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Chemistry Semester 1 Midterm Review

Total questions: 92

Worksheet time: 2hrs 32mins

Name
Class
Date
1.

A subatomic particle with a positive charge that is in the nucleus of an atom is called a (a)   .

Choose from the below words
neutron
proton
electron
valence electron
2.

What is a subatomic particle without an electric charge, located in the nucleus of an atom?

a)

neutron

b)

proton

c)

electron

d)

valence electron

3.

What is a subatomic particle with a negative charge? It is found in the electron cloud surrounding the nucleus.

a)

neutron

b)

proton

c)

electron

d)

electron cloud

4.

What is the center of an atom containing protons and neutrons?

a)

nucleus

b)

neutron

c)

proton

d)

electron cloud

5.

Match the following particles with their electrical charges.

a)

+1

1.

Proton

b)

0

2.

Neutron

c)

-1

3.

Electron

d)

+2

4.

Alpha particle

6.
In order for an atom to be neutral what has to be true?
a)
The atom has more protons than neutrons
b)
The atom has more neutrons than protons
c)
The atom has the same number of protons and neutrons
d)
The atom has the same number of protons and electrons
7.
What subatomic particles would you find in the nucleus of an atom?
a)
Protons only
b)
Protons and Neutrons
c)
Neutrons and Electrons
d)
Protons and Electrons 
8.

How many electrons does this atom have?

a)

2

b)

4

c)

6

d)

10

9.
Question Image

Match the following components of an atom with where most of the mass is located.

a)

in the nucleus

1.

Where is most of the mass in an atom located?

b)

in the protons

2.

Where are positively charged particles found?

c)

in the neutrons

3.

Where are neutral particles found?

d)

in the electrons

4.

Where are negatively charged particles found?

10.

What is the atomic number?

a)

the number of protons in the nucleus

b)

the number of protons and neutrons in the nucleus

c)

the number of neutrons in the nucleus

d)

the number of protons in the energy levels

11.

What is the mass number?

a)

the number of protons in the nucleus

b)

the number of protons and neutrons in the nucleus

c)

the number of neutrons in the nucleus

d)

the number of protons and electrons in the atom

12.

What is the mass number of this atom?

a)

1

b)

3

c)

4

d)

7

13.
What does the C represent?
a)
atomic mass
b)
atomic number
c)
element name
d)
chemical symbol 
14.

What does the 6 represent?

a)

Atomic mass

b)

atomic number

c)

chemical symbol

d)

element name

15.
How is the number of neutrons in the nucleus of an atom calculated?
a)
Add the number of e- and p+ together
b)
Subtract the number of e- from p+
c)
Subtract the number of p+ from the mass number
d)
Add the mass number to the number of e-
16.

An atom has 10 protons, 15 neutrons and 10 electrons, its mass number is (a)   .

Choose from the below words
20
10
35
25
17.

This is an atom of (a)   .

Choose from the below words
nitrogen
lithium
beryllium
carbon
18.
The top number in this isotope notation is
a)
the mass number
b)
the atomic number
c)
the atomic mass
d)
the neutron number
19.
According to the isotopic notation for copper-63, how many neutrons are present in this type of atom?
a)
29
b)
34
c)
63
d)
92
20.
The following element has _____________ electrons.
a)
114
b)
289
c)
175
d)
403
21.

What element does this Bohr model represent?

a)

Chromium

b)

Magnesium

c)

Carbon

d)

Krypton

22.
What group does this element belong to?
a)
Group 1: Alkali metals
b)
Group 18: Noble Gases
c)
Group 2: Alkaline-Earth Metals
d)
Group 17: Halogens
23.
How many valence electrons?
a)
2
b)
3
c)
5
d)
10
24.
What's a valence electron?
a)
electrons in the second energy level
b)
electrons in the outermost energy level
c)
the atomic number
d)
electrons in the first level
25.
What is an isotope? 
a)
A charged atom
b)
An atom with different amounts of neutrons
c)
An atom with different amounts of protons
d)
A neutral atom
26.
What is the name of the pictured isotope?
a)
Chlorine-Schmorine
b)
Chlorine-17
c)
Chlorine-35
d)
Chlorine-18
27.

Potassium-39 has how many neutrons?

a)

19

b)

18

c)

20

d)

21

28.
In the Bohr model of the atom, what is the maximum number of electrons in the first shell?
a)
1
b)
2
c)
6
d)
8
29.
Look at the periodic table that is provided. Where would nonmetals be located? 
a)
to the left of the table in blue
b)
to the right of the table in pink
c)
in the zigzag line in yellow
30.
Silicon is a semiconductor and has properties of both metals and nonmetals. What type of element is Silicon? 
a)
Metal
b)
Nonmetal
c)
Metalloid
d)
Pretty
31.
Which of the following is a good conductor of heat?
a)
Metal
b)
Nonmetal
c)
Metalloid
32.
Question Image

Match the following elements with their respective families.

a)

Alkali Metals

1.

Li, Na, K, Rb, Cs, Fr

b)

Alkaline Earth Metals

2.

Be, Mg, Ca, Sr, Ba, Ra

c)

Halogens

3.

F, Cl, Br, I, At

d)

Noble Gases

4.

He, Ne, Ar, Kr, Xe, Rn

33.

What family is highlighted in the picture?

a)

Boron Group

b)

Alkaline Earth Metals

c)

Transition Metals

d)

Lanthanides

34.

The horizontal rows on the periodic table are called

a)

groups

b)

families

c)

periods

d)

atomic numbers

35.
In the modern periodic table elements are arranged by:
a)
atomic mass
b)
atomic number
c)
valence electrons
d)
number of isotopes
36.
Which of the following is a halogen?
a)
Krypton
b)
Bromine
c)
Potassium
d)
Bismuth
37.

How many electron energy levels does this element have?

a)

1

b)

2

c)

3

d)

0

38.
Electronegativity is the...
a)
energy needed to remove the outermost electron.
b)
ability of an atom to attract electrons from another atom.
39.

As you move down a GROUP on the periodic table the atomic radius get bigger. This is because ____________.

a)

The atoms have more neutrons in the nucleus.

b)

The atoms have more protons in the nucleus.

c)

The atoms have more energy levels for the electrons

d)

The atoms have greater repulsion forces between the protons and electrons

40.
Which atom has the largest atomic radius?
a)
potassium
b)
rubidium 
c)
francium
d)
cesium
41.
As you move across the periodic table atoms tend to get smaller because, ______________.
a)
the atoms have more mass.
b)
the atoms have less mass
c)
the atoms have more protons.
d)
the atoms have less electrons.
42.
Atoms that have a high electronegativity, _______________.
a)
give up their electrons more easily.
b)
hold on to their electrons more tightly.
c)
have more electron shells.
43.
Ionization energy is...
a)
the energy required to add an electron to a specific atom
b)
how much energy it takes to remove an electron from an atom
c)
the energy required to shield the outer electrons from the nucleus
d)
a measure of the ability of an atom to attract electrons
44.
Which group has the greatest number of valence electrons?
a)
1
b)
14
c)
18
d)
16
45.

Put the following in order of increasing ionization energy: Neon, Lithium, Carbon

a)
Lithium, Carbon, Neon
b)
Carbon, Lithium, Neon
c)
Neon, Carbon, Lithium
d)
Lithium, Neon, Carbon
46.
As you move down the periodic table atoms get bigger.  This is because ____________.
a)
The atoms have more mass.
b)
The atoms have more protons.
c)
The atoms have more energy levels
d)
The atoms have more nuetrons
47.
The element with the largest electronegativity in the halogens is - 
a)
At
b)
F
c)
Cl
d)
Br
48.

The element with the lowest electronegativity in Period 3 is -

a)

Na

b)

Cl

c)

Ar

d)

Mg

49.

The electronegativity of Cl is the highest in Period 3. Why?

a)

Cl is the largest and has the greatest effective nuclear charge

b)

Cl is the smallest and has the lowest effective nuclear charge

c)

Cl is the largest and has the lowest effective nuclear charge

d)

Cl is the smallest and has the greatest effective nuclear charge

50.
Which periodic group has the smallest atomic radius?
a)
Alkali metals
b)
Halogens
c)
Noble Gases
d)
Transition metals
51.

A measure of the size of an atom, and is generally defined as the distance from the nucleus to the outermost electron orbit

a)

chemical reactivity

b)

atomic radius

c)

energy levels

d)

orbit

52.
Francium (Fr) has the lowest ionization energy in Group 1 because - 
a)
it has the smallest number of valence electrons
b)
it has the greatest atomic mass
c)
it has the greatest number of protons, so it attracts its electrons the strongest
d)
its 1 valence electron is very far from the nucleus, so little energy is needed to remove it
53.

a change in the chemical composition and identity of a substance

a)

Physical Change

b)

Chemical Change

c)

Physical and Chemical Change

d)

Matter

54.

a change that alters a substance without changing its chemical composition or its identity

a)

Chemical Change

b)

Physical Change

c)

Chemical and Physical Change

d)

Matter

55.

a characteristic of a pure substance that describes how it interacts with other substances

a)

chemical property

b)

physical property

c)

intensive property

d)

extensive property

56.

a characteristic of a pure substance that can be observed or measured without changing the substance’s chemical identity

a)

chemical property

b)

physical property

c)

intensive property

d)

extensive property

57.

tendency of a substance to undergo chemical changes

a)

Ductility

b)

Malleability

c)

Compressibility

d)

Reactivity

58.

anything that has mass and takes up space

a)

Compressibility

b)

Malleability

c)

Reactivity

d)

Matter

59.

a physical property that does not depend on the amount of substance present

a)

chemical property

b)

physical property

c)

intensive property

d)

extensive property

60.

a physical property that depends on the amount of matter present

a)

chemical property

b)

physical property

c)

intensive property

d)

extensive property

61.

is the measure of how much a given volume of matter decreases when placed under pressure

a)

malleability

b)

ductility

c)

compessibility

d)

solubility

62.

the mass of a substance per unit volume

a)

viscosity

b)

solubility

c)

density

d)

reactivity

63.

 a sample of matter with both definite and constant composition and distinct chemical properties

a)

Pure Substance

b)

Mixture

c)

Matter

d)

Density

64.

Indefinite shape and definite volume describe which state of matter

a)

Solid

b)

Liquid

c)

Gas

d)

Plasma

65.

Definite shape and definite volume describe which state of matter

a)

Solid

b)

Liquid

c)

Gas

d)

Plasma

66.

Indefinite shape and indefinite volume describe which state of matter

a)

Solid

b)

Liquid

c)

Gas

d)

Plasma

67.

Color, hardness, malleability, solubility, electrical conductivity, density, melting point, and boiling point are examples of

a)

Physical Properties

b)

Chemical Properties

68.

Reactivity, flammability, and the ability to rust are examples of

a)

Physical Properties

b)

Chemical Properties

69.

Density is the comparison of the mass and volume of an object. A 2 foot wood plank has a density of 0.85 g/cm3. What is the density of the wood if the wood plank is cut into a 1 foot section?

a)

1.7 g/cm3

b)

0.85 g/cm3

c)

0.425g/cm3

d)

0.085g/cm3

70.

_____________ are composed of more than one substance while _____________ are made up of one type of substance.

a)

Pure substances, mixtures

b)

Pure substances, homogenous substances

c)

Mixtures, pure substances

d)

Mixtures, heterogeneous

71.

Formation of ice is a (a)  

Choose from the below words
physical change
chemical change
72.

Reaction between acid and sucrose

a)

physical change

b)

chemical change

73.

Mass, Size, Shape, Volume, and Number of Moles

a)

Intensive Properties

b)

Extensive Properties

74.

Elements and Compounds are known as ....

a)

Pure Substances

b)

Mixtures

75.

When two or more elements chemicall combine to form new properties the substance is called a ...

a)

element

b)

compound

c)

homogeneous mixture

d)

heterogeneous mixture

76.
In physical changes, substances might change in __________ but not in __________.
a)
appearance, composition
b)
volume, state of matter
c)
texture, color
d)
weight, mass
77.

Choose the best description below for the image

a)

physical change

b)

chemical change

78.

Choose the best description below for the image

a)

physical change

b)

chemical change

79.

Choose the best description below for the image

a)

physical change

b)

chemical change

80.
Matter can not be created nor destroyed: it can only be
a)
Destroyed a little bit
b)
Invisible
c)
Transformed, changed
d)
None of the above
81.

A student heated a 10 gram sample of a chemical in an open container. A chemical reaction occurred, and the mass of the sample was measured again. The mass of the sample was found to be less than before the reaction. Which of the following best explains the decrease in mass of the sample?

a)

The heat caused the chemical to become less dense.

b)

The reaction gave off more heat than was added.

c)

Some of the lighter particles were destroyed.

d)

Some of the particles escaped as a gas formed.

82.

A student dissolved 25 grams of salt into 1,000 grams of water. What should the mass of the saltwater mixture be?

a)

975 grams

b)

1,000 grams

c)

1,025 grams

d)

2,500 grams

83.
Look at this image.  Which object has the LOWEST density in water? How? 
a)
The Ping Pong Ball because it floats to the top 
b)
The bolt because it has sunk to the bottom
c)
The soda cap because it is not just full of air like the Ping Pong ball
84.

What mixture is an heterogeneous mixture?

a)

Soluble coffee in water

b)

Sand and water

c)

Perfume

d)

Apple juice

85.

The mixtures where components CAN NOT be distinguished at simple sight:

a)

Homogeneous

b)

Heterogeneous

c)

Homogeneous and heterogeneous

d)

None

86.
What atom matches this electron configuration?
1s22s22p63s23p64s23d10
a)
Zinc
b)
Copper
c)
Nickel
d)
Germanium
87.
What atom matches this electron configuration?
1s22s22p63s2
a)
Neon
b)
Magnesium
c)
Aluminum
d)
Potassium
88.
What electron configuration matches an oxygen atom?
a)
1s22s22p63s2, 3p64s23d104p5
b)
1s22s22p4
c)
1s22s22p6
d)
1s22s22p63s23p64s23d1
89.

The 4 orbitals are

a)

s, p, d, f

b)

a, b, c, d

c)

2, 4, 6, 8

90.
What is the shorthand electron configuration for Sulfur atom?
a)
[Ar] 3p4
b)
[He] 3s23p4
c)
[Ne] 3s23p4
d)
[Na] 3s23p3
91.

The element pictured is (a)   .

Choose from the below words
neon
fluorine
magnesium
argon
92.

Match each concept with its corresponding representation on the periodic table:

a)

an energy level

1.

Each row on the periodic table represents:

b)

a sublevel

2.

Each block on the periodic table represents:

c)

an electron

3.

Each element on the periodic table represents:

d)

an orbital

4.

Each section within a block on the periodic table represents:

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