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(1 point) Hydrogen fluoride (HF) has a lower molecular weight compared to hydrogen chloride (HCl), yet its boiling temperature is much higher. Choose the best explanation for this phenomenon: . A. The chlorine atom has a lower electronegativity than fluorine, thereby making the bond within the molecule weaker OB. The equilibrium distance between atoms within the HF molecule is smaller than that for the HCI molecule C. None of these OD. Two types of secondary (or intermolecular) bonding are present between hydrogen fluoride molecules, whereas only one type of secondary bonding is present between hydrogen chloride molecules O E. The bond between hydrogen and chlorine has greater ionic character compared to that of hydrogen and fluorine OF. none of the above

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Answer:

The correct option is: D. Two types of secondary (or intermolecular) bonding are present between hydrogen fluoride molecules, whereas only one type of secondary bonding is present between hydrogen chloride molecules

Explanation:

Boiling point of a chemical substance depends on the molecular mass and the intermolecular forces, which are the interactive forces present between chemical species

1. The molecular mass of hydrogen fluoride (HF) is less than hydrogen chloride (HCl).

2. But the intermolecular forces present between the HF molecules are stronger than the intermolecular forces present between the HCl molecules.

This is because hydrogen fluoride exhibits two types of intermolecular forces: strong hydrogen bonding and dipole-dipole interactions. Whereas, hydrogen chloride exhibits only one type of intermolecular force i.e. dipole-dipole interactions.

Therefore, as a net result, the boiling point of HF is higher than the boiling point of HCl.

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