As Chemistry: Unit 1 - Module 3 (The Periodic Table)

Front 1

Define periodicity

Back 1

A regular periodic variation of properties of elements with atomic numbers and periodic table position.

Front 2

Name some periodic properties.

Back 2

- Atomic Radius
- First Ionisation Energy

Front 3

What happens to atomic radius as you go across the period?

Back 3

- atomic radius decreases
- nuclear charge increases
- nuclear attraction increases
- electron shielding does not change

Front 4

What happens to atomic radius as you go down the group?

Back 4

- atomic radius increases
- electron shells increases
- nuclear attraction decreases
- electron shielding increases

Front 5

What happens to first ionisation energy as you go across the period?

Back 5

- Nuclear charge increases
- Nuclear attraction increases
- Energy required increases

Front 6

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

Back 6

- Atomic radius increases
- Nuclear attraction decreases
- Electron shielding decreases
- Energy required decreases

Front 7

Define charge density

Back 7

The closeness of an atom and its low atomic radius in metallically bonded elements

Front 8

Define the Group 2 elements

Back 8

Alkaline Earth Metals

Front 9

What happens to solubility of Group 2 elements as you go down the group?

Back 9

it increases

Front 10

What happens to the capability of thermal decomposition of Group 2 elements as you go down the group?

Back 10

It gets harder to achieve

Front 11

What are the physical properties of Group 2 elements?

Back 11

- Metallic Bonds
- High melting and boiling points
- Low charge densities
- Forms colourless compounds

Front 12

What are Group 2 elements?

Back 12

Reducing agents

Front 13

What happens to the reactivity of Group 2 elements of you go down the group and why?

Back 13

- Reactivity Increases
- Atomic Radius Increases
- Electron Shielding Decreases
- Nuclear charge has little effect
- Outer electron is lost more easily

Front 14

What happens when Group 2 elements react with Oxygen?

Back 14

a vigorous redox reaction which forms an oxide

Front 15

What happens when Group 2 elements react with water?

Back 15

a gentle redox reaction which forms a hydroxide and hydrogen

Front 16

Name some uses of Group 2 Hydroxides.

Back 16

CaOH = used to reduce acidity of soil
Mg(OH)2 = used as milk of magnesia to neutralise stomach acid

Front 17

What is the test to identify a Halogen?

Back 17

Dissolve it in water and add cyclohexane.

Front 18

What is the test to identify a Halide ion?

Back 18

Add silver nitrate.

Front 19

What colour change occurs when you dissolve Chlorine in:

a) Water
b) Cyclohexane

Back 19

a) Pale Green
b) Pale Green

Front 20

What colour change occurs when you dissolve Bromine in:

a) Water
b) Cyclohexane

Back 20

a) Orange
b) Orange

Front 21

What colour change occurs when you dissolve Iodine in:

a) Water
b) Cyclohexane

Back 21

a) Brown
b) Violet

Front 22

What colour precipitate occurs when you add silver nitrate to Chloride ions?

Back 22

White

Front 23

What colour precipitate occurs when you add silver nitrate to Bromide ions?

Back 23

Cream

Front 24

What colour precipitate occurs when you add silver nitrate to Iodide ions?

Back 24

Yellow

Front 25

What is the name given to the Group 7 elements?

Back 25

The Halogens

Front 26

What happens to reactivity as you go down Group 7 and why?

Back 26

- Reactivity decreases
- Atomic Radius increases
- Electron Shielding increases
- Ability to gain electron into p-Subshell decreases

Front 27

What charge and type of bonding occurs in Halode ions?

Back 27

Covalent Bonding with a charge of -1

Front 28

What is a displacement reaction?

Back 28

A reaction where a more reactive element displaces a less reactive element from an aqueous solution of the latter's ions

Front 29

Describe the states of the Group 7 halogens at room temperature:

a) Flourine
b) Chlorine
c) Bromine
d) Iodine
e) Astatine

Back 29

a) Yellow gas
b) Green gas
c) Brown liquid
d) Blacky grey solid
e) Solid

Front 30

What is sublimation?

Back 30

When an element changes from Solid to gas without becoming a liquid.

Front 31

What is disproportionation?

Back 31

When an element in a redox reaction is both oxidised and reduced simultaneous

Front 32

What are the tests, and results, for finding an acid?

Back 32

a) Dissolve metal in acid, fizzes producing Hydrogen
b) Dissolve carbonate in acid, fizzes producing carbon dioxide

Front 33

What are the tests, and results, for finding a Carbonate?

Back 33

a) Add Acid - dissolves and produces carbon dioxide
b) Heat and pass through limewater - decreased mass and milky to show presence of Carbon dioxide

Front 34

What is the reaction for the disproportionation of chlorine in water?

Back 34

Cl2(aq) + H20(l) = HCLO(aq) + HCL(aq)

Front 35

What is the reaction for the disproportionation of chlorine in Sodium hydroxide?

Back 35

Cl2(aq) + 2NaOH(aq) = NaCl(aq) + NaCLO(aq) + H20(l)

Front 36

What is the trend across Period 2 of the periodic table for melting point and why?

Back 36

Increases up to Carbon, then suddenly drops and then increases again

Up to carbon it is giant metallic then carbon is giant covalent (the highest), which drops to simple molecules of only van der waals forces

Front 37

What is a second test that can be carried out to identify halides?

Back 37

First, add Silver Nitrate and then the Addition of aqueous NH3:

Cl - Precipitate should dissolve to give a colourless solution

I - precipitate is insoluble in any concentration of NH3

Br - Dilute NH3 shows little change, but concentrate NH3 should dissolve the precipitate

Front 38

Why can't Iodine oxidise or displace Chlorine (chloride) or bromine (bromide) in a reaction?

Back 38

Because it is less reactive than both of these elements and therefore cannot displace them