Intermolecular Forces in Hydrogen

The video explores the intermolecular forces in hydrogen gas (H2), also known as molecular or diatomic hydrogen. It begins by confirming the absence of ions in H2, as the molecule is neutral. The video then explains that H2 is non-polar due to identical electronegativity in its hydrogen atoms. Finally, it discusses London dispersion forces, the only intermolecular forces present in H2, which occur due to temporary dipoles in non-polar molecules.

What is the first step in analyzing the intermolecular forces in H2?

• Identifying the color of the gas

• Determining the boiling point

• Checking for the presence of ions

• Measuring the molecular weight

What is the charge of the H2 molecule?

• Negative

• Positive

• Neutral

• Both positive and negative

What is another name for hydrogen gas?

• Hydrogen ion

• Atomic hydrogen

• Molecular hydrogen

• Triatomic hydrogen

Why is H2 considered a non-polar molecule?

• It has a high electronegativity difference

• It contains a metal

• It has no difference in electronegativity between atoms

• It has a symmetrical shape

What type of intermolecular forces are present in H2?

• Hydrogen bonding

• Dipole-dipole interactions

• London dispersion forces

• Ionic bonds

How are London dispersion forces formed in H2?

• Through permanent dipoles

• By inducing a dipole in a neighboring molecule

• By sharing electrons

• Through ionic interactions

What is the role of temporary dipoles in London dispersion forces?

• They create permanent bonds

• They stabilize the molecule

• They increase the molecule's mass

• They induce dipoles in neighboring molecules