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Flashcards in Electron Structure Deck (24)
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1

How many electrons fit in one shell up to n=4?

2,8,18,32

2

What are shells?

Energy levels

3

What happens to the energy level as the shell number increases

Energy increases

4

What is the principle quantum number?

The shell number or energy level number

5

What are shells made out of

Made up of atomic orbitals

6

What is am atomic orbital?

A region around the nucleus that can hold up to 2 electrons, with opposite spins.

7

What types of orbital are there

S, p, d, f

8

S orbital

Spherical
Each can hold up to 2 electrons
Each shell from n=1 contains 1 orbital
The greater the shell number, the greater the radius of its s orbital

9

P orbital

Dumbbell shaped
Each orbital can hold up to 2 electrons
3 separate p orbitals at right angles to each other, px, py, pz
The greater the shell number, the further the p orbital is from the nucleus

10

D and F orbitals

n=3 contains 5 d orbitals
n=4 contains 7 f orbitals

11

What is the relationship between orbitals and sub shells?

A new type of orbital is added for each additional shell.

12

What are sub shells

Orbitals of the same type are grouped together as sub shells.

13

What is the relationship between new shells and orbitals

Each new shell gains a new type of orbital

14

What is the relationship between orbital number and type of orbital

The number of orbitals increase with each new type of orbital.

15

What is the relationship between electron numbers and orbitals?

2 electrons fit into each orbital, so the number of electrons in each sub shell increases. It is double the number of orbitals with each type of electrons

16

What is the order of filling orbitals?

1s, 2s, 2p, 3s, 3p, 4s, 3d, 4p, 4d, 4f

17

What is the relationship between filling orbitals and the type of orbital

Orbitals fill in in order of increasing energy.
4s is lower than 3d
Once 4s is filled, it falls into a lower energy state.

18

How do fill the orbitals with electrons?

Each orbital can hold up to 2 electrons.
Draw electrons in boxes.
Electrons repel each other, have opposite spins.
Orbitals with same energy are occupied singly first, prevents any repulsion between paired electrons until there is no further orbital available at the energy level.
Full orbitals are stable

19

Electron configuration

Shows how sub shells are occupied by electrons

20

What is the electron configuration of Krypton

1s2, 2s2, 2p6, 3s2, 3p6, 4s2, 3d10, 4p6

21

What do the letters mean

Sub shells

22

What do the superscript numbers mean

Electrons

23

What is the short hand configuration?

Write the noble gas before the element and the electron configuration.

24

How would you write the electron configuration of ions?

Add electrons if an anion
Take away electrons if a cation
4s fills and loses before 3d
Once 4s is filled, 3D falls below 4s in energy level