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Semester 1 Exam Review

Total questions: 136

Worksheet time: 6hrs 35mins

Name
Class
Date
1.
This variable in an experiment is the one being deliberately changed by the scientist. 
a)
dependent variable
b)
independent variable
c)
data
d)
control group
2.
A student wants to test the effects of type of exercise on heart rate.  What is the dependent variable?
a)
heart rate
b)
type of exercise
c)
amount of exercise
d)
time of day exercise occurs
3.
The dependent variable in an experiment is what you ________________. 
a)
Change
b)
Measure
4.
Theory or Law???  Explanation of a wide range of observations?
a)
Theory
b)
Law
5.
Theory or Law???  Changes with new observations.
a)
Theory
b)
Law
6.
Theory or Law???  Is a DESCRIPTION of what a scientists expects to happen every time under a certain set of conditions.
a)
Law
b)
Theory
7.
What is the dependent variable in the following experiment? Plants grow more when exposed to classical music
a)
Exposure to classical music
b)
Normal exposure to noises with no music
c)
height of plant
8.
What is the independent variable in the following experiment? Plants grow more when exposed to classical music
a)
Exposure to classical music
b)
height of plant
c)
Normal exposure to noises with no music
9.
What are the states of matter?
a)
solid, liquid, and juice
b)
solid and liquid
c)
solid and gas
d)
solid, liquid, and gas
10.
An example of a physical property is 
a)
flammability
b)
acidic
c)
color
d)
ability to rust
11.
Changing the way matter looks without changing it into NEW matter is a:
a)
Chemical change
b)
Physical change
c)
Energy change
d)
BOTH a chemical and a physical change
12.
Water freezing to ice is an example of a:
a)
Physical change
b)
Chemical change
13.
Burning wood to ash is an example of a:
a)
Physical change
b)
Chemical change
14.
Smashing a piece of candy into smaller pieces is an example of a:
a)
Physical change
b)
Chemical change
15.

A __________________ does not have a definite shape. It sometimes takes the shape of its container and sometimes moves freely wherever it can. These molecules are not connected to each other and take up whatever space is available.

a)

gas

b)

solid

c)

liquid

d)

matter

16.

A _________________ does not have a definite shape. It takes the shape of the container it is in. It does have a definite volume and mass.

a)

gas

b)

solid

c)

ooblek

d)

liquid

17.

240 cm = ___________ m

a)

2400

b)

24

c)

2.4

d)

0.24

18.

2,804 mg = ___________ g

a)

0.2804

b)

2.804

c)

28.04

d)

280.4

19.

3 km = ___________ mm

a)

30

b)

300

c)

3,000

d)

3,000,000

20.

68 cm = ___________ mm

a)

0.68

b)

6.8

c)

68

d)

680

21.

330 cm = ___________ m

a)

3,300

b)

33

c)

3.3

d)

0.33

22.

183 cm = ___________ m

a)

0.183

b)

1.83

c)

18.3

d)

1,830

23.
How many minutes are in a year?
a)
31,536,000 min
b)
525,600min
c)
52,560min
24.
How many inches are in 1 mile?
(Hint:  5280 ft = 1 mi)
a)
66,330 in
b)
63,360 in
c)
63,660 in
d)
63,066 in
25.

Convert 62 miles/hour to feet/second

a)

5,456 feet/second

b)

.003 feet/second

c)

90.9 feet/second

d)

909 feet/second

26.

A bicycle has a speed of 6.00 m/s. What is its speed in km/h?

a)

21.6 km/h

b)

16.67 km/h

c)

2.16 km/h

d)

1.67 km/h

27.
The density of lead is 11.342 g/mL.  What would be the volume of a 200.0 g sample of this metal?
a)
0.05671 g
b)
17.63 g
c)
2268 g
d)
Not enough information
28.
What is the mass of a 350 cm3 sample of pure silicon with a density of 2.336 g/cm3?
a)
820 g
b)
0.0067 g
c)
150 g
29.
What is the formula for density?
a)
density = mass x volume
b)
density = mass / volume
c)
density = mass + volume
d)
density = mass - volume
30.
Find the density of a 2 cm x 2 cm x 2 cm cube with a mass of 64 g.
a)
6 cm3
b)
12 g/cm3
c)
128 g/cm3
d)
8  g/cm3
31.

Subatomic particles with a negative charge

a)

Electrons

b)

Neutrons

c)

Protons

d)

Quarks

32.
subatomic particles found on the outermost shell & responsible for the atom's reactivity
a)
neutrons
b)
valence electrons
c)
isotopes
d)
ions
33.
Subatomic particles with a positive charge
a)
neutrons
b)
atomic mass
c)
protons
d)
isotopes
34.
Value representing the number of protons in an element
a)
Atomic Mass
b)
Mass Number
c)
Valence Electrons
d)
Atomic Number
35.
Atoms of the same element with a different number of neutrons
a)
Ion
b)
Gluons
c)
Isotope
d)
Quarks
36.
A charged atom
a)
Ion
b)
Isotope
c)
Electron Cloud
d)
Quark
37.
The smallest particle of an element that shows all the properties of that element.
a)
Subatomic Particles
b)
Atom
c)
Quarks
d)
Gluons
38.
A tiny but very dense, positively charged portion of the atom that holds most of the atomic mass
a)
Electron Shells
b)
Orbitals
c)
Electron Cloud
d)
Nucleus
39.
Discovered the electron within the atom
a)
Thomson
b)
Chadwick 
c)
Schrodinger & Heisenberg
d)
Dalton
40.
Rutherford's gold foil experiment provided evidence that...
a)
negative and positive charges are spread evenly throughout the atom.
b)
alpha particles have a positive charge.
c)
gold is not a dense as previously thought.
d)
there is a dense positively charged nucleus at the center of an atom.
41.
Who discovered the nucleus using the gold foil experiment?
a)
Democritus
b)
Robert Millikan
c)
James Chadwick
d)
Ernest Rutherford
42.
The first person to propose a theory about an atom called the Atomos Theory was
a)
Democritus
b)
Rutherford
c)
Dalton
d)
Aristotle
43.
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
44.
What is the mass number defined as?
a)
the number of protons
b)
the number of protons and neutrons
c)
the number of neutrons
d)
the number of protons and electrons
45.
What is the atomic number of this atom?
a)
1
b)
3
c)
4
d)
7
46.

How many protons are in a sodium atom, Na? (tap to enlarge the periodic table)

a)

Sodium has 1 proton.

b)

Sodium has 3 protons.

c)

Sodium has 11 protons

47.

Which subatomic particle has a negative charge in the atom?

a)

proton

b)

neutron

c)

electron

d)

quark

48.

How many neutrons does C-14 [atomic #6] contain? (tap to enlarge the image)

a)

6

b)

7

c)

14

d)

8

49.

If an atom has 10 electrons, how many protons does it have?

a)

0

b)

1

c)

10

d)

5

50.
What does the 1.00794 stand for?
a)
Hydrogen
b)
atomic number
c)
atomic mass
d)
atomic explosion
51.

Calculate the average atomic mass of the element iron (Fe) using the following data:

[Isotope / % abundance]

[Iron 54 / 6% ] [Iron 56 / 92% ] [ Iron 57 / 2% ]

a)

53.7 amu

b)

54.9 amu

c)

5592.0 amu

d)

55.9 amu

52.
How many neutrons does the isotope of lithium have?
a)
8
b)
3
c)
4
d)
5
53.
How many protons does this isotope of titanium have?
a)
48
b)
22
c)
26
d)
70
54.

How many electrons can there be in one orbital?

a)

2

b)

4

c)

6

d)

10

55.

Which element has 2 valence electrons?

a)

beryllium

b)

helium

c)

sodium

d)

boron

e)

silicon

56.

Which of the following elements has a full outer energy level of electrons?

a)

krypton

b)

strontium

c)

iodine

d)

sodium

57.

Which of the following elements has 5 valence electrons?

a)

boron

b)

phosphorus

c)

magnesium

d)

chlorine

58.
What is this element?
1s22s22p63s2
a)
Neon
b)
Magnesium
c)
Aluminum
d)
Potassium
59.
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
60.
What is the electron configuration for Bromine (Br)
a)
1s2, 2s2, 2p6, 3s2, 3p6, 4s2, 3d1
b)
1s2, 2s2, 2p4
c)
1s2, 2s2, 2p6, 3s2, 3p6, 4s2, 3d10, 4p5
d)
1s2, 2s2, 2p6
61.
How many electrons can the first energy level hold?
a)
1
b)
2
c)
8
d)
0
62.
What is the noble gas shorthand electron for Sulfur atom?
a)
[Ar] 3p4
b)
[He] 3s23p4
c)
[Ne] 3s23p4
d)
[Na] 3s23p4
63.
Electrons filling orbitals with more than one sublevel will be equally distributed to each sublevel before any of the sublevels receives a 2nd electron is known as what rule?
a)
Aufbau Principle
b)
Pauli Exclusion Principle
c)
Hund's Rule
64.
Orbitals can hold a maximum of two electrons each with opposite spins is which rule?
a)
Aufbau Principle
b)
Pauli Exclusion Principle
c)
Hund's Rule
65.
What does the 6 represent?
a)
atomic mass
b)
atomic number
c)
element name
d)
chemical symbol 
66.
Which one of these is not a noble gas?
a)
Helium
b)
Radon
c)
Iodine
d)
Krypton
67.
What is the atomic number of Oxygen?
a)
6
b)
7
c)
8
d)
9
68.

what group number are the halogens

a)

18

b)

1

c)

2

d)

17

69.

what group number are the noble gases

a)

17

b)

18

c)

14

d)

15

70.
An element's identity is determined by the number of
a)
electrons.
b)
protons.
c)
neutrons.
d)
valence.
71.

The vertical (up and down) columns in the Periodic Table are called

a)

groups

b)

towers

c)

periods

d)

atomic numbers

72.
The Modern Periodic Table of Elements is arranged by
a)
atomic mass
b)
atomic number
c)
valence electrons
d)
number of isotopes
73.
Sodium (Na) is found in period 
a)
3
b)
2
c)
4
d)
1
74.
As you move down a group, atomic radius increases because - 
a)
you add more and more neutrons
b)
you add more and more protons
c)
you add more and more shells (energy levels)
d)
you add more atomic mass
75.
Electronegativity is...
a)
the ability of an atom to attract/ accept 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. 
76.
Electronegativity __________ from left to right within a period and __________ from top to bottom within a group.
a)
decreases, increases 
b)
increases, increases
c)
increases, decreases 
d)
stays the same, increases
77.

How many valence electrons does carbon have?

a)

4

b)

5

c)

6

d)

7

78.

USE THE PERIODIC TABLE

How many valence electrons does sodium have?

a)

1

b)

2

c)

3

d)

4

79.

USE THE PERIODIC TABLE

How many valence electrons does Phosphorus have?

a)

31

b)

5

c)

15

d)

4

80.

What is it called when one or more electrons are transferred from one atom to another?

a)

Covalent Bond

b)

Ionic bond

c)

Ion

d)

Anion

81.

What is a cation?

a)

A negatively charged ion

b)

An atom with no charge

c)

A positively charged ion

d)

A stable atom on the periodic table

82.

What is an anion?

a)

A negatively charged particle

b)

An atom with no charge

c)

A positively charged ion

d)

A stable atom found on the periodic table

83.

What is it called when two atoms share an electron?

a)

Ionic Bonding

b)

Covalent bonding

c)

Oxidation Number

d)

Valence Electron

84.

True or False. The highest energy level in an atom is closer to the nucleus.

a)

True

b)

False

85.

Where are valence electrons located in an atom?

a)

On the outermost energy level

b)

On the innermost energy level

c)

In the nucleus

86.

What is a method for representing an atom's valence electrons using dots around the element symbol?

a)

Lewis Dot Structure

b)

Bohr Diagram

c)

Ion Formation

87.

Where are the noble gases located on the periodic table?

a)

In the middle of the periodic table

b)

On the bottom of the periodic table

c)

On the left hand side of the periodic table

d)

On the right hand side of the periodic table

88.
What is an ion?
a)
A Charged Atom
b)
A Large Atom
c)
A Small Atom
d)
A Cute Atom
89.
Why are ions formed?
a)
To make our lives difficult
b)
Because atoms want 8 valence electrons
c)
Because atoms have the same number of protons and electrons
d)
Because atoms gained neutrons
90.
An atom becomes _________ when it gains electrons.
a)
Positive
b)
Negative
c)
Neutral
d)
Invinsible
91.
An atom becomes _______ when it loses electrons.
a)
Positive
b)
Negative
c)
Neutral
d)
Invinsible
92.
What is a Rubidium ion's symbol?
a)
Rb-
b)
Rb+
c)
Rb-2
d)
Rb+2
93.
What is the ionic symbol for a phosphorus atom?
a)
P-3
b)
P+3
c)
P-2
d)
P+2
94.

The name of FeCl₂ is

a)

iron chloride

b)

iron (II) chloride

c)

iron (I) chloride

d)

iron dichloride

95.

LiBr is called

a)

lithium bromine

b)

lithium (I) bromine

c)

lithium bromide

d)

lithuim (I) bromide

96.

Which of these combinations is an ionic compound made of?

a)

Metal and Metal

b)

Nonmetal and Nonmetal

c)

Metal and Nonmetal

d)

Cation and Cation

97.

Name the following ionic compound: BeCl2

a)

beryllium chlorine

b)

beryllium II chloride

c)

beryllium chloride

d)

beryllium dichloride

98.

When naming ionic compounds with transition metals you need to include roman numerals to show the _____ of the metal..

a)

atomic number

b)

mass number

c)

charge

d)

ionization energy

99.

What is the name of the compound Na2(SO4)?

a)

Sodium sulfate

b)

Sodium sulfide

c)

Sodium sulfite

d)

Sodium sulfuroxide

100.

The name of the compound Ca3(PO4)2

a)

calcium phosphate

b)

tricalcium diphosphate

c)

calcium phosphorus oxide

d)

calcium phosphide

101.
phosphorus trichloride
a)
KCl3
b)
PCl3
c)
K3Cl
d)
P3Cl
102.
silicon dioxide
a)
SO2
b)
NaO2
c)
SiO2
d)
SiO
103.
SiCl4
a)
silicon tetrachloride
b)
silicon quadchloride
c)
monosilicon tetrachloride
d)
silicon chloride
104.
The chemical formula of tetraphosphorus heptaoxide is
a)
F₄O₁₀
b)
P₄O7
c)
PO
d)
P₁₀O₄
105.
The name of SO₃ compound is
a)
sulfate
b)
sulfur oxide
c)
sulfur trioxide
d)
monosulfur trioxide
106.
BrO3
a)
bromine oxide
b)
monobromine trioxide
c)
bromine trioxide
d)
bromine (III) oxide
107.
Name the acid: HC2H3O2
a)
Acetic Acid
b)
Acetous Acid
c)
Hydrogen Acetate
d)
Hydrogen Dicarbon Trihydrogen Dioxygen
108.
What is the formula for phosphorous acid?
a)
H3PO4
b)
H2PO4
c)
H3P
d)
H3PO3
109.
What is the formula for Nitric Acid?
a)
HNO2
b)
HNO3
c)
HNO4
d)
H2NO3
110.
Name HF
a)
hydrofluoric acid
b)
Hypofluoric acid
c)
hydrogen fluorine acid
d)
fluoric acid
111.
The mass of one mole of substance is called...
a)
molecular mass
b)
mole constant
c)
molar mass
d)
atomic weight
112.
What is the molar mass of sodium?
a)
11
b)
23
c)
45.98
d)
3
113.
What is the molar mass of CO2?
a)
12
b)
16
c)
32
d)
44
114.
How many particles are in a mole?
a)
602
b)
602 million
c)
602 moles
d)
6.02 x 1023
115.
Molar mass is in units of ________.
a)
grams
b)
grams/mole
c)
mole
d)
moles/gram
116.
What is the molar mass of AuCl3?
a)
96 g
b)
130 g
c)
232.5 g
d)
303.3 g
117.
What is the definition for Avogadro's number?
a)
number of grams per one mole of a substance
b)
whole number ratio that is a multiple of a chemical formula
c)
simplest, whole number ratio of a chemical formula
d)
6.02 x 10^23 particles per one mole of a substance
118.
What is the mass of 2.50 mol of oxygen gas O2?
a)
40.0 g
b)
80.0 g
c)
16.0 g
d)
32.0 g
119.
If I have 6.02 x1023 molecules of CO2, what is the mass?
a)
44.0 g
b)
2.65 x1023 g
c)
1.37 x1022 g
d)
96.0 g
120.
How many molecules are in 32.4 grams of phosphorous pentoxide?
a)
1.76 x 1023 molecules
b)
0.29 moles
c)
1.76 x 1022 molecules
d)
0.29 molecules
121.
What is the percent by mass of sodium in NaCl?
a)
39%
b)
61%
c)
35%
d)
65%
122.
What is the percent composition by mass of magnesium in the compound MgSO4 (gram formula mass = 120 g/mol)?
a)
20%
b)
27%
c)
46%
d)
53%
123.
How many grams are in 3.3 mol of Potassium Sulfide?
a)
360 g
b)
454 g
c)
238 g
d)
132 g
124.
magnesium carbonate
a)
Mg2C
b)
Mg2CO4
c)
Mg2(CO3)2
d)
MgCO3
125.

Which has more molecules?

a)

1 mole H2O

b)

1 mole CH4

c)

1 mole Cl2

d)

They're are all the same.

126.

36.0 g of beryllium (Be) contains how many moles?

a)

0.25 mol

b)

4.0 mol

c)

45 mol

d)

320 mol

127.

What is the molar mass of (NH4)3PO4

a)

113.02 g/mol

b)

124.13 g/mol

c)

149.12 g/mol

d)

137.00 g/mol

128.

What is the molar mass of one mole of HCl?

a)

79.92 grams per mole of HCl

b)

36.46 grams per mole of HCl

c)

35.45 grams per mole of HCl

d)

1.01 grams per mole of HCl

129.
What is the mass of 0.89 mol of CaCl2?
a)
111 grams
b)
0.008 grams
c)
98.9 grams
d)
none of the choices
130.
How many moles are present in 32.3 grams of carbon dioxide (CO2)?
a)
44.01 moles
b)
1421.52 moles
c)
32.3 moles
d)
0.73 moles
131.
A compound consists of 72.2% magnesium(Mg) and 27.8% nitrogen(N) by mass. What is the empirical formula?
a)
Mg4N3
b)
MgN2
c)
Mg3N2 
d)
MgN
132.
You are given the following percentages: 40.05% S and 59.95% O. Find the empirical formula for these elements.
a)
SO
b)
SO2
c)
SO3
d)
SO4
133.
What is the empirical formula if you have 81.82% carbon and 18.18% hydrogen?
a)
C3H8
b)
CH4
c)
C2H2
d)
C4H10
134.
A formula with the lowest whole # ratio of elements in a compound is called
a)
Molecular Formula
b)
Chemical Formula
c)
Empirical Formula 
d)
Distance Formula
135.
What is the percentage of chlorine in sodium chloride? (NaCl)
a)
60.7%
b)
39.3%
c)
60%
d)
40%
136.
Glycerol has a molar mass of 92.09g/mol. Its percent composition is: 39.12% C, 8.75% H, and 51.12% O. What is the molecular formula for glycerol?
a)
C2H3O2
b)
CH2O
c)
C2H4O2
d)
C3H8O3

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