9.4. Reactivity series
A subsection of Chemistry, 5070, through 9. Metals
Listing 10 of 158 questions
The Periodic Table is an arrangement of elements in groups and periods. Describe how the position of an element in the Periodic Table is related to its electronic configuration. Aluminium is an element in Group III of the Periodic Table. Deduce the electronic configuration of the aluminium ion. Aluminium reacts with oxygen to form aluminium oxide, Al2O3. Construct the equation for this reaction. Aluminium oxide reacts with both acids and alkalis. Name the type of oxide which reacts with both acids and alkalis. Draw a ‘dot-and-cross’ diagram of a molecule of oxygen. Only draw the outer shell electrons. Describe and explain the difference in the rate of diffusion of the gases oxygen and nitrogen. Oxygen reacts with hydrogen to form water. Sulfur reacts with hydrogen to form hydrogen sulfide. Some properties of hydrogen sulfide are listed. • It is a gas at room temperature. • It reacts with aqueous sodium hydroxide. • It is a reducing agent. • It burns in air. Describe four ways in which the properties of water differ from those of hydrogen sulfide. 1. 2. 3. 4.
5070_w18_qp_21
THEORY
2018
Paper 2, Variant 1
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Chromium is a transition element. Sodium is an element in Group I of the Periodic Table. Explain how both chromium and sodium conduct electricity. Describe two differences in the physical properties of chromium and sodium. 1. 2. An alloy of iron and chromium is stronger than pure iron. Use ideas about the structure of metals to explain why the alloy is stronger. Molten chromium reacts with steam to form chromium(oxide, Cr2O3, and hydrogen. Construct the equation for this reaction. The structure of an ion containing chromium is shown. Cr O O O O –O O Cr O O O O O– O Write the formula for this ion. Adding dilute acid to yellow CrO4 2–forms orange Cr2O7 2–. The ionic equation for this reaction is shown. 2CrO4 2–+ 2H+Cr2O7 2–+ H2Oyellow orange Describe and explain what you would observe when a few drops of concentrated aqueous sodium hydroxide are added to the orange solution. Suggest why a change in pressure has no effect on the reaction shown.
5070_w18_qp_21
THEORY
2018
Paper 2, Variant 1
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A student adds large pieces of copper(carbonate to dilute hydrochloric acid. The copper(carbonate is in excess. Complete the equation by adding state symbols for the products. CuCO3+ 2HCl CuCl 2( ) + H2O( ) + CO2( ) shows how the mass of the reaction mixture changes with time as the reaction proceeds. 199.0 199.2 199.4 time / min 199.6 199.8 mass of reaction mixture / g 200.0 In another experiment, powdered copper(carbonate is used instead of large pieces of copper(carbonate. All other conditions and the mass of copper(carbonate stay the same. Draw a line on the grid in to show how the mass of the reaction mixture changes with time. The initial experiment is repeated using large pieces of copper(carbonate and hydrochloric acid of a higher concentration. All other conditions stay the same. Describe and explain the difference in rate of reaction when hydrochloric acid of a higher concentration is used. Excess copper(carbonate is added to 22.0 cm3 of 0.500 mol / dm3 hydrochloric acid. Calculate the volume of carbon dioxide released measured at room temperature and pressure. Give your answer to two significant figures. volume of carbon dioxide gas = dm3 Describe the observations made when: • a few drops of aqueous ammonia are added to an aqueous solution containing copper(ions • excess aqueous ammonia is added to an aqueous solution containing copper(ions. An ionic compound of copper has the formula Cu2O. Deduce the oxidation number of copper in Cu2O. Describe how to prepare crystals of ammonium chloride by reacting aqueous ammonia with dilute hydrochloric acid.
5070_w24_qp_21
THEORY
2024
Paper 2, Variant 1
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Questions Discovered
158