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Chemistry Chemical Bonding

Total questions: 100

Worksheet time: 2hrs 33mins

Name
Class
Date
1.

Bond that forms due to electron TRANSFER (atoms gaining/losing electrons)

a)

covalent bond

b)

hydrogen bond

c)

metallic bond

d)

ionic bond

2.

Bond that forms due to electron SHARING.

a)

covalent bond

b)

hydrogen bond

c)

metallic bond

d)

ionic bond

3.

Bond that forms when electrons delocalize forming the "electron sea."

a)

covalent bond

b)

hydrogen bond

c)

metallic bond

d)

ionic bond

4.

This type of bond typically forms between a metal and a non-metal.

a)

covalent

b)

hydrogen

c)

metallic

d)

ionic

5.

Heitler and London introduced which theory?

a)

VSEPR Theory

b)

Valence Bond Theory

c)

Molecular Orbital Theory

d)

Covalent Theory

6.

Energy released during bond formation is called

a)

Bond Creation Energy

b)

Disassociation Energy

c)

Binding Energy of Molecules

d)

Bond Enthalpy

7.

Greater the overlap of the orbitals, _________________________

a)

lesser the bond strength

b)

greater the bond strength

c)

bond strength remains the same

d)

no bond formation

8.
If electrons are shared unequally then the bond is....
a)
Non-polar covalent
b)
Ionic
c)
Non-polar ionic
d)
Polar covalent
9.
 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
10.
Which of the following shapes has an unshared pairs of electrons on the central atom? 
a)
Bipyramidal
b)
Bent
c)
Trigonal Planar
d)
Tetrahedral
11.
What molecule could this be? 
a)
BF3
b)
CH4
c)
H2O
d)
CO2
12.
What molecule could this be? 
a)
H2O
b)
CCl4
c)
PCl5
d)
NaCl
13.
VSEPR theory is to
a)
determine the number of bonding and lone pairs electrons
b)
determine the number of ECC
c)
determine the shape and geometry of molecule
d)
determine the lewis structure of molecule
14.

What is the hybridization of a linear molecule?

a)

sp

b)

sp2

c)

sp3

d)

sp3d

15.

What is the hybridization of the Carbon atom indicated by the arrow?

a)

sp hybridization

b)

sp2 hybridization

c)

sp3 hybridization

d)

dsp3 hybridization

16.
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
17.
How many are shared in a double bond?
a)
2
b)
4 pairs
c)
6
d)
4
18.

Draw the Lewis Dot structure for ICl2- and determine its predicted molecular geometry.

a)

see-saw

b)

trigonal bipyramidal

c)

linear

d)

bent

19.
Which of these is covalent?
a)
NaCl
b)
Pb(NO3)2
c)
CO2
d)
AlCl3
20.

Atoms that are sp2 hybridized form ____ pi bond(s).

a)

0

b)

1

c)

2

d)

3

e)

4

21.

A π (pi) bond is the result of the

a)

overlap of two s orbitals

b)

overlap of an s orbital and a p orbital

c)

overlap of two p orbitals along their axes

d)

sidewise overlap of two parallel p orbitals

e)

sidewise overlap of two s orbitals

22.
Carbon atom undergo
a)
sp hybridization
b)
sp2 hybridization
c)
sp3 hybridization
d)
dsp3 hybridization
23.

What is the hybridization of the carbon (C) atoms in this molecule?

a)

sp3

b)

sp2

c)

sp

d)

unhybridized

24.

What is the bond angle for the CH4 molecule?

a)

120°

b)

107°

c)

109.5°

d)

90°

25.
What is the VSEPR theory used to predict?
a)
Bond Strength
b)
Polarity
c)
Molecular Shape
d)
Electronegativity
26.

BMO is formed due to

a)

Constructive Interference

b)

Destructive Interference

c)

Different sign of wave function

d)

Both 2 & 3

27.

NBMO is formed due to

a)

Constructive Interference

b)

Destructive Interference

c)

Non matching symmetry

d)

Both 1 & 2

28.

Sigma bond is formed when overlapping takes place along (if z-axis is inter nuclear axis)

a)

x-axis

b)

y-axis

c)

z-axis

d)

All axis

29.

Which sub shell has more stability????

a)

3d

b)

4p

c)

5s

d)

4d

30.

Which orbital has nodal plane????

a)

BMO

b)

ABMO

c)

NBMO

d)

All of these

31.

Which is pie bond combination????

a)

2s-2s

b)

2s-2px

c)

2px-2px

d)

None of these

32.

If 3 AOS take part in bonding, they results in

a)

1 BMO , 2 ABM0

b)

3 NBMO

c)

1 BMO, 1 ABMO

d)

1 BMO, 1 ABMO, 1 NBMO

33.

Which Quantum Number is used to describe Sub shell????

a)

n

b)

l

c)

m

d)

s

34.

What is value of SUBSIDIARY Quantum Number for 3d subshell

a)

0

b)

1

c)

2

d)

3

35.

What do you understand from the term 'Molecular Orbital' from the perspective of coordination chemistry?

a)

Mixing of atomic orbitals to form new set of orbitals

b)

Overlapping between orbitals of ligands to form new orbitals

c)

Overlapping between orbitals of ligands and orbitals of metal to form new orbitals

d)

Electrostatic attraction between metal and ligands

36.

For octahedral complexes with sigma overlapping, what is the total number of electrons in the molecular orbitals?

a)

8 electron from ligands + electrons in d orbital of metal

b)

12 electron from ligands + all electrons of the metal

c)

12 electron from ligands + electrons in d orbital of metal

d)

18 electron from ligands + electrons in d orbital of metal

37.

Which of the following are the pi-acceptor ligands?

a)

CN-

b)

CO

c)

Cl

d)

NO2-

38.

What is total number of electrons in molecular orbitals of tetrahedral complex?

a)

12 electrons from ligands + all electrons from metal

b)

12 electrons from ligands + electrons in d orbital of metal

c)

8 electrons from ligands + all electrons from metal

d)

8 electrons from ligands + electrons in d orbital of metal

39.

Which statement is false? A sigma molecular orbital

a)

may result from overlap of p atomic orbitals perpendicular to the molecular axis (side-on)

b)

may result from overlap of p atomic orbitals along the molecular axis (head-on)

c)

may result from overlap of two s atomic orbitals

d)

may result from overlap of one s and one p atomic orbitals

40.

Significance of bond order

a)

To indicate bond strength

b)

To indicate bond length

c)

To indicate the existence of a molecule

d)

All of the mentioned

41.

According to Molecular Orbital Theory, the shape and size of a molecular orbital depends upon _________

a)

Shape and size of the combining atomic orbitals

b)

Numbers of the combining atomic orbitals

c)

Orientation of the combining atomic orbitals

d)

All of the mentioned

42.

Choose the incorrect statement from the following options.

a)

In bonding molecular orbital, electron density is low in the region between the nuclei of bonded atoms

b)

The energy of antibonding molecular orbital is higher than that of atomic orbitals from which it is formed

c)

Every electron in bonding molecular orbital contributes toward stability of the molecule

d)

Antibonding takes place when lobes of atomic orbitals have different signs

43.

The filling of molecular orbital takes place according to __________

a)

The Aufbau Principle

b)

Pauli Exclusion Principle

c)

Hund’s rule of maximum multiplicity

d)

All of the mentioned

44.

Antibonding molecular orbitals are produced by

a)

constructive interaction of atomic orbitals.

b)

destructive interaction of atomic orbitals.

c)

the overlap of the atomic orbitals of two negative ions

d)

none of these

45.

Give the orbital designation.

a)

σ2p

b)

π2p

c)

σ*2p

d)

π*2p

46.

Give the orbital designation.

a)

π2p

b)

π*2p

c)

σ2p

d)

σ*2p

47.

Draw the Lewis Dot structure for ICl2- and determine its predicted molecular geometry.

a)

see-saw

b)

trigonal bipyramidal

c)

linear

d)

bent

48.

Which of the following is octahedral?

a)

SCl6

b)

XeI4

c)

NBr5

d)

CH4

49.

Two carbon atoms form a linear shaped ethene, C2H4, molecule when bonded with four other hydrogen atoms. Prior to bonding, the carbon atom

a)

does not hybridise

b)

undergoes sp hybridisation

c)

undergoes sp2 hybridisation

d)

undergoes sp3 hybridisation

50.

Which of the following hybrid orbitals is used by the central atom for bonding in CO32-?

a)

sp2

b)

sp3

c)

sp3d

d)

sp3d2

51.

The molecule that uses sp3d hybrid orbital on the central atom is

a)

BCl3

b)

NCl3

c)

ICl3

d)

PCl3

52.

Molecule CO2

a)

undergoes sp2 hybridisation

b)

has 2 σ bond and 2 π bond

c)

undergoes sp3d hybridisation

d)

is trigonal planar molecule

53.

What is the hybridization of PF5?

a)

sp3

b)

sp3d

c)

sp3d2

d)

sp2

54.
Sulfur atom undergo
a)
sp hybridization
b)
sp2 hybridization
c)
sp3 hybridization
d)
dsp3 hybridization
55.
Nitrogen atom undergo
a)
sp hybridization
b)
sp2 hybridization
c)
sp3 hybridization
d)
dsp3 hybridization
56.
This term describes the energy used to break a covalent bond
a)
energy of activation
b)
bond dissociation energy
c)
electronegativity
d)
resonance energy
57.

Which of the following does not determine the shape of a molecule?

a)

electron pairs around the central atom

b)

lone pair of electrons on other attached atoms

c)

lone pair of electrons around the central atom

d)

number of attached atoms

58.

What name is given to the shape shown in the picture?

a)

bent

b)

trigonal planar

c)

triangular

d)

trigonal pyramidal

59.

What is the bond angle in the shape shown here?

a)

109.5o

b)

120o

c)

107o

d)

104.5o

60.

What is the approximate bond angle in nitrogen fluoride, NF3?

a)

90o

b)

120o

c)

107o

d)

60o

61.

The 109.5o bond angle around each carbon atom in ethane is mainly due to?

a)

the lone pair of electrons on each carbon atom

b)

the sigma bonds around each carbon atom

c)

the four electron regions around each carbon atom

d)

the sp3 hybridised orbitals on each carbon atom

62.

Which species has a shape that is influenced by the presence of one or more lone pairs of electrons around the central atom?

a)

AlCl3

b)

ClF3

c)

IF6+

d)

PCl6–

63.

Which species has one or more bond angle(s) of 90°?

a)

CH4

b)

NH4+

c)

ClF4−

d)

AlCl4−

64.

Which is the most likely bond angle around the oxygen atom in ethanol?

a)

104.5°

b)

109.5°

c)

120°

d)

180°

65.

Which of these species is not planar?

a)

HCHO

b)

CH3+

c)

CH3OH

d)

C2H4

66.

Which of these species has a trigonal planar structure?

a)

PH3

b)

BCl3

c)

H3O+

d)

CH3−

67.

In which one of the following species is the shape influenced by the presence of one or more lone pairs of electrons?

a)

NH2-

b)

NH4+

c)

[CH3NH3]+

d)

[Co(NH3)6]2+

68.

Which one of the following molecules is not planar?

a)

BF3

b)

NCl3

c)

C2H4

d)

HCHO

69.

Which one of the following is the most likely value for the bond angle α shown in the diagram of SF4?

a)

118°

b)

101°

c)

90°

d)

88°

70.

Which one of the following molecules or ions is pyramidal in shape?

a)

BF3

b)

CH3+

c)

CH3-

d)

SF3-

71.

The acronym VSEPR stand for

a)

very strong electron pair repulsion.

b)

varied symmetry electrostatic proton reaction.

c)

venomous snakes enjoy pink ribbons.

d)

valence shell electron pair repulsion.

72.

VSEPR theory is used to predict

a)

the number of unshared pairs of electrons in a Lewis structure.

b)

the number of multiple bonds in a Lewis structure.

c)

the three-dimensional geometry of a molecule.

d)

the three-dimensional crystal lattice structure of ionic compounds.

73.

Any molecule with only two atoms must be linear. Three-atom molecules such as BeCl2 can also be linear. For linear molecules, the bond angle is

a)

360°360\degree

b)

180°180\degree

c)

120°120\degree

d)

90°90\degree

74.
Who could this be? 
a)
CO2
b)
NH3
c)
H2S
d)
CH4
75.

What shape would this have?

a)

Trigonal planar

b)

Pyramidal

c)

Tetrahedral

d)

Bent

76.
How many lone pairs are in this molecule's structure?
a)
6
b)
2
c)
0
d)
4
77.
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
78.
What molecular shape is the structure shown here? (BeCl2)
a)
linear
b)
bent
c)
trigonal planar
d)
tetrahedral
79.

What is the molecular geometry/shape of HCN?

a)

linear

b)

trigonal planar

c)

bent

d)

tetrahedral

80.

What is the molecular geometry/shape of a molecule with 4 shared pairs and 0 unshared pairs?

a)

Linear

b)

Bent

c)

Trigonal Pyramidal

d)

Tetrahedral

81.

Which molecule has non-linear shape?

a)

BeCl2

b)

HCN

c)

CO2

d)

PF5

82.

Application of VSEPR theory leads to the prediction that the shape of the IF3 is

a)

T-shaped

b)

Trigonal planar

c)

Bent

d)

Tetrahedral

83.

The bond angle of Cl-O-Cl in Cl2O molecule is approximately

a)

109o

b)

107o

c)

104o

d)

180o

84.

The pair that has the same geometry is

a)

NH2- and BeH2

b)

NH2- and H2O

c)

H2O and BeH2

d)

NH2- , H2O and BeH2

85.

According to the VSEPR theory, which of the following molecules should be trigonal bipyramidal?

a)

PCl3

b)

XeF3

c)

SF6

d)

PF5

86.

Based on valence shell electron pair repulsion (VSEPR), the shape of ClF3 molecule is

a)

T-shaped

b)

Trigonal planar

c)

Bent

d)

Tetrahedral

87.

According to MOT the number of Molecular orbitals formed is equal to

a)

Multiple of the overlapping atomic orbitals

b)

Half of the overlapping atomic orbitals

c)

Same number of the overlapping atomic orbitals

d)

No matter of formation of molecular orbitals

88.

The maximum number of electrons can be accommodated in a molecular orbital are-----------

a)

4

b)

2

c)

6

d)

8

89.

According to VBT, the formation of a stable bond requires

a)

The electrons should have opposite spins

b)

The two atoms should be close to each other

c)

The greater overlapping of the electron clouds

d)

All of the mentioned

90.

The energy of Bonding molecular orbitals -----------in correspondent with overlapping atomic orbitals.

a)

Greater

b)

Lesser

c)

Same

d)

Not applicable

91.

The number of electrons for n= 4 quantum number

a)

2

b)

6

c)

16

d)

18

92.

Which of the following has a full valence shell?

a)

Oxygen

b)

Neon

c)

Barium

d)

Carbon

93.

----------------orbitals that have the same energy

a)

Bonding MO

b)

Degenerate Orbitals

c)

Anti-Bonding MO

d)

Atomic Orbitals

94.

-----------------molecular orbital located outside of the region between two nuclei

a)

Degenerate Orbitals

b)

Bonding Molecular

c)

Antibonding Orbital

95.

What are the bond angles in this molecule?

a)

all are exactly 90o

b)

all are slightly more than 90o

c)

all are slightly less than 90o

d)

more information is needed

e)

some of the bonds are 90o, others are 120o

96.
This structure is called...
a)
tetrahedral
b)
Trigonal pyramidal
c)
Seesaw
d)
Bent/Angular
97.
Xe atom undergo
a)
sp hybridization
b)
sp2 hybridization
c)
sp3 hybridization
d)
dsp3 hybridization
98.

Heitler and London introduced which theory?

a)

VSEPR Theory

b)

Valence Bond Theory

c)

Molecular Orbital Theory

d)

Covalent Theory

99.

States that “the repulsion between electron pairs causes molecular shapes to adjust so that the valence-electron pairs stay as far apart as possible”.

a)

VSEPR theory

b)

Dalton theory

c)

Particle theory

100.

A molecular orbital that can be occupied by two electrons of a covalent bond is called a bonding orbital.

a)

True

b)

False

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