Group 2

Calcium reacts in cold water more quickly than magnesium because more energy is required to remove the outer electrons in magnesium. This occurs even though calcium atoms have a greater nuclear charge.

Explain why more energy is required to remove the outer electrons in magnesium than in calcium.

$0.001\text{ mol}$ of strontium reacts with an excess of cold water. When the reaction is complete a colourless solution is seen.

Construct the equation for the reaction of strontium with cold water. Include state symbols.

$0.005\text{ mol}$ of calcium and $0.005\text{ mol}$ of strontium are added separately to two beakers. Each beaker contains $100\text{ cm}^3$ of cold water.
At the end of each reaction a white solid and a colourless solution are seen in both beakers.

Predict which element, calcium or strontium, produces the more alkaline solution. Explain your answer.

Describe one observation when magnesium carbonate is added to excess dilute sulfuric acid.

From the information given, state two similarities and one difference that metal $\text{X}$ and its compounds have with Group 2 metals and their compounds.

similarity 1

similarity 2

difference 1

Write the formula of the oxide of $\text{X}$.

Write an equation for the reaction of $\text{XCO}_3$ when it is heated.

State the formula of each of the calcium compounds U to Y.

U ..............................................
V ..............................................
W ..............................................
X ..............................................
Y ..............................................

Compound Y may be converted into compound V.

Outline how this reaction would be carried out in a school or college laboratory using a small sample of Y.

Construct balanced equations for the following reactions.

calcium to compound U

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compound V to compound W

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compound U to compound Y

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Construct a balanced equation for the effect of heat on solid compound W.

Suggest the formula of an aqueous reagent, other than an acid, for reaction 1.

What would be observed when each of the following reactions is carried out in a test-tube?

the formation of X from Ca(s)

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the formation of X from V

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State the formula of each of the barium compounds R to W.

R ................................... S ....................................

T ................................... U ....................................

V ................................... W ...................................

Write balanced equations for the following reactions.

compound T to compound W

the roasting of V in air

Suggest a gaseous reagent for the conversion of T into V and write a balanced equation for the reaction.

reagent .....................................................................................................................

equation ...................................................................................................................

Suggest the formula of an aqueous reagent, other than an acid, for reaction 1.

Suggest the identity of the solid Y.

Use your answers to (i) and (ii) to construct an equation for the reaction of X with $\text{H}_2\text{SO}_4$.

the element that forms a soluble hydroxide and an insoluble sulfate,

State and explain the conditions needed for magnesium to react with oxygen.

State what would be seen during the reaction in (b)(i).

Write an equation for the reaction of magnesium with cold water.
Include state symbols.

Write an equation for the thermal decomposition of magnesium nitrate.

The thermal decomposition of calcium carbonate forms a solid product that is industrially important. This solid product reacts with water to form a compound commonly known as slaked lime.

Write equations for the thermal decomposition of calcium carbonate and the reaction of the solid product to form slaked lime.

thermal decomposition .......................................................................................................

formation of slaked lime ......................................................................................................

Describe this use and explain what makes these two compounds suitable for it.

Write an ionic equation to illustrate this use of calcium carbonate.

Describe and explain the trend in reactivity of these three elements with cold water.

Give the equation for the reaction of magnesium with cold water.

Suggest why the water eventually turns cloudy during the reaction of magnesium with cold water.

Suggest the equation for the reaction of hot magnesium with steam.

Give the equation for the reaction of magnesium oxide with nitric acid.

State the trend in thermal stability of the nitrates of Group II.

Give the equation for the thermal decomposition of magnesium nitrate.

Apart from lithium nitrate, the nitrates of the Group I elements decompose in a different way to those of the Group II elements.

The equation for the thermal decomposition of potassium nitrate is

By identifying any changes in oxidation number, explain which element is reduced and which is oxidised in this decomposition.

Write equations to show how calcium carbonate can be converted into calcium hydroxide by a two-step process.

Write an equation for the reaction of magnesium with cold water.

Suggest why the solution is cloudy after the reaction of magnesium with cold water.

Explain why there is a general increase in reactivity from Mg to Ba.

Give two observations for the reaction of magnesium with oxygen. Write an equation for this reaction. Include state symbols.

Write an equation for the reaction of magnesium with sulfuric acid.

Magnesium reacts with oxygen to form magnesium oxide.

State two observations that would be made when magnesium is heated strongly and placed in a gas jar of pure oxygen.

Give the equation to show how magnesium oxide relieves acid indigestion.

Name the type of reaction that occurs in (b)(i).

Write an equation for this reaction. Include state symbols.

Name the type of reaction occurring during this process.

Identify the anion in salt L.

Identify the element M and write an ionic equation for the formation of the white precipitate with sulfuric acid.

Give the formula of salt L and use it to write an equation for the thermal decomposition of salt L.

Write ionic equations for the neutralisation of acid by each of calcium hydroxide and calcium carbonate.

Suggest and explain why calcium carbonate is a better choice than calcium hydroxide for this purpose in areas of high rainfall.

Magnesium reacts with both cold water and steam.

Give the formula of the magnesium-containing product of each of these reactions.

State the variation in solubilities of group 2 hydroxides.

State what is observed in reaction 1.

Suggest a reactant for reaction 2.

Identify A.

$\text{Ba(OH)}_2$ is made by the reaction of $\text{Ba}$ with water.

Write an equation for this reaction.

State which compound decomposes first when barytocalcite is heated.

Explain your answer.

Construct an equation for the complete thermal decomposition of barytocalcite.

The formula of barytocalcite is $\text{BaCa(CO}_3)_2$.

State the variation in solubilities of group 2 hydroxides.

State what is observed in reaction 1.

Suggest a reactant for reaction 2.

Identify A.

Ba(OH)₂ is made by the reaction of Ba with water.

Write an equation for this reaction.

State which compound decomposes first when barytocalcite is heated.

Explain your answer.

Construct an equation for the complete thermal decomposition of barytocalcite.

The formula of barytocalcite is BaCa(CO₃)₂.

BaCa(CO₃)₂ ................................................................................................................