Understanding London Dispersion Forces and Dipoles

What are London dispersion forces also known as?

• Van der Waals forces

• Ionic bonds

• Coulombic forces

• Hydrogen bonds

What happens to a neutral atom when it becomes a temporary dipole?

• It loses electrons permanently

• It becomes a different element

• It temporarily has uneven electron distribution

• It gains a permanent charge

How does a temporary dipole affect a nearby neutral atom?

• It causes the neutral atom to lose protons

• It induces a dipole by distorting the electron cloud

• It causes the neutral atom to gain electrons

• It has no effect on the neutral atom

What is the main characteristic of London dispersion forces?

• They are strong and permanent

• They are weak and temporary

• They only occur in ionic compounds

• They are stronger than covalent bonds

In which type of molecules are London dispersion forces dominant?

• Polar molecules

• Ionic compounds

• Non-polar molecules

• Metallic compounds

Why do different halogens have varying boiling points?

• Because of varying London dispersion forces

• Due to differences in color

• Because of different covalent bond strengths

• Due to differences in atomic mass

What is the relationship between the number of electrons and the strength of London dispersion forces?

• More electrons mean weaker forces

• Fewer electrons mean stronger forces

• More electrons mean stronger forces

• The number of electrons has no effect

Which halogen has the strongest London dispersion forces?

• Fluorine

• Chlorine

• Iodine

• Bromine

What is the boiling point of fluorine gas?

• -188°C

• -34°C

• 59°C

• 114°C

What happens to London dispersion forces as you move down Group 7 in the periodic table?

• They remain constant

• They disappear

• They decrease

• They increase