electron configuration
- Created by: Margaret Hobart
- Created on: 22-04-21 08:57
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- electron configuration
- 1s2, 2s2,2p6, 3s2, 3p6, 4s2, 3d10, 4p6, 4d10
- lowest energy sub-shells filled first
- 4s sub shell filled before 3d because it has lower energy
- an orbital can hold two electrons, one goes clockwise, one goes anticlockwise
- Bus rule
- ionisation energies
- 1st IE is the amount of energy required to remove 1 mol of electrons from 1 mol of a gaseous atom
- the lower the IE the easier is is to form an ion
- X(ne1)+ (g) -> Xn+(g) + e-
- factors affecting IE
- atomic radius: less attraction between e- and nucleus; less energy needed to remove e-; smaller iE
- charge on nucleus: more protons; more charge; more energy needed to remove e-; larger IE
- shielding: more shells; more shielding; less energy needed to remove e-; smaller IE
- successive ionisation is the energy needed to remove 1e- from each ion in one mol of gaseous 1+ ions to form 1 mol gaseous 2+ ions
- trends
- ionisation increases across period 3
- protons increase; atomic radius decreases; shielding stays the same
- anomalies: Al and S
- Al: Al outer e- in 3p orbital which is further from nucleus than 3s; 3p shielded by 3s
- S: sheilding is the same; in P e- is being removed from singly occupied orbital whereas in S there's 2 e- in orbital; repulsion
- evidence for sub-shells
- ionisation decreases down the group
- more shielding; atomic radius increases
- ionisation increases across period 3
- 1st IE is the amount of energy required to remove 1 mol of electrons from 1 mol of a gaseous atom
- 1s2, 2s2,2p6, 3s2, 3p6, 4s2, 3d10, 4p6, 4d10
- ionisation decreases down the group
- more shielding; atomic radius increases
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