A hydrogen atom must be in a molecule with a highly electronegative atom (like nitrogen, oxygen, or fluorine) for hydrogen bonding to occur. Here are the steps:

1. The hydrogen atom is part of a molecule (like water, ammonia, or hydrogen fluoride) where it is covalently bonded to a highly electronegative atom. This means the hydrogen and the electronegative atom share a pair of electrons.

2. Because the electronegative atom (like oxygen in water) is so electronegative, it pulls the shared electrons closer to itself. This creates a dipole, where the electronegative atom becomes slightly negative (δ-) and the hydrogen atom becomes slightly positive (δ+).

3. This slightly positive hydrogen atom can then form a hydrogen bond with another electronegative atom in a different molecule. The hydrogen bond is the electrostatic attraction between the δ+ hydrogen atom and the δ- electronegative atom.

4. This hydrogen bond is not as strong as a covalent bond, but it is stronger than other types of intermolecular forces like London dispersion forces or dipole-dipole interactions. This is why substances with hydrogen bonding (like water) have higher boiling points than similar substances without hydrogen bonding.

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A hydrogen atom must be in a molecule with a highly electronegative atom (like nitrogen, oxygen, or fluorine) for hydrogen bonding to occur. Here are the steps:

1. The hydrogen atom is part of a molecule (like water, ammonia, or hydrogen fluoride) where it is covalently bonded to a highly electronegative atom. This means the hydrogen and the electronegative atom share a pair of electrons.

2. Because the electronegative atom (like oxygen in water) is so electronegative, it pulls the shared electrons closer to itself. This creates a dipole, where the electronegative atom becomes slightly negative (δ-) and the hydrogen atom becomes slightly positive (δ+).

3. This slightly positive hydrogen atom can then form a hydrogen bond with another electronegative atom in a different molecule. The hydrogen bond is the electrostatic attraction between the δ+ hydrogen atom and the δ- electronegative atom.

4. This hydrogen bond is not as strong as a covalent bond, but it is stronger than other types of intermolecular forces like London dispersion forces or dipole-dipole interactions. This is why substances with hydrogen bonding (like water) have higher boiling points than similar substances without hydrogen bonding.

Knowee AI · Accepted Answer

A hydrogen atom must be in a molecule with a highly electronegative atom (like nitrogen, oxygen, or fluorine) for hydrogen bonding to occur. Here are the steps:

1. The hydrogen atom is part of a molecule (like water, ammonia, or hydrogen fluoride) where it is covalently bonded to a highly electronegative atom. This means the hydrogen and the electronegative atom share a pair of electrons.

2. Because the electronegative atom (like oxygen in water) is so electronegative, it pulls the shared electrons closer to itself. This creates a dipole, where the electronegative atom becomes slightly negative (δ-) and the hydrogen atom becomes slightly positive (δ+).

3. This slightly positive hydrogen atom can then form a hydrogen bond with another electronegative atom in a different molecule. The hydrogen bond is the electrostatic attraction between the δ+ hydrogen atom and the δ- electronegative atom.

4. This hydrogen bond is not as strong as a covalent bond, but it is stronger than other types of intermolecular forces like London dispersion forces or dipole-dipole interactions. This is why substances with hydrogen bonding (like water) have higher boiling points than similar substances without hydrogen bonding.

What does a hydrogen atom need to be in for hydrogen bonding to occur?

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