(b) Restatement: Explain halogen trend.
- Observed melting point order: I > Br > Cl > F
- All halogens are nonmetals
- Intramolecular forces =covalent bonding
- Intermolecular forces =dispersion (van der Waals) forces, which exist between
molecules - Dispersion forces result from “temporary” dipoles caused by polarization of
electron clouds - As one moves up the group, the electron clouds become smaller
- Smaller electron clouds result in higher charge density
- As one moves up the group, electron clouds are less readily polarized
- Less readily polarized clouds result in weaker dispersion forces holding molecules
to other molecules - Therefore, attractive forces between molecules decrease as one moves up the
group, resulting in lower melting points
(c) Restatement: Predict melting point order (high to low) CsI, NaCl, LiF, and KBr and
explain. - LiF > NaCl > KBr > CsI
- All compounds contain a metal and a nonmetal
- Predicted order has ionic bonds
- Larger ionic radius results in lower charge density
- Lower charge density results in smaller attractive forces
- Smaller attractive forces result in lower melting point
Questions Commonly Asked About the AP Chemistry Exam
8684-X Ch01.F 2/14/01 2:49 PM Page 11