Electron Structure

Question 1

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

Answer 1

2,8,18,32

Question 2

What are shells?

Answer 2

Energy levels

Question 3

What happens to the energy level as the shell number increases

Answer 3

Energy increases

Question 4

What is the principle quantum number?

Answer 4

The shell number or energy level number

Question 5

What are shells made out of

Answer 5

Made up of atomic orbitals

Question 6

What is am atomic orbital?

Answer 6

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

Question 7

What types of orbital are there

Answer 7

S, p, d, f

Question 8

S orbital

Answer 8

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

Question 9

P orbital

Answer 9

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

Question 10

D and F orbitals

Answer 10

n=3 contains 5 d orbitals

n=4 contains 7 f orbitals

Question 11

What is the relationship between orbitals and sub shells?

Answer 11

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

Question 12

What are sub shells

Answer 12

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

Question 13

What is the relationship between new shells and orbitals

Answer 13

Each new shell gains a new type of orbital

Question 14

What is the relationship between orbital number and type of orbital

Answer 14

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

Question 15

What is the relationship between electron numbers and orbitals?

Answer 15

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

Question 16

What is the order of filling orbitals?

Answer 16

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

Question 17

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

Answer 17

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

Question 18

How do fill the orbitals with electrons?

Answer 18

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

Question 19

Electron configuration

Answer 19

Shows how sub shells are occupied by electrons

Question 20

What is the electron configuration of Krypton

Answer 20

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

Question 21

What do the letters mean

Answer 21

Sub shells

Question 22

What do the superscript numbers mean

Answer 22

Electrons

Question 23

What is the short hand configuration?

Answer 23

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

Question 24

How would you write the electron configuration of ions?

Answer 24

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