Chemistry As Level - 10.1.3 - Electrons And Energy Levels

Front 1

Main level 1, sublevels:

Back 1

s

Front 2

Main level 2, sublevels:

Back 2

s,p

Front 3

Main level 3, sublevels:

Back 3

s,p,d

Front 4

Main level 4, sublevels:

Back 4

s,p,d,f

Front 5

How many electrons can fit into each level:

Back 5

2n^2 (2,8,18,32) but 4s gets two electrons when 3p has 8, before 3d starts to fill.

Front 6

How many electrons can fit into each sub-level?

Back 6

2,6,10.

Front 7

How are electron configuration diagrams drawn?

Back 7

1s at bottom, moves up levels. 3d above 4s. Electrons ^down^down arrows. Go into sublevels unpaired before pairing takes place.

Front 8

Electron configuration e.g.:

Back 8

1s^2 2s^2 2p^6 3s^2 3p^1.. Save time by [Ar] or [Ne] - only after.

Front 9

Copper is exception to energy level rule:

Back 9

[Ar] 4s^1 3d^10

Front 10

Chromium is exception to energy level rule:

Back 10

[Ar] 4s^1 3d^5

Front 11

Blocks of elements

Back 11

electron within highest energy is in an s/d/f/p sub-level. Periodic table shaded.

Front 12

4s

Back 12

fills up before 3d, loses electrons before 3d.

Front 13

Ion electron configuration:

Back 13

different - lost or gained electrons

Front 14

Orbitals

Back 14

can't know exact location of electron - found from electron density measurement that there are regions where it is highly probably to find an electron of certain energe. High probably to find an electron = orbital.

Front 15

sub-levels and orbitals

Back 15

Each of the s p and d sub-levels corresponds to a different shaped orbital. Each orbital can hold 2 electrons which spin in different difections.

Front 16

Shape of s orbitals

Back 16

s - spheres getting larger per shell

Front 17

Shape of p orbitals

Back 17

p>x orbital on x axis - diagonal when z at top
p>y horizontal when z at top.
p>z straight up. Hourglass.