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Chemistry Fall Final Review 2024

Total questions: 172

Worksheet time: 2hrs 21mins

Name
Class
Date
1.

What is the best graph to use when graphing data that is showing something happening over time?

a)

Bar graph

b)

Line graph

c)

Pie chart

d)

Histogram

2.

What is the best graph to use when graphing data that is given in percentages (parts of a whole)?

a)

Bar graph

b)

Line graph

c)

Pie chart

d)

Scatter plot

3.

A hypothesis is a testable statement developed from observations.

a)

A guess based on intuition

b)

A testable statement developed from observations

c)

A proven fact

d)

A random idea

4.

What is the purpose of a controlled experiment?

a)

To test multiple variables at once

b)

To isolate and test the effect of a single variable

c)

To prove a hypothesis correct

d)

To collect as much data as possible

5.

What is the INDEPENDENT variable in an experiment?

a)

The variable that is measured

b)

The variable that is changed or controlled

c)

The variable that remains constant

d)

The variable that is dependent on others

6.

What is the DENSITY of an object? What are the UNITS used to measure density?

a)

Mass per unit volume, measured in kg/m³

b)

Volume per unit mass, measured in m³/kg

c)

Mass per unit area, measured in kg/m²

d)

Volume per unit area, measured in m²/kg

7.

What are the three major subatomic particles that comprise (make up) an atom?

a)

Protons, neutrons, electrons

b)

Atoms, molecules, ions

c)

Quarks, leptons, bosons

d)

Nuclei, shells, orbitals

8.

What is 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 electrons

d)

Atoms with different numbers of protons and neutrons

9.

What is the electron configuration for Sulfur and what is the shorthand/Noble gas configuration for Sulfur?

a)

1s² 2s² 2p⁶ 3s² 3p⁴; [Ne] 3s² 3p⁴

b)

1s² 2s² 2p⁶ 3s² 3p⁶; [Ar] 3s² 3p⁶

c)

1s² 2s² 2p⁶ 3s² 3p²; [He] 2s² 2p⁶

d)

1s² 2s² 2p⁶ 3s² 3p³; [Ne] 3s² 3p³

10.

What are the two names for vertical rows in the periodic table?

a)

Groups and Periods

b)

Columns and Rows

c)

Families and Series

d)

Lines and Sections

11.

What is the name for the horizontal rows in the periodic table?

a)

Groups

b)

Periods

c)

Columns

d)

Families

12.

Which elements on the periodic table might have more than one charge if they become ionic?

a)

Alkali metals

b)

Transition metals

c)

Noble gases

d)

Halogens

13.

Are these multi charge elements metals or nonmetals?

a)

Metals

b)

Nonmetals

c)

Metalloids

d)

Noble gases

14.

Where are p elements found?

a)

In the s block

b)

In the p block

c)

In the d block

d)

In the f block

15.

Which element has the greatest electronegativity?

a)

Fluorine, because it is the most reactive

b)

Oxygen, because it is a gas

c)

Chlorine, because it is a halogen

d)

Helium, because it is a noble gas

16.

Which element has the LARGEST atomic radius on the periodic table?

a)

Helium, because it is a noble gas

b)

Francium, because it is at the bottom of the group

c)

Hydrogen, because it is the lightest

d)

Carbon, because it is in the middle of the table

17.

What is the difference between a cation and an anion?

a)

Cations are negative, anions are positive

b)

Cations are positive, anions are negative

c)

Cations are neutral, anions are charged

d)

Cations are charged, anions are neutral

18.

What are the rules for NAMING an ionic compound?

a)

Use prefixes for both elements

b)

Name the metal first, then the nonmetal with an -ide ending

c)

Name the nonmetal first, then the metal with an -ide ending

d)

Use Roman numerals for both elements

19.
How many significant figures: 216 m
a)
1
b)
2
c)
3
d)
0
20.
How many significant figures: 2016 m
a)
1
b)
2
c)
3
d)
4
21.
How many significant figures: 153.0 mL
a)
1
b)
2
c)
3
d)
4
22.
How many significant figures: 0.012 km
a)
1
b)
2
c)
3
d)
4
23.
How many significant figures: 1000 mL
a)
1
b)
2
c)
3
d)
4
24.
How many significant figures: 100.000 cL
a)
1
b)
3
c)
5
d)
6
25.

Which of the following is true about a scientific theory?

a)

a scientific theory is an explanation

b)

scientific theories will eventually become scientific laws

c)

scientific theories are not supported by evidence

d)

scientific theories are usually rejected because they are only theories

26.

What is the difference between a scientific theory and a scientific law?

a)

Theories and laws are the same thing: there is no difference.

b)

A theory will eventually become a law after a long period of time.

c)

A theory is an explanation of the natural world and a law is a description of the natural world.

d)

Theories and laws switch back and forth depending on the situation.

27.

Which of the following best describes a hypothesis?

a)

A hypothesis is an educated guess to a parent's question.

b)

A hypothesis is the probability an event will occur such as winning the lottery.

c)

A hypothesis is a prediction about what will happen based on observations and evidence.

d)

A hypothesis occurs when you fall into freezing water and become very, very cold.

28.

Explains something we see in the natural world that has been verified through repeated experiments or testing.

a)

hypothesis

b)

law

c)

theory

d)

Inference

29.

This variable is the one thing that changed on purpose...

a)

Dependent Variable

b)

Control

c)

Independent Variable

30.

What is the DEPENDENT variable (effect) in this experiment?


"Does eating breakfast improve test scores?"

a)

eating breakfast or not

b)

the grade you got on the test

c)

what time you get up in the morning

d)

how tasty the breakfast is

31.

You are testing how the amount you water a plant affects its growth. What would be the INDEPENDENT VARIABLE in this experiment.

a)

They type of pot you put the plants in.

b)

The amount you water each plant.

c)

The amount of sunlight the plants get.

d)

The amount the plant grows.

32.

What are the constant variables?

a)

what we are changing or testing

b)

what we are observing or measuring

c)

what we keep the same to make the experiment fair

33.

Which correctly describes the smallest amount of an element?

a)

Atom

b)

Molecule

c)

Compound

d)

Proton

34.

How would H2O be classified? Check all that apply.

a)

Atom

b)

Molecule

c)

Compound

35.

How would O2 be qualified. Check all answers that apply.

a)

Atom

b)

Molecule

c)

Compound

36.
What is the number of protons that the element in this image contain?
a)
14
b)
7
c)
15
d)
18
37.
What is the number of protons that the element in this image contain?
a)
14
b)
7
c)
15
d)
18
38.
The positive particles of an atom are 
a)
Electrons 
b)
Positrons 
c)
Neutrons 
d)
Protons 
39.
The central region of an atom where its neutrons and protons are is its _______.
a)
Nucleus 
b)
Electron cloud
c)
Core 
d)
Center 
40.
An atom with atomic number 6 would have how many protons?
a)
6
b)
12
c)
3
d)
Cannot be determined 
41.
Particles in an atom that are neutral and have no charge are ______. 
a)
Negatrons 
b)
Electrons 
c)
Neutrons 
d)
Protons 
42.
Which of the following is a negatively charged subatomic particle?
a)
Electron
b)
Proton
c)
Neutron
d)
Quark
43.
The particles that are found in the nucleus of an atom are _____.
a)
Neutrons and electrons
b)
Electrons only
c)
Protons and neutrons
d)
Protons and electrons
44.
The atomic number of an elements is the total number of which particles in the nucleus?
a)
Neutrons
b)
Protons
c)
Electrons
d)
Protons and electrons
45.
Where are electrons of an atom found?
a)
Nucleus
b)
Electron Cloud
c)
Some are in the nucleus and some in the electron cloud.
d)
They are moving everywhere.
46.
Most of the mass in an atom is concentrated in the _____.
a)
Electrons
b)
Nucleus
c)
Protons
d)
Empty space
47.
What are the 3 particles that make-up the atom?
a)
Protons, neutrons, and isotopes
b)
Neutrons, isotopes, and electrons
c)
Positives, negatives, and electrons
d)
Protons, neutrons, and electrons
48.

What does the 1.00794 stand for?

a)

Hydrogen

b)

atomic number

c)

atomic mass

d)

atomic explosion

49.

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

50.

If an atom has 10 protons, 10 neutrons, and 10 electrons, what is the mass of the atom?

a)

10

b)

20

c)

30

51.
What is the atomic mass of "F"
a)
9
b)
18
c)
17
d)
19
52.
How many protons are in an atom of carbon?
a)
12.01
b)
8
c)
6
d)
14
53.

Which number here is the atomic number?

a)

5

b)

10.811

54.
What did Democritus, Dalton, Thomson, Rutherford, and Bohr all have in common?
a)
They were all cool dudes.
b)
They each identified new isotopes of atoms.
c)
They each contributed to the development of the atomic theory.
d)
They each designed a new building.
55.
What did Democritus, Dalton, Thomson, Rutherford, and Bohr all have in common?
a)
They were all cool dudes.
b)
They each identified new isotopes of atoms.
c)
They each contributed to the development of the atomic theory.
d)
They each designed a new building.
56.
all matter is made of what 
a)
energy 
b)
atoms 
c)
electrons 
d)
compounds 
57.
The positive particles of an atom are 
a)
electrons 
b)
positrons 
c)
neutrons 
d)
protons 
58.
the central region of an atom where its neutrons and protons are is its 
a)
nucleus 
b)
electron cloud
c)
core 
d)
center 
59.
True or False? Neutrons have a negative charge
a)
True
b)
False
60.
Element or compound?
O2
a)
Element
b)
Compound
61.
 What is at the center of every atom? 
a)
nucleus
b)
neutron
c)
proton
d)
all of these 
62.
 An atom is neutral if...    
a)
The number of protons = electrons
b)
The number of neutrons = protons
c)
The number of protons∠ electrons
d)
 Electrons+Neutrons = 0
63.
The smallest common particle in the atom...   
a)
electron
b)
proton
c)
nucleus 
d)
neutron
64.
Neutrons are important because...      
a)
They hold the nucleus together
b)
They have a positive charge
c)
 They orbit outside of the atom
d)
All of these
65.
____ with specific characteristics and is made up of only one atom 
a)
protron
b)
8
c)
chemical
d)
Element
66.
vertical columns in the periodic table are _________ of elements with similar properties. 
a)
groups
b)
periods
67.
_______ are horizontal  rows of elements that contain increasing numbers of protons and electrons.
a)
groups
b)
periods
68.
an atom with atomic number 6 would have how many protons 
a)
6
b)
12
c)
3
d)
cannot be determined 
69.
Which element is this on the periodic table?
a)
3rd element
b)
7th element
c)
13th element
d)
6th element
70.
Which of the following determines the identity of an element?
a)
atomic number 
b)
mass number
c)
atomic mass
d)
overall charge
71.
Two atoms of the same element but with different mass numbers are called________
a)
electrons
b)
isotopes
c)
variables
d)
electron cloud
72.
What does the 1.00794 stand for?
a)
Hydrogen
b)
atomic number
c)
atomic mass
d)
atomic explosion
73.

The _ is a small, dense region at the center of the atom. It consists of positive protons and neutral neutrons, so it has an overall positive charge.

a)

protons

b)

neutrons

c)

nucleus

d)

electrons

74.

Physical science is the study of matter and energy. It includes all but:

a)

physics

b)

biology

c)

chemistry

75.
What makes something radioactive?
a)
elements with an atomic number above 81
b)
an unstable nucleus
c)
contaminated sewage
d)
It decays over time
76.
The half life of iodine-131 is 8.040 days. What percentage of an iodine-131 sample will remain after 40.20 days?
a)
312.5%
b)
31.25%
c)
.3125%
d)
3.125%
77.
Takes two small nuclei and combines them into a larger nucleus
a)
fission
b)
fusion
78.
The splitting of a nucleus into smaller nuclei is
a)
fusion
b)
fission
c)
half-life
d)
gamma radiation
79.
How is nuclear fusion different from nuclear fission?
a)
In fusion, the product is a larger atomic nucleus.
b)
Fission produces energy but fusion does not.
c)
Fusion produces energy but fission does not.
d)
In fission, the product is a larger atomic nucleus.
80.

When nuclei decay, massive amounts of __________ is released.

a)

energy

b)

electrons

c)

protons

d)

neutrons

81.

Process by which nuclei having small masses combine to form a nucleus with a heavier mass is...

a)

nuclear fission

b)

a chemical reaction

c)

nuclear fusion

d)

a chain reaction

82.

The force that holds neutrons and protons together in the nucleus is known as the:

a)

weak nuclear force

b)

hydrogen bonding

c)

strong nuclear force

d)

electronegative force

83.

Atoms of the same element that have different numbers of neutrons and different mass numbers:

a)

nucleons

b)

isotopes

c)

gamma rays

d)

ions

84.

You have 20 grams of uranium that has a half-life of 2 seconds, how much will be left after 4 seconds?

a)

5 grams

b)

2 seconds

c)

6 grams

d)

8 grams

85.
The time taken for half of an amount of radioactive atoms to decay.
a)
Nuclear fusion
b)
Full-life
c)
Dead time
d)
Half-life
86.

Nuclear fission of uranium-235 can start a chain reaction by

a)

releasing enough thermal energy to start nuclear fission in neighboring atoms

b)

producing two smaller atoms that can then strike and split neighboring atoms

c)

producing neutrons that can then strike and split neighboring atoms

d)

combining two atoms with low mass to form one large atom

87.
What atom matches this electron configuration?
1s22s22p63s23p64s23d10
a)
Zinc
b)
Copper
c)
Nickel
d)
Germanium
88.

Each row on the periodic table represents:

a)

an energy level

b)

a sublevel

c)

an electron

d)

an orbital

89.

Which periodic table family below has their last, most energetic electron in their electron configuration in the s-block?

a)

Alkaline Earth

b)

Halogens

c)

Noble Gases

d)

Transition Metals

90.
How many electrons can the first energy level hold?
a)
1
b)
2
c)
8
d)
0
91.
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
92.
What is the noble gas configuration for beryllium?
a)
[He]1s2
b)
[He]2s2
c)
[Li]2s1
d)
[Li]2s2
93.
What is the noble gas configuration for Neon?
a)
[Ne]
b)
[He]2s22p6
c)
[F]2p1
d)
[Ne]2s21p6
94.
The electron configuration of an atom is 1s22s22p6.  The number of electrons in the atom is 
a)
3
b)
6
c)
8
d)
10
95.
What atom matches this electron configuration?
1s22s22p63s2
a)
Neon
b)
Magnesium
c)
Aluminum
d)
Potassium
96.
There are 4 different types of subshells (orbitals) s,p,d,f.
a)
true
b)
false
97.
What is the noble gas shorthand electron for Sulfur atom?
a)
[Ar] 3p4
b)
[He] 3s23p4
c)
[Ne] 3s23p4
d)
[Na] 3s23p4
98.
What is the charge of an atom that has lost one electron?
a)
-1
b)
-2
c)
+1
d)
+2
99.
What is the charge of an atom that has gained one electron?
a)
-1
b)
-2
c)
+1
d)
+2
100.
How many electron can be found in a p orbital?
a)
2
b)
3
c)
4
d)
6
101.
What is the electronic configuration of sodium?
a)
1s22s22p63s1
b)
[Ne]3s1
c)
1s22s22p7
d)
Both A and B are correct
102.
Which of the following is the correct electron configuration for a carbon atom?
a)
1s2 2s2 2p6 3s2 3p2
b)
1s2 2s2 2p6 3s2 3p6
c)
1s2 2s2 2p2
d)
1s2 2s2 2p6 3s2 3p6 4s2 4p2
103.
Which of the following elements is a noble gas?
a)
1s2 2s2
b)
1s2 2s2 2p5
c)
1s2 2s2 2p6 3s2 3p6
d)
1s2 2s2 2p6 3s1
104.
How many electrons does Si contain? (click to see image)
a)
14
b)
28
c)
2
d)
4
105.
The number of protons and electrons are the same as
a)
Neutrons
b)
Atomic number
c)
atomic mass
d)
Electron shells
106.

Which of the following is a positively charged particle found in the nucleus of an atom?

a)

Electron

b)

Proton

c)

Neutron

d)

Quark

107.

Which particle carries no charge?

a)

Neutrons

b)

Electrons

c)

Protons

108.

The 4 orbitals are

a)

s, p, d, f

b)

a, b, c, d

c)

2, 4, 6, 8

109.
How many electrons can the d sublevel hold?
a)
8
b)
10
c)
2
d)
4
110.

What does Hund's rule state?

a)

An orbital can contain two electrons only if the electrons have opposite spins.

b)

An orbital can contain two electrons only if all other orbitals at that sublevel are empty.

c)

An orbital can contain two electrons only if the electrons have different energy levels.

d)

An orbital can contain two electrons only if all other orbitals in that sublevel contain at least one electron.

111.

What does the sign represent with respect to electrons?

a)

opposite spin of two electrons

b)

different principal energy levels of two electrons

c)

distances of two electrons from the nucleus

d)

attraction between two electrons

112.

According to the Pauli exclusion principle, when can two electrons occupy the same orbital?

a)

only if there is no place else to put them

b)

only if they have the same spin

c)

only if they have opposite spins

d)

only if they are alike in all their properties

113.

Electron configuration of hydrogen (H)

a)

1s11s^1  

b)

1s21s^2  

c)

2s12s^1  

d)

2s2 2p12s^2\ 2p^1  

114.

Electron configuration of helium (He)

a)

1s11s^1  

b)

1s21s^2  

c)

2s12s^1  

d)

2s2 2p12s^2\ 2p^1  

115.
An electron occupies the lowest energy orbital that can receive it.
a)
Hund’s rule
b)
Pauli exclusion principle
c)
Bohr model of the atom
d)
Aufbau principle
116.

Energy levels are denoted by:

a)

letters

b)

numbers

c)

a combination of letters and numbers

d)

subscripts

117.
Which is associated with more energy? 
a)
2p
b)
2s
c)
3p
d)
1s
118.

Write the electron configuration

a)

1s22s22p6

b)

1s12s12p3

c)

1s22s22p63s2

d)

1s22s22p63s3

119.

Write the electron configuration for the element.

a)

1s12s12p33s1

b)

1s22s22p53s1

c)

1s2s2p3s

d)

1s22s22p63s1

120.

Check all of the following that could actually exist in a correctly written electron configuration.

a)

4s3

b)

3p4

c)

2p8

d)

6d3

e)

1s1

121.

What period is Lead (Pb) in?

a)

6

b)

4

c)

Metals

d)

4A

122.

How many electrons does Barium (Ba) have?

a)

13

b)

2

c)

71

d)

56

123.

What is the ionic charge of Phosphorus (P)?

a)

+5

b)

-3

c)

+3

d)

-5

124.

How many electrons does a Strontium (Sr) ION have?

a)

38

b)

10

c)

8

d)

36

125.

How many neutrons does Bromine (Br) have?

a)

35

b)

80

c)

45

d)

7

126.

What is group name of the most reactive metals?

a)

Noble gases

b)

Halogens

c)

Alkali metals

d)

Alkaline earth metals

127.

Why are halogens so reactive?

a)

They want to get rid of their only valance electron

b)

They only need one more electron

c)

They are non reactive, they have a full shell

128.

Which scientist created the first periodic table?

a)

Dmitri Mendeleev

b)

Isaac Newton

c)

Albert Einstein

d)

John Dalton

129.

Metals are found on the ____ side of a periodic table and nonmetals are found on the ___ side.

a)

left, right

b)

right, left

130.

This orbital diagram represents:

a)

Carbon

b)

Boron

c)

Nitrogen

d)

Oxygen

131.

This orbital diagram represents

a)

Nitrogen

b)

Oxygen

c)

Carbon

d)

Neon

132.

What is incorrect about this orbital diagram?

a)

Both arrows in the 2p box should be pointing up

b)

There are too many electrons in the 1s orbital

c)

In the 2p boxes, there should only be 1 electron in the first 2p box and one in the 2nd 2p box

d)

All the arrows should be pointing up

133.
Which element is depicted from this orbital diagram
a)
Fluorine
b)
Neon
c)
Chlorine
d)
Argon
134.
Ionic bonds are between...
a)
Metal and Non-metal
b)
Non-metal and Non-metal
c)
Metal and Metal
135.

When magnesium burns in oxygen it produces MgO. Use the ionic formula to name the compound produced.

a)

Magnesium oxygen

b)

Oxygen magnesium

c)

Magnesium oxide

d)

Oxygen magnesiumide

136.

According to the Octet Rule, atoms of elements react with each other in order to attain ____ electrons in their outermost energy level or shell.

a)

2

b)

4

c)

6

d)

8

e)

10

137.

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-

138.

Lithium is in group 1 of the periodic table, which ion would it form?

a)

Li-

b)

Li2-

c)

Li+

d)

Li2+

139.
If my charge becomes 2+ what does that say about me?
a)
I am stealing 2 electrons
b)
I am losing 2 electrons
c)
I am in period 2
d)
I have an atomic # of 2
140.
A cation is a ____ ion.
a)
negative
b)
positive
141.
A anion will be a ____ ion.
a)
negative
b)
positive
142.

NaC2H3O2

(a)  

143.

Magnesium hydroxide

(a)  

144.

MnOH

(a)  

145.

Al2O3

(a)  

146.

Which of the following would be the correct formula for a compound of Aluminum and Fluorine?

a)

AlF3

b)

Al2F3

c)

AlF2

d)

AlFI

147.

A metal will always ____ electrons

a)

Lose

b)

Take

c)

Give

d)

Hold

148.

Which particle is involved in bonding?

a)

Neutron

b)

Proton

c)

Electron

d)

Photon

149.

Which of these has five valence electrons?

a)

Nitrogen

b)

Oxygen

c)

Hydrogen

d)

Chlorine

150.

An atom with seven valence electrons is a:

a)

Noble Gas

b)

Metal

c)

Nonmetal

d)

Transition Metal

151.

An atom of Beryllium can bond to two atoms of:

a)

Nitrogen

b)

Oxygen

c)

Chlorine

d)

Sulfur

152.

What is the net charge of an ionic compound?

a)

Four

b)

Zero

c)

One

d)

Eight

153.

Alkali Metals cannot form ionic bonds with:

a)

Sulfur

b)

Alkaline Earth Metals

c)

Oxygen

d)

Halogens

154.

Nonmetals will ____ electrons

a)

Give

b)

Take

c)

Gain

d)

Lose

155.

Ionic Compounds are named without prefixes.

a)

True

b)

False

156.

 

An element gains two electrons. This element is:

a)

An anion with a +2 charge

b)

A cation with a +2 charge

c)

An anion with a -2 charge

d)

A cation with a -2 charge.

157.

An elements loses one electron to become a cation. This element is a:

a)

Alkaline Earth Metal

b)

Halogen

c)

Alkali Metal

d)

Metalloid

158.

In a Bohr model, the valence electrons are placed on the:

a)

Nucleus

b)

Outer Shell

c)

Inner Shell

d)

Middle Shell

159.

A compound that has a formula of SrF2 is named:

a)

Calcium Fluoride

b)

Strontium Fluoride

c)

Fluorine Strontide

d)

Strontium Difluoride

160.

A negative ion is called a(n):

(a)  

161.

The positive ions tend to _____________ electrons.

a)

lose

b)

gain

162.

The negative ions tend to _____________ electrons.

a)

lose

b)

gain

163.

When an atom loses an electron, it becomes a

a)

positive ion

b)

negative ion

c)

neutral ion

d)

neutral atom

164.
Ionic bonds are between...
a)
Metal and Non-metal
b)
Non-metal and Non-metal
c)
Metal and Metal
165.
CO2
a)
Ionic
b)
Covalent
c)
Polyatomic Ion 
d)
Metallic 
166.
SO4
a)
Covalent
b)
Ionic
c)
Metallic
d)
Polyatomic Ion
167.
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
168.
Ionic bonds form between metals and ____.
a)
metalloids
b)
metals
c)
nonmetals
169.

Beryllium and sulfur will form a ______ bond

a)

ionic

b)

covalent

c)

metalloid

170.

Sodium and Bromine will make a _____ bond.

a)

ionic

b)

covalent

c)

metallic

171.

Carbon and Oxygen will make a ___________ bond.

a)

ionic

b)

covalent

c)

metallic

172.

Nitrogen and Oxygen will make a ____________ bond

a)

ionic

b)

covalent

c)

metallic

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