Answer :
To determine the strongest intermolecular force present in each of the given molecules, we must evaluate their structures and the types of interactions they can form. Intermolecular forces include Hydrogen bonding, Dipole-Dipole interactions, and London Dispersion forces. Let's analyze each molecule in detail:
1. Water (H₂O):
- Water has a highly polar O-H bond and a bent molecular geometry, leading to significant polarizability.
- The strongest intermolecular force present in water is Hydrogen Bonding due to the presence of hydrogen atoms bonded to highly electronegative oxygen atoms.
2. Acetone (CH₃)₂CO:
- Acetone has a polar carbonyl (C=O) group, making the molecule polar.
- The strongest intermolecular force in acetone is Dipole-Dipole interactions due to the significant polarity of the carbonyl group.
3. Methane (CH₄):
- Methane is a non-polar molecule as it has a symmetric tetrahedral structure.
- The strongest intermolecular force in methane is London Dispersion forces, which arise due to temporary dipoles induced by momentary fluctuations in electron density.
4. Benzene (C₆H₆):
- Benzene is a non-polar molecule with a planar ring structure consisting of alternating double bonds (delocalized π-electrons).
- The strongest intermolecular force in benzene is London Dispersion forces, which are typical for non-polar molecules.
5. Ammonia (NH₃):
- Ammonia has a trigonal pyramidal structure with a lone pair of electrons on the nitrogen atom, making the molecule polar.
- The strongest intermolecular force in ammonia is Hydrogen Bonding due to the presence of hydrogen atoms bonded to a highly electronegative nitrogen atom.
6. Methanol (CH₃OH):
- Methanol consists of a hydroxyl group (-OH), which makes the molecule quite polar.
- The strongest intermolecular force in methanol is Hydrogen Bonding due to the presence of hydrogen atoms bonded to oxygen.
7. Chloromethane (CH₃Cl):
- Chloromethane has a polar C-Cl bond, resulting in an overall dipole moment.
- The strongest intermolecular force in chloromethane is Dipole-Dipole interactions because of the molecule's polarity.
In summary, the strongest intermolecular forces for each molecule are:
1. Water (H₂O): Hydrogen Bonding
2. Acetone ((CH₃)₂CO): Dipole-Dipole interactions
3. Methane (CH₄): London Dispersion forces
4. Benzene (C₆H₆): London Dispersion forces
5. Ammonia (NH₃): Hydrogen Bonding
6. Methanol (CH₃OH): Hydrogen Bonding
7. Chloromethane (CH₃Cl): Dipole-Dipole interactions
1. Water (H₂O):
- Water has a highly polar O-H bond and a bent molecular geometry, leading to significant polarizability.
- The strongest intermolecular force present in water is Hydrogen Bonding due to the presence of hydrogen atoms bonded to highly electronegative oxygen atoms.
2. Acetone (CH₃)₂CO:
- Acetone has a polar carbonyl (C=O) group, making the molecule polar.
- The strongest intermolecular force in acetone is Dipole-Dipole interactions due to the significant polarity of the carbonyl group.
3. Methane (CH₄):
- Methane is a non-polar molecule as it has a symmetric tetrahedral structure.
- The strongest intermolecular force in methane is London Dispersion forces, which arise due to temporary dipoles induced by momentary fluctuations in electron density.
4. Benzene (C₆H₆):
- Benzene is a non-polar molecule with a planar ring structure consisting of alternating double bonds (delocalized π-electrons).
- The strongest intermolecular force in benzene is London Dispersion forces, which are typical for non-polar molecules.
5. Ammonia (NH₃):
- Ammonia has a trigonal pyramidal structure with a lone pair of electrons on the nitrogen atom, making the molecule polar.
- The strongest intermolecular force in ammonia is Hydrogen Bonding due to the presence of hydrogen atoms bonded to a highly electronegative nitrogen atom.
6. Methanol (CH₃OH):
- Methanol consists of a hydroxyl group (-OH), which makes the molecule quite polar.
- The strongest intermolecular force in methanol is Hydrogen Bonding due to the presence of hydrogen atoms bonded to oxygen.
7. Chloromethane (CH₃Cl):
- Chloromethane has a polar C-Cl bond, resulting in an overall dipole moment.
- The strongest intermolecular force in chloromethane is Dipole-Dipole interactions because of the molecule's polarity.
In summary, the strongest intermolecular forces for each molecule are:
1. Water (H₂O): Hydrogen Bonding
2. Acetone ((CH₃)₂CO): Dipole-Dipole interactions
3. Methane (CH₄): London Dispersion forces
4. Benzene (C₆H₆): London Dispersion forces
5. Ammonia (NH₃): Hydrogen Bonding
6. Methanol (CH₃OH): Hydrogen Bonding
7. Chloromethane (CH₃Cl): Dipole-Dipole interactions
