Chemical Bonding and Molecular Structure Test

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Chemical Bonding and Molecular Structure Test - 6

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Weekly Quiz Competition

Question 1
4 / -1

Which of the following compounds shows maximum hydrogen bonding?

A
HF

B
H₂O

C
NH

D
CH₃OH

Solution

Greater the electro negativity and smaller the size of the atom, stronger is the H-bond
Question 2
4 / -1

Hydrogen bond between two atoms is formed due to

A
Displacement of electrons towards more electronegative atom resulting in fractional positive chargeon hydrogen

B
Displacement of electrons towards hydrogenatom resulting in a polar molecule

C
Formation of a bond between hydrogen atoms of one molecule and the other

D
Existence of an attractive force which binds hydrogen atoms together.

Solution

Hydrogen bonding occurs when H atom is linked to an electronegative atom like F, O or N. It is the force of attraction between small positive charge developed on H atom and small negative charge developed on electronegative atom due to displacement of electrons towards more electronegative atom.
Question 3
4 / -1

Which of the following statements is true about hydrogen bonding?

A
Cl and N have comparable electronegativities yet there is no H-bonding in HCl because size of Cl is large

B
Intermolecular H-bonding results in decrease in m.p. and b.p

C
Ice has maximum density at 0⁰C due toH-bonding

D
KHCI₂₍HCI^-₂) exists but KHF₂(HF^-₂) does not exist due to lack of H-bonding in HCl

Solution

For hydrogen bonding, the size of the atom should be small.
Question 4
4 / -1

Which of the following has strongest bond?

A
HF

B
HCl

C
HBr

D
HI

Solution

Due to largest difference in electronegativity, H—F bond is strongest.
Question 5
4 / -1

Which of the following observations can be explained on the basis of hydrogen bonding?
(i) H—F has higher boiling point than other halogen acids.
(ii) H₂O has highest boiling point among hydrides of group 16 elements.
(iii) NH₃ has lower boiling point than PH₃.

A
(i), (ii) and (iii)

B
(i) and (iii)

C
(ii) and (iii)

D
(i) and (ii)

Solution

Statement (iii) is not true since NH₃ has higher boiling point than PH₃ due to hydrogen bonding.
Question 6
4 / -1

Paramagnetism is shown by the molecules which have

A
Paired electrons

B
Unpaired electrons

C
Lone pair of electrons

D
Bond order more than one.

Solution

Presence of unpaired electrons makes a
molecule paramagnetic. More the number of unpaired electrons, higher is the paramagnetism.
Question 7
4 / -1

Though covalent in nature, methanol is soluble in water, why?

A
Methanol is transparent like water

B
Due to hydrogen bonding between methanol and water molecules

C
Due to van der Waals' forces between methanoland water

D
Due to covalent attraction forces

Solution

In methanol, R is —CH₃ group.
Hydrogen bonding between methanol and water.
Question 8
4 / -1

The ice floats on water because

A
Solids have lesser density than liquids

B
It has open-cage like structure in which lesser molecules are packed per mL than water

C
Ice is lighter than water

D
When ice is formed water molecules come closer and start floating.

Solution

Density of ice is less than water due to an open cage structure formed by hydrogen bonding.
Question 9
4 / -1

Which of the following molecules shows intramolecular hydrogen bonding?

A
o-Nitrophenol

B
p-Nitrophenol

C
Benzoic acid

D
Ethanol

Solution
Question 10
4 / -1

Which of the following statements is not true?

A
Intermolecular hydrogen bonds are formed between two different molecules of compounds

B
Intramolecular hydrogen bonds are formed between two different molecules of the same compound

C
Intramolecular hydrogen bonds are formed within the same molecule

D
Hydrogen bonds have strong influence on the physical properties of a compound

Solution

Intramolecular hydrogen bonds are formed within the same molecule.

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Chemical Bonding and Molecular Structure Test - 6

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Chemical Bonding and Molecular Structure Test - 6

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Question 1

HF

H2O

NH

CH3OH

Solution

Question 2

Displacement of electrons towards more electronegative atom resulting in fractional positive chargeon hydrogen

Displacement of electrons towards hydrogenatom resulting in a polar molecule

Formation of a bond between hydrogen atoms of one molecule and the other

Existence of an attractive force which binds hydrogen atoms together.

Solution

Question 3

Cl and N have comparable electronegativities yet there is no H-bonding in HCl because size of Cl is large

Intermolecular H-bonding results in decrease in m.p. and b.p

Ice has maximum density at 00C due toH-bonding

KHCI2(HCI-2) exists but KHF2(HF-2) does not exist due to lack of H-bonding in HCl

Solution

Question 4

HF

HCl

HBr

HI

Solution

Question 5

(i), (ii) and (iii)

(i) and (iii)

(ii) and (iii)

(i) and (ii)

Solution

Question 6

Paired electrons

Unpaired electrons

Lone pair of electrons

Bond order more than one.

Solution

Question 7

Methanol is transparent like water

Due to hydrogen bonding between methanol and water molecules

Due to van der Waals' forces between methanoland water

Due to covalent attraction forces

Solution

Question 8

Solids have lesser density than liquids

It has open-cage like structure in which lesser molecules are packed per mL than water

Ice is lighter than water

When ice is formed water molecules come closer and start floating.

Solution

Question 9

o-Nitrophenol

p-Nitrophenol

Benzoic acid

Ethanol

Solution

Question 10

Intermolecular hydrogen bonds are formed between two different molecules of compounds

Intramolecular hydrogen bonds are formed between two different molecules of the same compound

Intramolecular hydrogen bonds are formed within the same molecule

Hydrogen bonds have strong influence on the physical properties of a compound

Solution

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H₂O

CH₃OH

Ice has maximum density at 0⁰C due toH-bonding

KHCI₂₍HCI^-₂) exists but KHF₂(HF^-₂) does not exist due to lack of H-bonding in HCl