Energy Levels, Sublevels, and Orbitals
Define Sublevel.
S, P, D, F - each energy level has a certain number of these, and each has a different shape and number of orbitals
Electron Configuration- Oxygen
⬆️⬇️ ⬆️⬇️ ⬆️⬇️ ⬆️ ⬆️
1s2 2s2 2p4
Noble gas- Chlorine
[Xe] 6s2 4f14 5d7
Define orbital notation.
Each orbital can hold 2 electrons with opposite spins
What is the Aufbau Principle?
Electrons occupy the orbitals of the lowest energy leve
How many Sublevels are there?
4
Electron Configuration- helium
⬆️⬇️
1s2
Noble gas- Irdium
[Xe] 3s2 3p3
What is this?
⬆️⬇️
Orbital notation
What is Pauli Exclusion?
An atomic orbital may have, at most, 2 electrons with different spins
Define energy levels.
Fixed amount of energy in a system that describes quantum mechanics
- molecule, atoms, electrons, nucleus
Electron configuration- lithium
⬆️⬇️ ⬆️
1s2 2s1
Noble gas - oxygen
[He] 2s2 2p4
Half arrows represent what?
⬆️
Electrons within orbitals
What is Hund’s Rule?
Electrons occupy orbitals of the same energy levels in a way that makes the number of electrons with the same spin direction
How many orbitals do the orbitals s, p, d, f have?
Electron configuration- carbon
⬆️⬇️ ⬆️⬇️
1s2 2s2
Noble gas- boron
[He] 2s2 2p1
Orbital notation- nitrogen
⬆️⬇️ ⬆️⬇️ ⬆️ ⬆️ ⬆️
1s2 2s2 2p3
No two electrons are alike. Two electrons in the same orbital must have opposite spins.
Pauli’s Exclusion Principle
There can be only — electrons in each orbital.
2
Electron configuration- hydrogen
⬆️
1s1
Noble gas- zinc
[Ar] 3d10 4s2
Orbital notation- sodium
⬆️⬇️ ⬆️⬇️ ⬆️⬇️ ⬆️⬇️ ⬆️⬇️ ⬆️
1s2 2s2 2p5
Electrons in the same sublevel occupy empty orbitals first before pairing up; unpaired electrons have the same spin.
Hund’s Rule