1.5 - electron arrangements Flashcards
what are main energy levels divided into
sub-levels or orbitals
what are the different orbitals
s
p
d
f
which orbital has the lowest energy
s
which orbital has the highest energy
f
what does each sub-level consist of
electron orbitals
what can each orbital hold
2 electrons
what do the electrons in each orbital have
opposite spins (anti-clockwise and clock-wise)
what are orbitals
regions of space that electrons are most likely to be in.
what does degenerate mean
of equal energy
what is the max number of electrons s orbital can hold
2
what is the max number of electrons p orbital can hold
6
what is the max number of electrons d orbital can hold
10
what is the max number of electrons f orbital can hold
14
what is the energies of the sub-levels
4f
4d
4p
3d
4s
3p
3s
what is a probability function
it give rise to a 3D shape where we say the electrons “exist” between
What is The Aubfau principle
States that the lowest energy sub-levels must be occupied first.
what is the electron configuration order
SSP
SPS
DPS
DPSF
What is The Pauli exclusion principle
States that each orbital can contain no more than a maximum of two electrons.
What is Hund’s Rule
states that single electrons occupy all empty orbitals within a sub-level before they start to form pairs in orbitals.
What is Electron spin
Each orbital contains two electrons which spin in opposite directions
what happens as the electrons spin
on their axes, the moving charge results in formation of a magnetic field
what happens when 2 electrons enter the same orbital
there is repulsion between them due to their negative charges.
when is the most stable configuration
with single electrons in different orbitals.
What is a half-filled or filled 3d orbital have
a special stability it creates a lower energy configuration
what 2 elements do this apply for
copper and chromium (Fe2+)
