2.2 & 2.3 Group 2 & 7

Question 1

Does reducing strength of a halide, which is a reducing agent increase down a group

Answer 1

Yes
Ionic radius decreases
There is a weaker attraction between outer electron and nucleus

Question 2

The reducing ability of the halides can be demonstrated through their reactions with H2SO4. What are three possible products and their observations

Answer 2

SO2 (acidic gas)
S (yellow solid)
H2S (bad egg smell)

Question 3

Observation when I2 or Br2 is formed

Answer 3

I2 : black solid
Br2 : brown fumes

Question 4

Fluorine and chlorine are too weak as reducing agents to reduce, H2SO4. Write the acid base reaction for each halide with H2SO4 and write their observation

Answer 4

H+ + F− → HF
Observation: Misty fumes of HF gas
H+ + Cl− →HCl
Observation: Misty fumes of HCl gas

Question 5

Describe how you would test for halides

Answer 5

Question 6

Do Halogens have a stronger oxidisng agent down the group

Answer 6

No, weaker as you go down the group
Weaker bond between nucleus and incoming electron

Question 7

State the use of chlorine, why it’s added in low concentrations and it’s reaction with water

Answer 7

Question 8

Write equations for when Magnesium reacts with water and with steam. State the observations

Answer 8

Question 9

Write equation for extraction of magnesium of Ti from TiCl4
State role of magnesium in this reaction

Answer 9

Question 10

State trend of solubility group 2 hydroxides down the group
Describe how to test for magnesium hydroxide and ionic equations

Answer 10

Question 11

Use of magnesium hydroxide

Answer 11

Neutralise stomach acid
Or indigestion relief

Question 12

Describe trend of solubility of group 2 sulphates down the group. State use of barium sulphate and write ionic equations and it’s observations for barium sulphate

Answer 12

Question 13

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Question 14

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Question 15

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Question 16

What is used to test for ammonium ions. State observation

Answer 16

Heat with NaOH
Damp litmus paper turns from red to blue

Question 17

Least soluble group 2 hydroxides and least soluble group 2 sulfate

Answer 17

Mg(OH)2 & BaSO4

Question 18

Differences between reaction of magnesium with water and steam

Answer 18

Question 19

How do other group 2 hydroxides react with cold water and state observations

Answer 19

Question 20

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Question 21

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Question 22

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Question 23

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Question 24

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Question 25

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Question 26

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Question 27

Different gases are produced when solution B reacts in Test 1 and 2. Suggest identity of these gases

Answer 27

Test 1 : CO2 Test 2 : NH3

Question 28

Answer 28

D Br2 is an orange Solution I2 is a dark brown solution

Question 29

Answer 29

A

Question 30

Answer 30

Question 31

Answer 31

A) incorrect, Chloride ions not strong enough reducing agents H2SO4 to reduce B) Incorrect, Bromide ions can reduce H2SO4, only to sulfur dioxide, not sulfur. It's iodide ions that reduce it to sulfur C) Not feasible as iodine less reactive than bromine. Less reactive halogen cannot reduce a more reactive halogen D) Chlorine more reactive than iodine. So iodide ions can be oxidised to I2 while chlorine reduced to Cl^-

Question 32

Answer 32

You know A & B can be produced from ionic equation in the eqaution you know between chlorine and water In sunlight : 2Cl2 + 2H2O -> 4HCL + O2 Answer is D

Question 33

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Question 34

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Question 35

How to test for ammonium nitrate - outline a test tube reaction - state observation - write equation

Answer 35

Add warm NaOH, then hold down red litmus paper at mouth of the tube. Red litmus paper at the mouth of the tube will turn blue NH4^+ + OH^- -> NH3 + H2O

Question 36

How to test for potassium sulfate - outline a test tube reaction - state observation - write equation

Answer 36

- add acidified BaCl2 - white ppt Ba^2+ + SO4^2- --> BaSO4

Question 37

Answer 37

Question 38

Answer 38

Cl2 + H2O -> HCl + HClO In sunlight : 2Cl2 + 2H2O -> 4HCl + O2 So hydrogen (H2) Not produced Answer : C

Question 39

Answer 39

A