Vocabulary Week 2 Flashcard

Atomic Emission Spectrum
The pattern formed when light from an element passes through a prism by separating the frequencies
Electromagnetic Radiation
All types of electromagnetic waves including radio waves, infrared waves, visible light,  ultraviolet light waves, x-rays, and gamma rays
Wavelength
Distance between crests of a wave, ?, units are m
Frequency
Number of wave cycles, ?, units per seconds or S-1 or Hz(Hertz)
c
The Speed of light, 2.998 X 108 m/s
c

 

 = ?? (This is the equation to find wavelength or frequency)

 

Spectrum
All the colors of the Rainbow
Ground State
Lowest possible energy level an electron can be in
Photons
Packets or ‘quantu’ of light
Electron Configurations
The arrangements of electrons into orbitals
Energy Levels
The specific energy levels an electron in an atom can have
Ion
An atom/group of atoms with a positive or negative charge
Cation
An ion with a positive charge
Anion
An ion with a negative charge
Atomic Orbitals
a region in space in which there is a high probability of finding an electron
Quantum Numbers
Coordinates used to describe the orbitals where electrons can be found
n
Principle Quantum Number, describes energy level, cant = 0, can equal any other integer, ex: 1, 2, 3, 4, etc.
l
Angular Quantum Number, describes sub shell, can be an integer between 0 and n – 1 , ex: if n = 3, then l = 0, 1, 2.
ml
Magnetic Quantum Number, describes the specific orbital or ‘cloud’ with the sub shell, can be an integer between -1 and +1, ex: if n = 3, then l = -2, -1, 0, 1, 2.
ms
Describes the spin, can only be spin or opposite spin, ms = +½ or -½
Sublevel
Sections electron can occup, s, p, d, f
Aufbau Principle
Electrons occupy the orbital of lowest energy first
Pauli Exclusion Principle
Two electrons per orbital
Hund’s Rule
Electrons don’t pair up until they have to

Get instant access to
all materials

Become a Member