Intermolecular Forces in Halogens

The video discusses the intermolecular forces in diatomic iodine (I2), focusing on the absence of ions and polarity due to identical iodine atoms. It explains that I2 exhibits London dispersion forces, which are temporary dipoles occurring in non-polar molecules like I2. These forces are stronger in larger atoms, such as iodine, compared to smaller halogens like fluorine or chlorine.

What is the physical state of I2 under standard conditions?

• Solid

• Plasma

• Liquid

• Gas

Why is I2 considered non-polar?

• It has a high electronegativity difference.

• It has a complex molecular structure.

• It contains ions.

• It consists of identical atoms.

What type of intermolecular force is present in I2?

• Dipole-dipole interactions

• Hydrogen bonding

• London dispersion forces

• Ionic bonding

What causes London dispersion forces in I2?

• Temporary dipoles

• Permanent dipoles

• Covalent bonds

• Ionic charges

How do the dispersion forces in iodine compare to those in fluorine?

• Non-existent

• Equal in strength

• Stronger due to larger size

• Weaker due to smaller size

Which factor increases the strength of dispersion forces in halogens?

• Lower atomic mass

• Larger atomic size

• Smaller atomic radius

• Higher electronegativity

What is the primary reason for the ease of polarizability in larger atoms like iodine?

• Larger electron cloud

• Greater atomic mass

• Higher electronegativity

• Stronger covalent bonds

Which of the following halogens would have the weakest dispersion forces?

• Bromine

• Chlorine

• Iodine

• Fluorine