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Chemistry Midterm Review

Total questions: 149

Worksheet time: 2hrs 17mins

Name
Class
Date
1.
How many neutrons does the isotope of lithium have?
a)
8
b)
3
c)
4
d)
5
2.
In a correctly written symbol what would be located in the "A" position?
a)
number of neutrons
b)
atomic number
c)
number of electrons 
d)
mass number
3.
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
4.
How many protons does this isotope of titanium have?
a)
48
b)
22
c)
26
d)
70
5.
If the number of electrons in an atom changes you make a(n) __________________.
a)
ion
b)
isotope
c)
new element
d)
isomer
6.
Ions are: 
a)
atoms with a positive or negative charge
b)
atoms with no charge
c)
atoms with ONLY a positive charge
d)
atoms with ONLY a negative charge
7.
How many electrons are in an atom that has an atomic number of 34, an atomic mass of 74 and a charge of -2?
a)
34
b)
36
c)
2
d)
40
8.
Two isotopes of carbon are carbon-12 and carbon-14.  These isotopes differ from one another by two protons.
a)
true
b)
false
9.
How many neutrons in C-14?
a)
6
b)
7
c)
14
d)
8
10.
which atom has  4 neutrons?
a)
Li-6
b)
Li-7
c)
Li-8
d)
they have the same # of neutrons
11.
How many neutrons does the isotope below have?     89 36Kr
a)
53
b)
36
c)
89
d)
125
12.
If X is the symbol for an element, which of the following two symbols represent    isotopes of the same element?     I. 7735X  II. 7733X  III. 8137X  IV. 8135 X
a)
I and II
b)
III and IV
c)
I and IV
d)
I and III
13.
An atom is electrically neutral when
a)
protons and neutrons are the same
b)
protons and electrons are the same
c)
neutrons and electrons are the same
d)
neutrons balance the protons and electrons
14.
Four isotopes of lead include lead-204, lead-206, lead-207, and lead-208.  The average atomic mass of lead is 207.2.  Which isotope of lead is likely to be the most abundant.
a)
204
b)
206
c)
207
d)
208
15.
How many neutrons does an atom of the isotope Neon-22 have?
a)
12
b)
10
c)
22
d)
20
16.
What do these isotopes of carbon all have in common?
a)
neutrons & mass number
b)
atomic number and neutrons
c)
atomic number and electrons
d)
protons, atomic number, and mass number
17.
Isotopes are atoms of the same element with different #’s of __________ & therefore different __________.
a)
n0 ;  atomic #’s
b)
p+ ; atomic #’s
c)
e- ; atomic masses
d)
n0 ; atomic masses
18.

The atomic number of an element is 14. What is the likely arrangement of the valence and core electrons in a neutral atom of this element?

a)

There are 2 valence electrons and 12 core electrons.

b)

There are 4 valence electrons and 10 core electrons.

c)

There are 5 valence electrons and 10 core electrons.

d)

There are 6 valence electrons and 8 core electrons.

19.

How many valence electrons does the chlorine atom have?

a)

3

b)

4

c)

8

d)

7

20.

This could be the dot diagram of

a)

Mg

b)

Cl

c)

C

d)

O

21.

This is a correct dot diagram for neon (Ne)

a)

true

b)

false

22.
This could be the dot diagram of
a)
Mg
b)
Cl
c)
C
d)
O
23.

How many electrons should sodium, atomic number 11, have around its Lewis dot model?

a)

1

b)

2

c)

3

d)

4

24.

How many valence electrons does Aluminum Have?

a)

1 Valence electron

b)

2 Valence electron

c)

3 Valence electron

d)

4 Valence electron

e)

5 Valence electron

25.

How would you draw a Lewis dot diagram for Magnesium?

a)
b)
c)
d)
26.

Which of these is correct?

a)
b)
c)
27.

Which Danish physicist proposed an atomic model that described electrons as moving in circular orbits around the nucleus?

a)

Niels Bohr

b)

Stephen Hawking

c)

Tycho Brahe

d)

Carl Sagan

28.

The amount of energy required to move an electron from one energy level to another is a _______ of energy. 

a)

atomic emission spectrum

b)

quantum

c)

energy level

d)

Ground State

29.

What is the lowest possible energy level that an electron can occupy?

a)

Lower energy level

b)

Excited State 

c)

Ground State

d)

Depressive State

30.

How does an electron get from a lower energy level to an excited state (higher energy level)? 

a)

It absorbs light

b)

it simply can do whatever it wants

c)

that's how the statistics describe it

d)

It emits light 

31.

Which of the following electronic transitions in the oxygen atom will result in light emission?

a)

ni​=1⟶nf​=2

b)

ni=3⟶nf=2ni​

c)

ni=1⟶nf=3

d)

ni=2⟶nf=3

32.

If the hydrogen atom emits red, blue-green, blue, and violet light, how many energy levels does it have in the visible region of the spectrum?

a)

3

b)

4

c)

5

d)

6

33.

How many electrons can occupy the lowest energy level? 

a)

1 only

b)

up to 2

c)

up to 4

d)

up to 8

34.

How many electrons can occupy the second energy level? 

a)

up to 2

b)

up to 4

c)

up to 6

d)

up to 8

35.

How many electrons are in the outer most energy level of Boron?

a)

1

b)

2

c)

3

d)

4

36.

How many electrons are in the outermost energy level of Chlorine (Cl)

a)

1

b)

3

c)

5

d)

7

37.

The quantum mechanical model describes the ______________ location of an electron and its __________ structure. (Select TWO ANSWERS)

a)

Most likely (probable)

b)

Definite

c)

2D

d)

3D

38.
1.  What is the shape of an s orbital?
a)
sphere
b)
dumbbell
c)
double dumbbell
d)
TOO COMPLEX TO KNOW IT.
39.
What is the shape of a p orbital?
a)
sphere
b)
it's just too complex to thing about it
c)
dumbbell
d)
I don't know this stuff.
40.
How many electrons can each p orbital hold?
a)
6
b)
3
c)
2
d)
4
41.
How many d orbitals are there in a given sublevel?
a)
1
b)
3
c)
5
d)
7
42.
How many p orbitals are there in a sublevel?
a)
2
b)
1
c)
4
d)
3
43.
How many electrons can the d sublevel hold?
a)
8
b)
10
c)
2
d)
4
44.
Which is associated with more energy? 
a)
2p
b)
2s
c)
3p
d)
1s
45.
Which orbital has the least amount of energy? 
a)
p orbital
b)
d orbital
c)
s orbital 
d)
What is an orbital?
46.

How many atoms are in 1 molecule of H2O?

a)

1

b)

2

c)

3

d)

4

47.

How many atoms are in 1 molecule of CH4?

a)

2

b)

3

c)

4

d)

5

48.

Which molecule has more atoms in it: CO or CO2?

a)

CO

b)

CO2

c)

They have the same number of atoms

49.

The simplest form of matter containing only one type of atom with its own particular set of properties is called a(n) ___.

a)

element

b)

ion

c)

mass

d)

molecule

50.

A combination of two or more atoms that can be the same or different is called a(n) ___.

a)

element

b)

isotope

c)

ion

d)

molecule

51.

The state of matter exhibiting the highest amount of kinetic energy is the __________ state.

a)

gas

b)

liquid

c)

solid

52.

Water vapor is in gaseous form. Water vapor molecules are held together by ________ attractive forces than ice.

a)

stronger

b)

the same

c)

weaker

53.

For a given element, in which state of matter would you expect it to have the greatest amount of POTENTIAL energy?

a)

gas

b)

liquid

c)

solid

54.

Which of the following are examples of matter? (select all that apply)

a)

electricity

b)

American flag

c)

temperature

d)

water

55.

Which of the following are examples of energy? (select all that apply)

a)

atoms

b)

heat

c)

kinetic

d)

potential

e)

zebra

56.
Which is a metal?
a)
Rhodium (Rh)
b)
Arsenic (As)
c)
Hydrogen
d)
Argon (Ar)
57.
Which is an alkaline earth metal?
a)
Calcium
b)
Rubidium
c)
Carbon
d)
Iodine
58.
Argon (Ar)
a)
alkali metal
b)
alkaline earth metal
c)
halogen
d)
noble gas
59.
Which of the following is the atomic number of an alkali metal?
a)
31
b)
20
c)
18
d)
19
60.
Which properties are characteristic of the Group 1 metals?
a)
high reactivity and the formation of unstable compounds
b)
low reactivity and the formation of unstable compounds
c)
high reactivity and the formation of stable compounds
d)
low reactivity and the formation of stable compounds
61.
What group on the Periodic Table contains the elements of the alkaline earth family?
a)
1
b)
2
c)
17
d)
18
62.
Which of the following in not a diatomic element?
a)
hydrogen
b)
carbon
c)
nitrogen
d)
oxygen
63.
What Periodic Table family is represented by the Lewis dot diagram?
a)
Halogens
b)
Alkali Metals
c)
Transition Metals
d)
Noble Gases
64.
Which of the following is the most reactive group of non-metals? 
a)
Alkali
b)
Alkali Earth
c)
Halogen
d)
Noble Gas
65.
How many valence electrons does an alkaline earth metal have? 
a)
1
b)
2
c)
7
d)
8
66.
How many valence electrons does a halogen have? 
a)
1
b)
2
c)
7
d)
8
67.

The elements in this family are soft, silvery, and very reactive with water.

a)

Alkaline Earth Metals

b)

Alkali Metals

c)

Transition Metals

d)

Lanthanides

68.

What group is the family found? These halides are very reactive and almost have full outer energy level/shell.

a)

1

b)

2

c)

16

d)

17

69.

The is family has properties of both metals and nonmetals.

a)

Alkali

b)

Halogens

c)

Nonmetals

d)

Metalloids

70.

This type of element is dull, brittle solids and gases, insulators, poor conductors of heat and electricity, as well as having low melting points.

a)

metals

b)

metalloids

c)

nonmetals

71.

Sulfur is a...

a)

metal

b)

nonmetal

c)

metalloid

72.
Radium (Ra)
a)
alkali metal
b)
alkaline earth metal
c)
halogen
d)
noble gas
73.
An atom that has the electron configuration of 1s22s22p63s23p64s23d5 is classified as
a)
A transition element
b)
a noble gas
c)
an alkali metal
d)
an alkaline earth metal
74.
Which element is not in the Alkali metal family?
a)
Li
b)
H
c)
Fr
d)
Cs 
75.
Gold (Au)
a)
Transition Metal
b)
Alkali Metal
c)
Alkaline Earth Metal
d)
Heavy Metal
76.

What is the atomic number of Cu?

a)

25

b)

26

c)

27

d)

29

77.

An element with 21 protons in each atom has an atomic number of:

a)

12

b)

21

c)

2

d)

24

78.

Which element has a mass number of 12 and contains 6 neutrons?

a)

Gallium

b)

Copper

c)

Carbon

d)

Sodium

79.

What is the mass number of a nitrogen atom that has 8 neutrons?

a)

15

b)

14

c)

22

d)

8

80.

What is true about the carbon atom depicted in the image?

a)

This carbon atom has 13 protons

b)

There are 13 subatomic particles in the electron cloud

c)

The mass number of this carbon atom is 13

d)

The atomic number of this carbon atom is 13

81.

(Multiple Answer Question)


Select the element(s) that has 8 valence electrons.

a)

Ne

b)

Br

c)

Kr

d)

Xe

82.

How many valence electrons does Boron have?

a)

1

b)

2

c)

3

d)

4

e)

5

83.

How many valence electrons does carbon have?

a)

4

b)

5

c)

6

d)

7

84.

USE THE PERIODIC TABLE

Find the element that has 5 Valence Electrons and 4 energy levels.


(Hint: Energy Levels = Number of Electrons Shells or Periods)

a)

Arsenic - As

b)

Selenium - Se

c)

Calcium - Ca

d)

Vanadium - V

85.

Two objects that are similarly charged will...

a)

attract.

b)

repel.

c)

not experience an electric force.

d)

implode.

86.

The Lewis Dot structure for aluminum would have ______ electrons.

a)

13

b)

3

c)

8

d)

27

87.

Valence electrons are those that are

a)

closest to the nucleus.

b)

freely floating between atoms.

c)

in the outermost energy level of the atom.

d)

unable to become involved in chemical bonding.

88.

Atoms that have gained electrons form

a)

cations.

b)

anions.

c)

negions.

d)

positrons.

89.

What is a cation's charge?

a)

positive

b)

negative

c)

neutral

d)

depends on the element

90.

This could be the dot diagram of

a)

Mg

b)

Cl

c)

C

d)

O

91.

How would you draw a Lewis dot diagram for Magnesium?

a)
b)
c)
d)
92.

What is the goal of the Lewis Dot Structure?

a)

To determine the electron position.

b)

To show the element's valence electrons & bonding capabilities.

c)

To find the atomic mass of an element.

d)

To search for the number of electrons in an individual atom.

93.
This is a correct dot diagram for fluorine (F)
a)
true
b)
false
94.
What element is represented in this Bohr Model? 
a)
Carbon
b)
Hydrogen
c)
Aluminum
d)
Lithium
95.

The majority of an atom's mass exists where?

a)

In the nucleus

b)

In the electron cloud

c)

In the space between the nucleus and the electrons

d)

In the neutrons

96.
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.
97.
The element with the smallest ionization energy in Period 6 is - 
a)
Rn
b)
Cs
c)
Os
d)
Tm
98.
Which has the greater Electronegativity: 
N or C?
a)
C
b)
N
99.
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. 
100.
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
101.
Families all have similar 
a)
Names
b)
atomic numbers
c)
atomic masses
d)
properties
102.
What is the name of family I
a)
Alkaline Earth Metals
b)
Boron Family
c)
Alkali Metals
d)
Halogen Family
103.
Group B is known as the:
a)
Inner Metals
b)
Transition Metals
c)
Weirdos
d)
Changelings 
104.
The energy required to remove electrons is the definition of: 
a)
Electronegativity
b)
Atomic Number
c)
Atomic Radius
d)
Ionization
105.
The atom with the largest atomic radius in Group 18 is - 
a)
Ar
b)
He
c)
Kr
d)
Rn
106.
As you move across the periodic table from left to right, the atomic radius decreases.  This is because - 
a)
the number of protons increases, so attraction to electrons increases
b)
the number of energy levels increases
c)
the number of electrons increases
d)
the atomic mass increases
107.
The atom with the largest atomic radius in Period 4 (row 4) is - 
a)
K
b)
Kr
c)
Fe
d)
Fe
108.
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
109.
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
110.

Na ionizes to a charge of _______

a)

+1

b)

+2

c)

-1

d)

-2

111.

Li ionizes to a charge of _________

a)

+2

b)

+1

c)

-1

d)

-2

112.

K ionizes to a charge of _________.

a)

+1

b)

+2

c)

-1

d)

-2

113.

Rb ionizes to a charge of _________.

a)

+2

b)

+1

c)

-1

d)

-2

114.

Be ionizes to a charge of ________.

a)

+1

b)

+2

c)

-1

d)

-2

115.

Mg ionizes to a charge of ______.

a)

+1

b)

+2

c)

-1

d)

-2

116.

Ca ionizes to a charge of _______.

a)

+1

b)

+2

c)

-1

d)

-2

117.

Sr ionizes to a charge of _________.

a)

+1

b)

+2

c)

-1

d)

-2

118.

Al ionizes to a charge of _______.

a)

+3

b)

-3

c)

+2

d)

-2

119.

N ionizes to a charge of _______.

a)

+3

b)

-3

c)

+2

d)

-2

120.

P ionizes to a charge of _______.

a)

+3

b)

-3

c)

+2

d)

-2

121.

As ionizes to a charge of _______.

a)

-3

b)

+3

c)

-2

d)

+2

122.

O ionizes to a charge of ________.

a)

+1

b)

+2

c)

-1

d)

-2

123.

S ionizes to a charge of _______.

a)

-2

b)

-1

c)

+1

d)

+2

124.

Se ionizes to a charge of _____.

a)

-2

b)

-1

c)

+1

d)

+2

125.

Te ionizes to a charge of ________.

a)

-2

b)

-1

c)

+2

d)

+1

126.

F ionizes to a charge of ________.

a)

-2

b)

-1

c)

+1

d)

+2

127.

Cl ionizes to a charge of _________.

a)

-2

b)

-1

c)

+1

d)

+2

128.

Br ionizes to a charge of ________

a)

-1

b)

-2

c)

+1

d)

+2

129.

I ionizes to a charge of _______.

a)

-1

b)

-2

c)

+1

d)

+2

130.

Which of the following could NOT form an ionic compound? Check all that apply.

a)

Li+ and Cl-

b)

F- and O2-

c)

Ba2+ and Ag+

d)

Mg2+ and S2-

131.

Which of the following could form an ionic compound? Check all that apply.

a)

Na+ and F-

b)

S2- and O2-

c)

Ca2+ and Fe3+

d)

Mg2+ and Cl-

132.

In an ionic bond, the ions are held together because...

a)

the positive nucleus of each ion attracts the other ion's negatively charged electrons

b)

the ions have opposite charges

c)

as the electron moved from one atom to another it pulled the atom along with it

d)

electrons are being shared

133.

Which element(s) will lose valence electrons to form an ion? Check all that apply.

a)

Phosphorus

b)

Iron

c)

Barium

d)

Neon

134.

Which element(s) will form negative ions? Check all that apply.

a)

Potassium

b)

Sulfur

c)

Iodine

d)

Magnesium

135.

Which of the following pairs of elements could NOT react to form an ionic compound?

a)

Carbon and Oxygen

b)

Potassium and Fluorine

c)

Silver and Oxygen

d)

Aluminum and Chlorine

136.

Calcium Fluoride has a chemical formula of CaF2. What does the chemical formula tell you?

a)

There are 2 Calcium ions for every 1 Fluoride ion in the crystal

b)

There is 1 Calcium ion for every 2 Fluoride ions in the crystal

137.

The following ionic crystal has 6 Fe ions (red) and 9 O ions (blue). What is the formula for this ionic crystal?

a)

FeO

b)

Fe2O3

c)

Fe3O2

d)

Fe6O9

138.

The following ionic crystal has 4 Sr ions (red) and 8 Br ions (blue). What is the formula for this ionic crystal?

a)

SrBr

b)

SrBr2

c)

Sr2Br

d)

Sr4Br8

139.

The following ionic crystal has 4 Al ions (red) and 6 O ions (blue). What is the formula for this ionic crystal?

a)

Al3O2

b)

Al4O5

c)

Al4O6

d)

Al2O3

140.

In which part of the periodic table are metals mostly found?

a)

At the top

b)

On the left

c)

On the right

141.

Which of these describes the arrangement of particles in a metal?

a)

Closely packed electrons with delocalised ions

b)

Alternating layers of metal ions and electrons

c)

Layers of metal ions surrounded by delocalised electrons

142.

How many electrons are delocalised in a metal?

a)

1

b)

2

c)

As many as are in the outer shell

143.

What does a metallic bond consist of?

a)

Forces between metal ions and delocalised electrons

b)

Pairs of metal atoms joined together by strong bonds

c)

Forces between oppositely charged metal ions

144.

Which of the following is NOT a property of a typical metal?

a)

Poor conductor of electricity

b)

High melting point

c)

Shiny

145.

What does 'malleable' mean?

a)

Able to be drawn into wires

b)

Able to conduct electricity

c)

Able to be hammered into thin sheets

146.

Which of these metals does NOT have a high melting point?

a)

Magnesium

b)

Mercury

c)

Silver

147.

Why are metals ductile?

a)

Because the metal is arranged in layers

b)

Because the metal ions are closely packed

c)

Because the metal can conduct electricity

148.

Why do metals conduct electricity?

a)

They have free-moving atoms

b)

They have free-moving ions

c)

They have free-moving electrons

149.

Why do metals have high melting points?

a)

Metallic bonds are weak and metals have a simple structure

b)

Metallic bonds are strong and metals have a lattice structure

c)

Metallic bonds are strong and metals have a simple structure

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