chemistry : class12 Intermolecular forces : Physical properties of haloalkanes : Haloalkanes and Haloarenes MCQ Questions and Answers
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Intermolecular forces
MCQ questions and answers.
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MCQ Questions
1. Which intermolecular force is present between haloalkane molecules because of their polar carbon-halogen bonds?
A.
Dipole-dipole attraction
B.
Hydrogen bonding
C.
Ionic attraction
D.
Metallic bonding
Correct Answer:
Dipole-dipole attraction
Explanation:
Haloalkanes contain polar carbon-halogen bonds, so their molecules experience dipole-dipole attractions.
2. Which intermolecular force is present in all haloalkanes, including nonpolar ones?
A.
Hydrogen bonding
B.
London dispersion force
C.
Ionic attraction
D.
Covalent bonding between molecules
Correct Answer:
London dispersion force
Explanation:
London dispersion forces arise from temporary fluctuations in electron distribution and are present in all molecules.
3. Why do haloalkanes generally have higher boiling points than hydrocarbons of similar molecular mass?
A.
Haloalkanes have stronger intermolecular attractions due to their polar bonds
B.
Haloalkanes form ionic lattices
C.
Haloalkanes form hydrogen bonds with themselves
D.
Haloalkanes have metallic bonding
Correct Answer:
Haloalkanes have stronger intermolecular attractions due to their polar bonds
Explanation:
The polar carbon-halogen bonds produce dipole-dipole attractions, which can raise the boiling point compared with similar hydrocarbons.
4. Which intermolecular force is mainly responsible for the attraction between molecules of chloromethane?
A.
Dipole-dipole attraction
B.
Hydrogen bonding
C.
Ion-dipole attraction
D.
Metallic attraction
Correct Answer:
Dipole-dipole attraction
Explanation:
Chloromethane is a polar molecule, so its molecules attract one another through dipole-dipole forces, in addition to dispersion forces.
5. What happens to London dispersion forces when the number of electrons in haloalkane molecules increases?
A.
They generally become stronger
B.
They disappear completely
C.
They change into ionic bonds
D.
They become hydrogen bonds
Correct Answer:
They generally become stronger
Explanation:
A larger number of electrons makes the electron cloud more polarizable, strengthening London dispersion forces.
6. Which type of intermolecular force is not normally present between pure haloalkane molecules?
A.
London dispersion force
B.
Dipole-dipole attraction
C.
Hydrogen bonding
D.
Temporary dipole attraction
Correct Answer:
Hydrogen bonding
Explanation:
Haloalkane molecules do not usually contain hydrogen bonded to nitrogen, oxygen, or fluorine, so they do not form hydrogen bonds with one another.
7. Why can a haloalkane with a larger halogen atom have stronger intermolecular attractions than a similar haloalkane with a smaller halogen atom?
A.
Its electron cloud is more polarizable
B.
It forms more ionic bonds
C.
It forms hydrogen bonds
D.
It has metallic electrons
Correct Answer:
Its electron cloud is more polarizable
Explanation:
Larger halogen atoms have more easily distorted electron clouds, which increases London dispersion forces between molecules.
8. Which statement correctly describes the intermolecular forces in bromoethane?
A.
It has dipole-dipole and London dispersion forces
B.
It has only hydrogen bonding
C.
It has only ionic attraction
D.
It has no intermolecular forces
Correct Answer:
It has dipole-dipole and London dispersion forces
Explanation:
Bromoethane is polar because of its carbon-bromine bond and also contains electrons that produce London dispersion forces.
9. Stronger intermolecular forces between haloalkane molecules generally cause which change in boiling point?
A.
The boiling point increases
B.
The boiling point becomes zero
C.
The boiling point decreases to room temperature
D.
The boiling point is unaffected
Correct Answer:
The boiling point increases
Explanation:
More energy is needed to separate molecules held together by stronger intermolecular forces, resulting in a higher boiling point.
10. Which property of a haloalkane molecule allows it to experience dipole-dipole attraction?
A.
A permanent separation of charge
B.
The presence of a metal lattice
C.
Complete absence of electrons
D.
Formation of hydrogen ions
Correct Answer:
A permanent separation of charge
Explanation:
A polar carbon-halogen bond creates partial positive and partial negative ends, producing a permanent dipole that allows dipole-dipole attraction.
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