chapter 5/ Electron STEPHEN TUMMONDS
Electron Configurations
1s
2s 2p
6s 6p 6d
3s 3p 3d
5s 5p 5d 5f
4s 4p 4d 4f
7s 7p
Models of the electron
Plum Pudding - Thomson
Orbital Modle - Bohr
Todays modle: Electron cloud modle
Electrons "orbit" the nucleus in specific paths like the planets orbit the sun
Electrons stuck in a sphere
Quantum Mechanical Model
Tells how likely it is to find an electron in various locations around the nucleus
Atomic Orbitals
Principal Energy Levels
n=2
n=3
n=1
n=4
2 sublevels
1 sublevel
3 sublevels
4 sublevels
1s (1 orbital
2s (1 ordital), 2p (3 orbital)
3s (1 rbital), 3p (3 orbitals), 3d (5 orbitals)
4s (1 orbital), 4p (3 orbitals), 4d (5 orbitals), 4f (7 orbitals)
Maximum electrons for each level
n2 = 8
n3 = 18
n1 = 2
n4 = 32
The Principles and Rules
Heisenberg's Uncertainty Principle
It is impossible to know the location and velocity of an election at the same time
Hund's Rule
Electrons spin opposite direction in an orbital
Paul's Exclusion Principle
1 or 2 elections per orbital
Aufbau Principle
Elections occupy the lowest energy level first
Bucket filling with water bottom to the top
Electromagnetic Spectrum
Series of waves
Ground State
Light is energy
Energy Added - Excited State
Atomic Emission Spectra
When atoms absorb energy, electrons move into higher energy levels. They will then lose energy and emit light when they return to lower energy levels.
Electron Jumps from High To Low State
Light emitted as electron jumps
The bigger the jump, the more light is emitted
Electron is the lowest possible energy level
Visible Light (SPECTRUM
High Frequency/ small wavelength - Gamma Rays
Low Frequency/ Big Wavelength - Radio Waves
Low Energy - R O Y G B I P - High Energy
Light particles are called photons
Light energy given off in waves
electrons
have -1 charge
outside the nucleus in the elctron cloud
small (1840 electrons = mass of proton/neutron)
Neutral atom -> p+=e-
orbiting (moving)