Chemistry Chapter 4 Entry Test MCQs
Topic 4:
Intermolecular Forces of attraction
1. Naphthalene is soluble in carbon tetrachloride due to the force
a. Debye forces
b. Hydrogen bonding
c. Van der Waals’s force
d. Dipole – dipole force
2. Which one of the following arrangements represents the correct order of increasing interactions?
a. London forces, Dipole – Dipole, Hydrogen bonding
b. Hydrogen bonding, London forces, Dipole – Dipole
c. Dipole – Dipole, London forces, Hydrogen bonding
d. London force, Hydrogen bonding, Dipole – Dipole
3. Hydrogen bonding links one spiral (DNA) to the other. The H-bonding is more dominant between
a. O and H
b. C and H
c. O and N
d. N and H
4. The compound soluble in water not through hydrogen bonding is
a. Urea
b. Sugar
c. Glucose
d. Salt
5. The polarizabilities of elements mostly increase down the group due to the
a. Increase in the number of shell
b. Increase in the atomic number
c. The behaviour of element remains the same
d. Increase in the number of protons
6. London forces are more significant in
a. Ionic solids
b. Polar molecules
c. Non polar molecules
d. Metals
7. Kerosene is liquid at room temperature due to
a. Dipole-dipole forces
b. Hydrogen bonding
c. Molecular size
d. Organic nature
8. Which one of the following exhibits dipole-dipole attraction between molecules?
a. CO2
b. SnCl2
c. BCl3
d. CH4
9. Rather than gases liquid contains __
a. High molecular motion
b. Fix shape
c. Weak forces of attraction
d. Fix volume
10. The strongest H-bond is
a. H −N−δ—H+δ −N
b. H −O−δ—H+δ −O
c. H −Cl−δ—H+δ −Cl
d. H −F−δ—H+δ −F
11. The intermolecular attractive forces vary in the order
a. Alcohol < Water < Ether
b. Water < Alcohol < Ether
c. Water < Ether < Alcohol
d. Ether < Alcohol < Water
12. The strength of H – Bond is how many times less than that of a covalent bond?
a. 30 times
b. 10 times
c. 40 times
d. 20 times
13. The angle formed between H – Bonds and covalent bonds in HF molecules is equal to:
a. 900
b. 600
c. 1800
d. 1200
14. Which of the following molecules will not form a hydrogen bond with another of its own molecules?
a. CH3NH2
b. CH3CHO
c. NH3
d. CH3OH
15. Among hydrides of group VA, which has highest boiling point:
a. AsH3
b. PH3
c. NH3
d. SbH3
16. The chloroform and acetone are miscible due to hydrogen bonding. The type of force between chloroform molecules is
a. Van der Waals’s force
b. Hydrogen bonding
c. Debye forces
d. Dipole – dipole force
17. London dispersion forces are the only forces present among the
a. Molecules of NH3
b. Molecules of waxy solid hydrocarbons
c. Molecules of Noble gases at high temperature
d. Molecules of Alcohol in vapour phase
18. Density of liquid water _ if temperature decreases from 25oC to 0oC
a. Increases
b. Decreases
c. First decreases and then increases
d. First increases and then decreases
19. Which of the followings does not match?
a. CH3COCH3 and CH3COCH3 → dipole-dipole force
b. H2O and Na+ → Ion dipole force
c. C6H12O6 and H2O → Hydrogen bonding
d. HCl and Ar → Dipole-dipole force
20. A substance that is soluble in water due to dipole-induced dipole force
a. Kr
b. C6H12O6
c. H2S
d. HCl
21. Which of the following H-bonds is expected to be of maximum strength?
a. H-S… . H
b. H-O… .H
c. H-Cl… .H
d. H-N….H
22. Water becomes less dense with temperature decreasing:
a. below 4oC
b. upto 10oC
c. up to 4oC
d. upto 100oC
23. The predominant forces among which of the following molecules are London dispersion forces?
a. Water
b. Diethyl ether
c. Glycerol
d. Ethanol
24. Which intermolecular force is the strongest?
a. Dipole-dipole interactions
b. London dispersion forces
c. Metallic bonding
d. Hydrogen bonding
25. Ice floats on the surface of water due to
a. hexagonal structure of ice
b. tetrahedral structure of water
c. planar structure of ice
d. polarity in water