Class of August 29th - Electron Configuration and Oribitals

Picked up on the "2.2 Electron Configuration" spreadsheet. Things covered in this lesson included; Emission Spectra, Electromagnetic Spectrum, Electron Arrangements (2n^2) and Orbitals.

Emission Spectra

• The spectrum of light emitted when electricity is passed through an element
• The glow from objects comes from when electricity goes through an element and the electrons go up an energy level. When they come back down they release protons.

Electromagnetic Spectrum

• When the wavelength increases in the electromagnetic spectrum the frequency decreases, and visa versa. 
• the wavelength from longest to shortest goes from: Radio - Microwave - Sub mm - Infrared - Visible - Ultraviolet - Xray - Gamma Ray 

Electron Arrangements

• Pre-IB understanding taught that electron shells would be filled 2,8,8,8... etc. This actually a flithy lie
• Each energy level is made up of different types of orbitals
• The four types are s, p, d, f
• Each orbitals are made up from 2 electrons.
• s has only one shape of orbital, p has 3, d has 5, and f has 7.
• To work out which shell has which amount of orbitals you can use this diagram and follow the arrows to allocate the electrons:

• The only 2 exceptions form this diagram are when you are dealing with Cr and Cu or dealing with an first row transition element that is ionised.