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Admissions tests / ESAT / Chemistry

27 questions in 40 minutes. Multiple choice. No calculator.

ESAT Chemistry

The Chemistry module runs from atomic structure and the Periodic Table through quantitative chemistry, bonding, group chemistry, acids, rates, energetics, electrolysis and organic chemistry. It assumes all of the Mathematics 1 content, and the quantitative strands are where the marks move.

270 original practice questions across 18 sets, grouped by the strand of the published specification each one covers. Every question carries a full worked solution.

  • Each module is separately timed. Time not used on one module is not carried into the next.
  • No calculator. An erasable booklet is provided for working.

Atomic structure and the Periodic Table

Structure of the atom, isotopes, electronic configuration, the arrangement of Periods and Groups, and trends across and down the table.

What the specification says (11 points)
  • C1.1 Describe the structure of the atom as a central nucleus (containing protons and neutrons) surrounded by electrons moving in shells/energy levels.
  • C1.2 Know the relative masses and charges of protons, neutrons and electrons, and recognise that most of the mass of an atom is in the nucleus.
  • C1.3 Know and be able to use the terms atomic number and mass number, together with standard notation, and so be able to calculate the number of protons, neutrons and electrons in any atom or ion.
  • C1.4 Use the atomic number to write the electron configurations of the first 20 elements in the Periodic Table (H to Ca) in comma-separated format (e.g. 2,8,8,1 for a potassium atom).
  • C1.5 Know the definition of isotopes as atoms of an element with the same number of protons but different numbers of neutrons (so having different mass numbers). Use data, including that from a mass spectrometer, to identify the number and abundances of different isotopes of elements.
  • C1.6 Know and use the concept of relative atomic mass, Ar, including calculating values from given data.
  • C2.1 Know that Periods are horizontal rows and Groups are vertical columns.
  • C2.2 Know that the elements are arranged in the order of increasing atomic number.
  • C2.3 Recall the position of metals and non-metals in the Periodic Table: alkali metals (Group 1), alkaline earth metals (Group 2), common non-metals in Group 16, the halogens (Group 17), the noble gases (Group 18) and the transition metals. NOTE: IUPAC conventions are used and Groups are labelled 1-18.
  • C2.4 Know and use the relationship between the position of an atom in the Periodic Table (Group and Period) and the electron configuration of the atom.
  • C2.5 Understand that elements in the same Group have similar chemical properties and that down a metal Group reactivity increases, and down a non-metal Group reactivity decreases.

Quantitative chemistry and redox

Chemical equations, relative molar mass, moles, concentration, yields, limiting reagents, empirical formulae, and oxidation and reduction.

What the specification says (22 points)
  • C3.1 Understand that in a chemical reaction, new substances are formed by the rearrangement of atoms and their electrons, but no nuclei are destroyed or created.
  • C3.2 Know the chemical formulae of simple, common ionic and covalent compounds.
  • C3.3 Know and use state symbols: solid (s), liquid (l), gas (g), aqueous solution (aq).
  • C3.4 Be able to construct and balance a chemical equation, including ionic and half-equations.
  • C3.5 Understand that chemical reactions can be reversible and do not go to completion, reaching a state of equilibrium in a closed system. Know the factors that can affect the position of an equilibrium (concentration of reactants/products, temperature, overall pressure) and predict the effect of changing these factors.
  • C4.1 Use Ar values to calculate the relative molar mass, Mr.
  • C4.2 Know that Avogadro's number gives the number of particles in one mole of a substance.
  • C4.3 Know that one mole of a substance is the Ar or Mr in grams, and perform conversions of grams to moles and vice versa (including working in tonnes and kilograms). Know that the amount of a substance corresponds to the number of moles.
  • C4.4 Calculate the percentage composition by mass of a compound using given Ar values.
  • C4.5 Know that the empirical formula is the simplest integer ratio of atoms in a compound. Find the empirical formula from a variety of data, such as percentage composition by mass or reacting masses. Find the molecular formula from the empirical formula if given the Mr value.
  • C4.6 Use balanced chemical equations to calculate the masses of reactants and products, including if there is a limiting reactant present.
  • C4.7 Be able to construct balanced chemical equations from reacting masses or gas volumes data.
  • C4.8 Understand that (for an ideal gas) one mole of a gas occupies a set volume at a given temperature and pressure (for example, 24 dm3 at room temperature and pressure), and perform conversions of volumes to number of moles and vice versa.
  • C4.9 Solutions: understand that concentration can be measured in mol dm-3 or g dm-3, and calculate the concentration given the number of moles (or mass) of solute and the volume of solution. Know the term saturated solution, calculate solubility and interpret solubility data.
  • C4.10 Use the concentrations of solutions (or find them from given data) and the reacting ratio from the balanced equation to perform titration calculations.
  • C4.11 Calculate the percentage yield of a reaction using the balanced chemical equation and percentage yield = (actual yield / predicted yield) x 100.
  • C5.1 Know that on a basic level, oxidation is the gain of oxygen and reduction is the removal of oxygen.
  • C5.2 Know and use the concept that oxidation and reduction are the transfer of electrons, i.e. reduction is the gain of electrons and oxidation is the loss of electrons.
  • C5.3 Determine and use the oxidation states of atoms in simple inorganic compounds.
  • C5.4 Identify any chemical equation that involves oxidation only, reduction only, redox (both), or no oxidation/reduction.
  • C5.5 Understand the concept of disproportionation and recognise reactions (or species) where this occurs.
  • C5.6 Understand the terms oxidising agent and reducing agent, and be able to identify them in reactions.

Bonding, structure and the groups

Elements, compounds and mixtures, ionic, covalent and metallic bonding, giant and simple structures, states of matter, and the chemistry of Groups 1, 17 and 18.

What the specification says (16 points)
  • C6.1 Define and understand the differences between elements, compounds and mixtures.
  • C6.2 Understand that atoms often react to form compounds which have the electron configuration of a noble gas (Group 18), and that the type of bonding depends on the atoms involved.
  • C6.3 Ionic bonding: know that ions are formed by transfer of electrons from atoms of metals to atoms of non-metals and that these ions attract to form ionic compounds; predict the charge of the most stable ions formed from elements in Groups 1, 2, 16 and 17 and aluminium; know the chemical formulae of common compound ions (e.g. carbonate and hydroxide); know that Roman numerals denote the oxidation state where an element can exist in more than one (e.g. iron(III) chloride); determine the formulae of ionic compounds from their constituent ions; understand the general physical properties of ionic compounds, such as melting point and conductivity.
  • C6.4 Covalent bonding: know that a covalent bond is formed when atoms share one or more pairs of electrons, generally between non-metals; understand that covalently bonded substances can be small molecules (e.g. water, ammonia, methane) or giant structures (e.g. diamond, graphite, silicon dioxide); understand the general physical properties of substances composed of small molecules or existing as giant covalent structures.
  • C6.5 Metallic bonding: understand that solid metals exist as a giant structure of positively charged ions surrounded by delocalised (free) electrons; understand the general physical properties of metals, such as melting point and conductivity.
  • C6.6 Understand that intermolecular forces can exist between molecules, and that these forces must be overcome in melting and boiling.
  • C6.7 Be able to relate structure and bonding to physical properties, such as melting point and conductivity.
  • C7.1 Know the physical and chemical properties of the alkali metals (Group 1), the halogens (Group 17) and the noble gases (Group 18).
  • C7.2 Describe the trends in chemical reactivity and physical properties of the alkali metals (Group 1) and make predictions based on those trends, including knowledge of the relative positions of lithium, sodium and potassium.
  • C7.3 The halogens (Group 17): describe the trends in chemical reactivity and physical properties and make predictions based on those trends, including the relative positions of fluorine, chlorine, bromine and iodine; explain what is meant by a displacement reaction, in terms of reactivity competition, between halogens and halide ions.
  • C8.1 Know that chemical processes are required to displace constituent elements from their compounds.
  • C8.2 Know that physical processes are required to separate mixtures, including miscible/immiscible liquids and dissolved/insoluble solids.
  • C8.3 Know when to apply the following separation techniques: simple/fractional distillation, paper chromatography (including use of Rf values), use of a separating funnel, centrifugation, dissolving, filtration, evaporation and crystallisation.
  • C8.4 Know how to establish the purity of a substance using chromatography.
  • C15.1 Be able to describe the packing and movement of particles in the three states of matter: solid, liquid and gas.
  • C15.2 Understand the changes to the packing and movement of particles in freezing, melting, boiling/evaporating and condensing; understand that the energy required for these processes is related to the bonding and structure of the substance, including a consideration of intermolecular forces.

Acids, rates and energetics

Acids and bases, neutralisation and salts, the qualitative and quantitative effects on rate, catalysts, and exothermic and endothermic change with energy profiles.

What the specification says (14 points)
  • C9.1 Acids: define an acid as a substance that can form H+(aq) ions or that is an H+ donor; describe reactions with metals, carbonates, metal hydroxides and metal oxides in which salts are formed; understand the terms strong, weak, dilute and concentrated; know that some oxides of non-metals react with water to form acidic solutions; recall that pH is a measure of H+ ion concentration and that a change of 1 on the pH scale corresponds to a change by a factor of 10 in H+ ion concentration; know that one mole of some acidic substances can form/donate more than one mole of H+ ions, including the use of the terms mono-, di-, tri- and polyprotic.
  • C9.2 Bases: define a base as a substance that can form OH-(aq) ions or that is an H+ acceptor; understand the terms strong, weak, dilute and concentrated; know that some oxides and hydroxides of metals react with water to form alkaline solutions.
  • C9.3 Know that the reaction of an acid with a base can lead to neutralisation and is often exothermic.
  • C10.1 Describe the qualitative effects on a rate of reaction of concentration, temperature, particle size, a catalyst and, for gases, pressure.
  • C10.2 Know that the rate of reaction can be found by measuring the loss of a reactant or the gain of a product, or by measurement of a physical property over time, and identify which measurement can be used in a given situation.
  • C10.3 Interpret data in graphical form concerning the rate of a reaction.
  • C10.4 Use collision theory to explain changes in the rate of a reaction.
  • C10.5 Understand that particles must have sufficient energy when they collide to react, that this energy is called the activation energy (Ea), and identify the activation energy on an energy level diagram.
  • C10.6 Know that catalysts are not used up in a reaction, are chemically unchanged at the end of a reaction, provide an alternative route (reaction mechanism) with a lower activation energy (and interpret this effect on an energy level diagram), and do not affect the position of an equilibrium.
  • C11.1 Understand the concepts of an exothermic reaction, for which the enthalpy change is negative, and an endothermic reaction, for which the enthalpy change is positive.
  • C11.2 Know that if a reversible reaction is exothermic in one direction, it is endothermic in the other direction.
  • C11.3 Be able to interpret energy level diagrams.
  • C11.4 Be able to calculate energy changes from specific heat capacities and changes in temperature in calorimetry experiments.
  • C11.5 Know that bond breaking is endothermic and bond formation is exothermic, and use bond energy data to calculate energy changes.

Electrochemistry and organic chemistry

Electrodes, electrolysis and its products, the reactivity series and extraction of metals, crude oil and fractional distillation, alkanes, alkenes, alcohols and carboxylic acids, and polymers.

What the specification says (18 points)
  • C12.1 Understand the terms electrode, cathode (negative electrode), anode (positive electrode) and electrolyte.
  • C12.2 Understand why direct current (dc), and not alternating current (ac), is used in electrolysis.
  • C12.3 Understand that in electrolysis at the cathode the cations receive electrons (reduction) to change into atoms or molecules, and at the anode the anions lose electrons to form atoms or molecules (oxidation).
  • C12.4 Understand and predict the products of the electrolysis of aqueous solutions (including those of salts), including situations where more than one ion/molecule is attracted to a single electrode, and of molten binary compounds.
  • C12.5 Be able to write half-equations for the processes taking place at each electrode.
  • C12.6 Explain how electrolysis is used to electroplate objects.
  • C13.1 Organic general concepts: know that crude oil is the main source of hydrocarbons and is separated into fractions by fractional distillation (names and uses of specific fractions not expected); understand the link between carbon chain length and boiling points, viscosity and flammability; know the use of longer chain alkanes in cracking to form shorter chain alkanes and alkenes and write balanced equations; understand structural isomerism and recognise examples; understand and use the terms molecular formula, full structural formula (displayed structure) and condensed structural formula; understand and use the terms complete combustion and incomplete combustion and write balanced equations; know the IUPAC guidelines for the systematic naming of carbon compounds and apply them to name all the compounds in this section; know and understand the terms homologous series and functional group.
  • C13.2 Alkanes (saturated hydrocarbons): describe alkanes as a homologous series with the general formula CnH2n+2; be able to name, or recognise from the name, the C1 to C6 straight-chain alkanes.
  • C13.3 Alkenes (unsaturated hydrocarbons): describe alkenes as a homologous series with a double bond and the general formula CnH2n; name, or recognise from the name, C2 to C6 straight-chain alkenes including the position of the double bond; recognise and use the test for unsaturation with bromine water; know that addition reactions take place with hydrogen, halogens, hydrogen halides and steam, write the balanced equations and recognise the formulae of the products formed. (Mechanisms and consideration of carbocation stability are NOT required.)
  • C13.4a Addition polymerisation, polyalkenes: know that alkenes or other molecules with a C=C bond may react with each other to form long-chain saturated molecules called polymers by addition reactions called polymerisation, and that the unsaturated molecules are called monomers; given an unsaturated monomer molecule, recognise the structure of the polymer and vice versa; recognise the repeating unit of these polymers.
  • C13.4b Condensation polymerisation, polyesters and polyamides (to include amino acids forming proteins): given the monomer molecules, recognise the structure of the polymer and vice versa; recognise the repeating unit. Understand the terms biodegradable and non-biodegradable when applied to polymers.
  • C13.5 Alcohols: describe alcohols as a homologous series with the general formula CnH2n+1OH; name, or recognise from the name, C1 to C6 straight-chain alcohols including the position of the -OH group; describe the reaction of alcohols with sodium metal.
  • C13.6 Carboxylic acids: describe carboxylic acids as a homologous series with the general formula CnH2n+1COOH; name, or recognise from the name, C1 to C6 straight-chain carboxylic acids; describe the chemical properties of carboxylic acids as those of weak acids, and predict their reactions and determine the formulae of their salts; know that carboxylic acids react with alcohols in the presence of an acid catalyst to produce esters.
  • C14.1 Understand that the reactivity of a metal is linked to its tendency to form positive ions and the ease of extraction of the metal.
  • C14.2 Be able to use displacement reactions to establish the order of reactivity of metals and vice versa.
  • C14.3 Describe how the uses of metals are related to their physical and chemical properties (e.g. Al, Fe, Cu, Ag, Au, Ti), and understand that alloys can be formed to produce materials with specific properties.
  • C14.4 Know that most metal ores are the oxides of the metal, and that the extraction of metals always involves reduction processes.
  • C14.5 Know that common properties of transition metals include: they are able to form stable ions in different oxidation states; they often form coloured compounds; they are often used as catalysts (as ions or atoms).

Chemical analysis and the atmosphere

Tests for gases and ions, separation techniques, chromatography, the composition of dry air and fractional distillation of air.

What the specification says (9 points)
  • C16.1 Know and recognise the tests for gases: hydrogen (explodes with a 'squeaky pop' when a burning splint is held at the open end of a test tube); oxygen (relights a glowing splint); carbon dioxide (limewater turns cloudy when shaken with the gas); chlorine (damp blue litmus paper turns red and then is bleached).
  • C16.2 Know, recognise and describe the tests for anions: carbonates using a dilute acid; halides using an aqueous solution of silver nitrate in the presence of dilute nitric acid (chlorides white precipitate, bromides cream precipitate, iodides yellow precipitate); sulfates using an aqueous solution of barium chloride in the presence of dilute hydrochloric acid.
  • C16.3 Know and recognise the test for metal cations using aqueous sodium hydroxide: Al3+, Ca2+ and Mg2+ each form a white precipitate; Cu2+ forms a blue precipitate; Fe2+ forms a green precipitate; Fe3+ forms a brown precipitate.
  • C16.4 Recall and recognise the flame test for the cations of the following metals: Li (crimson red), Na (yellow-orange), K (lilac), Ca (red-orange), Cu (green).
  • C16.5 Know and recognise the test for the presence of water using anhydrous copper(II) sulfate (colour change from white to blue).
  • C17.1 Know and be able to use the composition of dry air, and understand that fractional distillation can be used to separate the components of air.
  • C17.2 Know the origins and describe the effects of greenhouse gases such as CO2 and CH4.
  • C17.3 Know the origins and effects of gaseous pollutants such as CO, CO2, SO2 and NOx.
  • C17.4 Know the purpose of chlorine and fluoride ions in the treatment of drinking water.

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