0620_m16_qp_42
A paper of Chemistry, 0620
Questions:
7
Year:
2016
Paper:
4
Variant:
2
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1
The table below gives information about particles. Complete the table. The first line has been done for you. particle number of protons number of electrons electronic configuration charge on particle A 2,8 2+ B 2,8,8 1– C 2,8,8 D Gallium is a Group III element. Define the term element. The following are gallium atoms. Ga Ga Complete the following table. atom number of protons number of neutrons number of electrons Ga Ga
2. Atoms, elements and compounds  →  2.2. Atomic structure and the Periodic Table
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2
Rubidium, Rb, is a Group I element. It has similar physical and chemical properties to the other elements in Group I. Predict how many electrons there are in the outer shell of a rubidium atom. Predict one physical property of rubidium which is the same as that of a transition element such as iron. Predict two physical properties of rubidium which are different to those of a transition element such as iron. When rubidium is added to cold water a reaction occurs. Suggest two observations that would be made when rubidium is added to cold water. What would be the colour of the solution if methyl orange was added to it after the reaction? Write a chemical equation for the reaction between rubidium and water. Put the Group I elements, caesium, lithium, potassium, rubidium and sodium in their order of reactivity with water. Put the most reactive element first. most reactive least reactive Suggest one safety measure that should be used when rubidium is added to cold water. The phosphate ion has the formula PO4 3–. Deduce the formula of rubidium phosphate.
8. The Periodic Table  →  8.1. Arrangement of elements
9. Metals  →  9.4. Reactivity series
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3
Carbon dioxide and silicon(oxide are oxides of Group IV elements. Complete the following table. carbon dioxide silicon(oxide formula SiO2 melting point / °C –56 physical state at 25 °C gas conduction of electricity non-conductor structure macromolecular Name the type of bonds that exist between the atoms in silicon(oxide. Explain why silicon(oxide has a very high melting point. Explain, in terms of attractive forces between particles, why carbon dioxide has a very low melting point. Explain, in terms of particles, why carbon dioxide is a non-conductor of electricity. Suggest a chemical equation for the reaction between sodium hydroxide solution and carbon dioxide. Name the type of chemical reaction in which carbon dioxide is produced from fossil fuels. Name the chemical process in which green plants convert carbon dioxide into carbohydrates. Name the chemical process in which living things produce carbon dioxide.
10. Chemistry of the environment  →  10.3. Air quality and climate
2. Atoms, elements and compounds  →  2.6. Giant covalent structures
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4
Hydrogen peroxide, H2O2, decomposes into water and oxygen in the presence of a catalyst, manganese(oxide. 2H2O2→ 2H2O+ O2What is meant by the term catalyst? A student studies the rate of decomposition of hydrogen peroxide using the apparatus shown. The student uses 20 cm3 of 0.1 mol / dm3 hydrogen peroxide and 1.0 g of manganese(oxide. The student measures the volume of oxygen given off at regular time intervals until the reaction stops. A graph of the results is shown. hydrogen peroxide catalyst gas syringe volume of oxygen produced / cm3 time / s When is the rate of reaction highest? Suggest one method of increasing the rate of reaction using the same amounts of hydrogen peroxide and manganese(oxide. Calculate the number of moles of hydrogen peroxide used in this experiment. mol Use your answer to and the equation to calculate the number of moles of oxygen produced in the reaction. 2H2O2→ 2H2O+ O2mol Calculate the volume (at r.t.p.) of oxygen produced. dm3 What would be the effect on the volume of oxygen produced if the mass of catalyst was increased? Deduce the volume of oxygen that would be produced if 20 cm3 of 0.2 mol / dm3 hydrogen peroxide was used instead of 20 cm3 of 0.1 mol / dm3 hydrogen peroxide. dm3 The student carries out a second experiment to investigate whether another substance, copper(oxide, is a better catalyst than manganese(oxide. Describe how the second experiment is carried out. You should state clearly how you would make sure that the catalyst is the only variable.
6. Chemical reactions  →  6.2. Rate of reaction
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5
This question is about compounds of nitrogen. Describe the Haber Process giving reaction conditions and a chemical equation. Reference to rate and yield is not required. Give one use of ammonia. The diagram shows the structure of a hydrazine molecule. N H H N H H Draw the electron arrangement of a hydrazine molecule. Show the outer shell electrons only. Hydrazine is a base. Define the term base. Complete the chemical equation to show that hydrazine acts as a base when added to water. N2H4 + H2O → + Nitrogen dioxide is an atmospheric pollutant. State one environmental problem caused by nitrogen dioxide. Explain how oxides of nitrogen, such as nitrogen dioxide, are formed in car engines.
6. Chemical reactions  →  6.3. Reversible reactions and equilibrium
10. Chemistry of the environment  →  10.3. Air quality and climate
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6
Iron pyrite, FeS2, is known as Fool’s Gold because it is a shiny yellow solid which is similar in appearance to gold. Iron pyrite is an ionic compound. Gold is a metallic element. Iron pyrite, FeS2, contains positive and negative ions. The positive ion is Fe2+. Deduce the formula of the negative ion. A student is provided with a sample of iron pyrite and a sample of gold. Suggest how the student could distinguish between the two substances. Sulfur dioxide is produced on a large scale by heating iron pyrite strongly in air. The iron pyrite reacts with oxygen in the air producing iron(oxide, Fe2O3, and sulfur dioxide. Construct a chemical equation for the reaction between iron pyrite and oxygen. Give one use of sulfur dioxide.
9. Metals  →  9.4. Reactivity series
6. Chemical reactions  →  6.4. Redox
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7
Alkanes and alkenes are examples of hydrocarbons. What is meant by the term hydrocarbon? Give the general formula of straight-chain alkanes, alkenes. A compound X contains carbon, hydrogen and oxygen only. X contains 54.54% of carbon by mass, 9.09% of hydrogen by mass and 36.37% of oxygen by mass. Calculate the empirical formula of compound X. Compound X has a relative molecular mass of 88. Deduce the molecular formula of compound X. An ester has the molecular formula C3H6O2. Name and give the structural formulae of two esters with the molecular formula C3H6O2. name of ester structural formula Name the ester produced from the reaction of propanoic acid and methanol. A polyester is represented by the structure shown. C O C O O O What type of polymerisation is used for the production of polyesters? Which simple molecule is removed when the polyester is formed? Complete the diagrams below to show the structures of the monomers used to produce the polyester. Show all atoms and bonds. C C O O
11. Organic chemistry  →  11.2. Naming organic compounds
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