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what is the maximum number of electrons in each of the first 4 shells
1-2
2-8
3-18
4-32
what is the formula for working out the maximum number of electrons in a shell
2n²
orbital definition
a region around the nucleus that can hold up to 2 electrons with opposite spins
what is an orbital
a region in space where there is a high probability of finding an electron
what are the different types of orbitals
s,p,d,f
what is the shape of an s orbital
sphere
what is the shape of a p orbital
dumbbell
what is a sub-shell
orbitals of the same type grouped together
how many electrons can each type of orbital hold (maximum)
s-2
p-6
d-10
f-14
what is the model used to show electrons with spins in orbitals
‘electrons in box’
what is the order of sub-shells in an electron configuration (36 electrons)
1s 2s 2p 3s 3p 4s 3d 4p
why does the 4s sun-shell fill up before the 3d sub-shell
has a lower energy level and sub-shells are filled from the lowest energy
ionisation energy definition
the energy required to remove one electron from each atom in one mole of gaseous atoms to form one mole of gaseous 1+ ions
factors affecting ionisation energy
atomic radius
nuclear charge
electron shielding
how does atomic radius affect ionisation energy
greater distance between nucleus and outermost electron = less nuclear attraction= easier to loose an electron = lower ionisation energy
how does electron shielding affect ionisation energy
less electron shielding = greater nuclear attraction
how does nuclear charge affect ionisation energy
greater nuclear charge= greater nuclear attraction = greater ionisation energy
trend in first IE down a group
1st IE decreases down a group as atomic radius increases and electron shielding increases, decreasing the nuclear attraction
trend in 1st IE across a period
1st IE increases across a period as nuclear charge increases and atomic radius decreases resulting in a lower nuclear charge
