Electronic Configuration Flashcards
What is an orbital?
A region of space that can hold two electrons.
How many s-orbitals occur in every energy level?
One.
How many p-orbitals occur in every energy level?
Three.
How many d-orbitals are there?
Five.
How many electrons can an s-orbital hold in total?
Two.
How many electrons can a p-orbital hold in total?
Six.
How many electrons can a d-orbital hold in total?
10
What is the order of the first 10 sublevels?
1s 2s 2p 3s 3p 4s 3d 4p 5s 5p
What is the Aufbau Rule?
It states that the sub shells are filled in order of energy and the lowest energy levels are filled first.
What is the Pauli Exclusion Principle?
It states that an orbital cannot contain more than two electrons and then only if they have opposite spins.
What is Hund’s Rule of Maximum Multiplicity?
It states that the orbitals of a sub-shell must be occupied singly and with parallel spin before being occupied in pairs.
What are the two exceptions to electronic configuration and why?
Chromium (Cr) and Copper (Cu):
The 4s orbital is half filled because a completely full or half full d sub-level is more stable than a partially filled d sub-level. An electrons from the 4s orbital rises to a 3d orbital.
What shape are s-orbitals?
Spherically shaped.
What shape are p-orbitals?
Dumbbell shaped.
