The intermolecular forces that act between a hydrogen bromide molecule and a hydrogen iodide molecule are:

1. Dipole-Dipole Interaction: Both hydrogen bromide (HBr) and hydrogen iodide (HI) are polar molecules. This means they have a positive end (the hydrogen atom) and a negative end (the bromine or iodine atom). The positive end of one molecule is attracted to the negative end of another, which is known as a dipole-dipole interaction.

2. London Dispersion Forces: These are temporary attractive forces that result when the electrons in two adjacent atoms occupy positions that make the atoms form temporary dipoles. These forces are present in all molecules, whether they are polar or nonpolar.

So, the intermolecular forces between a hydrogen bromide molecule and a hydrogen iodide molecule are dipole-dipole interactions and London dispersion forces.

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The intermolecular forces that act between a hydrogen bromide molecule and a hydrogen iodide molecule are:

1. Dipole-Dipole Interaction: Both hydrogen bromide (HBr) and hydrogen iodide (HI) are polar molecules. This means they have a positive end (the hydrogen atom) and a negative end (the bromine or iodine atom). The positive end of one molecule is attracted to the negative end of another, which is known as a dipole-dipole interaction.

2. London Dispersion Forces: These are temporary attractive forces that result when the electrons in two adjacent atoms occupy positions that make the atoms form temporary dipoles. These forces are present in all molecules, whether they are polar or nonpolar.

So, the intermolecular forces between a hydrogen bromide molecule and a hydrogen iodide molecule are dipole-dipole interactions and London dispersion forces.

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The intermolecular forces that act between a hydrogen bromide molecule and a hydrogen iodide molecule are:

1. Dipole-Dipole Interaction: Both hydrogen bromide (HBr) and hydrogen iodide (HI) are polar molecules. This means they have a positive end (the hydrogen atom) and a negative end (the bromine or iodine atom). The positive end of one molecule is attracted to the negative end of another, which is known as a dipole-dipole interaction.

2. London Dispersion Forces: These are temporary attractive forces that result when the electrons in two adjacent atoms occupy positions that make the atoms form temporary dipoles. These forces are present in all molecules, whether they are polar or nonpolar.

So, the intermolecular forces between a hydrogen bromide molecule and a hydrogen iodide molecule are dipole-dipole interactions and London dispersion forces.

What kind of intermolecular forces act between a hydrogen bromide molecule and a hydrogen iodide molecule?Note: If there is more than one type of intermolecular force that acts, be sure to list them all, with a comma between the name of each force.

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