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TEST5 Bonding & Naming REVIEWF23

Total questions: 47

Worksheet time: 35mins

Name
Class
Date
1.
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.
2.
Intermolecular force present in HCl?
a)
dipole dipole
b)
dispersion
c)
H-bond
d)
ionic
3.
Ionic Bonding involves...
a)
The transfer of protons
b)
The transfer of nuetrons 
c)
The transfer of electrons
d)
None Of the above
4.

Which substance has the weakest intermolecular forces?

a)

Substance A, boiling point of 75 °C

b)

Substance B, boiling point of 105 °C

c)

Substance C, boiling point of 25 °C

d)

Substance d, boiling point of 45 °C

5.

The weaker the intermolecular forces of a substance the _____________ the boiling point

a)

higher

b)

lower

6.
Which of the following statements correctly explains why hydrogen bonding is such a strong intermolecular force?
a)
There is an attraction between a small, weakly electronegative hydrogen atom and a large, strongly electronegative atom of fluorine, nitrogen, or oxygen
b)
There is an attraction between a small, highly electronegative hydrogen atom and a large, highly electronegative fluorine atom
c)
There is an attraction between the hydrogen and oxygen atoms, only
d)
There is an attraction between the hydrogen and nitrogen atoms, only
7.

Water has an unusually high boiling point for a molecular compound because it has

a)

hydrogen bonding

b)

ion-ion attractions

c)

a high density

d)

a large gram formula mass

8.

In a polar covalent bond, the electrons gather around...

a)

Mostly the atom with the greatest electronegativity

b)

The atom with the lowest electronegativity

c)

Each atom equally

d)

Only the atom with the greatest electronegativity

9.

In a nonpolar covalent bond, the electrons gather around...

a)

Mostly the atom with the greatest electronegativity

b)

The atom with the lowest electronegativity

c)

Each atom Equally

d)

Only the atom with the greatest electronegativity

10.

The polarity of a bond is determined by...

a)

The sum of the electronegativities of the two atoms

b)

The difference in the electronegativities of the two atoms

c)

The charges of the atoms

d)

The number of electrons shared in the bond

11.
Rank these in order of strength:
covalent bond
London forces
hydrogen bond
dipole-dipole attraction
a)
dipole-dipole>covalent bond>hydrogen bond>London
b)
London>dipole-diple>hydrogen bond>covalent bond
c)
covalent bond>hydrogen bond>dipole-dipole>London
d)
hydrogen bond>dipole-dipole>London>covalent bond
12.
Intermolecular forces are the forces
a)
within molecules
b)
between molecules
13.

This is an example of a(n) __________.

a)

Hydrogen Bonding

b)

Dipole

c)

Nonpolar Molecule

d)

Intermolecular Force

14.

The forces that hold the atoms in a CCl4 molecule together are _______, and the forces that hold the molecules together in sample are _________.

a)

intermolecular (covalent); intramolecular (dipole-dipole)

b)

intermolecular (dipole-dipole); intramolecular (dipole-dipole)

c)

intramolecular (covalent); intermolecular (London Dispersion)

d)

intramolecular (covalent); intermolecular (dipole-dipole)

15.

Which of the following types of bonding results in materials which are malleable and ductile?

a)

ionic bonding

b)

metallic bonding

c)

covalent bonding

16.

Which of the following types of bonding results in materials which have the highest melting and boiling points?

a)

ionic bonding

b)

metallic bonding

c)

covalent bonding

17.

In the case of metallic bonding, the greater the number of delocalized electrons, the ________ the metallic bond strength.

a)

weaker

b)

stronger

18.

Which type of bond is polar?

a)

Cl - Cl

b)

C - Cl

19.

What type of force?

a)

intermolecular

b)

intramolecular

20.

What type of force?

a)

intermolecular

b)

intramolecular

21.

What type of bond/force?

a)

nonpolar covalent because of a low difference in electronegativity

b)

polar covalent because of a high difference in electronegativity

c)

metallic because of a low difference in electronegativity

d)

ionic because of a high difference in electronegativity

22.

What type of bond/force?

a)

nonpolar covalent because of a high difference in electronegativity

b)

nonpolar covalent because of a low difference in electronegativity

c)

ionic because of a high difference in electronegativity

d)

ionic because of a low difference in electronegativity

23.

Two elements and their electronegativities are shown.

X- 1.1

Y- 2.9

What type of bond would they form and why?

a)

nonpolar covalent because the EN difference is greater than 1.5

b)

polar covalent because the EN difference is greater than 1.5

c)

ionic because the EN difference is between 0.5 and 1.5

d)

metallic because they would share all electrons equally

24.

Based on the table, which substance has the strongest intermolecular forces?

a)

Sample 1

b)

Sample 2

c)

Sample 3

d)

Sample 4

25.

According to the VSEPR theory, ... want to ... each other.

a)

protons, repel

b)

protons, attract

c)

electrons, repel

d)

electrons, attract

26.
What is the VSEPR theory used to predict?
a)
Bond Strength
b)
Polarity
c)
Molecular Shape
d)
Electronegativity
27.

What molecular geometry would PH3 have?

a)

Trigonal Pyramidal

b)

Trigonal Bipyramidal

c)

Bent

d)

Linear

28.

What is the molecular shape of OCl2?

a)

linear

b)

bent

c)

tetrahedral

d)

trigonal planar

29.
How many electrons are shared in a triple bond?
a)
6
b)
3
c)
6 pairs
d)
5
30.

Which of these molecules is trigonal planar?

a)

Hydrogen Sulfide (H2S)

b)

Carbon Dioxide (CO2)

c)

Phosphorus Trichloride (PCl3)

d)

Formaldehyde (CH2O)

31.

What is the central atom for formaldehyde (CH2O)?

a)

Carbon

b)

Hydrogen

c)

Oxygen

d)

There is no central atom

32.

How many BONDS are in the diagram of this molecule

(a)  

33.

How many TOTAL VALENCE ELECTRONS are in the diagram of this molecule

(a)  

34.

The effect of lone pairs of electrons on molecular geometry is

a)

to push other atoms closer together because lone pairs are

localized on only one nucleus, so they spread out more.

b)

to allow the other atoms to be further apart because lone pairs

take up less space than bonding pairs.

c)

to create an aysmmetical distribution of the electrons within

the atom, thus creating a polar molecule by creating dipoles.

d)

to help to create resonance structures through the formation of

pi bonds.

35.

The name of FeCl₂ is

a)

iron chloride

b)

iron (II) chloride

c)

iron (I) chloride

d)

iron dichloride

36.

Name the following ionic compound: BeCl2

a)

beryllium chlorine

b)

beryllium II chloride

c)

beryllium chloride

d)

beryllium dichloride

37.
phosphorus trichloride
a)
KCl3
b)
PCl3
c)
K3Cl
d)
P3Cl
38.

What is the name for CO

a)

Carbon Oxide

b)

Carbon Oxygen

c)

Carbon Monoxide

d)

Carbon Dioxide

39.
True or false: When naming ionic compounds, use prefixes to indicate subscripts
a)
True
b)
False
40.
What is the name for SrO?
a)
strontium monoxide
b)
strontium oxide
c)
strontium (II) oxide
d)
strontium oxygen (II)
41.
Iron(II) oxide would be written in formula form as 
a)
Fe2O3
b)
FeO
c)
Fe3O2
d)
cannot be determined 
42.
What is the chemical formula for Tetrasulfur pentoxide?
a)
SO
b)
S4O
c)
S4O5
d)
S5O4
43.
What is the name of a mutivalent ionic compound made from copper (Cu2+) and oxygen?
a)
copper oxygen.
b)
copper oxide.
c)
dicopper oxide.
d)
copper(II) oxide.
44.
How do the following two elements bond together?
K1+  S2- 
a)
KS
b)
K8S
c)
K6S3
d)
K2S
45.
How do the following two elements bond together?
Cr3+  O2-         
a)
CrO
b)
Cr3O2
c)
Cr2O3
d)
CrO3
46.
This could be the dot diagram of
a)
Mg
b)
Cl
c)
C
d)
O
47.
Which of the following is the correct Lewis dot structure for the molecule fluorine (F2)?
a)
A
b)
B
c)
C
d)
D

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