London Dispersion Forces and Molecular Geometry

Flashcards about London Dispersion Forces and The VSEPR Theory

London Dispersion Forces

intermolecular force; If only London dispersion forces are considered, H₂S should have a higher boiling point than H₂O because it has a higher molar mass.

Hydrogen Bonding

intermolecular force; Accounts for the higher boiling point of H₂O; stronger than London dispersion forces.

Intermolecular Forces

Forces of attraction between molecules (e.g., hydrogen bonding, dipole-dipole interactions, London dispersion forces).

Haber Process

Industrial production of ammonia (NH3) from H2 and N2. NH3 is separated by cooling the gaseous mixture to condense only the NH3.

Liquefaction of Gases

Cooling gases to the point where they change into a liquid state.

Metallic Solid

Good electrical conductor, insoluble in water.

Ionic Solid

Conductive only when melted or dissolved, soluble in water, melting point is above 300°C.

Molecular Solid

Poor electrical conductor, low melting point (below 300°C), soluble in water.

Network covalent solid

High melting points (1600-3000°C), non-conductive, insoluble in water.

VSEPR Theory

Valence Shell Electron Pair Repulsion theory; predicts the shape of molecules based on the repulsion between electron pairs around a central atom.

Polar Molecule

A molecule with an uneven distribution of electron density, resulting in a net dipole moment.

Nonpolar Molecule

A molecule with an even distribution of electron density, resulting in no net dipole moment.

Viscosity, Surface Tension, Hardness

Macroscopic properties of a substance explained by the organization and strength of attraction between particles.

van der Waals forces

A general term for intermolecular forces, including dipole-dipole attractions, hydrogen bonds, and London dispersion forces. NOT covalent bonds.

Electronegativity

The ability of an atom to attract electrons in a chemical bond.

Lewis Structure for Ammonia

Nitrogen has one unshared pair of electrons in the correct Lewis structure for ammonia (NH3).

Water Molecular Shape

Bent

Octet Rule

Tendency of elements (such as Oxygen) to gain two electrons to satisfy the octet rule.

Diatomic Elements with Double Bonds

Oxygen