OCR A-Level Chemistry AS Breadth in chemistry (01), June 2018
Every question from OCR A-Level Chemistry AS Breadth in chemistry (01), June 2018 (H032): 25 questions, 70 marks, each with its mark scheme and topic.
- Question 1 1 mark
Determine the formula of the compound formed when sodium reacts with element X, given the electron configuration of element X.
Module 2: Foundations in chemistry · 2.2 Electrons, bonding and structure · 2.1 Atoms and reactions
- Question 2 1 mark
Calculate the number of oxygen atoms in 88.0 g of CO2
Module 2: Foundations in chemistry · 2.1 Atoms and reactions
- Question 3 1 mark
Identify the compound with a given percentage composition by mass from four multiple-choice options.
Module 2: Foundations in chemistry · 2.1 Atoms and reactions
- Question 4 1 mark
Calculate the mass of sodium that reacts with water to produce 960 cm3 of hydrogen gas at RTP based on a given chemical equation.
Module 2: Foundations in chemistry · 2.1 Atoms and reactions
- Question 5 1 mark
Identify which chemical equation does not represent a neutralisation reaction among the four given options.
Module 2: Foundations in chemistry · 2.1 Atoms and reactions
- Question 6 1 mark
Determine the oxidation number of iron in K2FeO4.
Module 2: Foundations in chemistry · 2.1 Atoms and reactions
- Question 7 1 mark
Identify which given chemical reaction shows the oxidation of sulfur.
Module 3: Periodic table and energy · 3.1 The periodic table
- Question 8 1 mark
Identify the property that determines the order of elements in the Periodic Table.
Module 2: Foundations in chemistry · Module 3: Periodic table and energy · 2.1 Atoms and reactions · 3.1 The periodic table
- Question 9 1 mark
Deduce the formula of the chloride of element Y using its first five successive ionisation energies.
Module 2: Foundations in chemistry · Module 3: Periodic table and energy · 2.1 Atoms and reactions · 2.2 Electrons, bonding and structure · 3.1 The periodic table
- Question 10 1 mark
Identify which element has induced dipole-dipole interactions (London forces) in its solid lattice among boron, magnesium, silicon, and sulfur.
Module 2: Foundations in chemistry · Module 3: Periodic table and energy · 2.2 Electrons, bonding and structure · 3.1 The periodic table
- Question 11 1 mark
Calculate the standard enthalpy change of combustion of aluminium sulfide using standard enthalpy changes of formation.
Module 3: Periodic table and energy · 3.2 Physical chemistry
- Question 12 1 mark
Identify which experimental error caused the calculated enthalpy change of combustion of methanol to be more exothermic than the data book value.
Module 3: Periodic table and energy · Practical Activity Groups · 3.2 Physical chemistry · PAG 3: Enthalpy determination
- Question 13 1 mark
Deduce the changes in pressure and temperature required to shift the equilibrium position towards the products for the given reversible reaction.
Module 3: Periodic table and energy · 3.2 Physical chemistry
- Question 14 1 mark
Identify the correct expression for the equilibrium constant Kc for the reversible reaction between nitrogen and hydrogen to form ammonia.
Module 5: Physical chemistry and transition elements · 5.1 Rates, equilibrium and pH
- Question 15 1 mark
Identify the formula of a compound that reacts with 8 mol of O2 for complete combustion from multiple choice options.
Module 2: Foundations in chemistry · 2.1 Atoms and reactions
- Question 16 1 mark
Determine the number of tertiary alcohol structural isomers with the molecular formula C6H14O.
Module 4: Core organic chemistry · 4.2 Alcohols, haloalkanes and analysis
- Question 17 1 mark
Determine the molecular formula of naphthalene from its skeletal structure.
Module 6: Organic chemistry and analysis · 6.1 Aromatic compounds, carbonyls and acids
- Question 18 1 mark
Identify the product formed from the reaction of pent-2-ene with bromine
Module 4: Core organic chemistry · 4.1 Basic concepts and hydrocarbons
- Question 19 1 mark
Identify the correct E/Z isomerism for two double bonds in a given branched alkene molecule from multiple-choice options
Module 4: Core organic chemistry · 4.1 Basic concepts and hydrocarbons
- Question 20 1 mark
Identify which alcohol is likely to have a fragment ion at m/z = 31 in its mass spectrum from a given list of four structural formulas.
Module 4: Core organic chemistry · Module 6: Organic chemistry and analysis · 4.2 Alcohols, haloalkanes and analysis · 6.3 Analysis
- Question 21 8 marks
Calculate the relative atomic mass of silicon, determine atomic structure, draw a dot-and-cross diagram, predict the shape of phosgene, and explain why elements belong to the p-block.
Module 2: Foundations in chemistry · Module 3: Periodic table and energy · 2.1 Atoms and reactions · 2.2 Electrons, bonding and structure · 3.1 The periodic table
- Question 22 13 marks
Calculate the mass of magnesium needed to react with phosphoric acid, determine the volume of phosphine gas produced using the ideal gas equation, and write related chemical equations.
Module 2: Foundations in chemistry · Module 3: Periodic table and energy · 2.1 Atoms and reactions · 3.2 Physical chemistry
- Question 23 10 marks
Calculate the enthalpy change for the reaction between magnesium and silver nitrate, explain how to test if the reaction went to completion using sodium chloride, and use the Boltzmann distribution model to explain the effect of temperature on reaction rate.
Module 3: Periodic table and energy · Module 5: Physical chemistry and transition elements · Practical Activity Groups · 3.2 Physical chemistry · 5.1 Rates, equilibrium and pH · PAG 3: Enthalpy determination
- Question 24 10 marks
Explain structural isomerism and boiling point trends of saturated hydrocarbons A, B, and C, and analyse their reactions with chlorine.
Module 4: Core organic chemistry · 4.1 Basic concepts and hydrocarbons
- Question 25 9 marks
Deduce the products of alcohol reactions, name the alcohol, outline the haloalkane hydrolysis mechanism, and explain IR spectroscopy changes for the functional group conversion.
Module 4: Core organic chemistry · Module 6: Organic chemistry and analysis · 4.2 Alcohols, haloalkanes and analysis · 6.3 Analysis