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FX Chem 20 Bonding Unit Review

Total questions: 60

Worksheet time: 1hrs 26mins

Name
Class
Date
1.

Identify the IMF exist in CH4

a)

dipole-dipole forces

b)

london forces

c)

ion-dipole forces

d)

hydrogen bonding

2.

Identify the IMF exist in HBr

a)

london dispersion forces

b)

hydrogen bonding

c)

dipole-dipole forces

d)

ion-dipole forces

3.

To form a hydrogen bonding, Hydrogen needs to attract to the highly electronegative elements such us _____, _____, and ____

a)

chlorine, fluorine, and oxygen

b)

fluorine, oxygen, and sulfur

c)

fluorine, bromine, and oxygen

d)

fluorine, oxygen, and nitrogen

4.

Forces that holds atoms together within the molecule

a)

intermolecular forces

b)

intramolecular forces

5.

Dipole-Dipole forces are stronger than _______ and weaker than _________ interactions.

a)

london dispersion, hydrogen bonding

b)

hydrogen bonding, london dispersion

c)

ionic bonds, london dispersion

6.

Which of the following has the lowest boiling point?

a)

PH3

b)

H2O

c)

SiH4

d)

NH3

7.

Forces that holds molecules together

a)

intramolecular forces

b)

intermolecular forces

8.
What explains the very high melting and boiling point of water
a)
Strong dipole-dipole bonds between water molecules
b)
Strong hydrogen bonds between water molecules
c)
Dispersion forces which are present in all molecules
d)
Asymmetrical shape of the polar bonds.
9.
Does HCl have hydrogen bonding?
a)
yes
b)
no
10.

Intermolecular forces for: NH3

a)

dispersion forces only

b)

dispersion forces and hydrogen bonding

c)

dispersion forces, dipole-dipole forces, and hydrogen bonding

d)

hydrogen bonding only

11.
London forces are stronger in heavier atoms or molecules, and weaker in lighter atoms or molecules.  Which of these has the strongest London forces?
a)
F2
b)
Br2
c)
I2
d)
Cl2
12.

What types of intermolecular forces will be present between two molecules of acetone?

a)

Dispersion forces only

b)

dipole-dipole forces & dispersion forces

c)

dispersion forces, dipole-dipole forces, and hydrogen bonding

d)

dispersion forces and hydrogen bonding

13.

Which substance would be expected to dissolve in polar water? Remember: like dissolves like - which of these molecules is also polar?

a)

NH3

b)

CH4

c)

CO2

d)

CH3CH2CH2CH3

14.

Intermolecular force due to the formation of temporary dipole moments in molecules.

a)

dispersion forces

b)

dipole-dipole forces

c)

hydrogen bonding

15.

CCl4 has how many double bonds?

a)

0

b)

1

c)

2

d)

3

16.
Which of the following is the correct Lewis dot structure for the molecule fluorine (F2)?
a)
A
b)
B
c)
C
d)
D
17.

What bond is formed when a metal transfers electrons to a nonmetal?

a)

Covalent bond

b)

Ionic bond

c)

Metallic bond

18.

MgCl2

a)

Ionic

b)

Covalent

c)

Metallic

19.

This is a correct Lewis dot diagram for fluorine (F)

a)
true
b)
false
20.
What molecular shape is the structure shown here? (H2O)
a)
tetrahedral
b)
trigonal planar
c)
bent
d)
trigonal pyramidal
21.

Choose the correct shape for this molecule:

a)

Trigonal planar

b)

Trigonal pyramidal

c)

Bent

d)

Tetrahedral

22.
What are valence electrons?
a)
The innermost electrons
b)
The outermost electrons
c)
The bonds between two atoms
d)
When electrons are balanced
23.
What is the octet rule?
a)
Elements can only have 8 electrons in its outermost shell
b)
The elements must form an octopus like structure
c)
Is the outermost electrons
d)
Elements can only have 6 electrons in its outermost shell
24.

Name this element.

a)

Neon

b)

Magnesium

c)

Sodium

d)

Manganese

25.

What is the basis of a metallic bond?

a)

the attraction of neutral metal atoms.

b)

the attraction between protons and neutrons.

c)

the attraction between positive metal ions and interlocking electrons.

d)

the attraction between positive metal ions and free moving electrons.

26.

Why do metals conduct electricity?

a)

They are shiny

b)

The electrons are delocalised and able to move

c)

The electrons are held tightly within the lattice

d)

The electrons are shared between two metal ions

27.

What is the molecular geometry of this molecule

a)

tetrahedral

b)

Linear

c)

trigonal bipyramidal

d)

bent

28.

What is the MOLECULAR geometry for this molecule?

a)

Linear

b)

Bent

c)

trigonal planar

d)

square planar

29.
 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
30.
What is the VSEPR theory used to predict?
a)
Bond Strength
b)
Polarity
c)
Molecular Shape
d)
Electronegativity
31.
Who could this molecule be?
a)
CH4
b)
CO2
c)
PCl5
d)
BF3
32.
Who could this be?
a)
H2O
b)
NH3
c)
CO2
d)
CH4
33.

What molecular geometry would PH3 have?

a)

Trigonal Pyramidal

b)

Trigonal Bipyramidal

c)

Bent

d)

Linear

34.

Is this molecule polar?

a)

No

b)

Yes

35.

What shape would this have?

a)

Trigonal planar

b)

Pyramidal

c)

Tetrahedral

d)

Bent

36.
Will this molecule be polar or nonpolar? CS2
a)
polar
b)
nonpolar
37.

What molecular geometry is the structure shown here? (BCl3)

a)

linear

b)

trigonal planar

c)

tetrahedral

d)

trigonal pyramidal

38.
A bond where electrons are NOT shared equally? 
a)
polar covalent
b)
nonpolar covalent
39.

What is the molecular geometry/shape of a molecule with 3 shared pairs and 0 unshared pairs?

a)

Linear

b)

Trigonal Planar

c)

Trigonal Pyramidal

d)

Tetrahedral

40.

For polarity to occur in a bond, you need two elements with a difference in their electronegativities of ___

a)

0.5 or less

b)

between 0.5 and 1.6

c)

less than 1.6

d)

greater than 1.6

41.

Liquids made up of polar molecules are really good at dissolving ___

a)

metallic solids

b)

lipids and fats

c)

molecular solids

d)

solids composed of polar or ionic compounds

42.

What type of bond would form between O and O?

a)

Polar Covalent

b)

Non-Polar Covalent

c)

Ionic

43.

What type of bond would form between Li and O?

a)

Polar Covalent

b)

Non-Polar Covalent

c)

Ionic

44.

The bond between C and Cl is polar covalent. That means

a)

there is a pair of electrons shared equally between them

b)

there is a pair of electrons shared unequally between them

c)

an electron will be stolen from one and given to the other

45.

The bond between K and N is ionic. Which atom will steal the electrons from the other?

a)

K will steal electrons from N and become (+)

b)

K will steal electrons from N and become (-)

c)

N will steal electrons from K and become (+)

d)

N will steal electrons from K and become (-)

46.

The bond between C and H is non-polar covalent. That means

a)

there is a pair of electrons shared equally between them

b)

there is a pair of electrons shared unequally between them

c)

an electron will be stolen from one and given to the other

47.

What type of bond contains atoms with "partial" charges?

a)

Polar Covalent

b)

Non-Polar Covalent

c)

Ionic

48.

LiBr is called

a)

lithium bromine

b)

lithium (I) bromine

c)

lithium bromide

d)

lithuim (I) bromide

49.

Name the following ionic compound: BeCl2

a)

beryllium chlorine

b)

beryllium II chloride

c)

beryllium chloride

d)

beryllium dichloride

50.
Valence electrons are: 
a)
Electrons farthest away from the nucleus
b)
Electrons closest to the nucleus
c)
Electrons that just come and go - they don't stay with the atom
d)
Electrons in the second shell
51.

According to the diagram below, how many bonds will this atom be able to make?

a)
1
b)
2
c)
3
d)
4
52.
This could be the dot diagram of 
a)
Ne
b)
Si
c)
Al
d)
Be
53.
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
54.

As you look down a group, ionization energy and electronegativity

a)

increases

b)

decreases

55.
What is ionization energy?
a)
Energy needed to destroy an atom
b)
Energy required to remove an electron
c)
Energy needed to split an electron
d)
Energy required to add an electron
56.
Electronegativity is...
a)
how good an atom is at attracting 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. 
57.
Which of the following is the least electronegative element?
a)
oxygen
b)
potassium
c)
fluorine
d)
nitrogen
58.

These bonds represent the strongest bonds and are limited to a few hard substances like glass and diamonds. There is no free movement of electrons. Uses include semiconductors and ceramics

a)

covalent network Bonds

b)

ionic bonds

c)

metallic bonds

d)

covalent bonds

59.
a)

1

b)

2

c)

3

d)

4

60.

This is the correct lewis dot structure for sodium floride

a)

True

b)

False

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