A-LEVEL Chemistry: 3.2.2: Group 2

Question 1

As you go Down Group 2, Atomic Radius ___.

Answer 1

Increases.

Question 2

As you go Down Group 2, the Atoms have ___ Shells of Electrons, Making the Atom ___.

Answer 2

More, Bigger.

Question 3

As you go Down Group 2, the MPs ___. Why is this?

Answer 3

Decrease.
Because the Metallic Bonding Weakens as the Atomic Size Increases.
The Distance Between the Positive Ions & the Negative Delocalised Electrons Increases. Therefore, the Electrostatic Forces of Attraction Weakens, & MPs Decrease.

Question 4

As you go Down Group 2, The Distance Between the Positive Ions & the Negative Delocalised Electrons ___. Therefore, the Electrostatic Forces of Attraction ___, & MPs ___.

Answer 4

Increases, Weaken, Decrease.

Question 5

The Outermost Electrons are Held More ___ by the Atom. Why is this? What other Factor is there in Addition to this?

Answer 5

Weakly.

Because they are Successively Further Away from the Nucleus, in Additional Shells.

In Addition, the Outer-Shell Electrons Experience More Shielding, Due to More Inwards Electrons. Hence, their Attraction to the Nucleus Decreases, & they Become Easier to Lose.

Question 6

As you go Down Group 2, the Reactivity of the Metals ___. Why is this?

Answer 6

Increases.
Because Electrons get Easier to Remove.

Question 7

The Group 2 Metals Will Burn in ___. What do they Burn with?

Answer 7

Oxygen.
They Burn with Bright Coloured Flames.

Question 8

Explain the Reaction Between Magnesium & Steam: (3)

Answer 8

-Mg(s) + H2O(g) —–> MgO(s) + H2(g)

-Mg Burns with a Bright White Flame.

-MgO Appears as a White Power.

Question 9

Explain the Reaction Between Magnesium & Water: (3)

Answer 9

• Mg + 2H2O —–> Mg(OH)2 + H2

-Much Slower Reaction than Mg & Steam.

-No Flame.

Question 10

Most Group 2 Metals Will React with Cold Water with Increasing Vigour Down the Group to Form…

Answer 10

Hydroxides.

Question 11

What would you Observe when Most Group 2 Metals React with Cold Water? (4)

Answer 11

-Fizzing (gets More Vigorous as you go Down Group 2).

-The Metal Dissolving (Faster Down Group 2).

-The Solution Heating Up (More Down Group 2).

-Precipitate Forming (Less Precipitate Forms as you go Down Group 2).

Question 12

Titanium is Extracted by Reaction with a ___ ___ Metal. eg:

Answer 12

More Reactive.
eg: Magnesium.

Question 13

Why Can’t you Extract Titanium with Carbon?

Answer 13

Because Instead of Displacing it, Titanium Carbide (TiC) is Formed.

Question 14

Why Can’t Titanium be Extracted by Electrolysis?

Answer 14

Because it has to be Very Pure.

Question 15

Steps in Extracting Titanium by Displacement Reaction: (3)

Answer 15

-TiO2(s) is Converted to TiCl4(l) at 900’C.

-The TiCL4(l) is Purified by Fractional Distillation in an Argon Atmosphere.

-The Ti is Extracted by Mg in an Argon Atmosphere at 500’C.

Question 16

What Can be Used to Remove SO2 from the Waste Gases from Furnaces (eg Coal Fired Power Stations) by Flue Gas Desulfurisation?

Answer 16

Calcium Oxide.

Question 17

As you go Down Group 2, the Solubility of Group 2 Hydroxides ___.

Answer 17

Increases.

Question 18

All Group 2 Hydroxides, when Not Soluble, Appear as…

Answer 18

White Precipitates.

Question 19

Magnesium Hydroxide is Classed as ___ in Water.

Answer 19

Insoluble.

Question 20

Calcium Hydroxide is Classed as ___ ___ in Water, & Will Appear as a ___ ___.

Answer 20

Partially Soluble, White Precipitate.

Question 21

Barium Hydroxide would ___ Dissolve in Water.

Answer 21

Easily.

Question 22

As you go Down Group 2, the Solubility of Group 2 Sulfates ___.

Answer 22

Decreases.

Question 23

What is Used as a Reagent to Test for the Presence of Sulfate Ions?

Answer 23

Barium Chloride (BaCl2) Solution Acidified with Hydrochloric Acid.

Question 24

What happens if Acidified Barium Chloride (BaCl2) is Added to a Solution that Contains Sulfate Ions?

Answer 24

White Precipitate of Barium Sulfate Forms.

Question 25

Why Must you Acidify Barium Chloride (BaCL2) Solution in Hydrochloric Acid Before Using it as a Reagent to Test for the Presence of Sulfate Ions?

Answer 25

Because the Hydrochloric Acid is Needed to React with Carbonate Impurities that are Often found in Salts which would Form a White Barium Carbonate Precipitate & so give a False Result.

Question 26

Why Can’t you Use Sulfuric Acid to Acidify Barium Chloride (BaCl2) Solution before Using it to Test for the Presence of Sulfate Ions?

Answer 26

Because it Contains Sulfate Ions, & so would give a False Positive Result.

Question 27

Insoluble Salts Can be Made by Mixing Appropriate Solutions of ___, so that a ___ is Formed.

Answer 27

Ions, Precipitate.

Question 28

What is a ‘Precipitation Reaction’? Give an Example.

Answer 28

A Precipitation Reaction is a Reaction that Produces Insoluble Salts by Reacting Appropriate Solutions of Ions so that a Precipitate is Formed.

eg: Barium Nitrate (aq) + Sodium Sulfate (aq) —–> Barium Sulfate (s) + Sodium Nitrate (aq)

Question 29

When Making an Insoluble Salt, Normally the Salt would be Removed by ___, Washed with ___ ___ to Remove ___ ___, & then Dried on ___ ___.

Answer 29

Filtration, Distilled Water, Soluble Impurities, Filter Paper.