2.2.1 Electron Structure Flashcards Preview

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Flashcards in 2.2.1 Electron Structure Deck (15)
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1

Number of electrons that can fill first 4 electron shells

1 -> 2
2 -> 8
3 -> 18
4 -> 32

2

Orbital

a region of space around the nucleus that can hold up to 2 electrons with opposite spins

3

Shape of S orbital

spherical

4

Shape of P orbital

dumbbell

5

number of orbitals in s,p,d sub-shells

s -> 1
p -> 3
d -> 5

6

number of electrons in s,p,d sub-shells

s -> 2
p -> 6
d -> 10

7

Writing electron configuration (order)

1s2s2p3s3p4s3d4p4d

8

Degenerate

Orbitals with the same energy

9

Electrons in a box

one box is an orbital containing 2 electrons with opposite spins
fill up one electron in a box at a time

10

Why does 4s come before 3d?

4s is at a lower energy and electrons will enter a lower energy level first

11

Why do the electrons fill up one one box at a time in an energy level?

due to repulsion, they have the same charge and so want to stay as far away from each other as possible

12

Electron spins

electrons have spins, 2 electrons can't have the same spin in an orbital

13

Writing ion configuration

cations- remove electrons from highest energy levels first
lose 4s electrons before 3d electrons
anions- just add on electrons

14

Noble gases and configuration

use nearest past noble gas to write configuration (makes it shorter)

15

Why are the electronic configurations for Cu and Cr different?

4s1 then fill up 3d subshell because it makes it more stable to have a full 3d shell