Question

the lewis diagram of c₂h₅cl is shown. which of the following is a type of intermolecular force that occurs in a sample of c₂h₅cl?
(a) the students claim is correct; a large amount of energy is needed to break all of the covalent bonds within the molecules.
(b) the students claim is correct; a large amount of energy is needed to break all of the intermolecular attractive forces between atoms within the molecules.
(c) the students claim is incorrect; the high boiling point is due to the strong intermolecular forces, such as hydrogen bonds, that must be overcome.
(d) the students claim is incorrect; the high boiling point is due to the hydrogen bonds between atoms within each molecule.

Explanation:

• Option A: Covalent bonds within molecules are intramolecular forces. Boiling point is related to intermolecular forces (forces between molecules), not intramolecular forces. So this option is incorrect.
• Option B: Hydrogen - bonding is a type of intermolecular force. But for \(C_2H_5Cl\), there is no hydrogen bonding (hydrogen bonding occurs when \(H\) is bonded to \(N\), \(O\), or \(F\)).
• Option C: The high boiling point of \(C_2H_5Cl\) is due to intermolecular forces (such as dipole - dipole forces, since \(C_2H_5Cl\) is a polar molecule). Breaking these intermolecular forces requires energy. Intramolecular bonds (covalent bonds within the molecule) are not broken during boiling.
• Option D: This option correctly identifies that the student's claim is incorrect because the high boiling point is due to intermolecular forces (not intramolecular bonds).

Answer:

D. The student's claim is incorrect; the high boiling point is due to the bonds, that must be overcome.