Atomic Structure & Bonding Overview

This set of flashcards covers key vocabulary related to atomic structure, bonding, and molecular behavior, as discussed in the lecture notes.

Atomic Theory

The theory that matter is composed of small particles called atoms and describes their behavior and properties.

Ionic Bond

A chemical bond formed through the transfer of electrons from a metal to a non-metal, creating charged ions.

Covalent Bond

A bond formed when two non-metals share one or more pairs of electrons.

Electron Configuration

The distribution of electrons among the orbitals of an atom.

Periodic Table

An arrangement of elements in order of increasing atomic number that shows periodic trends in properties.

Quantum Number

A number that describes the properties of atomic orbitals and the electrons in those orbitals.

Valence Electrons

The electrons in the outermost principal quantum level involved in chemical bonding.

Hybridization

The mixing of atomic orbitals to create new hybrid orbitals for bonding.

Bohr Model

A model of the hydrogen atom proposing that electrons travel in fixed orbits around the nucleus.

Intermolecular Forces

Forces that occur between molecules, influencing physical properties such as boiling and melting points.

Nuclear Reaction

A process in which an atomic nucleus changes, either by decay or nuclear fission/fusion.

Activation Energy

The minimum energy required for a chemical reaction to occur.

Dynamic Equilibrium

A state in which the rate of the forward reaction equals the rate of the reverse reaction in a reversible process.

Electromagnetic Radiation

Energy that travels in waves and includes visible light, radio waves, and gamma rays.

Dipole-Dipole Forces

Forces between polar molecules that result from the attraction of opposite charges.

Hydrogen Bonding

A strong type of dipole-dipole interaction that occurs when hydrogen is bonded to highly electronegative atoms.

Quantum Mechanical Model

A model of the atom that describes electrons as wave functions and incorporates the uncertainty principle.

Phase Change

The transition of matter from one state (solid, liquid, gas) to another, such as melting or boiling.

Molar Heat of Vaporization

The amount of energy required to vaporize one mole of a liquid at its boiling point.

Kinetic Theory

The theory stating that all matter is made of particles in constant motion, influencing properties like temperature and pressure.

Le Chatelier's Principle

The principle stating that if a stress is applied to a system at equilibrium, the system will adjust to counteract that stress.