Unit One, Chapter Three - Orbital Notations Flashcards
1
Q
Why are copper and chromium different?
A
More electrons in the d-orbitals than usual to allow for symmetry around the nucleus
2
Q
Define isoelectronic
A
Particles which have the same electronic configuration
3
Q
How to write electronic configuration
A
Shell number → orbital → no. of electrons
4
Q
Aufbau principle
A
Orbitals are filled in order of increasing energy (in diagonal lines from top right to bottom left)
5
Q
Hund’s rule
A
When degenerate orbitals are available, electrons fill each singly, keeping spins parallel before spin pairing starts
6
Q
Pauli exclusion principle
A
No two electrons in one atom can have the same set of four quantum numbers
7
Q
What are degenerate orbitals?
A
Orbitals that have the same energy
8
Q
The orbitals within each subshell of an isolated atom are…
A
…Degenerate
