Topic 2 Flashcards
What is the order for electronic configuration?
1s 2s 2p 3s 3p 4s 3D
How many electrons can each sub shell hold?
S: 2
P: 6
D:10
F:14
What does degenerate mean?
When orbitals in a subshell has equal energies
What is the aufbau principle?
It states that the orbitals are filled in order of increasing energy.
What is Hunds rule?
It states that when degenerate orbitals are available, electrons will fill each singly, with parallel spins, before pairing occurs.
What is the Pauli exclusion principle?
It states that no two electrons can have the same set of four quantum numbers.
How is the periodic table arranged into S,P,D, and F blocks?
Left side S block
Transition metals D block
Right side P block
Bottom part F block
What is the principal quantum number?
Main energy level of an electron.
How is the angular momentum number found?
Indicates the type of orbital the electron resides in.
S - 0
P - 1
D - 2
F - 3
How is the magnetic quantum number found out?
Indicates orientation of the orbital.
0 is always an option.
What is the spin magnetic number?
Always either +1/2 or -1/2
How can Anomalies in the ionisation energies be explained?
By considering the electronic configurations
What is pattern between electronic configuration and ionisation energy?
The more stable the electronic configuration, the higher the ionisation energy.
