Studied by 3 people
Frequency
Number of wavelenght per second
Wavelenght
Distance between corresponding points
Magnetic radiation
Describes as waves travel at the speed of light in a vacuum
Short wavelenght
High energy ,high frequency
High energy
High frequence and short wavelenght
Long wavelenght
Low frequency and low energy
Increasing energy in colours
Red, orange, yellow, green, blue, indigo, violet
Emission spectra
by heating an element , that forces the electrons to go to the excited state
series of sharp, bright lines on a dark background
The lines get closer together at higher frequencys
Absorbition spectrum
all colours merging into eachother
Are obtained by bombarding an element with light of many wavelenght and detecting which wavelenght are absorbed
Groundstate
Lowest energy level (n=1)
Excited state
Highest energy level electrons gains energy
How many electrons are there in each energy levels
N=1 is 2 electrons
N=2 is 8 electrons
N=3 is 18 electrons
N=4 is 32 electrons
What type of orbitals are there and what shape do they have
S- orbital and p-orbital
S orbital are sperial
P-orbital are dumbells
