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Strength of chemical bonds

Total questions: 70

Worksheet time: 1hrs 7mins

Name
Class
Date
1.

True or False: Shorter bonds are stronger bonds with larger bond energy.

a)

True

b)

False

2.

True or False: Double and triple bonds are longer, weaker bonds than single bonds.

a)

True

b)

False

3.

Which of these would require the least energy in order to break the bonds?

a)

single bond

b)

double bond

c)

triple bond

4.

Longer bonds are _ than shorter bonds

a)

weaker

b)

stronger

5.

Shorter bonds are _ than longer bonds.

a)

weaker

b)

stronger

6.

When the bond is stronger, the bond energy is

a)

smaller

b)

larger

7.

When the bond is weaker, the bond energy is

a)

smaller

b)

bigger

8.

The energy required to break a bond and break atoms of a molecule apart

a)

bond length

b)

bond energy

c)

bond strength

d)

none of these

9.

Which of these is the shortest bond?

a)

single bond

b)

double bond

c)

triple bond

10.

Which of these is the strongest bond?

a)

single bond

b)

double bond

c)

triple bond

11.

True or False: Energy is required to break a bond and energy is released when new bond(s) form.

a)

True

b)

False

12.

Why do all bonds form?

a)

so the number of protons equals the number of electrons

b)

so an atom can become unstable

c)

to fill the outermost energy level

13.
What elements have zero electronegativity?
a)
metals
b)
nonmetals
c)
metalloids
d)
noble gases
14.

What type of bond is depicted in the image?

a)

Covalent

b)

Polar Covalent

c)

Ionic

15.

What type of bond is depicted in the image?

a)

Covalent

b)

Polar Covalent

c)

Ionic

16.

What type of bond is depicted in the image?

a)

Covalent

b)

Polar Covalent

c)

Ionic

17.

Which bond shares electrons evenly?

a)

non polar Covalent

b)

Polar Covalent

c)

Ionic

18.

Which bond shares electrons unevenly?

a)

Covalent

b)

Polar Covalent

c)

Ionic

19.

Which bond involves "stealing" electrons?

a)

Covalent

b)

Polar Covalent

c)

Ionic

20.

What does the word "polar" refer to?

a)

together, mutually, in common

b)

valence electrons

c)

an atom or molecule with a net electric charge due to the loss or gain of one or more electrons.

d)

To have a positive and negative end like a magnet

21.

Measure of the tendency of an atom to attract a bonding pair of electrons is known as...

a)

electronegativity

b)

bond polarity

c)

angular momentum

d)

valence electrons

22.

The difference in electronegativity affects the type of bond will be formed. What type of bond would be formed with a difference of 0.3?

a)

Covalent

b)

Polar Covalent

c)

Ionic

23.

The difference in electronegativity affects the type of bond will be formed. What type of bond would be formed with a difference of 2.0?

a)

Covalent

b)

Polar Covalent

c)

Ionic

24.

The difference in electronegativity affects the type of bond will be formed. What type of bond would be formed with a difference of 0.6?

a)

Covalent

b)

Polar Covalent

c)

Ionic

25.

True or False: The smaller the difference in electronegativity, the more polar the bond

a)

True

b)

False

26.

As you look from left to right across a period, electronegativity

a)

increases

b)

decreases

27.

As you look down a group, electronegativity

a)

increases

b)

decreases

28.

The positive ions tend to _____________ electrons.

a)

lose

b)

gain

29.

The negative ions tend to _____________ electrons.

a)

lose

b)

gain

30.

Why are sodium and chlorine attracted to each other?

a)

they have opposite charges

b)

they both have negative charges

c)

they both have positive charges

31.

How do bonds make elements stable?

a)

so the number of protons equals the number of electrons

b)

make other atoms unstable

c)

fill the outermost energy level

32.
What type of bond is illustrated above?
a)
Metallic
b)
Ionic
c)
Covalent
d)
Wiggly
33.
What type of bond is present when electrons are freely shared between metal atoms?
a)
Metallic
b)
Ionic
c)
Covalent
d)
Hippie
34.
A solid substance is an excellent conductor of electricity. The chemical bonds in this substance are most likely?
a)
ionic, because the valence electrons are shared between atoms
b)
covalent, because the valence electrons are mobile
c)
metallic, because the valence electrons are stationary
d)
metallic, because the valence electrons are mobile
35.
 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
36.
What is the VSEPR theory used to predict?
a)
Bond Strength
b)
Polarity
c)
Molecular Shape
d)
Electronegativity
37.

What 3-D VSEPR shape does this molecule exhibit?

a)

linear

b)

tetrahedral

c)

trigonal pyramidal

d)

trigonal planar

38.

Which Lewis Dot Model drawing correctly shows an O2 molecule?

a)
b)
c)
d)
39.
What is the VSEPR shape of H2S?
a)
linear
b)
trigonal planar
c)
bent
d)
tetrahedral
40.
How many electrons are shared in a double bond?
a)
1
b)
2
c)
4
d)
6
41.

Which type of molecular shape is shown by this molecule?

a)

trigonal pyramidal

b)

tetrahedral

c)

bent

d)

trigonal planar

42.
Low melting point and low solubility in water are general properties of ______________________ compounds
a)
ionic
b)
covalent
c)
chemical
d)
glucose
43.

Which is the correct molecular structure for carbon dioxide?

a)
b)
c)
d)
44.
What is the MOLECULAR geometry of the central oxygen?
a)
Linear
b)
Trigonal Planar
c)
Bent
d)
Tetrahedral
45.
Which of the following molecular shapes would have a bond angle of 180 Degrees?
a)
Bent
b)
Trigonal Planar
c)
Tetrahedral
d)
Linear
46.
What molecular shape is the structure shown here? (BCl3)
a)
linear
b)
trigonal planar
c)
tetrahedral
d)
trigonal pyramidal
47.
What molecular shape is the structure shown here? (NH4+)
a)
linear
b)
trigonal planar
c)
tetrahedral
d)
trigonal pyramidal
48.
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
49.
A formula with the lowest whole # ratio of elements in a compound is called
a)
Molecular Formula
b)
Chemical Formula
c)
Empirical Formula 
d)
Distance Formula
50.

What is the empirical formula for C4H6?

a)

CH

b)

CH3

c)

C2H3

d)

C4H6

51.

What is the empirical formula for N2S3?

a)

NS

b)

N3S2

c)

N2S3

d)

N1S1.5

52.

C2F6

Choose the correct empirical formula...

a)

CF

b)

C2F6

c)

C6F2

d)

CF3

53.
A chemical formula that shows the actual # and kinds of atoms present in one molecule of a compound is called_________
a)
ionic formula
b)
covalent formula
c)
empirical formula
d)
molecular formula
54.
Find the percent composition of N2S2.
a)
N: 69.6%  S: 30.4%
b)
N:36% S: 75.6%
c)
N: 96.6% S: 3.4%
d)
N: 30.4% S: 69.6%
55.

Whats the empirical formula of a molecule containing 40.0 % C, 6.7% H, and 53.3% oxygen?

a)

CHO

b)

CH2O

c)

CH30

d)

C2HO2

56.

What is the molecular formula if the empirical formula is CH2O and the molecular molar mass is 120?

a)

CH2O

b)

C2H4O2

c)

C4H8O4

d)

C6H12O6

57.

What is the molecular formula of a compound with an empirical formula of C2OH4 and a molecular mass of 88 grams per mole?

a)

C2O4H8

b)

C8O2H4

c)

C4O2H8

d)

C4O8H2

58.
What is the molecular formula if the empirical formula is C2H5 and the molecular molar mass is 58.14 g/mol?
a)
C2H5
b)
C4H10
c)
C1H2.5
d)
C4H8
59.
A hydrate of magnesium chloride is present and the following data is collected:
mass of crucible = 22.130 grams
mass of crucible + hydrate = 25.290 grams
mass of crucible and contents after heating = 23.491 grams
What is the complete formula of this hydrate?
a)
MgCl2 · 7H2O
b)
MgCl2 · 11H2O
c)
MgCl2 · 6H2O
d)
MgCl2 · 13H2O
60.
Crucible, cover: 17.8 g
Crucible, cover, and hydrate: 23.9g
Crucible, cover, and salt: 21.5g
Calculate % of water lost.
a)
90.0%
b)
60.7%
c)
39.3%
d)
45.5%
61.

What is the correct chemical formula for barium hydroxide octahydrate?

a)

Ba(OH)2 . 8H2O

b)

Ba(OH)2 . H2O

c)

8Ba(OH)2 . H2O

d)

Ba . 8(OH)2

62.

What is the best method for removing water from a hydrated compound?

a)

freezing

b)

filtration

c)

distillation

d)

heating

63.
What is the empirical formula for the following:
32.40% sodium, 22.5% sulfur; 45.1 % oxygen, 37.75% water?
a)
Na2SO4H6O3
b)
Na2SO4 . 2H2O
c)
Na2SO4 . 3H2O
d)
Na2SO4 . (H2O)3
64.
Na2CO3 · 10H2O is known as sodium sulfate ______
a)
Hydroxide
b)
Hydrate
c)
Decahydrate
d)
None of the above
65.
Cr(NO3)3 ⋅ 9H2O
a)
chromium nitrate nonahydrate
b)
chromium nitrogen trioxide nonahydrate
c)
chromium (III) nitrate nonahydrate
d)
chromium (I) tritrioxide heptahydrate
66.
An empirical formula:
a)
is a formula that calculates the coefficients of a compound in a balanced equation.
b)
is the simplest whole-number ratio of moles of elements in the compound.
67.

What is the percent by mass of Oxygen in water? H2O.

a)

33 %

b)

88.9%

c)

11.1%

d)

50%

68.

What is the percent by mass of Carbon in sugar C12H22O11 ?

a)

144.0

b)

42.1

c)

12.01

d)

342.0

69.

Indigo the dye used to color blue jeans is prepared using sodium amide. Sodium amid contains the following percentages by mass of the following elements: 5.17% Hydrogen, 35.9% Nitrogen and 58.9% sodium. What is the empirical formula for Sodium amide?

a)

NaNH

b)

Na2NH

c)

NaNH2

d)

NaN2H2

70.

Atoms form bonds in order to

a)

become more stable

b)

have the highest energy possible.

c)

repel like charges

d)

make chemistry students angry.

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