Chapter 5 (Ellie Ward)
Models of the Electron
Quantum Mechanical Model
The Principles and rules
Electron Configurations
4s 4p 4d 4t
5s 5p 4d 5t
3s 3p 3d
6s 6p 6d
2s 2p
7s 7p
1s
Thomson's: Electrons stuck in a sphere
Bohr: Electron "orbit" the nucleus in specific paths like the planets orbit the sun
Today's Model: Electron Cloud Model
Aufbau Principle
Pauli Exclusion Principle
Hund's Rule
Heisenberg Uncertainty Principle
One electron enters each orbital until all the orbitals contain one electron with the same spin direction
The rule that electrons occupy the orbitals of lowest energy first
An atomic orbital may describe at most two electrons, each with opposite spin direction
It is impossible to know exactly both the velocity and the position of a particle at the same time
Electromagnetic spectrum
Series of waves
Ground State
Light is energy
Added Energy
Light energy given off in waves // Light particles are called photons
Visible light (Spectrum) //Low Energy-R O Y G B I P-High Energy
High Frequency/Small Wavelength - Gamma Rays
Low Frequency/Big Wavelength - Radio Waves
Electron in the lowest possible energy level.
Electron Jumps from High
To Low State
Atomic Emission Spectra
Light emitted as electron jumps. // The Bigger the jump, the
more light is emitted.
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.
tells how likely it is to find an electron in
various locations around the nucleus.
Atomic Orbitals
Principal Energy Levels
Maximum electrons for each level
n=1//1 sublevel//1s (1 orbital)
n=4//4 Sublevels//4s (1 orbital), 4p (3 orbitals), 4d (5 orbitals), 4f (7 orbitals)
n=2//2 Sublevels//2s (1 orbital), 2p (3 orbitals)
n=3//3 Sublevels//3s (1 orbital), 3p (3 orbitals), 3d (5 orbitals)
n2 = 8
n3 = 18
n1 = 2
n4 = 32