unit 1a: electronic configuration and the periodic table Flashcards
pauli exclusion principle
no two electrons in one atom can have the same set of 4 quantum numbers, this means no orbital can hold more than two electrons and those electrons must have opposite spins
aufbau principle
electrons fill orbitals in order of increasing energy (1s > 2s > 2p > 3s > 3p > 4s > 3d > 4p
hunds rule of maximum multiplicity
when degenerate orbitals are available, electrons fill each singly keeping their spins parallel before spin pairing occurs
spectroscopic notation
uses numbers to represent the energy level, letters to represent the subshell, and superscript to represent the number of electrons in each subshell
orbital box notation
uses boxes to represent orbitals, and arrows to represent electrons
forming ions
electrons are added or removed from the highest energy orbital available
note about 4s and 3d filling
the 4th subshell is always filled before the 3d and the 4s subshell always empties before the 3d
transition metals which do not follow the aufbau principle
chromium and copper
chromium’s configuration
[Ar] 3d^5 4s^1 due to stability of half filled d subshell
coppers configuration
[Ar] 3d^10 4s^1 due to the extra stability of a filled d subshell
blocks
the periodic table can be divided into blocks, based on the outermost subshell being filled
s-block
groups 1+2 and helium
p-block
groups 3-8 except helium
d-block
transition metals
f-block
lanthanides and actinides
