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Question 1
The elements in group 2 from Mg to Ba can be used to show the trends in properties down a group in the periodic table. |
a) | State and explain the trend in first ionisation energy for atoms of the elements down group 2 from Mg to Ba.
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b) | The group 2 elements react with water. State the trend in reactivity with water of the elements down group 2 from Mg to Ba.
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c) | Write an equation for the reaction of calcium with water. State symbols are not required.
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d) | Give the formula of the hydroxide of the element in group 2 from Mg to Ba that is least soluble in water.
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Question 2
The trend in the first and second ionisation energies of group 2 elements can be linked to the increase in chemical reactivity down the group. The table below shows the first and second ionisation energies of magneisum and calcium. |
a) | Write an equation, including state symbols, to represent the second ionsation energy of calcium.
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b) | Explain why the first ionisation energy of calcium is lower than the first ionisation energy of magnesium.
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Question 3
A chemist reacts a group 2 metal, M, with water and measures the volume of gas produced. The digram below shows the apparatus used by the chemist. |
a) | Write an equation for the reaction of M with water.
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b) | 0.150 g of the metal produces 89.8 cm3 of hydrogen measured at room temperature and pressure. Identify the group 2 metal, M.
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c) | The chemist plans to repeat the experiment using the same mass of calcium metal. Predict whether the volume of hydrogen produced would be greater than, less than, or the same as, the volume in the first experiment. Explain your answer.
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Question 4
Group 2 elements and their compounds have a range of uses. |
a) | From Mg(OH)2 to Ba(OH)2, the solubility in water: A increases B decreases C stays the same
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b) | From Mg to Ba, the outer shell electronic configuration: A increases B decreases C stays the same
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c) | From MgSO4 to BaSO4, the solubility in water: A increases B decreases C stays the same
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d) | Explain why beryllium has a higher melting point than magnesium.
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Question 5
The metals of group 2 and their compounds have several uses. Milk of magnesia, Mg(OH)2 is used as an indigestion remedy to neutralise excess stomach acid. |
a) | Write a balanced symbol equation, including state symbols, for the reaction between magnesium and cold water.
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b) | Write an ionic equation for the neutralisation of stomach acid with milk of magnesia.
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c) | Calcium hydroxide is used in agriculture to neutralise acidic soils. Give two reasons why calcium hydroxide is a better choice than magnesium hydroxide for this purpose.
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Question 6
An aqueous solution Z is a salt of a group 2 metal. Aqueous solutions of sodium hydroxide and acidified barium chloride are added to separate samples of solution Z. The table below shows the observations. |
a) | Suggest the identity of the group 2 metal ion present in solution Z. Write an ionic equation, including state symbols, for the reaction that takes place when sodium hydroxide is added to solution Z.
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b) | Suggest the identity of the negative ion present in solution Z. Write an ionic equation, including state symbols, for the reaction that takes places when acidified barium chloride is added to solution Z.
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c) | Solution Z is acidified with dilute hydrochloric acid before barium chloride is added. Suggest a reason for this.
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Question 7
Strontium chloride is a component of toothpaste for sensitive teeth. |
a) | Write a balanced symbol equation, including state symbols, for the reaction between strontium and hydrochloric acid to form strontium chloride.
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b) | Explain, with the use of half equations, why this reaction is a redox process.
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c) | Describe and explain the trend in reactivity of group 2 elements with hydrochloric acid.
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Question 8
This question is about group 2 elements and their oxides. Magnesium burns in oxygen to form an ionic compound. |
a) | Write the electronic configuration of an atom of magnesium.
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b) | Explain why the following reaction is a redox process: 2Mg(s) + O2(g) ➔ 2MgO(s) Identify the changes in oxidation number.
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c) | State and explain the trend in pH of the solution formed when the group 2 oxides are added to water.
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Question 9
P is a salt of a group 2 element M. When P is heated a brown gas is released and a white solid remains. The white solid dissolves in water to form a colourless solution of the metal hydroxide M(OH)2. Addition of dilute sulfuric acid produces a white precipitate. |
a) | Identify the negative ion in salt P
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b) | Identify element M and write an ionic equation for the formation of the white precipitate with sulfuric acid.
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c) | Give the formula of salt P and use it to write an equation for the thermal decomposition of salt P.
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d) | Salt P can be formed in a neutralisation reaction between nitric acid and salt Q. This reaction produces a colourless gas that turns limewater cloudy. |
Identify the negative ion in salt Q.
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e) | Give the formula of salt Q and use it to write an equation for the reaction of salt Q with nitric acid.
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Question 10
a) | Describe the trend in the thermal stability of the group 2 nitrates down the group.
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b) | A sample of barium nitrate was heated strongly until no further change occurred. A white solid was formed. Write an equation for the action of heat on barium nitrate.
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c) | When water was added to the white solid produced in part b), an alkaline solution was produced. Identify the species responsible for making the solution alkaline. Write an equation to explain this observation.
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d) | When sulfuric acid was added to the alkaline solution produced in part c), a white precipitate formed. Identify the white precipitate. Write an equation to explain this observation.
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