Intermolecular Forces in HBr

The video tutorial explores the intermolecular forces in hydrogen bromide (HBr). It begins by identifying that HBr is a covalent compound with no ions present. The video then examines the polarity of HBr using its Lewis structure, highlighting that bromine's higher electronegativity makes HBr a polar molecule. The primary intermolecular force in HBr is identified as dipole-dipole interactions, with London dispersion forces also present. The tutorial concludes with a summary of these forces.

What type of bond is present in hydrogen bromide (HBr)?

• Hydrogen bond

• Covalent bond

• Metallic bond

• Ionic bond

Why are there no ions present in HBr?

• Because it is a metallic compound

• Because it is a polar compound

• Because it is an ionic compound

• Because it is a covalent compound

What makes HBr a polar molecule?

• The difference in electronegativity between hydrogen and bromine

• The presence of ions

• The equal sharing of electrons

• The presence of hydrogen bonds

Which element in HBr is more electronegative?

• Hydrogen

• Bromine

• Both have the same electronegativity

• Neither is electronegative

What is the primary intermolecular force in HBr?

• Hydrogen bonding

• Ionic bonding

• Dipole-dipole interactions

• Metallic bonding

Besides dipole-dipole interactions, what other intermolecular force is present in HBr?

• Covalent forces

• Hydrogen bonding

• London dispersion forces

• Ionic forces

Which of the following is NOT a factor in determining the intermolecular forces in HBr?

• Presence of ions

• Electronegativity difference

• Presence of hydrogen bonds

• Molecular polarity