Light, Energy, and Electrons Chapter Test

types of electromagnetic radiation

radio waves, microwaves, infrared radiation, (visible light), UV radiation, X-Rays, gamma rays

wavelength (m, nm)

The distance between two crests or troughs of a wave

frequency (hz)

the number of complete wavelengths that pass a point in a given time

C=λv

speed of light = wavelength x frequency

excited electrons

electrons that have absorbed energy and have moved farther from the nucleus to a higher energy level

when an electron loses energy

it releases light

photon

a discrete particle of pure light or electromagnetic radiation

E= hv

energy= planck's constant x frequency

planck's constant

6.63 x 10^-34 J-s

speed of light

3.00 x 10^8 m/s

relationship of photons and frequency

the energy of a photon is proportional to it's energy

grounded state

electrons release energy as light when it falls back to the original energy level

four orbitals

s, p, d, f

s subshell

1 orbital, 2 electrons, sphere shaped

p subshell

2 orbitals, 6 electrons, dumbbell shaped

d subshell

5 orbitals, 10 electrons, four leaf clover shaped

f subshells

7 orbitals, 14 electrons, 6 leaf clover shaped

orbital

the shell of an atom that can contain 2 electrons each

Aufbau Principle

fill in orbitals closest to nucleus first

pauli exclusion principle

electron in the same orbit or sub orbit must have opposite spins

hund's rule

fill in suborbitals with a single electron first, then pair

noble gas configuration

An outer main energy level occupied, in most cases, by 8 electrons

one electron produces

one line of light

different energy level absorbed means

different level of energy it's jumping to