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Spring '24 Chemistry Midterm Practice

Total questions: 185

Worksheet time: 4hrs 33mins

Name
Class
Date
1.
What atom matches this electron configuration?
1s22s22p63s23p64s23d10
a)
Zinc
b)
Copper
c)
Nickel
d)
Germanium
2.
What atom matches this electron configuration?
1s22s22p63s2
a)
Neon
b)
Magnesium
c)
Aluminum
d)
Potassium
3.
What electron configuration matches an oxygen atom?
a)
1s22s22p63s2, 3p64s23d104p5
b)
1s22s22p4
c)
1s22s22p6
d)
1s22s22p63s23p64s23d1
4.
How many electrons does Si contain? (click to see image)
a)
14
b)
28
c)
2
d)
4
5.

What do you start all electron configurations with?

a)

1s2

b)

1d10

c)

1f14

d)

1p6

6.

What do you start all electron configurations with?

a)

1s2

b)

1d10

c)

1f14

d)

1p6

7.
Which element is pictured?
a)
neon
b)
fluorine
c)
magnesium
d)
argon
8.

Choose the correct electron configuration for Beryllium (Be).

a)

1s1

b)

1s2 2s2

c)

1s2 2s2 2p1

9.

Choose the correct electron configuration for Chlorine (Cl).

a)

1s2 2s2 2p1

b)

1s2 2s2 2p6 3s2

c)

1s2 2s2 2p6 3s2 3p5

10.

Choose the correct electron configuration for Nickel (Ni).

a)

1s2 2s2 2p6 3s2 3p6 4s2 3d8

b)

1s2 2s2 2p6 3s2 3p6 4s2 3d2

c)

1s2 2s2 2p6 3s2 3p6 4s10

11.
How many electrons should Carbon have around its Lewis dot model?
a)
1
b)
3
c)
4
d)
5
12.
According to the octet rule most elements need _______ valence electrons.
a)
2
b)
8
c)
6
d)
18
13.

This is a Bohr Diagram of Aluminum. How many valence electrons does Aluminum have?

a)

3

b)

4

c)

5

14.

How many valence electrons does Tin (Sn) have?

a)

8

b)

7

c)

5

d)

4

15.

How many valence electrons does Lithium (Li) have?

a)

8

b)

1

c)

5

d)

2

16.
This could be the dot diagram of 
a)
Ne
b)
Si
c)
Al
d)
Be
17.

How many valence electrons?

a)

2

b)

3

c)

4

d)

5

18.
a)
7
b)
8
c)
9
d)
10
19.

This could be the dot diagram of

a)

Mg

b)

Cl

c)

C

d)

O

20.

How many valence electrons are in this element?

a)

7

b)

6

c)

5

d)

2

21.

What is the process by which one or more substances are changed into one or more different substances?

a)

chemical equation

b)

change in state

c)

physical change

d)

chemical reaction

22.

What happens during a chemical reaction?

a)

new elements are created

b)

atoms are destroyed

c)

atoms are rearranged

d)

elements are destroyed

23.

In the following reaction, identify the products:

3Mg + 2FeCl3 →\rightarrow   2Fe + 3MgCl2

a)

Mg and Fe

b)

FeCl3 and MgCl2

c)

Mg and FeCl3

d)

Fe and MgCl2

24.

What is the whole number that appears in front of a formula in a chemical equation?

a)

a coefficient

b)

an exponent

c)

a subscript

d)

a superscript

25.

How many hydrogens are in 2NH4CH3COO?

a)

3

b)

4

c)

7

d)

14

26.

What symbol is used to represent the phrase “reacts with” in a chemical equation?

a)

an arrow

b)

a plus sign

c)

a coefficient

d)

an equal sign

27.

In the following reaction, identify the reactants:

3Mg + 2FeCl3 →\rightarrow   2Fe + 3MgCl2

a)

Mg and Fe

b)

FeCl3 and MgCl2

c)

Mg and FeCl3

d)

Fe and MgCl2

28.

How many atoms of oxygen are represented in 2Ca(NO3)2?

a)

4

b)

6

c)

10

d)

12

29.

Balance the following equation. What is the coefficient in front of the Carbon monoxide (CO)?

C + SO2 →\rightarrow   CS2 + CO

a)

2

b)

3

c)

4

d)

5

30.

Balance the following equation. What coefficient should be used for manganese?

Al + MnO →\rightarrow   Al2O3 + Mn

a)

1

b)

2

c)

3

d)

4

31.

What type of reaction is this?

2C2H2 + 5O2 →\rightarrow   4CO2 + 2H2O?

a)

Single Replacement

b)

Double Replacement

c)

Combustion

d)

Decomposition

32.

What type of reaction is this?

H2 + Cl2 →\rightarrow   2HCl?

a)

synthesis

b)

decomposition

c)

double replacement

d)

single replacement

33.

Balance the following equation. What coefficient is in front of NH4NO3?

(NH4)2SO4 + Ba(NO3)2 → NH4NO3 + BaSO4

a)

1

b)

2

c)

3

d)

4

34.

What is the best category to describe the reaction

KHCO3 →\rightarrow   CO2 + KOH?

a)

synthesis

b)

decomposition

c)

single replacement

d)

double replacement

35.

Balance the following equation. What coefficient goes in front of KOH?

KHCO3 →\rightarrow  CO2 + KOH?

a)

1

b)

2

c)

3

d)

4

36.
Cu + 2Ag(NO3) → 2Ag + Cu(NO3)
a)
Synthesis Reaction
b)
Decomposition Reaction
c)
Single Displacement Reaction
d)
Double Displacement Reaction
37.

The Law of Conservation of Matter

a)

tells how many atoms of an element are contained in one molecule or formula unit.

b)

the starting materials in a chemical reaction

c)

the new substances that are formed in a chemical reaction

d)

A law stating that atoms are not created or destroyed during a chemical reaction.

38.

What are the coefficients that would properly balance this equation?

__AgNO3 + __H2S --> __Ag2S+ __HNO3

a)

2,1 --> 1,2

b)

1,2 --> 1,1

c)

1,2 --> 1,2

d)

1,2 --> 2,1

39.

BONUS: Balance this reaction: ____ C5H14 + ____ O2 ----> ____ CO2 + ____ H2O

a)
1,8,5,7
b)
2,12,5,14
c)
3,27,15,24
d)
2,17,10,14
40.
KNO3 --> KNO2 + O2
What coefficients are needed to balance the reaction?
a)
2, 2, 1
b)
2, 3, 2
c)
1, 2, 2
d)
1, 3, 1
41.
Balance this equation.
_CH4 + _O2 --> _CO2 + _H2O
a)
1,2,1,1
b)
2,1,2,1
c)
1,2,1,2
d)
0,2,0,2
42.
Balance this equation
_N2 + _H2 --> _NH3
a)
1,2,3
b)
1,3,2
c)
1,1,2
d)
2,1,1
43.
Balance this equation-
__P4 + __O2 --> __P2O3
a)
it is already balanced
b)
2, 1, 3
c)
1, 2, 3
d)
1, 3, 2
44.

_FeCl3+ _H2SO4 →\rightarrow  _Fe2(SO4)3+ _HCl

a)

2, 3, 1, 6

b)

2, 2, 1, 6

c)

2, 2, 1, 5

d)

2, 3, 1, 5

45.

Which coefficients will balance the equation?

__Al(NO3)3 + __NaOH --> __Al(OH)3 + __NaNO3

a)

3,1,1,3

b)

1,3,1,3

c)

1,1,1,3

d)

1,3,6,2

46.

What are the coefficients that would balance the equation

__ Na3P + __ CaF2 --> __ Ca3P2 + __ NaF

(when you answer, separate the numbers by commas...NO SPACES)

(a)  

47.

What are the coefficients that would balance the following equation

__ CoBr3 + __ CaSO4 --> __ CaBr2 + __ Co2(SO4)3

(when you answer, separate the numbers by commas...NO SPACES)

(a)  

48.

Determine the coefficients to balance the equation.

__Al +__HCl --> __H2 +__AlCl3

a)

2,6,3,2

b)

it's already balanced

c)

4,12,3,4

d)

2,1,4,5

49.

Balance the following equation:

___ SeCl6+ ___ O2→___ SeO2+____Cl2

a)

1, 1, 1, 3

b)

2, 1, 2, 1

c)

1, 2, 1, 2

d)

2, 2, 2, 4

50.
What is the little number after an element in a chemical equation called.
Example: H2
a)
Coefficient 
b)
Subscript
c)
Atom
d)
Equation
51.
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
52.
The more protons there are, the  ____ .
a)
Weaker the pull
b)
Smaller the electrons
c)
Stronger the pull
d)
The bigger the electrons
53.
Which one has the largest radius?
a)
Lithium (Li, atomic #3)
b)
Boron (B, atomic #5)
c)
Neon (Ne, atomic #10)
d)
Nitrogen (N, atomic #7)
54.

Which of these best explains the reasoning behind the trend that as you go across a period, size decreases?

a)

As you go across a period, more energy levels are added, which shrinks the atom.

b)

The added electrons in the nucleus give the atom a negative charge, which shrinks the atom.

c)

The added protons in the nucleus pull the electrons closer to them, which shrinks the atom.

d)

All of the above

55.

Which atom in the list below has the largest atomic radius?

a)

Argon (Ar)

b)

Helium (He)

c)

Krypton (Kr)

d)

Radon (Rn)

56.

Which element's atom is the smallest?

a)

Rhodium

b)

Silver

c)

Cadmium

d)

Tin

57.
Which of the following elements has the smallest atomic radius: Li, O, C, F?
a)
Li
b)
O
c)
C
d)
F
58.
Of the elements Ca, Be, Ba, and Sr, which has the largest atomic radius?
a)
Be
b)
Ba
c)
Ca
d)
Sr
59.

Across a period, Ionization energy ____a____

Down a group, ionisation energy ____b_____

a)

a : increase

b: decrease

b)

a : increase

b: increase

c)

a : decrease

b: decrease

60.

Which element has the greatest ionization energy: Aluminum (Al)    or    Chlorine (Cl)?

a)

Aluminum (Al)

b)

Chlorine (Cl)

61.
Which of the following is true about a sulfur atom and a chlorine atom?
a)
Sulfur is larger and has higher ionization energy.
b)
Sulfur is larger and has lower ionization energy.
c)
Sulfur is smaller and has higher ionization energy.
d)
Sulfur is smaller and has lower ionization energy.
62.
Which element has the greater ionization energy?
a)
Strontium
b)
Boron
63.
Which element has the greater ionization energy?
a)
Lead
b)
Silicon
64.
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
65.
Put the following in order of increasing ionization energy:Sodium, Oxygen, Boron
a)
Sodium, Boron, Oxygen
b)
Oxygen, Boron, Sodium
c)
Sodium, Oxygen, Boron
d)
Oxygen, Sodium, Boron
66.

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

67.

When going down a group, the atomic size increases. This means the first IE __________.

a)

increases

b)

decreases

c)

remains constant

d)

I am not sure

68.

Which element has the greater ionization energy?

a)

Iodine (I)

b)

Chlorine (Cl)

69.
Define electron affinity.
a)
The energy it takes to add an electron to an atom.
b)
The energy it takes to remove an electron from an atom.
70.
Elements closer to the noble gases have stronger attraction for electrons.
a)
True
b)
False
71.

As you move left to right across a period, electron affinity

a)

increases

b)

decreases

72.

As you move down a group, electron affinity

a)

increases

b)

decreases

73.

Which of these has a greater need for electrons?

a)

Ca

b)

Ba

74.

Which of these has a greater electron affinity?

a)

Na

b)

K

75.

Which of these has a greater electron affinity?

a)

P

b)

Cl

76.

Which of these has a greater electron affinity?

a)

Si

b)

Cl

77.

Which of these has a greater electron affinity?

a)

Li

b)

K

78.
Choose the set that goes from lowest to highest electronegativity?
a)
Cu, Mg, Sr, Ca
b)
F, Cl, Br, Si
c)
Cs, Rb, Ca, Mg
d)
Zn, Cd, Ag, Cu
79.
The element with the largest electronegativity in the halogens is - 
a)
At
b)
F
c)
Cl
d)
Br
80.
Which of the following is the least electronegative element?
a)
oxygen
b)
potassium
c)
fluorine
d)
nitrogen
81.
Which of the following is the most electronegative element?
a)
nitrogen
b)
phosphorus
c)
arsenic
d)
lithium
82.
Put these in order of increasing electronegativity:
Se, S, and O
a)
Se < S < O
b)
Se < O < S
c)
O < S < Se
d)
S < Se < O
83.
Chlorine and Fluorine are both very electronegative, as they are both missing a single electron from their valence energy level.  Why is Fluorine more electronegative than Chlorine? 
a)
Fluorine has less energy levels.
b)
Chlorine has more electrons in its outer shell
c)
Fluorine has more protons.
d)
None of these
84.
What elements have zero electronegativity?
a)
metals
b)
nonmetals
c)
metalloids
d)
noble gases
85.

Which element has a higher electronegativity value?

a)

Niobium

b)

Tin

c)

Cadmium

d)

Iodine

86.

Which element has a lower electronegativity value?

a)

Calcium

b)

Barium

87.

What does electronegativity do as you go across a period?

a)

decrease

b)

no pattern

c)

stay the same

d)

increase

88.

How do you write the formula for Sodium Chloride?

a)

NaCl2

b)

NaCl

c)

KI

89.

What is the name of LiF?

a)

Lithiide Fluorine

b)

Lithium Monofluride

c)

Lithium Fluoride

d)

Lithium Phosphine

90.

What is the formula for Gallium Nitride?

a)

GaN

b)

Ga (III) N

c)

GeN

d)

GaNi

91.

What is the formula for magnesium phosphide?

a)

Mg3P2

b)

Mg2P3

92.

What is the formula for potassium and oxygen?

a)
KO.
b)
K2O.
c)
K2O2.
d)
KO2.
93.
Name this compound: 
NaBr
a)
Bromide sodide
b)
Sodium bromide
c)
Sodium bromate
d)
Sodium bromite
94.

Name this compound:

KF

a)

Potassium fluoride

b)

Potassium monofluorite

c)

Fluorine potasside

d)

Potassium monofluoride

95.
What is the correct formula for Sodium Oxide?
a)
NaO
b)
NaO2
c)
Na2O
d)
Na2O2
96.

LiBr is called

a)

lithium monobromine

b)

lithium (I) bromine

c)

lithium bromide

d)

lithuim (I) bromide

97.

Name the ionic compound SnSe2

a)

Tin diselenide

b)

Tin (IV) Selenide

c)

Tin selenide

d)

Tin (II) triselenide

98.

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

a)

Sodium sulfate

b)

Sodium sulfide

c)

Sodium sulfite

d)

Sodium sulfuroxide

99.

What is the name of the compound Sc(OH)3?

a)

Scandium (III) hydroxide

b)

Scandium (I) hydroxide

c)

Scandium (II) hydroxide

d)

Scandium hydroxide

100.

The name of the compound Ca3(PO4)2

a)

calcium phosphate

b)

tricalcium diphosphate

c)

calcium phosphorus oxide

d)

calcium phosphide

101.

What is the name of the following compound: CuBr2

a)

copper bromine

b)

copper bromide

c)

copper (I) bromide

d)

copper (II) bromide

102.

What is the name of the following compound: K2SO4

a)

potassium sulfur

b)

potassium sulfate

c)

potassium (I) sulfate

d)

potassium (II) sulfide

103.

Which is the correct formula for the compound: lead (II) fluoride

a)

Pb2F

b)

PbF2

c)

PbF

d)

PbF7

104.

What is the what charge of lead in the compound: lead (IV) iodide

a)

+1

b)

+4

c)

+6

d)

-1

105.

Which of the following combinations would need roman numerals in the name?

a)

potassium + fluorine

b)

beryllium + oxygen

c)

boron + iodine

d)

lead + oxygen

106.

What is the correct molecular formula for barium hydroxide?

a)

Ba(OH)2

b)

Ba2OH

c)

BaOH

d)

Ba2OH

107.
What is the formula for copper(I) sulfate?
a)
CuSO3
b)
CuSO4
c)
Cu2SO3
d)
Cu2SO4
108.

An alpha particle is made up of

a)

2 protons and 4 neutrons

b)

1 proton and 1 neutron

c)

2 protons and 2 neutrons

d)

4 protons and 2 neutrons

109.

Gamma rays have

a)

no mass

b)

a huge mass

c)

a small mass

d)

an average mass

110.

The particle emitted in beta decay is a ____________________.

a)

a proton

b)

an electron

c)

a neutron

111.
Complete the nuclear equation and determine the type of decay that is occurring in this reaction. 
a)
alpha
b)
beta
c)
gamma
d)
none
112.

The % of the parent isotope remaining after 1 Half Life.

a)

50%

b)

25%

c)

12.5%

d)

6.25%

113.
What is Half-life?
a)
The amount of time it takes for some of the nuclei in a sample of the isotope to decay
b)
The amount of time it takes for half the electrons in a sample of the isotope to decay
c)
The amount of time it takes for half the nuclei in a sample of the isotope to decay
d)
the amount of time it takes to double the nuclei in a sample of the isotope to decay
114.
What is the half-life of iodine-131?
a)
32 days
b)
8 days
c)
16 days
d)
24 days
115.
If 10 mg of iodine 131 is given to a patient, how much is left after 24 days? The half-life of iodine-131 is 8 days.
a)
1.25mg
b)
1.25g
c)
10g
d)
10mg
116.
The half-life of strontium-90 is 25 years. How much strontium-90 will remain after 100 years if the initial amount is 4.0 g?
a)
3.0g
b)

2.5g

c)
0.3g
d)
0.25g
117.

What is the Half life of this isotope?

a)

5 seconds

b)

10 seconds

c)

15 seconds

d)

20 seconds

118.
Who discovered that the nucleus contains positively charged particles called protons?
a)
Ernest Rutherford
b)
James Chadwick
c)
Democritus
d)
Niels Bohr
119.
Who discovered the electron?
a)
Niels Bohr
b)
Democritus
c)
Joseph Thomson
d)
John Dalton
120.

Used the word "atomos" to decsribe the uncuttable (indivisible) atom.

a)

Democritus

b)

Thomson

c)

Bohr

d)

Dalton

121.

Proposed that electrons move around the nucleus in specific layers, or shells.

a)

Bohr

b)

Rutherford

c)

Chadwick

d)

Thomson

122.

This picture best represents ___________________ atomic model.

a)

Thomson's

b)

Dalton's

c)

Bohr's

d)

Chadwick's

123.

The scientist that discovered a positive center of an atom.

a)

Millikan

b)

Rutherford

c)

Dalton

d)

Thomson

124.
This model of the atom described atoms as tiny spheres that could not be broken down into smaller pieces.
a)
Dalton's model of the atom
b)
The "Plum Pudding Model" of the atom
c)
The Nuclear Model
d)
The Bohr Model
125.
What Greek philosopher first spoke about the idea of an atom?
a)
Democritus
b)
Dalton
c)
Thompson
d)
Rutherford
126.
Who performed the Gold Foil Experiment?
a)
J. J. Thomson
b)
Ernest Rutherford
c)
Neils Bohr
d)
John Dalton
127.

Who developed the idea that electrons are found in a cloud?

a)

Bohr

b)

Dalton

c)

Schrodinger

d)

Rutherford

128.

Which scientist discovered that the nucleus contained neutrons?

a)

bohr

b)

Rutherford

c)

Dalton

d)

Chadwick

129.
Who developed the Quantum Mechanical Model?
a)
Erwin Schrodinger
b)
Joseph Thomson
c)
James Chadwick
d)
Ernest Rutherford
130.
"Electrons have particle and wave-like properties."
a)
Planck
b)
Heisenberg
c)
de Broglie
d)
Schrodinger
131.
The position & momentum of the electron cannot be known at the same time. 
a)
Planck
b)
Heisenberg
c)
de Broglie
d)
Schrodinger
132.

Who created this atom model?

a)

Heisenberg and Schrodinger

b)

Thomson

c)

Rutherford

d)

Bohr

133.

Which scientist is given credit for discovering the electron?

a)

Bohr

b)

Dalton

c)

Thomson

d)

Rutherford

134.

Who discovered that electrons travel in specific orbits around the nucleus?

a)

Bohr

b)

Schrodinger

c)

Democritus

d)

Rutherford

135.

Who was the first person to say that matter was made of atoms, and these atoms could not be created or destroyed?

a)

Dalton

b)

Democritus

c)

Rutherford

d)

Thomson

136.

Whose model of the atom is known as the "plum pudding" model (aka the "chocolate chip cookie" model)?

a)

Rutherford

b)

Schrodinger

c)

Dalton

d)

Thomson

137.

Whose gold foil experiment led to his conclusion that the nucleus of an atom contained protons?

a)

Rutherford

b)

Bohr

c)

Thomson

d)

Dalton

138.

Who developed the idea that electrons are found in a cloud?

a)

Bohr

b)

Dalton

c)

Schrodinger

d)

Rutherford

139.

Whose model of the atom is represented in the image?

a)

Thomson

b)

Bohr

c)

Dalton

d)

Rutherford

140.

Whose model is the most modern interpretation of an atom?

a)

Dalton

b)

Democritus

c)

Rutherford

d)

Schrodinger

141.

The Cathode Ray Tube experiment led to this model that was developed by ___.

a)

JJ Thomson

b)

John Dalton

c)

Ernest Rutherford

d)

Democritus

142.

Protons have what type of charge?

a)

Positive

b)

Negative

c)

Neutral

143.

The nucleus is comprised of ___

a)

Protons and Electrons

b)

Protons and Neutrons

c)

Neutrons and Electrons

d)

Just Protons

144.

Neutrons have what kind of charge?

a)

Neutral

b)

Positive

c)

Negative

145.

Electrons have what kind of charge?

a)

Positive

b)

Negative

c)

Neutral

146.

Which option is NOT part of Dalton's Atomic Theory of Matter

a)

All matter is made of atoms

b)

Atoms join together with other atoms to make new substances

c)

Atoms have a defined nucleus

d)

Atoms of the same element are alike, and atoms of different elements are different.

147.

Which subatomic particle was found to be 2000 times lighter than a single hydrogen atom?

a)

The proton

b)

The electron

c)

The neutron

148.
How do covalent bonds form?
a)
Donating & receiving valence e- between atoms.
b)
Opposite slight charges attract each other between compounds.
c)
Scientists are still not sure how they form.
d)
Sharing valence e- between atoms.
149.
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
150.
What is the correct name for C4H6?
a)
Carbon Hexahydride
b)
Pentacarbon Pentahydride
c)
Hexacarbon Tetrahydride
d)
Tetracarbon Hexahydride
151.
What is the formula for Tricarbon Octahydride?
a)
Ca3O
b)
C2H8
c)
C3H8
d)
Ca3H8
152.
What is Sulfur Trichloride?
a)
SCl3
b)
SiCl3
c)
SCl4
d)
Si3Cl
153.
A covalent compound made of one sulfur and two oxygen atoms would be named
a)
sulfur dioxide.
b)
sulfur oxide.
c)
disulfur oxide.
d)
sulfide oxygen.
154.
The covalent compound N2O5 would be named
a)
nitrogen oxide.
b)
dinitrogen oxide.
c)
nitrogen pentoxide.
d)
dinitrogen pentoxide.
155.

How are covalent bonds formed?

a)

Sharing of electrons

b)

Giving of electrons

c)

Taking of electrons

d)

Transferring electrons

156.

How many total electrons are shared in a single bond such as one shown in this Hydrogen Molecule (H2)?

a)

1

b)

2

c)

3

d)

4

157.
Name the following compound: 
CO2
a)
monocarbon dioxide
b)
carbon oxide
c)
carbon dioxide
d)
oxygen carbonide
158.
In a covalent bond, one or more electrons are? 
a)
shared 
b)
lost 
c)
gained 
d)
transferred 
159.

In the water molecule shown, H2O, the electrons are NOT shared equally forming a slight positive side and a slight negative side. This is what kind of bond?

a)

Polar Covalent

b)

Non-Polar Covalent

c)

Ionic Covalent

d)

James Bond Covalent

160.

In the hydrogen molecule (H2) shown here, the electrons are share equally between the 2 hydrogen molecules. This is what kind of bond?

a)

Polar Covalent

b)

Non-Polar Covalent

c)

Ionic Covalent

d)

James Bond Covalent

161.

Dr. "HOFBrINCl" was the name of a famous professor who also taught me "Have No Fear Of Ice Cold Beverages."

Which of the following is NOT a diatomic molecule?

a)

Hydrogen

b)

Fluorine

c)

Boron

d)

Chlorine

162.
What is the correct formula for this molecule?
a)
NH
b)
N3H
c)
NH3
d)
NH4
163.
The chemical formula of dinitrogen textroxide is
a)
Ni₂O₄
b)
NiO
c)
N₂O₄
d)
NiO₂
164.
What is the correct name for NO?
a)
Mononitrogen Monoxide
b)
Nitrogen Monoxide
c)
Mononitrogen Dioxide
d)
Nitrogen Oxide
165.

A covalent compound made of one nitrogen and 3 bromine atoms would be named

a)

nitrogen bromide

b)

mononitrogen tribromide

c)

tribromine mononitride

d)

nitrogen tribromide

166.

Which of these is NOT a rule for naming covalent compounds?

a)

First element name stays the same

b)

Second element name changes ending to -ide

c)

Use Prefixes like "di-" or "tri-" etc on the names

d)

Always use every prefix on all elements

167.

How many valence electrons do atoms want to have in order to be stable?

a)

3

b)

1

c)

8

d)

4

168.

An atom that has gained or lost an electron is called a(n) _____.

a)

ion

b)

particle

c)

atom

169.

When ions LOSE electrons they become ____ charged.

a)

positively

b)

negatively

c)

same

170.

When ions GAIN electrons, they become _____ charged.

a)

postively

b)

negatively

c)

same

171.
In order to have a stable arrangement of 8 valence electrons, metal atoms are likely to _________electrons.
a)
gain
b)
lose
172.
Ionic bonds are between...
a)
Metal and Non-metal
b)
Non-metal and Non-metal
c)
Metal and Metal
173.
How are ionic bonds formed?
a)
Transfer of electrons
b)
Sharing of electrons
174.
Why do elements bond?
a)
To be friends
b)
To create a new element
c)
To become stable
175.
Where are the nonmetals located on the periodic table? 
a)
Blue
b)
Red
c)
Green
176.
Where are metals located on the periodic table?
a)
Blue
b)
Green
c)
Red
177.
Ionic bonds form between two ions that have...
a)
ionic compounds
b)
negative charges
c)
positive charges
d)
opposite charges
178.

What type of elements form cations?

a)

metals

b)

nonmetals

c)

metalloids?

179.

Anions

a)

Gain electrons, has an overall positive charge

b)

Lose electrons, has an overall positive charge

c)

Lose electrons, has an overall negative charge

d)

Gain electrons, has an overall negative charge

180.

Cations

a)

Gain electrons, has an overall positive charge

b)

Lose electrons, has an overall positive charge

c)

Lose electrons, has an overall negative charge

d)

Gain electrons, has an overall negative charge

181.

How does calcium become an calcium ion?

a)

it loses 2 electrons

b)

it gains 2 electrons

182.

How does magnesium become an magnesium ion?

a)

it loses 2 electrons

b)

it gains 2 electrons

183.

How does oxygen become an oxide ion?

a)

it loses 2 electrons

b)

it gains 2 electrons

184.
Is this ionic bond drawn correctly?
a)
Yes
b)
No
185.

How many Aluminum atoms are in Al2O3?

a)

3

b)

5

c)

2

d)

1

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