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Chemical Bonding and shapes

Total questions: 43

Worksheet time: 47mins

Name
Class
Date
1.
Which of the following has a full valence shell?
a)
Oxygen
b)
Neon
c)
Barium
d)
Carbon
2.
An ionic bond forms when atoms ___________ electrons.
a)
gain
b)
share
c)
increase
d)
transfer
3.
Chemical bonds form when atoms
a)
combined nuclei
b)
give up neutrons
c)
gain protons
d)
share or transfer electrons
4.
If an atom loses two electrons what charge will it have?
a)
+ 2
b)
 - 2
c)
+1
d)
-1
5.
How many valence electrons in this structure?
a)
6
b)
5
c)
4
d)
7
6.
What is the electron configuration of sodium?
a)
2.8
b)
2.8.2
c)
2.8.1
d)
11
7.
 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
8.

What is the molecular structure?

a)

Bent/Angular

b)

Linear

c)

Trigonal Planar

d)

Trigonal Pyramidal

9.

What is the molecular shape of the following?

a)

Bent

b)

Linear

c)

SeeSaw

d)

Octahedral

10.

What is the molecular shape of the following?

a)

Tetrahdral

b)

Trigonal Bipyramid

c)

See-Saw

d)

Bent

11.

What is the molecular shape of the following?

a)

Trigonal BiPyramid

b)

Tetrahedral

c)

Trigonal Planar

d)

T-Shape

12.
What is the shape of this molecule?
a)
Linear
b)
Bent
c)
Tetrahedral
d)
Trigonal Pyramidal
13.

Is this molecule polar or non-polar?

a)

Polar

b)

Non-polar

14.

Is this molecule polar or non-polar?

a)

Non-polar

b)

Polar

15.
What is the measure of a tetrahedral bond angle?
a)
90 Degrees
b)
109.5 Degrees
c)
120 Degrees
d)
180 Degrees
16.

The polarity of a bond between two elements can be best determined by

a)

The difference in electronegativity between the elements

b)

The difference in first ionization energy between the elements

c)

The number of electrons shared in the bond

d)

The difference in atomic radius between the elements

17.

Which of the following molecules has Π bonds?

a)

CO2

b)

BF3

c)

NH3

d)

H2O

18.
How many sigma and pi bonds does this have?
a)
1 sigma and 1 pi
b)
2 sigma and 1 pi
c)
1 sigma and 2 pi
d)
2 sigma and 2 pi
19.

Which of the following molecules are polar molecule?

a)

HCl

b)

H2O

c)

CH4

d)

NH3

20.
In chemical compounds, covalent bonds form when
a)
the electronegativity difference between two atoms is very large.
b)
electrons are completely transferred between two metals.
c)
pairs of electrons are shared between two nonmetal atoms.
d)
two nonmetal atoms are attracted to each other by opposite charges.
21.
Which of the following is a characteristic property of ionic compounds?
a)
They form hard, brittle crystals with characteristic shapes
b)
They have low melting points
c)
They have low boiling points
d)
They contain no charged particles
22.
Write the correct chemical formula for Ag +  and  Br -
a)
AgBr
b)
silver bromide
c)
Ag2Br2
d)
gold bromide
23.
Name the following ionic compound: MgSO4
a)
magnesium sulfoxide
b)
magnesium sulfide
c)
magnesium sulfate
d)
magnesium oxide
24.

Chemical bond formed from the electrostatic attraction between positive and negative ions

a)

covalent bond

b)

ionic bond

c)

metallic bond

25.

Use VSEPR theory to predict the shape of the hydrogen chloride molecule, HCl.

a)

tetrahedral

b)

linear

c)

bent

d)

trigonal planar

26.

Use VSEPR theory to predict the shape of the chlorate ion, ClO3–.

a)

trigonal planar

b)

octahedral

c)

trigonal pyramidal

d)

bent

27.
Which of the following is an example of an IONIC COMPOUND?
a)
NaCl
b)
H2O
c)
CO2
d)
NO
28.
Which is the correct name for CaBr2?
a)
Calcium Bromine
b)
Bromine Calcium
c)
Calcium Bromide
29.
The chemical formula of carbon tetrachloride is
a)
CCl
b)
C₄Cl
c)
CCl₄
d)
C(IV)Cl
30.

Which is the correct description about van der Waals' forces?

a)

They are the weakest of the intermolecular forces arising from instantaneous dipole - induced dipole interactions.

b)

They are the strongest of the intermolecular forces arising from dipole - dipole interactions.

31.

Which of the following molecules are held together by van der Waals’ forces and hydrogen bonds?

a)

Ammonia

b)

Carbon dioxide

c)

Chloromethane

d)

Hydrogen sulphide

32.
Which of the following is NOT considered a diatomic element?
a)
Carbon
b)
Nitrogen
c)
Chlorine
d)
Iodine
33.

What is considered a Hydrogen Bond?

a)

H-Pb

b)

H-Fe

c)

H-O

d)

All of the above

34.

Can ammonia, NH3 form hydrogen bonds?

a)

Yes

b)

No

35.
Which of the following has the highest boiling point?
a)
H2
b)
NH3
c)
N2
d)
O2
36.
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.
37.

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

38.

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

a)

higher

b)

lower

39.

________________________ have the strongest intermolecular forces of attraction.

a)

Dipole- Dipole

b)

Dispersion

c)

Hydrogen Bonds

40.
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
41.
The strength of temporary dipoles:
a)
increases with the size of molecules
b)
is greater than intremolecular forces
c)
is the strongest intermolecular force
42.
How many electrons are shared between two atoms that are triple bonded?
a)
6
b)
2
c)
4
d)
8
43.

Which type of IMF is responsible for the attraction pictured above?

a)

Dipole-Dipole Interaction

b)

Ion-Dipole Interaction

c)

Hydrogen Bonds

d)

Covalent Bond

e)

Ionic Bond

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