1.2 - Orbitals and electronic configurations Flashcards
how many electrons can exist in 1 orbital
2
what is the aufbau principle
electrons fill orbitals in order of increasing energy
what is hund’s rule
when degenerate orbitals are available, electrons fill each singly, keeping their spins parallel before spin pairing starts
what is the pauli exclusion principle
no 2 electrons in one atom can have the same set of 4 quantum numbers, therefore, no orbital can hold more than 2 electrons and these 2 electrons must have opposite spins
what are the different sizes and shapes of electron standing waves known as?
orbitals
how do standing waves vibrate
in time but not in space
name the titles of the 4 quantum numbers
principle quantum number
angular momentum quantum number
magnetic quantum number
spin magnetic quantum number
name the letters which stand for the 4 quantum numbers
n
l
mₗ
mₛ
describe what the principle quantum number determines
the main energy level for an electron and is related to the size of the orbital
describe what the angular momentum quantum number determines
the “shape” of the subshell
describe what the magnetic quantum number determines
the “orientation” of the orbital
describe what the spin magnetic quantum number determines
the direction of spin
what are the ranges of possible values for the 4 quantum numbers
n - any natural number
l - 0 - (n-1)
mₗ - (-l ) - (+l)
mₛ - -1/2, +1/2
how does the stability of an electronic configuration influence the ionisation energy of an atom?
The more stable
the electronic configuration, the higher the ionisation energy.
what are the arrangements for electron pairs around an atom with: 2, 3, 4, 5, 6 pairs
linear trigonal planar tetrahedral trigonal bipyramidal octahedral
