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100+ Questions on Chemical Bonding

Total questions: 103

Worksheet time: 3hrs 26mins

Name
Class
Date
1.

What are valence electrons?

a)

The total number of electrons in an atom

b)

The number of electrons in the outermost shell

c)

The number of electrons in the second shell

d)

The number of protons in the outermost shell

2.

How many valence electrons does carbon have?

a)

4

b)

5

c)

6

d)

7

3.

Atoms are electrically neutral when

a)

They have a minimal charge.

b)

They have a balanced number of protons and neutrons.

c)

They have a balanced number of protons and electrons.

d)

They have no valance electrons.

4.

If an electron is removed, an ion becomes

a)

An atom

b)

Positive

c)

Negative

d)

Neutral

5.

If an ion gains an electron, it becomes

a)

Positive

b)

Stable

c)

Atomic

d)

Negative

6.

Cations have what type of charge?

a)

Positive

b)

Negative

7.

Which of the following about cations is correct?

a)

Cations where named after cats.

b)

Cations form when an atom has a mostly empty outer shell.

c)

Cations are only non-metals.

d)

Cations are mostly negative.

8.

Anions have which type of charge?

a)

Positive

b)

Negative

9.

Anions occur when

a)

The inner shell is full.

b)

The outer shell is almost full.

c)

The outer shell is full.

d)

There is no outer shell.

10.

ALL anions are

a)

Metal

b)

Transitional Metals

c)

Nobel Gases

d)

Non-Metal

11.

What is the formula of an ionic compound formed from Lithium and Oxygen?

a)

Li2O

b)

LiO2

c)

2LiO

d)

Li2O

12.

What is the ion formed from Sulfur?

a)

S+2

b)

S-2

c)

S+6

d)

S-6

13.

A Bromine ion gains 1 electron, which of the following is the correct symbol for a Bromine ion?

a)

Br-1

b)

Br+1

c)

Br+7

d)

Br-7

14.

An atom can gain, but can't lose electrons.

a)

true

b)

false

15.
Why do ionic bonds form?
a)
so the number of protons equals the number of electrons
b)
to fill the outermost energy level
c)
so an atom can become unstable
16.
If an aluminum atom has 13 protons (+) and 10 electrons (-), what is it's charge?
a)
Al3+
b)
Al13+
c)
Al10+
d)
Al10-
17.
The attraction between oppositely charged ions is called a(n) _______________.
a)

ionic bond

b)

covalent bond

18.
What is the charge on a noble gas & why?
a)
0; they don't exchange electrons
b)
+1; they give away an electron
c)
-1; they gain an electron
d)
1; they form only single bonds
19.

What type of elements will form an ionic bond?

a)

Metals + Metals

b)

Nonmetals + Nonmetals

c)

Metals + Nonmetals

d)

None of the above

20.

This image shows the bonding between Lithium and Fluorine. What does the red arrow show?

a)

electrons being shared

b)

electrons being transferred to Fluorine

c)

electrons being transferred to Lithium

d)

electrons being destroyed

21.

An ionic bond is the attraction between: (Select ALL that apply)

a)

oppositely charged ions

b)

similarly charged ions

c)

metals and nonmetals

d)

neutral atoms

e)

cations and anions

22.

Looking at the periodic table, when the alkali metals form an ion what charge do they have?

a)

1-

b)

1+

c)

2-

d)

2+

e)

3-

23.

Looking at the periodic table, when the alkaline earth metals form an ion what charge do they have?

a)

1-

b)

1+

c)

2-

d)

2+

e)

3-

24.

Looking at the periodic table, when the halogens form an ion what charge do they have?

a)

1-

b)

1+

c)

2-

d)

2+

e)

3-

25.

Nitrogen, N, will form which of the following ions?

a)

N

b)

N-3

c)

N-5

d)

N+5

26.

What is another name of an ionic compound

a)

salt

b)

cation

c)

anion

d)

polyatomic ion

27.

Which of the following is the correct formula for Sodium Nitride ( [ Na ] + & [ N ] 3- )

a)

NaN3

b)

Na3N

c)

Na2N3

d)

Na3N2

28.

When assigning ionic charge it is always written as a...

a)

superscript

b)

subscript

c)

coefficient

d)

script

29.

When assigning the number of individual atoms in a chemical formula it is written as a...

a)

superscript

b)

subscript

c)

coefficient

d)

script

30.

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-

31.

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-

32.

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

a)

Phosphorus

b)

Iron

c)

Barium

d)

Neon

33.

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

a)

Potassium

b)

Sulfur

c)

Iodine

d)

Magnesium

34.

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

35.

What type of bonding does this picture show?

a)

Ionic

b)

Covalent

36.

What type of bonding does this picture show?

a)

Ionic

b)

Covalent

37.

Generally, atoms form bonds so that _______________.

a)

Each atom loses its electrons

b)

Each atom has a stable electron configuration

c)

Each atom has an unstable electron configuration

d)

Each atom gains electrons

38.

Generally low melting and boiling points

a)

Ionic compounds

b)

Covalent compounds

39.

Poor electrical conductivity

a)

Ionic compounds

b)

Covalent compounds

40.

Conducts electricity well when melted or dissolved

a)

Ionic compounds

b)

Covalent compounds

41.

Valence electrons are shared

a)

Ionic bonds

b)

Covalent bonds

42.
Where are the nonmetals located on the periodic table? 
a)
Blue
b)
Red
c)
Green
43.

The chemical bond between a non-metal and another non-metal will be a ________ bond.

a)

metal

b)

ionic

c)

covalent

d)

polar

44.

Carbon and Oxygen will make a ___________ bond.

a)

ionic

b)

covalent

c)

metallic

45.

MgO

a)

ionic

b)

covalent

c)

metallic

46.

NaCl

a)

ionic

b)

covalent

c)

metallic

47.

If two fluorine atoms bond they will make a _____ bond.

a)

ionic

b)

covalent

c)

metallic

48.

What is it called if there are three-pairs of electrons being shared?

a)

Triple Bond

b)

Three Single Bonds

c)

Tribond

d)

Double and Single Bond Combo

49.
What two types of atoms make a covalent bond?
a)
2 Nonmetals
b)
1 Nonmetal & 1 Metal
c)
2 Metals
d)
2 Noble Gases
50.
What is a diatomic element?
a)
a metal bonded with a nonmetal
b)
2 or more nonmetals bonded together
c)
2 or more metals bonded together
d)
2 atoms of the same element bonded together
51.
How many electrons are shared in a double bond?
a)
2
b)
4
c)
6
d)
8
52.

Which would be the only situation where valence electrons would be shared evenly?

a)

metals and nonmetals

b)

different nonmetals

c)

nonmetals of the same element

d)

metalloids of the same element

53.
Is Hydrogen considered a metal or a non-metal?
a)
Metal
b)
Non-metal
54.
Is carbon considered a metal or a non-metal?
a)
metal
b)
nonmetal
c)
other
55.
What is the correct formula for this molecule?
a)
NH
b)
N3H
c)
NH3
d)
NH4
56.
Which of the following is the correct Lewis dot structure for the molecule fluorine (F2)?
a)
A
b)
B
c)
C
d)
D
57.

This could be the dot diagram of

a)

Mg

b)

Cl

c)

C

d)

O

58.
This could be the dot diagram of
a)
P
b)
Ar
c)
Na
d)
B
59.

What is at the center of every atom?

a)

an electron

b)

a compound

c)

a molecule

d)

a nucleus

60.

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

61.

Which ones are acceptable for #13 Aluminum in Group 3A?

(Actually pick "2" that are acceptable)

a)
b)
c)
62.

Which is the correct molecular structure for carbon dioxide?

a)
b)
c)
d)
63.
Which of the following is the correct Lewis structure for water?
a)
A
b)
B
c)
C
64.
Three pairs of electrons are shared in a
a)
Single bond
b)
Double bond
c)
Triple bond
65.
 A lone pair is defined as
a)
A pair of bonding electrons
b)
One non-bonding electron
c)
A pair of non-bonding electrons
d)
A pair of electrons on the central atom
66.
Why do elements bond?
a)
To be friends
b)
To create a new element
c)
To become stable
67.

Is this compound ionic or covalent?

a)

ionic

b)

covalent

68.

No electronegativity difference between two atoms leads to a

a)

Polar covalent bond

b)

Non-polar covalent bond

c)

Ionic bond

d)

None of these

69.

In a polar covalent bond, the atom with a negative charge is less electronegative.

a)

true

b)

false

70.

Water is a polar molecule because of unequal sharing of electrons between the oxygen and hydrogen atoms bonded together.

a)

true

b)

false

71.

The percentage of partial ionic character depends upon the difference of the ______ of two atoms that join with each other through a covalent bond.

a)

Electron affinity

b)

Ionization energy

c)

Electronegativity

d)

Atomic size

72.

A bond in which the electrons are shared equally between the two atoms is a(n)________ bond.

a)

polar covalent

b)

nonpolar covalent

c)

hydrogen

d)

ionic

73.

In a polar covalent bond, the electrons spend more time around the atom...

a)

with the greatest electronegativity

b)

with the lowest electronegativity

c)

each atom equally

74.

Partial charges are present in which type of bond(s)?

a)

Ionic

b)

Nonpolar Covalent

c)

Polar Covalent

d)

Both Polar Covalent and Ionic

e)

All covalent

75.

Partial charges like the ones shown here are called:

a)

dipoles

b)

deltas

c)

ions

d)

magnetic poles

76.

In this Lewis structure, the symbol above F means...

a)

electrons are being transferred to Fluorine

b)

electrons are less attracted to F than H

c)

electrons are more attracted to F than H

d)

Fluorine has formed an anion

77.

Look at this covalent molecule as a whole. What type of molecule is it? (Is it symmetrical?)

a)

Polar

b)

Non-polar

c)

Ionic

78.

Look at this covalent molecule as a whole. What type of molecule is it? (Is it symmetrical?)

a)

Polar

b)

Nonpolar

c)

Ionic

79.

Look at this covalent molecule as a whole. What type of molecule is it? (Is it symmetrical?)

a)

Polar

b)

Nonpolar

c)

Ionic

80.

When you have Br-Br, what is the polarity?

a)

Polar

b)

nonpolar

c)

Ionic

81.

When you have Li-O, what is the polarity?

a)

nonpolar

b)

polar

c)

ionic

82.

When you have H-Cl, what is the polarity?

a)

nonpolar

b)

polar

c)

ionic

83.

Electronegativity (a)   as you go down a group.

84.

Which element has a higher electronegativity value?

a)

Niobium

b)

Tin

c)

Cadmium

d)

Iodine

85.

Which element has a lower electronegativity value?

a)

Calcium

b)

Barium

86.
VSEPR stands for ________ theory.
a)
Valence Structure of Electron Pyramids and Regression
b)
Varied Structures of Electrons Paired and Replaced
c)
Varied Shell Energy of Protons and Radiation
d)
Valence Shell Electron Pair Repulsion
87.
According to VSEPR, molecules adjust their shapes to keep which of the following as far away as possible?
a)
Pairs of valence electrons
b)
Inner shell electrons
c)
Mobile Electrons
d)
Electrons closest to the nucleus
88.

2 bonded atoms and 0 lone pairs

a)

linear

b)

trigonal planar

c)

bent

d)

tetrahedral

e)

trigonal pyramidal

89.
 A lone pair is defined as
a)
A pair of bonding electrons
b)
One non-bonding electron
c)
A pair of non-bonding electrons
d)
A pair of electrons on the central atom
90.

3 atoms bonded and 0 lone pairs

a)

linear

b)

trigonal planar

c)

bent

d)

tetrahedral

e)

trigonal pyramidal

91.
Who could this be?
a)
H2O
b)
NH3
c)
CO2
d)
CH4
92.

4 shared pairs and 0 unshared pairs

a)

true linear

b)

trigonal planar

c)

bent

d)

tetrahedral

e)

trigonal pyramidal

93.
Who could this be? 
a)
CO2
b)
NH3
c)
H2S
d)
CH4
94.
What molecular shape is the structure shown here? (H2O)
a)
tetrahedral
b)
trigonal planar
c)
bent
d)
trigonal pyramidal
95.
What is the VSEPR theory used to predict?
a)
Bond Strength
b)
Polarity
c)
Molecular Shape
d)
Electronegativity
96.
Which molecule would have this shape?
a)
BF3
b)
CH4
c)
PCl5
d)
CO2
97.
What molecule could this be? 
a)
BF3
b)
CH4
c)
H2O
d)
CO2
98.

What shape would PH3 have?

a)

Trigonal Planar

b)

Trigonal pyramidal

c)

Bent

d)

Linear

99.
What should you do if you break glass in the lab?
a)
Tell the teacher.
b)
Sweep up the glass.
c)
Pick up the glass with your hands.
d)
Ignore it; the teacher will clean it up when she sees it later.
100.
Goggles must be worn when using or working with a Bunsen Burner
a)
False
b)
True
101.

To produce the most heat, you should twist the collar until you see ______

a)

A dark blue cone

b)

An orange cone

c)

A yellow cone

d)

A light blue cone

102.
When in the lab you should wear...
a)
open-toed shoes.
b)
sandals.
c)
closed-toes shoes.
d)
no shoes.
103.

Which of the following items are considered safety equipment in our classroom?

a)

Eyewash Station

b)

Emergency Shower

c)

Fire Extinguisher

d)

All of the Above.

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