1.5 - electron arrangements

Question 1

what are main energy levels divided into

Answer 1

sub-levels or orbitals

Question 2

what are the different orbitals

Answer 2

s
p
d
f

Question 3

which orbital has the lowest energy

Answer 3

s

Question 4

which orbital has the highest energy

Answer 4

f

Question 5

what does each sub-level consist of

Answer 5

electron orbitals

Question 6

what can each orbital hold

Answer 6

2 electrons

Question 7

what do the electrons in each orbital have

Answer 7

opposite spins (anti-clockwise and clock-wise)

Question 8

what are orbitals

Answer 8

regions of space that electrons are most likely to be in.

Question 9

what does degenerate mean

Answer 9

of equal energy

Question 10

what is the max number of electrons s orbital can hold

Answer 10

2

Question 11

what is the max number of electrons p orbital can hold

Answer 11

6

Question 12

what is the max number of electrons d orbital can hold

Answer 12

10

Question 13

what is the max number of electrons f orbital can hold

Answer 13

14

Question 14

what is the energies of the sub-levels

Answer 14

4f
4d
4p
3d
4s
3p
3s

Question 15

what is a probability function

Answer 15

it give rise to a 3D shape where we say the electrons “exist” between

Question 16

What is The Aubfau principle

Answer 16

States that the lowest energy sub-levels must be occupied first.

Question 17

what is the electron configuration order

Answer 17

SSP
SPS
DPS
DPSF

Question 18

What is The Pauli exclusion principle

Answer 18

States that each orbital can contain no more than a maximum of two electrons.

Question 19

What is Hund’s Rule

Answer 19

states that single electrons occupy all empty orbitals within a sub-level before they start to form pairs in orbitals.

Question 20

What is Electron spin

Answer 20

Each orbital contains two electrons which spin in opposite directions

Question 21

what happens as the electrons spin

Answer 21

on their axes, the moving charge results in formation of a magnetic field

Question 22

what happens when 2 electrons enter the same orbital

Answer 22

there is repulsion between them due to their negative charges.

Question 23

when is the most stable configuration

Answer 23

with single electrons in different orbitals.

Question 24

What is a half-filled or filled 3d orbital have

Answer 24

a special stability it creates a lower energy configuration

Question 25

what 2 elements do this apply for

Answer 25

copper and chromium (Fe2+)