Pauli’s Exclusion Principle
Each orbital can hold up to 2 electrons
2 electrons must have opposite spins
Hund’s Rule
Can’t have 2 electrons in 1 orbital until all orbitals have 1 electron
Aufbau Principle
Electrons occupy orbitals of the lowest energy first
orbital diagram vs electron configuration vs kernel structure
Oribtal diagram: uses arrows to show electron placement (1s ^v), use lines to show different orbitals
Electron configuration: 1s^2
Kernel Structure: same as electron configuration but uses one of noble gases as a “shortcut”
shape of s orbital
Circle
shape of p orbital
infinity symbol
2 exceptions for electron configurations
copper and chromium
For stability
Both start with C, 24 and 29
Heisenburg Uncertainty Principle
The Break Bad character -Gavin
It’s impossible to know the velocity and location of a particle at the same time
blurrrr
Relationship between frequency and wavelength
Inversely proportional
one goes up, other goes down
Relationship between frequency and light energy
directly proportional
one goes up, other also goes up
Which color has the shortest wavelength
purple
which color has the longest wavelength
red
Absorption spectrum
- Jump in energy levels
- Excited State
- Further from nucleus
Emission Spectrum
- Released light energy
- Closer to nucleus
- ground state
emits: colors reflect back to colors shown
Shielding Electrons
Electrons not in the highest energy lvl
Valence Electrons
Electrons in the highest energy level
These all have same energy lvl number
Alkaline Earth Metal
2nd most reactive group metals
Metalloids
Boron, Silicon, Arsenic, Tellurium, Astatine, Germanium, Antimony
Stair step starting from Boron, no 118, and Germany down 1
Alkaline Metals
Most reactive metal group
Noble Gases
Very stable, least reactive
Halogens
Most reactive non-metal
Metal properties
- Conductive in heat and electricity
- solid at room temp
- shiny
- can be made into wires
Non-metals
- varying matter of state at room temp
