9701_s19_qp_23
A paper of Chemistry, 9701
Questions:
6
Year:
2019
Paper:
2
Variant:
3
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1
A sample contains three different types of atom: 40Ar , 40K 19 and 40Ca . State fully, in terms of the numbers of subatomic particles, what these three atoms have in common. State fully, in terms of the numbers of all subatomic particles, how these three atoms differ from each other. A sample of sulfur contains only two isotopes, 32S and 34S. The relative atomic mass of this sample is 32.09. isotope isotopic mass 32S 32.0 34S 34.0 Calculate the percentage abundance of the isotopes present in this sample.  % abundance 32S =  % abundance 34S =  The electronic configuration of a sulfur atom is 1s22s22p63s23p4. Identify which orbital in a sulfur atom has the lowest energy. Sketch the shape of a p orbital.  During the process of ionisation a sulfur atom loses an electron. SS++ e– ΔH = 1000 kJ mol–1 Identify the orbital from which this electron is removed. Explain your answer. orbital explanation  Complete the diagram to show the arrangement of electrons within the third shell of a phosphorus atom. 3s 3p  Explain why the first ionisation energy of sulfur is less than that of phosphorus. 
1. Atomic structure  →  1.3. Electrons, energy levels and atomic orbitals
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2
Iodine is an element in Group17 of the Periodic Table. At room temperature, iodine solid has a lattice structure. Describe the arrangement of the iodine molecules within the solid. List all of the forces of attraction present in solid iodine and identify which of these are overcome when solid iodine is heated to produce iodine vapour. forceof attraction present forceof attraction overcome  Iodine reacts with aluminium to form a white solid, Al 2I6. The diagram shows the arrangement of the outer electrons within a molecule of Al 2I6. Al Al I I I I I I How many co-ordinate (dative covalent) bonds are made when a molecule of Al 2I6 is formed from its atoms? Describe how co-ordinate (dative covalent) bonds form within this molecule. In a reaction between hydrogen iodide and concentrated sulfuric acid, the products are hydrogensulfide, sulfur, iodine and water. Write an equation for this reaction. You may wish to use oxidation numbers to help you. Explain, with reference to oxidation numbers, why this reaction is a redox reaction. 
3. Chemical bonding  →  3.4. Covalent bonding and coordinate (dative covalent) bonding
4. States of matter  →  4.2. Bonding and structure
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3
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. Acid indigestion is caused by an excess of hydrochloric acid in the stomach. Magnesium oxide is commonly found in indigestion tablets. Give the equation to show how magnesium oxide relieves acid indigestion. Name the type of reaction that occurs in . Magnesium oxide is described as a ceramic material. It has a high melting point. State and explain why ceramic materials such as magnesium oxide have high melting points. Magnesium oxide can be made from magnesium carbonate in a one-step reaction using heat. Write an equation for this reaction. Include state symbols. Name the type of reaction occurring during this process. 
10. Group 2  →  10.1. Similarities and trends in the properties of the Group 2 metals, magnesium to barium, and their compounds
3. Chemical bonding  →  3.2. Ionic bonding
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4
Release of sulfur dioxide, SO2, into the atmosphere causes acid rain. Explain why high levels of SO2 may be found in the atmosphere near power stations that burn fossil fuels. The SO2 released can be converted in the atmosphere into sulfuric acid, H2SO4, by reaction with nitrogen dioxide gas, NO2, and water, H2O. SO2 + NO2 NO + SO3 SO3 + H2O H2SO4 During one year, 1590 tonnes of SO2 was released into the atmosphere by a fossil-fuel burning power station. Use the equations to calculate how many tonnes of H2SO4 were formed in the atmosphere. Assume that all of the SO2 released was converted into H2SO4.  mass of H2SO4 = tonnes Describe how NO2 is also produced by these power stations. State one natural cause of NO2 being formed in the atmosphere. Explain why NO2 can be described as a catalyst in the oxidation of atmospheric SO2. 
12. Nitrogen and sulfur  →  12.1. Nitrogen and sulfur
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5
Halogenoalkanes react with a number of different reagents in nucleophilic substitution reactions. A sample of potassiumcyanide dissolved in ethanol is added to a sample of 1-bromobutane, CH3(CH2)3Br, and heated under reflux. A nucleophilic substitution reaction occurs and compoundA is formed. Name compoundA. What is meant by the term nucleophile? Identify the nucleophile in this reaction. Explain why this reaction is described as a substitution reaction. State the reagentand conditions needed for CH3(CH2)3Br to react to form CH3(CH2)3NH2. reagentconditions  Equal amounts of three different halogenoalkanes are added to three separate test‑tubes. An equal amount of aqueous silvernitrate and ethanol is added to each test‑tube. The time taken for a precipitate to form is recorded for each halogenoalkane. halogenoalkane time taken for precipitate to form / s (CH3)3CCl (CH3)3CBr (CH3)3CI Describe and explain the trend in reactivity of the different halogenoalkanes shown in this experiment. All three halogenoalkanes tend to react via the SN1 mechanism. Explain why the SN1 mechanism is favoured. Identify a halogenoalkane which tends to react with an aqueous solution of silver nitrate and ethanol via the SN2 mechanism. 
15. Halogen compounds  →  15.1. Halogenoalkanes
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6
Three alkenes, X, Y and Z, have the same molecular formula. Describe what is seen when aqueousbromine is added to X. X, Y and Z are reacted separately with hot, concentrated, acidified manganate(ions until no further reaction occurs. The carbon-containing products are shown in the table. alkene carbon-containing products X CO2 + (CH3)2CO Y CO2 + CH3CH2CO2H Z CH3CO2H Draw the structures of X, Y and Z. X Y Z  Deduce the molecular formula of X, Y and Z. The structures of V and W are shown. CH3(CH2)2CH2OH (CH3)3COH V W Name the class of compound that V and W each belong to. V W  V and W both react with sodium metal. Write an equation for the reaction of V with sodium metal. Name a reagent used to distinguish V from W. Describe any observations. reagent observations with V observations with W  
14. Hydrocarbons  →  14.2. Alkenes
14. Hydrocarbons  →  14.1. Alkanes
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