Topic 7 & 8

Question 1

What are the properties of giant metallic lattices?

Answer 1

1. High melting and boiling point.
2. Good electrical conductors.
3. Malleability
4. Ductility

Question 2

What is a ductile metal?

Answer 2

Metal that can be stretched eg. Wires.

Question 3

What is a malleable metal?

Answer 3

Metal that can be shaped into different forms

Question 4

Describe structure, forces and bonding between every element across period 2.

Answer 4

Li & Be: Giant covalent; Strong attraction between +ions and delocalised electrons; metallic bonding.

B & C: Giant covalent; strong forces between atoms; covalent bonding.

N2; O2; F2; Ne: Simple molecular; weak intermolecular forces between molecules; covalent intramolecular forces and intermolecular forces between molecules l.

Question 5

How are atoms arranged in the periodic table?

Answer 5

Increasing atomic number

Question 6

Define ‘Periodicity’

Answer 6

Repeating trends in chemical and physical properties.

Question 7

What change happens across a period?

Answer 7

Elements change from metals to non metals

Question 8

Define first ‘ionisation energy.’

Answer 8

Minimum energy required to remove one mole of electrons from one mole of an atom in its gaseous state.

Question 9

Write an equation to show first ionisation of Ca

Answer 9

Ca(g) —> Ca+ (g) + e-

Question 10

Name all factors affecting ionisation energy

Answer 10

1. Atomic Radius
2. Nuclear charge
3. Electron shielding

Question 11

Why does first ionisation decrease between group 2 to 3?

Answer 11

Group 3’s outer electrons are in p orbitals and Group 2’s are in s orbitals. P orbitals are further away so less attraction between nucleus and outer electrons.

Question 12

Why does first Ionisation decrease between the end of one period and the start of the next?

Answer 12

There is an increase of atomic radius and shielding.

Question 13

Why does first ionisation decrease down a group?

Answer 13

1. Increased shielding.

2. Increased atomic radius

Question 14

What is the common name of group 2 metals?

Answer 14

Alkaline earth metals

Question 15

What is the most reactive metal of group 2?

Answer 15

Barium

Question 16

State three physical properties of group 2 metals.

Answer 16

1. High melting points
2. Low density metals
3. Form colourless (white) compounds

Question 17

What subshell has the highest energy electrons in group 2?

Answer 17

S subshell

Question 18

What happens to reactivity down group 2? Why?

Answer 18

Reactivity increases

Because electrons are lost more easily due to increased atomic radius and shielding.

Question 19

What happens to first ionisation energy down group 2? Why?

Answer 19

1. Filled electron shells increase —> increases shielding
2. Increased atomic radius —> weaker force between nucleus and outer electron
3. Less energy required to remove the electron.

Question 20

State the reaction that takes place between a group 2 metal and oxygen.

Answer 20

Redox reaction

Question 21

Write the equation for the reaction of calcium and oxygen.

Answer 21

2Ca(s) + O2(g) —> 2CaO(s)

Question 22

What products are formed when group 2 elements react with water?

Answer 22

Metal Hydroxide and Hydrogen gas.

Question 23

What group 2 element doesn’t react with water?

Answer 23

Beryllium

Question 24

What group 2 element reacts very slowly with water?

Answer 24

Magnesium

Question 25

Name the type of reaction that takes place between group 2 metals and water.

Answer 25

Redox reactions.

Question 26

Write an equation showing the reaction between barium and water.

Answer 26

Ba(s) + 2H2O(l) —> Ba(OH)2(aq) + H2 (g)

Question 27

What is oxidised and reduced between group 2 metal and water?

Answer 27

Metal = oxidised | Hydrogen from water = reduced

Question 28

What products are formed when a group 2 metal reacts with a dilute acid?

Answer 28

Salt and hydrogen gas.

Question 29

Write a reaction between calcium and hydrochloric acid

Answer 29

Ca(s) + 2HCl(aq) —> CaCl2(s) + H2(g)

Question 30

What products are formed when group 2 reacts with a water?

Answer 30

Metal hydroxide

Question 31

State an equation for the reaction between a group 2 oxide and water.

Answer 31

MO(s) + H2O(l) —> M(OH)2(aq)

Question 32

What group 2 metal oxide is insoluble in water?

Answer 32

Beryllium oxide

Question 33

State the trend in hydroxide solubility down group 2.

Answer 33

1. Increases down group 2. Mg(OH)2 is slightly soluble 3. Ba(OH)2 creates a strong alkaline solution.

Question 34

State a use of Ca(OH)2. | Write an equation for the use.

Answer 34

Ca(OH)2(aq) + 2HCl(aq) —> 2H2O(l) + CaCl2(aq)

Question 35

What is Mg(OH)2 used for.

Answer 35

Antacid to treat indigestion

Question 36

What is calcium carbonate used for?

Answer 36

Found in Limestone and used for building construction.

Question 37

What is a drawback of using calcium carbonate in construction?

Answer 37

Group 2 metals react with acids.

Question 38

What group are known as the ‘halogens’?

Answer 38

Group 7

Question 39

State two properties of halogens.

Answer 39

1. Low melting & boiling points | 2. Exist as diatomic molecules eg. Cl2

Question 40

State the trend in boiling points down group 7, provide reasons for your answer.

Answer 40

Increases down the group. 1. Atomic size increases down the group 2. This means there are stronger london forces hence more energy needed to overcome these intermolecular forces.

Question 41

State the trend in reactivity down group 7, provide reasons for your answer.

Answer 41

Reactivity decrease down the group. 1. Increased atomic radius 2. Increased shielding 2. Ability to gain electron decreases.

Question 42

State the trend of oxidising ability down group 7. Provide reasons for your answer.

Answer 42

Decreases down a group. 1. Cl has smallest atomic radius meaning pull of nucleus is strongest compared to I. 2. Cl is easily reduced. 3. Cl is the best oxidising agent

Question 43

What is a ‘displacement reaction’

Answer 43

When a halogen displaces a less reactive halide.

Question 44

What colour is ‘Chlorine water’?

Answer 44

Pale green

Question 45

What colour is ‘bromine water’?

Answer 45

Orange

Question 46

What colour is ‘iodine in water’?

Answer 46

Brown

Question 47

What colour is chlorine in cyclohexane?

Answer 47

Pale green.

Question 48

What colour is bromine in cyclohexane?

Answer 48

Orange

Question 49

What colour is iodine in cyclohexane?

Answer 49

Violet

Question 50

Between halides Cl- Br- & I-, which ones can be oxidised by Cl2?

Answer 50

Br- and I- ions.

Question 51

State the equation of chlorine oxidising bromide ions.

Answer 51

Cl2(aq) + 2Br-(aq) —> 2Cl(aq) + Br2(aq)

Question 52

Show the equation for Cl2 oxidising 2I-

Answer 52

Cl2(aq) + 2I-(aq) —> 2Cl-(aq) + I2(aq)

Question 53

Between Cl-, Br- and I- which ones can be oxidised by bromine?

Answer 53

I- ions

Question 54

Show the equation for bromine oxidising iodide ions.

Answer 54

Br2 + 2I- —> 2Br- + I2

Question 55

Between Cl-, Br- and I- which of these can be oxidised by iodine?

Answer 55

None.

Question 56

What is ‘disproportionation’?

Answer 56

Oxidation and reduction of the same species in a redox reaction.

Question 57

Show the reaction of Cl2 and water.

Answer 57

Cl2(g) + H2O(l) —> HClO(aq) + HCl (aq)

Question 58

What type of reaction happens between chlorine and water?

Answer 58

Disproportionation. Chlorine is oxidised and reduced

Question 59

Why is chlorine added to drinking water?

Answer 59

Kills bacteria in the water

Question 60

What are the two forms of the chlorite ion?

Answer 60

ClO- is chlorate (I) ClO3- is chlorate (V)

Question 61

What is the formula for bleach?

Answer 61

NaClO

Question 62

Show the equation for the formation of bleach

Answer 62

Cl2 + 2NaOH(aq) —> NaCl + NaClO + H2O