Hydrogen Bonding and its Applications NEET Questions

Physical Chemistry - Chemical Bonding and Molecular Structure

Hydrogen Bonding and its Applications MCQ Questions


13.
Which of the following correctly describes the geometry around an oxygen atom in liquid water due to hydrogen bonding?
A.
Each O atom is surrounded by 6 other O atoms in an octahedral arrangement
B.
Each O atom is surrounded by 2 other O atoms in a linear arrangement
C.
There is no preferred geometry; arrangement is completely random
D.
Each O atom is surrounded by approximately 4 other O atoms in a roughly tetrahedral arrangement
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ANSWER :
D. Each O atom is surrounded by approximately 4 other O atoms in a roughly tetrahedral arrangement
14.
The boiling point order H₂O > HF > NH₃ is best explained by:
A.
Increasing molecular mass: H₂O > HF > NH₃
B.
Number of hydrogen bonds per molecule and overall hydrogen-bond network strength
C.
Order of electronegativity of the heavy atoms only
D.
Increasing covalent bond strength of X–H bonds
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ANSWER :
B. Number of hydrogen bonds per molecule and overall hydrogen-bond network strength
15.
DNA's double-helix structure is held together by:
A.
Covalent bonds between the two strands
B.
Ionic bonds between the phosphate groups
C.
Metallic bonds between the bases
D.
Hydrogen bonds between complementary base pairs (A–T and G–C)
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ANSWER :
D. Hydrogen bonds between complementary base pairs (A–T and G–C)
16.
Why does ice float on water?
A.
Air bubbles trapped in ice make it less dense
B.
Ice has stronger covalent bonds than liquid water
C.
Ice molecules are lighter than water molecules
D.
Hydrogen bonding produces an open, hexagonal cage-like structure in ice with more empty space than in liquid water, lowering its density
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ANSWER :
D. Hydrogen bonding produces an open, hexagonal cage-like structure in ice with more empty space than in liquid water, lowering its density
17.
The maximum density of water occurs at approximately:
A.
100°C
B.
4°C
C.
25°C
D.
0°C
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ANSWER :
B. 4°C
18.
Which of the following best explains why HF (b.p. 19.5°C) has a lower boiling point than H₂O (b.p. 100°C), even though F is more electronegative than O?
A.
Each H₂O molecule can form 4 hydrogen bonds (2 donor + 2 acceptor), while each HF molecule has only 1 H atom available for donating
B.
F is much smaller than O, making H-bonds in HF weaker
C.
HF has stronger covalent bonds, leaving less energy for H-bonding
D.
Water has a lower molecular mass than HF
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ANSWER :
A. Each H₂O molecule can form 4 hydrogen bonds (2 donor + 2 acceptor), while each HF molecule has only 1 H atom available for donating