Electron configuration

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