Numbers
CCEA A-Level Chemistry 1110
Formulae, Equations and Amounts of Substance
Atomic Structure
Topic overviewProtons, neutrons and electronsAtomic number, mass number and the composition of ionsIsotopes and relative isotopic massRelative atomic, molecular and formula massMass spectra and relative atomic mass calculationsMass spectra of diatomic elementsElectronic configuration and the building up principleOrbitals, electron spin and orbital shapesThe s-, p-, d- and f-blocks of the Periodic TableIonisation energies and their equationsTrends in ionisation energy as evidence for shells and subshells
Bonding
Topic overviewIonic bonding and electron transferDot and cross diagrams for ionic compoundsCovalent bonding and the shared pairLone pairs and co-ordinate bondingDot and cross diagrams for covalent molecules and ionsThe octet rule and its limitationsElectronegativity and bond polarityMetallic bonding
Intermolecular Forces and Structure
Shapes of Molecules and Ions
Redox
The Halogens
Acid-Base Titrations
Qualitative Tests
Formulae and Amounts of a Substance
Nomenclature and Isomerism in Organic Chemistry
Alkanes
Topic overviewAlkanes as saturated hydrocarbonsBoiling points of alkanes and van der Waals' forcesBoiling points of branched isomersComplete and incomplete combustion of alkanesPollutants from alkane fuels and the atmosphereCatalytic convertersRadicals, homolytic fission and heterolytic fissionFree radical substitution of alkanes
Alkenes
Topic overviewUnsaturated hydrocarbons and the bromine water testSigma and pi bonds in the carbon–carbon double bondElectron density at C=C, reactivity and catalytic hydrogenationAddition of chlorine and bromine to alkenesAddition of hydrogen chloride and hydrogen bromideElectrophiles, heterolytic fission and the addition mechanismCarbocation stability and Markovnikov additionAddition polymerisation of alkenes
Halogenoalkanes
Topic overviewClassification and boiling points of halogenoalkanesLaboratory preparation of a halogenoalkane from an alcoholNucleophiles and hydrolysis with aqueous alkaliReactions with ammonia and with potassium cyanideRelative rates of hydrolysis and carbon–halogen bond enthalpyElimination using ethanolic potassium hydroxideCFCs and the ozone layer
Alcohols
Infrared Spectroscopy
Energetics
Topic overviewExothermic and endothermic changesStandard conditions and the standard enthalpy changeEnthalpy level diagramsStandard enthalpies of combustion and formationStandard enthalpy of neutralisationMeasuring enthalpy changes by experimentEnthalpy calculations using q = mcΔTHess's Law and enthalpy cyclesIndirect enthalpy calculations using Hess's LawAverage bond enthalpies and their limitations
Kinetics
Equilibrium
Group II Elements and Their Compounds
Topic overviews-block character and electronic configurationTrends in atomic radius and first ionisation energyReactions of the elements with oxygen, water and dilute acidsThe oxides and their reactions with water and dilute acidsThermal stability of the carbonates and hydroxidesUses of magnesium oxide, calcium carbonate and limeSolubility trends and solubility curves
Lattice Enthalpy, Entropy and Free Energy
Topic overviewLattice enthalpy and the factors that control itBorn–Haber cycles for Group I halidesBorn–Haber cycles for Group II halides and oxidesEnthalpy of hydration and enthalpy of solutionCalculations on dissolving ionic compoundsEntropy and the limits of enthalpy changeStandard entropy change calculationsFree energy and the temperature of feasibility
Rates of Reaction
Equilibrium and Acid-Base Equilibria
Topic overviewEquilibrium concentrations from initial amountsKc expressions, values and unitsBrønsted–Lowry acids, bases and conjugate pairsKw, pH and the pH of strong acids and basesKa, pKa and the pH of weak acidsBuffer solutions and how they resist pH changeCalculating the pH of a buffer solutionTitration curves, indicators and the pH of salt solutions
Isomerism
Aldehydes and Ketones
Topic overviewStructure and naming of aldehydes and ketonesBoiling points and solubility of carbonyl compoundsPreparation from primary and secondary alcoholsReaction with hydrogen cyanide and the nucleophilic addition mechanismRacemic mixtures from nucleophilic addition2,4-dinitrophenylhydrazine and the identification of carbonylsDistinguishing aldehydes from ketones, and reduction with lithal
Carboxylic Acids
Derivatives of Carboxylic Acids
Topic overviewEsters and acyl chlorides: structure and namingBoiling points and solubility of monoestersMaking esters from alcohols with carboxylic acids or acyl chloridesThe laboratory preparation of a liquid esterFats and oils as esters of glycerolTransesterification, biodiesel and margarineReactions of acyl chlorides with water and alcohols
Aromatic Chemistry
Spectroscopy and Chromatography
Topic overviewThe mass spectrum: molecular ion and base peakFragmentation and the formulae of fragment ionsHigh resolution mass spectrometryNuclear magnetic resonance and the TMS standardChemically equivalent hydrogens and chemical shiftIntegration curvesSpin–spin splitting and the n+1 ruleDeducing a structure from an nmr spectrumPaper and thin-layer chromatographyGas–liquid chromatography
Volumetric Analysis
Transition Metals
Topic overviewThe characteristic properties of the transition metalsElectronic configurations of the metals and their ionsComplexes, ligands and coordination numberOxidation number, redox and disproportionationMonodentate, bidentate and polydentate ligandsLigand strength and the entropy of ligand replacementLigand replacement in copper(II) complexesThe colours of the aqueous transition metal ionsHydroxide precipitates with sodium hydroxidePrecipitates with aqueous ammonia and their dissolutionVanadium and the interconversion of its oxidation states
Electrode Potentials
Amines
Amides and Polymers
Amino Acids and Proteins
Atomic Structure
- 11 subtopics
- 33 things to know
- Unit AS 1
What Atomic Structure covers
Atomic Structure is examined in Unit AS 1, Basic Concepts in Physical and Inorganic Chemistry, and drawn on again in Unit AS 3, Basic Practical Chemistry. It covers protons, neutrons and electrons, atomic number, mass number and the composition of ions, isotopes and relative isotopic mass, relative atomic, molecular and formula mass, mass spectra and relative atomic mass calculations, mass spectra of diatomic elements, electronic configuration and the building up principle, orbitals, electron spin and orbital shapes, the s-, p-, d- and f-blocks of the Periodic Table, ionisation energies and their equations and Trends in ionisation energy as evidence for shells and subshells.
Where it is assessed
Unit AS 1
Basic Concepts in Physical and Inorganic Chemistry, and again in Unit AS 3, Basic Practical Chemistry.
Check the CCEA specification ↗The 11 subtopics
Each one has its own page.
- Protons, neutrons and electronsRelative mass and relative charge of a proton, relative mass and relative charge of a neutron and relative mass and relative charge of an electron.Open →
- Atomic number, mass number and the composition of ionsAtomic number of an element and mass number of an atom.Open →
- Isotopes and relative isotopic massTerm isotopes, relative isotopic mass and numbers of neutrons in the isotopes ³⁵Cl and ³⁷Cl.Open →
- Relative atomic, molecular and formula massRelative atomic mass, relative molecular mass and percentage by mass of nitrogen in ammonium nitrate, NH₄NO₃.Open →
- Mass spectra and relative atomic mass calculationsRecall questions on what the m/z axis and peak heights measure, why the sample is ionised, calculating relative atomic mass as a weighted mean from percentage abundances, working backwards from a known mass to find abundances, and why the abundances must total 100%.Open →
- Mass spectra of diatomic elementsRecall questions on why the spectrum of chlorine falls into atomic and molecular groups, the m/z values of each, which isotope combination gives each molecular peak, predicting the 9 : 6 : 1 ratio from probability, the double route to the mixed peak, and the corresponding spectrum of bromine.Open →
- Electronic configuration and the building up principleBuilding up principle and hund's rule for filling a subshell.Open →
- Orbitals, electron spin and orbital shapesTerm orbital, shape of an s orbital and shape of a p orbital.Open →
- The s-, p-, d- and f-blocks of the Periodic TableRecall questions on what determines an element's block, which groups make up the s- and p-blocks, where the d- and f-blocks sit, classifying magnesium, bromine and iron, why helium is placed in Group 0, and how block relates to position in a period.Open →
- Ionisation energies and their equationsFirst ionisation energy of an element and second ionisation energy of an element.Open →
- Trends in ionisation energy as evidence for shells and subshellsWhy first ionisation energy decreases down a group and general increase in first ionisation energy across a period.Open →
What you need to know
Answer each one before you reveal it.
Your recallNot started
Key term
Why is the volume of an atom far greater than the volume of its nucleus?
Key term
Define the atomic number of an element.
Key term
Define the term isotopes.
Key term
Why is the term relative formula mass used for an ionic compound rather than relative molecular mass?
Key term
What does the horizontal axis of a mass spectrum measure?
Key term
Why does the mass spectrum of chlorine gas show peaks in two separate groups?
Key term
State the building up principle.
Key term
Define the term orbital.
Key term
What determines the block to which an element belongs?
Key term
Write the general equation for the first ionisation energy of an element X.
Key term
State the three factors that determine the size of a first ionisation energy.
Key term
Define the mass number of an atom.
Key term
Why do the isotopes of an element have identical chemical properties?
Numbers
Calculate the relative molecular mass of sulfuric acid, H₂SO₄.
Key term
Why is the m/z value normally taken as the mass of the ion?
Key term
At which m/z values do the atomic peaks appear in the mass spectrum of chlorine?
Key term
Give the order in which the subshells are filled up to krypton.
Key term
How many electrons can occupy a single orbital, and what must be true of them?
Key term
Which groups make up the s-block?
Key term
Write the equation for the first ionisation energy of magnesium.
Key term
Explain why first ionisation energy decreases down a group.
Key term
Where in the atom is each of the three subatomic particles found?
Key term
How is the number of neutrons in an atom found from its atomic and mass numbers?
Key term
Give one physical property in which two isotopes of an element differ.
Numbers
Calculate the relative formula mass of calcium hydroxide, Ca(OH)₂.
Key term
What does the height of a peak in the mass spectrum of an element indicate?
Key term
At which m/z values do the molecular ion peaks appear in the mass spectrum of chlorine?
Numbers
How many electrons can be held in the s, p and d subshells?
Key term
Why must two electrons in the same orbital have opposite spins?
Key term
Which groups make up the p-block?
Key term
Write the equation for the second ionisation energy of magnesium.
Key term
Explain the general increase in first ionisation energy across a period.
Take Atomic Structure further
The same content, four other ways.
Questions from this topic
Each one with the model answer underneath.
- 1
Where in the atom is each of the three subatomic particles found?
Model answer
Protons and neutrons are found in the nucleus, and electrons occupy the space around the nucleus in shells.
- 2
State the relative mass and relative charge of a proton.
Model answer
A proton has a relative mass of 1 and a relative charge of +1.
- 3
State the relative mass and relative charge of a neutron.
Model answer
A neutron has a relative mass of 1 and a relative charge of 0.
- 4
State the relative mass and relative charge of an electron.
Model answer
An electron has a relative mass of about 1/1836 and a relative charge of −1.
- 5
Why is almost all the mass of an atom concentrated in the nucleus?
Model answer
Protons and neutrons each have a relative mass of 1 and both sit in the nucleus, while electrons have a mass close to zero on the same scale.
- 6
Explain why an atom has no overall charge.
Model answer
An atom contains equal numbers of protons and electrons, so the total positive charge exactly cancels the total negative charge.
What is inside Levo
Six ways to work the same material.
Atomic Structure revision questions
- What does Atomic Structure cover in CCEA A-Level Chemistry?
- 11 subtopics: protons, neutrons and electrons, atomic number, mass number and the composition of ions, isotopes and relative isotopic mass, relative atomic, molecular and formula mass, mass spectra and relative atomic mass calculations, mass spectra of diatomic elements, electronic configuration and the building up principle, orbitals, electron spin and orbital shapes, the s-, p-, d- and f-blocks of the periodic table, ionisation energies and their equations and trends in ionisation energy as evidence for shells and subshells. Each one has its own page with questions and model answers.
- How is Atomic Structure organised?
- By the CCEA 1110 specification, subtopic by subtopic, so it matches the order you are taught it in.
Every question in Atomic Structure, on a schedule.
Attempt a question from memory, write the correct version, then attempt it again. Levo records the jump between your first attempt and your last, and brings each question back on the day you are due to forget it.
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