A3 Inorganic Chemistry

Question 1

How do all electronic configurations of Group 2 elements end

Answer 1

S (^2)

Question 2

What happens to all group 2 elements in redox reactions

Answer 2

Oxidised to form 2+ ions

Question 3

General symbol equation for Group 2 elements reacting with dilute acid

Answer 3

Question 4

General symbol equation for Group 2 elements reacting with water

Answer 4

Question 5

General symbol equation for Group 2 elements reacting with oxygen

Answer 5

Question 6

State and explain the reactivity of Group 2 elements

Answer 6

• Reactivity increases down group
• More shells
• More sheilding
• Nuclur attraction decreases
• Ionisation energy decreases
• Less energy required to remove outer-shell electron

Question 7

Down Group 2, what happens to elements reducing power

Answer 7

Strong reducing agents

Question 8

State how solubility changes down the group and so the effect this has on the solution produced

Answer 8

• Solubility increases
• More alkaline solutions form
• Solutions have higher pH

Question 9

General symbol equation for metal oxide reacting with water

Answer 9

Question 10

What property of group 2 compounds make them useful

Answer 10

They are basic

Question 11

What is the use of calcium hydroxide in commerce, and what is the equation

Answer 11

• Neutralise soil acids in agriculture

Question 12

What is the use of magnesium hydroxide and calcium carbonate in commerce, and what are their equations

Answer 12

• Antacids to treat indigestion

Question 13

What electronic configurations do all group 7 elements end with

Answer 13

s(^2)p(^5)

Question 14

What happens to all group 7 elements in redox reactions

Answer 14

Reduced to form 1- ions

Question 15

How do all group 7 elements exist

Answer 15

Diatomic molecules

Question 16

Why does the boiling point of group 7 elements decrease down the group

Answer 16

• London forces become stronger
• More energy needed to break London forces

Question 17

State and explain the trend in reactivity down the group 7

Answer 17

• Reactivity decreases
• More shells
• Atomic radius increases
• More sheilding
• Nuclear attraction decreases
• Ionisation energy decreases
• More energy required to attract outer-shell electron

Question 18

Colour of chlorine regular

Answer 18

Colourless

Question 19

Colour of chlorine aqueous

Answer 19

Colourless

Question 20

Colour of chlorine organic

Answer 20

Colourless

Question 21

Colour of bromine regular

Answer 21

Red-Brown

Question 22

Colour of bromine aqueous

Answer 22

Orange

Question 23

Colour of bromine organic

Answer 23

Brown

Question 24

Colour of iodine regular

Answer 24

Dark grey

Question 25

Colour of iodine aqueous

Answer 25

Orange

Question 26

Colour of iodine organic

Answer 26

Violet

Question 27

Define Disproportionation

Answer 27

The reduction and oxidation of the same element in the same reaction

Question 28

Equation for chlorine reacting with cold, dilute aqeous sodium hydroxide, to form bleach

Answer 28

Question 29

Chemical formula and name for bleach

Answer 29

* NaClO * Sodium Chlorate (I)

Question 30

When chlorine is used to form bleach, what are the conditions required for sodium hydroxide

Answer 30

* Cold * Dilute

Question 31

Equation for chlorine used for water treatment

Answer 31

Question 32

Formula and name of acid created when chlorine is used for water treatment (not HCl)

Answer 32

* Chloric (I) acid * HClO

Question 33

Benefits of using chlorine for sterelising drinking water

Answer 33

Kills bacteria

Question 34

Risks with using chlorine for sterelising drinking water

Answer 34

* Chlorine gas is toxic * Chlorinated hydrocarbons formed which are carcinogenic

Question 35

How to test for halide ions and result

Answer 35

* Add HNO3 * Add AgNO3 * Add ammonia * Chloride ppt dissolved in dilute ammonia * Bromide ppt dissolved in concentrated ammonia * Iodide ppt insoluble in concentrated ammonia

Question 36

Equation for halide ion test

Answer 36

Question 37

How to test for carbonate ions, and result

Answer 37

* Add HCl * Bubble gas through limewater * Limewater turns cloudy

Question 38

Equation for carbonate ion test

Answer 38

Question 39

How to test for sulfate ions

Answer 39

* Add HCl to remove any carbonates * Add BaCl2 * White ppt will form

Question 40

Equation for sulfate ion test

Answer 40

Question 41

How to test for ammonium ions and result

Answer 41

* Add NaOH * Gently heat * Ammonia gas produced * Turns damp litmus blue

Question 42

Equation for ammonium ion test

Answer 42