Chapter 7.2: Atomic Spectra

Flashcards from Chapter 7.2 of Chemistry: The Molecular Nature of Matter and Change.

Line spectrum

Fine lines of light emitted by electrically excited gaseous atoms at specific wavelengths

• Differs from the expected continuous spectrum rainbow

Rydberg equation

An equation developed by Johannes Rydberg that predicts the position and wavelength of any line in a given hydrogen series

• States: 1/λ = R ⋅ (1/n²₁ - 1/n²₂)

  • R is the Rydberg constant, 1.097 ⋅ 10⁷ m^-1

Bohr model

A model developed by Niels Bohr to explain the existence of line spectra and orbitals through the conceptualization of stationary, ground, and excited states

• States that electrons move between distant discrete ground and excited stationary states while absorbing or emitting proportionally energetic photons in an energy change

• Explains how line and not continuous spectra appear due to the presence of quantization

  • Energy emittance is greater as transitions occur closer to the nucleus

• Gave rise to the formula of energy levels: E = -2.18 ⋅ 10^-18 J ⋅ (Z² / n²)

  • Can be used to find potential energy level differences, utilizing the formula E = hc/λ

Flame test

A test to determine to determine the emission spectrum profile of a substance via flame