Electron Configuration Test Review

Mr. Janick

Ground State

When electronsare at the normal electron configurations and at the lowest enegery state.

Excited electron

an electron that has gained energy and jumped energy levels from and inner and stable, lower energy state to a higher, unstable energy state.

Bright line spectra or absorption spectrum

pasing light through a prsim to separate the emitted color into its component color bands. the bands of color can be used to determine the electron configuration of any element and can be used like a chemical fingerprint to identify unkown substances.

wave speed

the speed of electromagnetic wave is 3.0×10^8 m/s in a vacuum.

Wavelength

the distance from peak to peak in a wave.

Frequency

The number of peaks that pass through a centain point in one second measured in hertz

Quanta/ Photons

bundles pf enegery contained by light that carry enegry but do nt have mass. the more bundles in a frequency, the more energy. Shorter wavlengths of light carry more energy than longer wavelengths.

Heisenberg uncertainty principle

the location and speed of a particle cannot be known at the same time.

The electromagnetic spectrum

Radio, microwave, infared, visible, ultraviolet, x-ray, gamma ray

pauli exclusion principle

in an atom or molecule, no two electrons can have the same four quantum numbers. an orbital can onlt contain two electrons that have opposite spin.

hands rule

every orbital in a subshell is singly occupied with one electron before anyone orbital is doublyoccupied, and all electrons in singly occupied areas have the same spin.

kernel electrons

the nucleus and all inner electrons, not including the outermost s and p electrons in that farthest enegry layer. they are not involved in chemical reactions.

valence electrons

the outermost layer of s and p electrons at the same energy level, determined the substances properties and is involved in chemical bonds