(a) List the following molecules in order of increasing polar- izability: GeCl4, CH4, SiCl4, SiH4, and GeBr4. (b) Predict the order of boiling points of the substances in part (a).

Verified step by step guidance

1. Identify the number of electrons and the molecular size of each molecule. Molecules with more electrons and larger molecular sizes generally have higher polarizability.
2. Compare the electronegativity of the atoms within each molecule. Molecules with less electronegative substituents (like Br compared to Cl or H) will generally have higher polarizability due to weaker hold on the electron cloud.
3. Arrange the molecules based on the trends identified: molecules with heavier atoms and more electrons will be more polarizable.
4. For boiling points, recognize that molecules with higher polarizability will have stronger London dispersion forces, which are a type of intermolecular force.
5. Predict the order of boiling points based on the strength of the intermolecular forces, where stronger dispersion forces lead to higher boiling points.

Key Concepts

Polarizability

Polarizability refers to the ability of an electron cloud around an atom or molecule to be distorted by an external electric field, leading to the formation of temporary dipoles. Larger atoms or molecules with more electrons generally exhibit higher polarizability due to their more diffuse electron clouds. This property is crucial for understanding intermolecular forces and how they influence physical properties like boiling points.

Intermolecular Forces

Intermolecular forces are the attractive forces between molecules that influence their physical properties, including boiling points. These forces include London dispersion forces, dipole-dipole interactions, and hydrogen bonding. In the context of the given molecules, the strength of these forces, which is affected by polarizability, will determine the order of boiling points.

Boiling Point Trends

Boiling point trends can be predicted based on molecular size, shape, and the strength of intermolecular forces. Generally, larger and more polarizable molecules have higher boiling points due to stronger London dispersion forces. Understanding these trends allows for the comparison of different substances and helps predict their physical behavior under varying conditions.