Chapter 6 Section 3 - Quantum Mechanics and Electron Behavior

These flashcards cover key concepts from Chapter 6 Section 3, focusing on quantum mechanics and electron behavior in atoms.

Bohr’s Model

A theory that explains the quantized energy levels of electrons in hydrogen but fails for multi-electron atoms.

Quantum Nature of Matter

Describes the wave-particle duality of matter, where particles like electrons exhibit wavelike properties.

de Broglie Wavelength

The equation λ = h/mv relates the wavelength (λ) of a particle to its mass (m) and velocity (v), where h is Plank’s constant.

Heisenberg’s Uncertainty Principle

States that we cannot simultaneously know the exact position and momentum of a particle.

Schrödinger Equation

A mathematical equation that describes how the quantum state of a physical system changes over time, used for determining the behavior of electrons.

Wavefunction

A mathematical function that describes the quantum state of a system; solutions provide probabilities of finding a particle in a particular location.

Orbitals

Regions in space around an atom's nucleus where there is a high probability of finding an electron.

Quantum Numbers

A set of values that describe the properties and energies of atomic orbitals and the electrons within them.

Ground Rules for Electron Configuration

1. Electrons fill the lowest energy orbitals first. 2. No more than two electrons can occupy an orbital, and they must have opposite spins. 3. Orbitals closer to the nucleus have lower energy.

Electron Configuration

A notation that shows the distribution of electrons across the various orbitals in an atom.