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Semester 1 Review

Total questions: 100

Worksheet time: 5hrs 31mins

Name
Class
Date
1.

A researcher is searching for a way to produce hydrogen for fuel cells that requires less energy input.

a)

Analytical Chemistry

b)

Biochemistry

c)

Organic Chemistry

d)

Physical Chemistry

2.

A medical researcher is trying to determine how digestion enzyme performance responds to changes in pH in rats.

a)

Organic Chemistry

b)

Analytical Chemistry

c)

Biochemistry

d)

Inorganic Chemistry

3.

A researcher is studying rocks to try to find the best way to separate out valuable (non-carbon) elements.

a)

Inorganic Chemistry

b)

Analytical Chemistry

c)

Physical Chemistry

d)

Biochemistry

4.

A pool store manager tests a water sample a customer has brought in to determine the concentrations of key chemicals.

a)

Organic Chemistry

b)

Analytical Chemistry

c)

Biochemistry

d)

Inorganic Chemistry

5.
A balloon filled with carbon dioxide contains a
a)
Atom
b)
Element
c)
Mixture
d)
Compound
6.
A balloon filled with Helium (He) contains a
a)
Atom
b)
Element
c)
Mixture
d)
Compound
7.
The basic unit of matter is
a)
a mixture
b)
a substance
c)
an atom
d)
a compound
8.
Which of these is a mixture?
a)
Uncooked chocolate chips and cookie dough blended together with a spoon.
b)
Distilled water
c)
A nugget of gold
d)
A molecule of Oxygen
9.
Atoms of an element always have a certain number of
a)
neutrons
b)
protons
c)
electrons
d)
ions
10.
Convert 17 m to cm:
a)
0.17 cm
b)
0.017 cm
c)
1,700 cm
d)
170 cm
11.
98 dm = ________mm
a)
98
b)
0.98
c)
980
d)
9800
12.

How many micrometers (μm) are in 0.0000678 kilometers?

a)

.000000000000000678

b)

678,000

c)

67.8

d)

6,780

13.

5.00 gallons = ___ hL

a)

19.0

b)

.190

c)

1900

d)

1900000

14.

6.70 ft= ___Km

a)

2.19

b)

20400.

c)

21900.

d)

.00204

15.

A block has a mass of 54g and a volume of 20. cm3. What is the density of the block?

a)

74 g/cm3

b)

1080 g/cm3

c)

34 g/cm3

d)

2.7 g/cm3

16.
Percent yield of a product is a measure of the reaction's ___________.
a)
efficiency
b)
heat production
c)
rate
d)
spontaneity
17.
The ratio of actual yield to theoretical yield written as a percent is _______________.
a)
percent composition
b)
hydrate
c)
percent yield
d)
limiting reactant
18.
The number in front of a compound or element is a 
a)
Subscript
b)
Coefficient
c)
Superscript
d)
Charge
19.

How many oxygen atoms are in this chemical formula?

a)

6 oxygen atoms

b)

2 oxygen atoms

c)

3 oxygen atoms

d)

4 oxygen atoms

20.
What is the Law of Conservation of mass?
a)
Mass is created in a chemical reaction
b)
Mass is created in a physical change
c)
New chemicals formed from a chemical reaction have a larger overall mass than the original reactants
d)
Mass is never created or destroyed
21.

Whose model of the atom describes the atom as a tiny charged core called the nucleus?

a)

Niels Bohr

b)

Ernst Rutherford

c)

Bill Nye

d)

Werner Heisenberg

22.

Who proposed the billiard ball model for the atom?

a)

Milikan

b)

Rutherford

c)

John Dalton

d)

Bohr

23.

Which scientist conducted experiments using alpha particles and thin gold foil, which later helped him develop his model for the atom?

a)

Ernest Rutherford

b)

Kneels Bore

c)

Erwin Schrodinger

d)

JJ Thomson

24.
Which scientist discovered the electron, which helped him develop a model of the atom?
a)
Niels Bohr
b)
John Dalton
c)
Ernst Rutherford
d)
J.J Thompson
25.

______________ properties can be observed or measured without changing the identity of the matter.

a)

Chemical

b)

Metallic

c)

Physical

d)

Flammability

26.

Iodine (I2) crystals would be expected to be ______________ because it is a ___________________.

a)

shiny, metal

b)

shiny, nonmetal

c)

malleable, metal

d)

brittle, nonmetal

27.
Nickel would be expected to be ____________________ because it is a __________________.
a)
conductive, metal
b)
conductive, nonmetal
c)
nonconductive, metal
d)
nonconductive, nonmetal
28.
What atom matches this electron configuration?
1s22s22p63s23p64s23d10
a)
Zinc
b)
Copper
c)
Nickel
d)
Germanium
29.

What electron configuration matches an oxygen atom?

a)

1s22s22p63s23p64s23d104p5

b)

1s22s22p4

c)

1s22s22p6

d)

1s22s22p63s23p4

30.

Oxidation occurs at the

a)

anode

b)

cathode

31.

Electrons are gained at the

a)

anode

b)

cathode

32.
What is the atomic number?
a)
the number of protons
b)
the number of protons and neutrons
c)
the number of neutrons
d)
the number of protons and electrons
33.
What is the atomic number of this nucleus?
a)
1
b)
3
c)
4
d)
7
34.
What is the mass number of this nucleus?
a)
1
b)
3
c)
4
d)
7
35.
An element has the mass number 12 and atomic number  6. The number of neutrons in it is:
a)
6
b)
10
c)
4
d)
8
36.
A wave with a large wavelength will have a ______ frequency and _____ energy
a)
high, low
b)
high, high
c)
low, high
d)
low, low
37.
Which has the SHORTEST wavelength and, therefore, the highest frequency/most energy
a)
Radio waves
b)
Ultraviolet Rays
c)
Gamma Rays
d)
X-rays
38.
Ionic Bonding involves...
a)
The transfer of protons
b)
The transfer of nuetrons 
c)
The transfer of electrons
d)
None Of the above
39.
Covalent compounds
a)
Share electrons
b)
transfer electrons
c)
contain a sea of electrons
d)
conduct electricity
40.
What two types of atoms make a covalent bond?
a)
2 Nonmetals
b)
1 Nonmetal and 1 Metal
c)
2 Metals
d)
2 Noble Gases
41.
What happens when an atom loses an electron?
a)
Neutral (no charge)
b)
Positive charge
c)
Negative charge
42.
What elements generally make an ionic bond?
a)
metal and nonmetal
b)
2 or more nonmetals
c)
metal
d)
none of the above
43.
Predict the bond that will form between Se and Cl.
a)
Ionic
b)
Covalent
44.
Predict the bond that will form between Sr and S.
a)
Ionic
b)
Covalent
45.
Which group of the periodic table is composed of inert (not reactive)  gases?
a)
alkali metals
b)
alkaline earth metals
c)
halogens
d)
noble gases
46.
Nonmetals can mostly be found in which area of the Periodic Table?
a)
The bottom section
b)
Along the staircase
c)
To the left of the staircase
d)
To the right of the staircase
47.

The name of the group of elements that are found in nature in naturally occurring compounds.

a)

Noble gases

b)

Halogens

c)

Alkaline earth metals

d)

Alkali metals

e)

Transition metals

48.

Which group are the halogens in?

a)

18

b)

17

c)

16

d)

13

49.
The family in the periodic table that contains the most reactive metals is the_______
a)
Alkaline Earth Metals
b)
Transition Metals 
c)
Alkali Metals
d)
Other Metals
50.
In what section would Transition Metals be found?
a)
orange
b)
light blue
c)
blue
d)
white
51.
a)
17
b)
18
c)
7
d)
3
52.
a)
19
b)
20
c)
1
d)
4
53.
a)
7
b)
5
c)
2
d)
15
54.

How many orbitals are there in the "d" sublevel?

a)

1

b)

3

c)

5

d)

7

55.

How many orbitals are in a "p" sublevel?

a)

1

b)

3

c)

5

d)

7

56.

What is the abbreviated configuration for gold?

a)

[Rn] 6p6

b)

[Rn] 7s2

c)

[Xe] 6s2 4f14 5d9

d)

[Xe] 6s2 4f14 5d10

57.

Which rule is being broken this orbital diagram?

a)

Aufbau Principle

b)

Pauli Exclusion Principle

c)

Hund's Rule

d)

The diagram is correct.

58.
Electrons occupy orbitals of lowest energy first is part of what electron configuration rule?
a)
Hund’s Rule
b)
Aufbau Principle
c)
Pauli Exclusion Principle
59.
Who created the uncertainty principle?
a)
Heisenberg
b)
DeBrogile
c)
Dalton
d)
Bohr
60.
Who rearranged the periodic table by using the number of protons each element has? 
a)
Bohr
b)
Einstein
c)
Moseley
d)
DeBrogile
61.

_________________ describes mathematically the wave properties of electrons and other very small particles.

a)

Heisenberg uncertainty principle

b)

Quantum theory

c)

Aufbau principle

d)

Pauli exclusion principle

62.

The principal quantum number is related too the _________ of an orbital

a)

spin

b)

shape

c)

orientation

d)

size and energy

63.

The angular momentum quantum number is related to the _________ of atomic orbitals

a)

size

b)

shape

c)

spin

d)

orientation

64.

The value of _______ is related to the orientation of the orbital in space and relative to other orbitals in the atom

a)

principal quantum numbers

b)

angular momentum quantum number

c)

magnetic quantum number

d)

absolute quantum number

65.

Electron spin quantum numbers can only have one of two values:

a)

1 and -1

b)

3/4 and -3/4

c)

2/5 and -2/5

d)

+ 1/2 and - 1/2

66.
Electron cloud model
a)
Bohr
b)
Chadwick
c)
Schrodinger
d)
Rutherford
67.

Which has the greater electronegativity value:

Cl or Al?

a)

Cl

b)

Al

68.
Which of the following will have a larger radius than Zinc?
a)
Gallium
b)
Aluminum
c)
Magnesium
d)
Strontium
69.
Electronegativity is...
a)
how good an atom is at attracting electrons
b)
the ability of an atom to lose electrons
c)
the energy required to remove an electron from a specific atom
d)
how easy it is to make friends. 
70.
Choose the correct shape for this molecule:
a)
Trigonal planar
b)
Trigonal pyramidal
c)
Tetrahedral
d)
Linear
71.
Choose the correct shape for this molecule:
a)
Bent
b)
Trigonal pyramidal
c)
Trigonal planar
d)
Linear
72.

Will this molecule be polar or nonpolar? CCl4

a)

polar

b)

nonpolar

c)

soluble

d)

insoluble

73.

Will this molecule be polar or nonpolar? PH3

a)

polar

b)

nonpolar

c)

soluble

d)

insoluble

74.
A bond where electrons are NOT shared equally? 
a)
polar covalent
b)
nonpolar covalent
75.
What is the correct formula for the compound, lithium oxide?
a)
LiO
b)
Li2O
c)
LiO2
d)
Li2O2
76.
Name CCl4
a)
carbon carbon tetraiodide
b)
carbon tetrachloride
c)
monocarbon tetrachloride
d)
water
77.

What is the name of CuCl2?

a)

copper (II) chloride

b)

copper chloride

c)

cupric chloride

d)

copper (I) chloride

e)

cuprous chloride

78.
How would you say HBr? 
a)
hydrobromic acid
b)
hydrogen bromide
c)
monohydrogen bromide
d)
hydrogen (I) bromide
79.
What is the name of H2SO4?
a)
dihydrogen sulfur tetraoxide
b)
dihydrogen sulfate
c)
hydrosulfuric acid
d)
sulfuric acid
80.
How would you say Ni3P2?
a)
nickel (II) phosphide
b)
nickel phosphide
c)
trinickel diphosphide
d)
nickel phosphorous
81.
Write the name for Mn(CO3)2 
a)
manganese (IV) carbonate
b)
manganese (II) carbonide
c)
manganese dicarbonate
d)
manganese carbonate
82.
Is the equation balanced?: 2H2O + O2 --> 4MgO + 3Fe
a)
Yes
b)
No
83.
Balance this equation
_Al +_HCl --> _H2 +_AlCl3
a)
2, 6, 3, 2
b)
it is already balanced
c)
4, 12, 3, 4
d)
2, 1, 4, 5
84.
Balance this equation-
_SeCl6+_O2>_SeO2+_Cl2
a)
1,2,1,2
b)
1,1,1,3
c)
1,2,1,1
d)
2,1,1,1
85.
Which of the following does NOT form a precipitate?
a)
AgNO3(aq) + 2KBr(aq) →
b)
LiNO3 (aq) + NaC2H3O2(aq) →
c)
Ca(NO3)2(aq) + K2CO3(aq) →
d)
 Ba(NO3)2 (aq) + Na2SO4(aq) →
86.
In a neutralization reaction, what are the products of a reaction between an acid and a base?
a)
another acid and base
b)
carbon dioxide and a salt
c)
water and a salt
d)
either two acids or two bases
87.
What precipitate forms when you mix barium nitrate with sodium sulfate?
a)
sodium nitrate 
b)
barium nitrate
c)
barium sulfate
d)
sodium sulfate
88.
If a pair of atoms that are covalently bonded have _____ electonegativity, then the electrons in the bond will be equally shared.  
a)
neither 
b)
different 
c)
the same
d)
similar
89.

What is the intermolecular force between two water molecules?

a)

Ion-Ion

b)

Hydrogen Bonds

c)

Ion-Dipole

d)

London Dispersion

90.

4Si + S8 --> 2Si2S4


What type of reaction is this?

a)

Synthesis

b)

Decomposition

c)

Single displacement

d)

Double displacement

91.
Fe + H2SO4 --> Fe2(SO4)3 + H2
a)
Synthesis (combination)
b)
Decomposition
c)
Single replacement
d)
Combustion
92.
The reaction below is an example of?
AgNO3 + NaCl → AgCl + NaNO3
a)
Single Replacement
b)
Double Replacement
c)
Decomposition
d)
Combustion
93.
What type of reaction is illustrated below?
2HI --> H2  +  I2
a)
synthesis
b)
decomposition
c)
single replacement
d)
double replacement
94.

Which of the following reactions involves the ions of two compounds exchanging places to form two new compounds?

a)

Synthesis

b)

Double replacement

c)

Combustion

d)

Single Displacement

95.
What type of reaction is C3H8 + 5O2 => 3CO2 + 4H2O?
a)
combination
b)
decomposition
c)
combustion
d)
both combination and decomposition
96.

substance that speeds up a chemical reaction but is not used up itself or permanently changed.

a)

enzyme

b)

catalyst

c)

activation energy

d)

chemical reaction

97.

What is the mass of 5.76 moles of sodium phosphate?

a)

164 g

b)

945 g

c)

984 g

d)

820 g

98.

How many moles are 98.3 grams of aluminum hydroxide?

a)

1.26 moles

b)

0.8 moles

c)

7,673.4 moles

d)

150 moles

99.

What percent of zinc phosphate is zinc?

a)

33.15%

b)

16.04%

c)

50.81%

d)

19.68%

100.

Find the percent composition of each element in dinitrogen disulfide.

a)

69.6% N, 30.4%S

b)

15.2% N, 84.8% S

c)

30.4% N, 69.6% S

d)

65.2% N, 34.8% S

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