C1 - Atomic Structure and the Periodic Table

Question 1

Describe the structure of an atom

Answer 1

A nucleus in the centre with electrons in shells around

Question 2

What is the charge of a proton?

Answer 2

+1

Question 3

What is the charge of a neutron?

Answer 3

0

Question 4

What is the charge of an electron?

Answer 4

-1

Question 5

What is the mass of a proton?

Answer 5

1

Question 6

What is the mass of a neutron?

Answer 6

1

Question 7

What is the mass of an electron?

Answer 7

0 (1/1836)

Question 8

What is the rule for amount of electrons in each shell?

Answer 8

2,8,8,2

Question 9

What does the atomic number mean (smaller number)?

Answer 9

Amount of protons in an atom

Question 10

What does the atomic mass mean (bigger number)?

Answer 10

Total amount of protons and neutrons in the nucleus of an atom

Question 11

What does the term ‘electronic configuration’ mean?

Answer 11

How electrons are arranged

Question 12

What are isotopes?

Answer 12

Atoms with the same number of protons but different numbers of neutrons

Question 13

What is the relative atomic mass?

Answer 13

An average of the different isotopes

Question 14

How would you calculate the relative atomic mass?

Answer 14

(percentagemass)+(percentagemass)etc/100

Question 15

What did Mendeleev do?

Answer 15

Create the periodic table - arranged elements in order of mass and spotted patterns

Question 16

What state are alkali metals (group 1) at room temperature?

Answer 16

Solid

Question 17

Do alkali metals (group 1) have a high or low melting point?

Answer 17

Low

Question 18

Are alkali metals (group 1) hard or soft?

Answer 18

Soft

Question 19

What happens when alkali metals (group 1) react with water?

Answer 19

They form hydroxides and hydrogen gas. They will move, float, fizz, potassium catches fire. Equation: metal + water -> metal hydroxide + hydrogen

Question 20

Why do alkali metals (group 1) get more reactive down the group?

Answer 20

They all want to lose the outer electron. Down the group, the outer electron is lost more easily because the atoms have more electron shells. This mean that the outer electron is further away from the nucleus so there is more shielding from inner electrons, resulting in a much weaker electrostatic attraction.

Question 21

How reactive are Nobel gases?

Answer 21

They are all unreactive (inert)

Question 22

Why are Nobel gases unreactive?

Answer 22

They already have a full outer shell. This means that they have many uses e.g. because they’re non-flammable

Question 23

Describe fluorine’s appearance

Answer 23

Pale yellow gas

Question 24

Describe chlorine’s appearance

Answer 24

Pale yellow-green gas

Question 25

Describe bromine’s appearance

Answer 25

Brown liquid

Question 26

Describe iodine’s appearance

Answer 26

Grey solid

Question 27

What does -ine refer to?

Answer 27

The element, which is diatomic (X₂)

Question 28

What does -ide refer to?

Answer 28

The anion (X-)

Question 29

What do a metal + halogen produce?

Answer 29

Metal halide

Question 30

What do hydrogen halides form when dissolved?

Answer 30

Acids

Question 31

Why does reactivity of halogens (group 7) decrease down the group?

Answer 31

It’s harder to gain an outer electron, can be proved with displacement reactions e.g. sodium bromide + fluorine -> sodium fluoride + bromine

Question 32

What does the group of an element mean?

Answer 32

The number of electrons in the outer shell

Question 33

What does the period of an element mean?

Answer 33

The number of electron shells