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Chemistry Mid-Term

Total questions: 155

Worksheet time: 3hrs 53mins

Name
Class
Date
1.

The law of conservation of mass states

a)

The mass of the products is never equal to the mass of the reactants.

b)

The mass of the products is less than the mass of the reactants

c)

The mass of the products is equal to the mass of the reactants

d)

The mass of the products is greater than the mass of the reactants

2.

Gold is a solid at room temperature. This is an example of a/n __ property

a)

nuclear

b)

electrical

c)

chemical

d)

physical

3.

An atom of chromium has 24 protons, 28 neutrons, and 24 electrons. How many subatomic particles are in the nucleus of a chromium atom?

a)

24

b)

28

c)

48

d)

52

4.

The average distance from Earth to the Moon is 384,401 km. How is the distance from Earth to the Moon expressed in scientific notation

a)

384 x 10^3 km

b)

3.84 x 10^3 km

c)

3.84 x 10 ^5 km

d)

3.84 x 10^6 km

5.

How do you calculate the mass number of an element?

a)
protons + electrons
b)
Protons + Neutrons
c)
Electrons + neutrons
d)
Electrons + Protons + Neutrons
6.
What is the charge of a neutron?
a)
positive
b)
negative
c)
neutral
d)
depends
7.
what is the charge of an electron?
a)
positive
b)
negative
c)
neutral
d)
depends
8.
What is the charge of a proton?
a)
positive
b)
negative
c)
neutral
d)
depends
9.
Rutherford and his gold foil shooting gallery discovered which subatomic particle?
a)
electron
b)
proton
c)
neutron
d)
nucleus
10.
Thomson and his cathode ray tube discovered which subatomic particle?
a)
Electron
b)
Proton
c)
Neutron
d)
Nucleus
11.
When constructing a bohr model, how many electrons can be placed in the first energy circle? 
a)
2
b)
4
c)
8
d)
Depends on the Group
12.
Using your periodic table. How many protons does Gold have? 
a)
196
b)
11
c)
79
d)
180
13.
The Period Number tells us ___________
a)
Valence Electrons
b)
Energy Shells
c)
Neutrons
d)
Protons
14.
The group number tells us the number of ____________
a)
Energy Shells
b)
Valence Electrons
c)
Protons
d)
Neutrons
15.
Find the average atomic mass of an element that has 3 different isotopes.
Atomic Mass            Relative Abundance
28 amu                     92.21 %
29 amu                     4.70 %
30 amu                     3.09%
a)
32.679
b)
28.1088
c)
26.548
d)
38.389
16.
Which of the following is not a subatomic particle?
a)
Neutron
b)
Nucleus
c)
Proton
d)

Electron

17.

A change in size, shape, or state of matter is a

a)
Chemical Property
b)
Physical Property
c)
Physical Change
d)
Chemical Change
18.
If the particles are tightly packed together and vibrating in place. What state of matter is the object?
a)
Solid
b)
Liquid
c)
Gas
d)
Vapor
19.

Which state of matter has neither definite shape nor volume?

a)
Solid
b)
Liquid
c)
Gas
d)
Water
20.
What is the volume of an object with a mass of 20 g and a density of .5 g/cm3
a)
40 cm3
b)
10 cm3
c)
.025 cm3
d)
17 cm3
21.
What is the mass of an object that has a volume of 52 cm3 and a density of 1.45 g/cm3? 
a)
.02 g
b)
75.4 g
c)
35.68 g
d)
.15 g
22.
What is the density of an object that has a mass of 1,500 g and a volume of 100 ml ?
a)
.066 g/ml
b)
150,000 g/ml
c)
15 g/ml
d)
1.5 g/ml
23.
Which of the following is not a physical change? 
a)
Tearing Paper
b)
Melting Ice
c)
Freezing water
d)
Burning Wood
24.
Which of the following below is not a physical property? 
a)
Density
b)
Combustion
c)
Length
d)
Solubility
25.
The equation to calculate Density is
a)
D= v/m
b)
D= V x M
c)
D = M / V
d)
D = ml/g 
26.
How many valence electrons does a bromine atom have?
a)
1
b)
2
c)
6
d)
7
27.

What element is will have the closest physical and chemical properties to Nitrogen (N)?

a)
Phosphorous (P)
b)
Carbon (C)
c)
Oxygen (O)
d)
Sulfur (S)
28.

What element is will have the closest physical and chemical properties to Sulfur (S)?

a)
Carbon (C)
b)
Phosphorous (P)
c)
Oxygen (O)
d)
Neon (Ne
29.
Each column in the periodic table is called a _________ .
a)
period
b)
group
c)
cluster
d)
unit
30.

What does the atomic radius increase down a group?

a)

There are more electrons and energy levels.

b)

There are fewer electrons and energy levels.

c)

There are more protons that need more energy levels.

d)

There are more neutrons that need more energy levels.

31.

What is the trend for atomic radius?

a)

It increases left to right on the Periodic Table and decreases down a group.

b)

It decreases left to right on the Periodic Table and increases down a group.

c)

It increases left to right on the Periodic Table and increases down a group.

d)

It decreases right to left on the Periodic Table and decreases down a group.

32.

Why does the atomic radius decrease across a period?

a)

There are more protons in the nucleus that pull electrons closer.

b)

There are more electrons in the nucleus that pull protons closer.

c)

There are more protons in the nucleus that pull neutrons closer.

d)

There are more neutrons in the nucleus that pull protons closer.

33.

Elements in the same group or family have

a)

the same number of valence electrons and different properties.

b)

the same number of valence electrons and similar properties

c)

different number of valence electrons and similar properties.

d)

different number of valence electrons and different properties.

34.

What is the short hand configuration for silicon?

a)

[Ar]2s22p2

b)

[Ne]2s22p2

c)

[Ne]3s23p2

d)

[Ne]3s23p4

35.

What is the short-hand electron configuration for sulfur?

a)

[Ar] 3p4

b)

[He] 3s2 3p4

c)

[Ne] 3s2 3p4

d)

[Na] 3s2 3p4

36.
Which electron configuration belongs to Chlorine (Cl)?
a)
1s2 2s2 2p6 3s2 3p5
b)
1s2 2s2 2p6 3s2 3p6
c)
1s2 2s2 2p6 3s2 3p7
37.
The electron configuration of an atom is 1s22s22p6.  The number of electrons in the atom is 
a)
3
b)
6
c)
8
d)
10
38.
What atom matches this electron configuration?
1s22s22p63s23p64s23d10
a)
Zinc
b)
Copper
c)
Nickel
d)
Germanium
39.

If the mass number of this chlorine atom is 36, how many neutrons does it have?

a)

17

b)

18

c)

19

d)

can't be determined

40.
If an atom has 10 protons, 10 neutrons, and 10 electrons, what is the mass of the atom?
a)
10
b)
20
c)
30
41.

If an atom has 12 protons, which of the following must it also have to be considered a neutral atom?

a)

12 neutrons

b)

12 electrons

c)

12 protons

d)

24 protons and neutrons

42.

What does the 1.00794 stand for?

a)

mass number

b)

atomic number

c)

average atomic mass

d)

number of protons

43.
Two atoms of the same element but with different mass numbers are called________
a)
electrons
b)
isotopes
c)
variables
d)
electron cloud
44.
What is the mass 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
45.
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
46.
If the number of protons equal the number of _____, the atom will have no charge
a)
protons
b)
neutrons
c)
electrons
d)
nucleus
47.

Table salt is an example of a/an

a)

Element

b)

Compound

c)
heterogeneous mixture
d)
homogeneous mixture
48.
Oxygen gas is an example of a.....
a)
pure element
b)
pure compound
c)
heterogeneous mixture
d)
homogeneous mixture
49.
Which of the following IS a mixture?
a)
air
b)
hydrogen
c)
water
d)
sugar
50.
Which of the following is not an element?
a)
water
b)
hydrogen
c)
carbon
d)
oxygen
51.
Mixture, such as mixed nuts or dry soup mix, in which different materials are unevenly distributed and are easily identified.
a)
suspension
b)
homogeneous mixture
c)
heterogeneous mixture
d)
colloid
52.
A mixture that is NOT evenly distributed is called ....
a)
Compounded
b)
Homogenous
c)
Heterogenous
d)
Salty
53.

Which changes are chemical changes? (Select all that apply.)

a)

boiling water to form steam

b)

adding sodium to water

c)

burning methane for heat

d)

melting ice-cream in summer

54.

How many electrons are there in the outer electronic shell of chlorine?

a)

5

b)

6

c)

7

d)

8

55.

Which of the following shows the correct quantum numbers (n; l; m) and electron configuration for the last electron in the following atoms? 

a)
P:[Ne]3s23p3
n=3; l=0; ml=0 
b)
Br: [Ar]4s2 3d10 4p5 
n=4; l=1;  ml = −2
c)
Na: [Ne]3s1
n=3; l=1; ml =−1
d)
Ga: [Ar]4s23d104p1
n = 4; l = 1; ml = −1 
56.

The electronegativity of an atom generally ______ going up columns and _____ going right  to left across rows.

a)

decreases; decreases

b)

increases; increases

c)

increases; decreases

d)

decreases; increases

57.
How many neutrons in C-14?
a)
6
b)
7
c)
14
d)
8
58.
How many protons does this isotope of titanium have?
a)
48
b)
22
c)
26
d)
70
59.
How many neutrons does the isotope of lithium have?
a)
8
b)
3
c)
4
d)
5
60.
What do these isotopes of carbon all have in common?
a)
neutrons & mass number
b)
atomic number and neutrons
c)

Number of protons

d)
protons, atomic number, and mass number
61.

which isotope has  4 neutrons?

a)
Li-6
b)
Li-7
c)
Li-8
d)
they have the same # of neutrons
62.
How many protons are in an atom of silver (Ag)?
a)
107
b)
108
c)
47
d)
61
63.
How many valence electrons do elements in group 17 have in their outer energy level?
a)
7
b)
17
c)
1
d)
0
64.
The group number tells us how many _________ there are in an element.
a)
groups
b)
valence electrons
c)
energy levels
d)
chemicals
65.
A sample of metal beads was measured to have a mass of 425g. The beads were placed in a graduated cylinder that initially had 100.mL of water.  After placing the beads in the graduated cylinder the water level rose to 148mL.  Given the following densities, select the most likely identity of the metal.
a)
Gold
19.3g/mL
b)
Copper
8.86g/mL
c)
Bronze
9.87g/mL
d)
Lead
11.37g/mL
66.
The number 2 × 1015 is
a)
greater than one. 
b)
smaller than 2.0 × 10−15. 
c)
less than one. 
d)
More information is needed. 
67.
What is the answer with the proper significant figures for the following equation?
(7.6 + 8.401) × 4.2 × 0.688 = 
a)
46.237 
b)
46.24 
c)
46 
d)
46.2
68.
Which of the following is a physical change? 
a)
Light is given off as two liquids mix.
b)
An iron nail rusts.
c)
A liquid evaporates. 
d)
Carbon dioxide is produced by burning gasoline. 
69.
How may significant digits are found in 765.000? 
a)
3
b)
4
c)
5
d)
6
70.
Where are Noble gases found on the periodic table?
a)
In the sky
b)
on the far right
c)
on the far left 
d)
in the dead middle
71.
The characteristics or properties of metals include
a)
shiny and solid
b)
ductile and malleable
c)

Good conductors

d)
all of the above
72.
The ________________ tells you how many energy levels are used in an element.
a)
group number
b)
atom
c)
protons
d)
period number
73.
Which particle does not contribute mass to the atom?
a)
Proton
b)
Neutron
c)
Electron
d)
Nucleus
74.
In the Pauli Exclusion Principle electrons must have opposite __________ to share an orbital.
a)
charges
b)
spins
c)
uncertainty
d)
quantum levels
75.
Which of the following statements is false
a)
Atoms can share electrons
b)
All atoms are the same
c)
In a neutral atom their are equal numbers of protons and electrons
d)
Isotopes have different numbers of neutrons but the same number of protons
76.
There is one s orbital and _____p orbitals for each quantum energy level or period.
a)
5
b)
7
c)
3
d)
1
77.
According to Hund's Rule electrons fill orbitals of a shape at an energy level...
a)
In pairs of electrons
b)
From highest energy levels to lowest
c)

Orbitals must fill one electron at a time before adding a second

d)
In no particular order.
78.
What is the symbol for an alpha particle?
a)
42He
b)
0-1e
c)
0+1 e
d)
10n
79.
What does the symbol -10e represent
a)
alpha
b)
beta
c)
gamma
d)
the zero element
80.

Which scientist described a positively charged core (“nucleus”) in the middle of a lot of empty space?

a)

Chadwick

b)

Thomson

c)

Rutherford

d)

Bohr

81.

If an element X has isotopes 14X (95% abundance), 15X (3% abundance), and 16X (2% abundance), what is the average atomic mass closest to?

a)

14.07

b)

15.00

c)

14.00

d)

16.00

82.

Which statement best describes the Quantum Mechanical model of the atom?

a)

Electrons are arranged on a large, solid, positive center.

b)

Electrons orbit around the nucleus in set paths.

c)

Electrons have properties similar to waves.

d)

Electrons make up most of the mass of an atom.

83.

How does the isotopes carbon-12 and carbon-14 differ?

a)

Carbon-12 has 12 neutrons; carbon-14 has 14 neutrons

b)

Carbon-12 has 6 protons; carbon-14 has 8 protons

c)

Carbon-12 has 6 neutrons; carbon-14 has 8 neutrons

d)

Carbon-12 has 6 protons; carbon-14 has 6 protons

84.

COFFEE IS

a)

Compound

b)

ELEMENT

c)

HOMOGENEOUS MIXTURE

d)

HETEREGENEOUS MIXTURE

85.

6. Chicken noodle soup is an example of

a)

Heterogeneous mixture

b)

Homogeneous mixture

86.
Gold is an example of a(n)
a)
Element 
b)
Compound 
c)
Nugget 
87.

Which event always involves a chemical change?

a)

boiling

b)

melting

c)

conducting

d)

burning

88.

Which characteristic of a substance is considered a chemical property?

a)

its boiling point

b)

its reactivity

c)

its density

d)

its conductivity

89.

Which of these metric units would you use to measure length?

a)

L

b)

mg

c)

kg

d)

m

90.

Which of the following metals is not a solid at room temperature?

a)

Copper

b)

Magnesium

c)

Mercury

91.

In which state of matter can materials take the shape of their container?

a)

Solids and liquids

b)

Liquid and gases

c)

Gases and solids

92.

Which of the following is NOT a physical property?

a)

Flammability

b)

Color

c)

Hardness

93.

The smallest particle of an element is a/an…

a)

Nucleus

b)

Electron

c)

Atom

94.

Helium, Gold, and Table salt are all examples of _________________________________.

a)

Compound

b)

Mixture

c)

Pure substance

95.

Very hot salsa for your tortilla chips would be an example of a _________________________________.

a)

Compound

b)

Mixture

c)

Solution

96.

Melting and Boiling points are

a)

Chemical Properties

b)

Physical Properties

c)

States of Matter

97.

A heterogeneous mixture is

a)

Parts are the same throughout

b)

Parts are not easily separated

c)

Parts are different throughout

98.

419,000 is equal to ________.

a)

4.19 x 10-2

b)

4.19 x 105

c)

4.19 x 10-5

99.

0.0419 is equal to ________.

a)

4.19 x 10-2

b)

4.19 x 105

c)

4.19 x 10-5

100.

Which value is equivalent to 5 x 106?

a)

Fifty thousand

b)

Five million

c)

Fifty million

101.

What type of mixture would fruit salad be?

a)

homogeneous

b)

heterogeneous

102.
Elements in the same column of the periodic table always have the same # of _______ as one another.
a)
Protons
b)
Neutrons
c)
Electrons
d)
Valence Electrons
103.

The nucleus of an atom contains which subatomic particles?

a)

protons and electrons

b)

protons and neutrons

c)

electrons and neutrons

d)

protons, electrons, and neutrons

104.
What quantities vary between isotopes of an element?
a)
protons, electrons, and atomic mass
b)
protons, electrons, and atomic number
c)
neutrons and electrons
d)
neutrons and atomic mass
105.

What is the term for the type of matter that cannot be broken down into simpler substances by chemical means?

a)

Element

b)

Compound

c)

Mixture

d)

Atom

106.

What is the term for the type of matter that can be separated into two or more substances by physical means?

a)

Element

b)

Compound

c)

Mixture

d)

Atom

107.

What type of matter is characterized by having a fixed shape and volume?

a)

Solid

b)

Liquid

c)

Gas

d)

Plasma

108.

What is the term for the amount of energy required to remove an electron from an atom?

a)

Ionization energy

b)

Electron affinity

c)

Atomic radius

d)

Electronegativity

109.

Which elements are stable?

a)

Group 1

b)

Group 8

c)

Group 18

110.

Which of the following can be separated by physical means?

a)

pure substances

b)

mixtures

c)

Elements

d)

Compounds

111.
According to the octet rule most elements need _______ valence electrons.
a)
2
b)
8
c)
6
d)
18
112.
How many electrons can the p sublevel hold?
a)
14
b)
10
c)
2
d)
6
113.
How many electrons can the d sublevel hold?
a)
14
b)
10
c)
2
d)
6
114.

Which Lewis electron-dot diagram represents a nitrogen atom in the ground state?

a)
b)
c)
d)
115.

How many valence electrons does Lithium have?

a)

1

b)

3

c)

None

d)

2

116.

Elements in group 3-12 are called

a)

Alkali Metals

b)

Alkaline Earth Metals

c)

Transition Metals

d)

Halogens

117.

Elements in group 2 are called

a)

Alkali Metals

b)

Alkaline Earth Metals

c)

Transition Metals

d)

Halogens

118.

Which group on the periodic table contains elements that are all gases at room temperature?

a)

Group 17

b)

Group 1

c)

Group 2

d)

Group 18

119.

What is the name of group number 1?

a)

halogens

b)

noble gases

c)

alkali metals

d)

alkaline earth metals

120.

what group number are the noble gases

a)

17

b)

18

c)

14

d)

15

121.

what group number are the halogens

a)

18

b)

1

c)

2

d)

17

122.

An unknown element is found to have properties similar to those of magnesium and calcium. Using your knowledge of periodic table groups, predict which group this element most likely belongs to.

a)

Group 1 (Alkali metals)

b)

Group 2 (Alkaline earth metals)

c)

Group 17 (Halogens)

d)

Group 18 (Noble gases)

123.

Which statement best describes the arrangement of elements in the modern periodic table?

a)

Elements are arranged in order of increasing atomic mass

b)

Elements are arranged in order of increasing atomic number

c)

Elements are arranged alphabetically

d)

Elements are arranged by color

124.

What is the horizontal row in the periodic table called?

a)

Group

b)

Family

c)

Period

d)

Block

125.

What is the definition of an isotope?

a)

Atoms with the same number of protons but different numbers of neutrons

b)

Atoms with different numbers of protons and electrons

c)

Atoms with the same number of neutrons but different numbers of protons

d)

Atoms with the same number of protons and neutrons

126.

What are the vertical columns in the periodic table called?

a)

Rows

b)

Groups

c)

Periods

d)

Blocks

127.
What is the symbol for Potassium?
a)
P
b)
K
c)
Pb
d)
Pd
128.
Who created the periodic table?
a)
Einstein
b)
Democritus
c)
Mendeleev
d)
Rutherford
129.
Refer to the illustration below. Neon’s outer energy level contains ___ electrons
a)
2
b)
8
c)
10
d)
20
130.
How many energy levels does potassium (K) have?
a)
1
b)
2
c)
3
d)
4
131.
Which of the following classification does nickel (Ni) belong to?
a)
alkali metal
b)
transition metal
c)
halogen
d)
noble gas
132.
Which of the following subatomic particles does not contribute to the mass of the atom?
a)
Proton
b)
Neutron
c)
Electron
133.
The elements oxygen (O), sulfur (S), and selenium (Se) are all located in column 16 of the periodic table. Which of the following is true of these elements?
a)
They all have the same atomic number.
b)
They all have the same atomic mass.
c)
They all have the same number of electrons.
d)
They all have the same number of valence electrons.
134.
Which two elements have similar chemical properties according to the periodic table?
a)
helium and argon
b)
oxygen and nitrogen
c)
lithium and calcium
d)
boron and Arsenic
135.
In the periodic table, which group or family of elements has only one valence electron in its outer shell?
a)
the alkali metals
b)
the noble gases
c)
the halogens
d)
the alkaline-earth metals
136.
Where on the periodic table are the MOST reactive nonmetals found?
a)
Group 15
b)
Group 1
c)
Groups 3-12
d)
Group 17
137.
Two unknown substances, a liquid and a solid, are mixed together, gas bubbles form. This is most likely what kind of change?
a)
Phase Change
b)
Nuclear Change
c)
Physical Change
d)
Chemical Change
138.
Digestion of food in your stomach
a)
Physical change
b)
Chemical change
139.
Popsicle melting on a hot summer day
a)
Physical change
b)
Chemical change
140.
Milk going sour
a)
Physical change
b)
Chemical change
141.
The Statue of Liberty turning green
a)
Physical change
b)
Chemical change
142.
Which of the following statements is true concerning all metalloids?
a)
They are extremely reactive.
b)
They have properties of both metals and non-metals.
c)
They are inert.
d)
They have 6 energy levels.
143.
Mendeleev noticed that if he organized the elements by atomic weight certain patterns emerged. For instance, elements in the same group (family) appeared to have the same ___.
a)
Valence electrons
b)
Energy levels
c)
Number of neutrons
d)
Atomic mass
144.
Which of the following statements is NOT true of krypton, argon and neon?
a)
They are inert.
b)
They have 8 valence electrons.
c)
They are reactive.
d)
They are noble gases.
145.
What is the name and group # of the most highly reactive metal group on the Periodic Table?
a)
Alkali Metals (group 1)
b)
Halogens (group 17)
c)
Noble gases (group 18)
d)
Alkaline Earth Metals (group 2)
146.
The atomic number is the same as the number of _______ or _______.
a)
neutrons and protons
b)
protons and electrons
c)
electrons and neutrons
d)
all of the above
147.
Examine the periodic table for the element nitrogen, chemical symbol N. Using your knowledge of the periodic table, which of these statements is correct about nitrogen?
a)
Nitrogen has the same number of energy levels as oxygen.
b)
Nitrogen’s elemental symbol is Ni.
c)
Nitrogen has fewer energy levels than boron.
d)
Nitrogen has the same number of valence electrons as fluorine.
148.
The state of matter that has definite volume but no definite shape is...
a)
Solid
b)
Liquid
c)
Gas
d)
Plasma
149.
In the isotope B-11, what does the 11 represent?
a)
Atomic number
b)
Mass number
c)
Average atomic mass
d)
Number of neutrons
150.
An unknown isotope contains 15 protons, 15 electrons, and 17 neutrons. What is the identity of this unknown isotope?
a)
P-15
b)
P-17
c)
P-30
d)
P-32
151.
Isotopes of the same element must have different numbers of____.
a)
Protons
b)
Neutrons
c)
Electrons
d)
Both A & B
152.

Round 0.010229 to four sig figs

a)

1022

b)

0.01023

c)

0.01022

153.

How many significant figures does the following number have: 0.002040 (Do not count leading zeros)

a)

6

b)

3

c)

4

d)

2

154.

0.932 g = ___________ mg

a)

9.32

b)

93.2

c)

932

d)

9,320

155.

240 cm = ___________m

a)

2400

b)

2.4

c)

24

d)

0.24

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