mg
 C. 2.044 g
 D. 204.4 mg
Which of the following is the mass in grams of
4.25 × 10³ mol of N2
 A. 2.35 × 10-4 g
 B. 1.52 × 102 g
 C. 5.95 × 104 g
 D. 1.19 × 105 g
(4.25 × 10³ mol of N2) x (28.012g/ 1 mol N2)
After the correct formula for a reactant in an
equation has been written, the —
 A. chemical formula cannot be altered
 B. subscripts of the formula are changed to
balance the equation
 C. chemical symbols in the formula must
appear only on the reactant side
 D. same chemical formula must be written on
the product side of the equation
Which of the following reactions involves two
or more substances combining to form a new
compound?
 A. single-replacement reaction
 B. synthesis reaction
 C. combustion reaction
 D. double-replacement reaction
Which of the following reactions involves one
element replacing an element in a compound
that is from the same activity series?
 A. combustion reaction
 B. decomposition reaction
 C. single-replacement reaction
 D. double-replacement reaction
Which of the following reactions involves a
single compound producing two or more
simpler substances?
 A. synthesis reaction
 B. decomposition reaction
 C. combustion reaction
 D. double-replacement reaction
Which of the following reactions involves the
ions of two compounds exchanging places to
form two new compounds?
 A. synthesis reaction
 B. single-replacement reaction
 C. double-replacement reaction
 D. combustion reaction
By predicting the outcome of the following
reactants mixing together in an aqueous
solution, what type of reaction will take place?
 Pb(NO3)2 (aq) + 2 KI (aq) -->
 A. double-replacement reaction
 B. synthesis reaction
 C. decomposition reaction
 D. single-replacement reaction
When an acid, such as carbonic acid, decomposes,
the products are —
 A. non-metal oxides and a salt
 B. non-metal oxides and water
 C. metal oxides and oxygen
 D. metal oxides and peroxide
Predict the products of the following reaction:
Na2O + CO2 -->
 A. Na2CO3
 B. Na + CO3
 C. NaCO2 + O2
 D. NaC + O3

Typically a synthesis reaction will occur that
is balanced
What are the advantages of using an activity
series in predicting the outcome of chemical
reactions?
 A. The freezing point of the elements can be
determined.
 B. Reactions can be categorized as either
exothermic or endothermic.
 C. The ionization energy can be calculated for
each element in the reaction.
 D. The reaction can be categorized as possible
or not possible.
Predict the outcome of the reaction where zinc
metal is added to a solution of potassium
chloride.
 A. No reaction occurs.
 B. Gaseous zinc is formed.
 C. Potassium calcide forms.
 D. Zinc chloride forms.

Zinc is below Potassium on the reactivity
series chart
Predict the outcome of the reaction where a
solution of silver nitrate is added to a solution
of sodium chloride.
 A. No reaction occurs
 B. Silver chloride forms
 C. Nitric acid is produced
 D. Calcium chloride is formed
In the solubility chart silver is insoluble in chlorine
so a precipitate will form. Nitrate is soluble with
sodium
According to the Law of Conservation of
Matter, the total mass of all the reacting
Substance is —
 A. more than the mass of all the products
 B. more than the total mass of all the
products and the reactants
 C. less than the total mass of all the products
 D. equal to the mass of all the products
What are the coefficients that would correctly
balance this reaction?
____Ni + ____C4H8N2O2 --> ____Ni(C4H8N2O2)2
 A. 1, 2, 1
 B. 2, 2, 1
 C. 2, 1, 1
 D. 2, 2, 2
What are the coefficients that would correctly
balance this equation?
____Zn + ____K2CrO4 -->____K + ____ZnCrO4
 A. 2, 1, 2, 1
 B. 1, 2, 3, 1
 C. 1, 2, 1, 2
 D. 1, 1, 2, 1
What is the balanced equation for the
combustion of magnesium?
 A. Mg (s) + O2 (g) --> MgO (g)
 B. Mg (s) + O2 (g) --> MgO2 (g)
 C. 2 Mg (s) + O2 (g) --> 2 MgO (s)
 D. Mg (s) + 2 O2 (g) --> MgO4
First the product must be balanced = MgO
Lavoisier used a variety of experiments to draw
conclusions regarding the chemical reactivity
of a number of elements. Critique the
following statements and select the
statement that was determined later to be
false.
 A. Water is formed from a reaction of
hydrogen (what he called phlogiston) and
oxygen.
 B. Sulfur, when burned, combines with air to
form new substances.
 C. Oxygen makes some substances acidic.
 D. The weight gained by the products of a
burning reaction came from the air.
The safest way to dilute concentrated
hydrochloric acid is to add  A. a series of small volumes of water to the
acid while stirring slowly
 B. the acid to water slowly while stirring
constantly
 C. the acid to a small volume of water and
then add more water
 D. dilute hydrochloric acid to a small volume
of the concentrated acid