Electronic Structure and Periodic Properties lecture 8

This set of flashcards covers key concepts from Chapter 3 on Electronic Structure and Periodic Properties, including the Bohr model, atomic spectra, and the Rydberg equation.

Electron Excitation

The process by which an electron absorbs energy and moves from a lower energy orbit to a higher energy orbit.

Photon Emission

The release of energy in the form of light when an electron transitions from a higher energy orbit to a lower energy orbit.

Ground State

The lowest energy orbit of an electron in an atom.

Excited State

Any energy state of an electron that is higher than the ground state.

Rydberg Equation

An equation used to predict the wavelengths of spectral lines produced by hydrogen; expressed as 1/λ = R(1/n₁² - 1/n₂²).

Atomic Spectra

The unique spectrum of lines corresponding to the emitted light of a gaseous element, akin to a fingerprint for identifying elements.

Continuous Spectrum

The spectrum of light that shows a smooth and continuous range of wavelengths.

Visible Light

A type of electromagnetic radiation that is visible to the human eye and includes colors ranging from red to violet.

Spectral Lines

Specific wavelengths of light emitted or absorbed by an atom, which appear as lines in its spectrum.