Atomic structure

Question 1

What’s the maximum amount of electrons that can fit on the s orbital?

Answer 1

2

Question 2

What’s the maximum amount of electrons that can fit on the p orbital?

Answer 2

6

Question 3

What’s the maximum amount of electrons that can fit on the d orbital?

Answer 3

10

Question 4

What’s the maximum amount of electrons that can fit on the f orbital?

Answer 4

14

Question 5

How many electrons can the first electron shell contain?

Answer 5

2

Question 6

How many electrons can the second electron shell contain?

Answer 6

8

Question 7

How many electrons can the third electron shell contain?

Answer 7

18

Question 8

How many electrons can the fourth electron shell contain?

Answer 8

32

Question 9

Why does the 4s subshell need to be filled before the 3D subshell?

Answer 9

Because the 4s subshell is closest to the nucleus and has a lower energy than the 3d subshell

Question 10

When is the 3d subshell most stable?

Answer 10

When it’s either half full or completely full

Question 11

What is the ionisation energy?

Answer 11

The amount of energy required to remove electrons from atoms

Question 12

Why does chromium’s 3d orbital take an electron from the 4s orbital?

Answer 12

Because this allows for less repulsion between the orbitals and helps to make chromium more stable.

Question 13

Which 2 atoms are exceptions to the orbital rules?

Answer 13

Chromium and copper

Question 14

Are lower energy levels closer or further away from the nucleus?

Answer 14

closer

Question 15

Are higher energy levels closer or further away from the nucleus?

Answer 15

further

Question 16

.

Answer 16

.

Question 17

Electrons in a shell are found in regions called what?

Answer 17

Atomic orbitals

Question 18

What is an electron?

Answer 18

A cloud of negative charge. this cloud of negative charge has the shape of the orbital occupied by the electrons.

Question 19

Which orbitals are filled first?

Answer 19

Orbitals with the lowest energy (closes to the nucleus)

Question 20

What is each block on the periodic table named after?

Answer 20

The subshell containing the highest energy electron for the elements in that block.

Question 21

What is the only electron shell involved in chemical reactions?

Answer 21

The outer electron shell

Question 22

Can the d subshell be involved in chemical reactions?

Answer 22

Yes

Question 23

What is the exam definition of the first ionisation energy?

Answer 23

The energy needed to remove 1 mole of electrons from 1 mole of atoms in their gaseous state to form 1 mole of 1+ ions(also in their gaseous state)

Question 24

What is the exam definition of the second ionisation energy?

Answer 24

The energy needed to remove 1 mole of electrons from one mole of 1+ ions in their gaseous state to form one mole of 2+ ions(also in their gaseous state)

Question 25

The greater the attraction between the outer electrons and the nucleus the greater the what?

Answer 25

The greater the ionisation energy because this attraction makes or more difficult for an electron to be lost

Question 26

What are the 3 factors affecting ionisation energy?

Answer 26

1) the distance between the nucleus and the outermost electrons

2) the charge on the nucleus

3) shielding

Question 27

How does the atomic radius affect ionisation energy?

Answer 27

As the atomic radius increases, the force of attraction between the positive nucleus and the outermost electrons decreases. This lowers the ionisation energy

Question 28

How does the charge of the nucleus affect the ionisation energy?

Answer 28

The greater the number of protons, the greater the force of attraction between the outer electrons and the nucleus

Question 29

How does shielding affect the ionisation energy?

Answer 29

Electrons in the outer shell are repelled by electrons in the inner shells. This shielding effect reduces the attraction between the outer electrons and the nucleus

Question 30

Why do successive ionisation energies increase?

Answer 30

Because each time an outer electron is removed , the remaining electrons in the outer shell are pulled slightly closer to the nucleus and the attraction increases . So slightly more energy is required to remove the next electron.

Question 31

What happens to the first ionisation energy as you go down a group?

Answer 31

It decreases

Question 32

Why does the first ionisation energy decrease as you go down a group?

Answer 32

-becuse moving down a group, the atomic radius increases. This means that the outer electron shell is further away from the nucleus.
-secondly, going down a group the number of internal energy levels also increase.this means that there’s more shielding between the nucleus and the outer electrons. Weaker attraction, lower ionisation energy

Question 33

What happens to the first ionisation energies across a period?

Answer 33

The first ionisation energies increase across a period

Question 34

Why do the first ionisation energies increase across a period?

Answer 34

The nuclear charge increases across a period as the number of protons increases. This increases the attraction between the nucleus and the outer electrons. Because of this, the atomic radius decreases across a period and it’s harder for outer electrons to be lost

Question 35

What do electrons in the same atomic orbital do to each other?

Answer 35

They repel each other

Question 36

Which period 2 elements don’t fit the pattern of ionisation energies increasing across a period?

Answer 36

Boron and oxygen

Question 37

Why doesn’t boron fit the pattern?

Answer 37

For boron, the outer electron needs to be removed from the 2p subshell which has a higher energy than the 2s subshell. So, less energy is required to remove boron’s outer electron in comparison to beryllium.

Question 38

Why doesn’t oxygen fit the pattern?

Answer 38

2 of the electrons in oxygens p subshell are in the same orbital and so they repel each other. So less energy is required to remove these electrons