What does it mean to call a substance amphoteric?

An amphoteric substance reacts with both acids and bases. It behaves as a base towards an acid and as an acid towards a base, so it dissolves in both.

Aluminium foil dissolves in warm dilute hydrochloric acid. Write the ionic equation and state what is seen.

2Al(s) + 6H⁺(aq) → 2Al³⁺(aq) + 3H₂(g). The grey metal dissolves with steady effervescence of a colourless gas, leaving a colourless solution.

Why does aluminium also dissolve in hot aqueous sodium hydroxide, and what is the aluminium-containing product?

Aluminium is amphoteric, so it is attacked by strong alkali as well as by acid: 2Al(s) + 2OH⁻(aq) + 6H₂O(l) → 2[Al(OH)₄]⁻(aq) + 3H₂(g). The product is the colourless tetrahydroxoaluminate(III) ion, and hydrogen is given off.

Write the equation for aluminium hydroxide dissolving in dilute nitric acid.

Al(OH)₃(s) + 3H⁺(aq) → Al³⁺(aq) + 3H₂O(l). The white precipitate dissolves to give a colourless solution.

Explain why aluminium hydroxide is described as amphoteric.

It dissolves in acid by accepting protons to give Al³⁺(aq), acting as a base, and it dissolves in alkali by accepting a hydroxide ion to give [Al(OH)₄]⁻, acting as an acid. Because it reacts in both ways it is amphoteric.

WJEC A-Level Chemistry 1410QS

Formulae and Equations

Topic overview Charges on common ions Building formulae for ionic and molecular compounds Assigning oxidation numbers Using oxidation numbers to follow redox changes Balancing equations and using state symbols Ionic and half equations

Basic Ideas About Atoms

Topic overview Radioactive decay and nuclear equations Alpha, beta and gamma radiation Half-life, dating and the uses of radioisotopes: half-life of radioactive decay Half-life, dating and the uses of radioisotopes: adverse consequences for living cells Ionisation energies and electronic structure Orbitals and the filling of sub-shells Atomic spectra and the energy of light: atomic emission spectrum of the hydrogen atom Atomic spectra and the energy of light: relationship between energy and frequency Atomic spectra and the energy of light: significance of the frequency

Chemical Calculations

Topic overview Relative masses and the mass spectrometer: relative atomic Relative masses and the mass spectrometer: how a mass spectrometer works Relative masses and the mass spectrometer: molecular ion The mole, the Avogadro constant and molar mass: relative mass terms and simple mass spectra The mole, the Avogadro constant and molar mass: moles and percentage composition by mass Empirical and molecular formulae Concentration, solubility and titration calculations: concentration in mol dm-3 and in g dm-3 Concentration, solubility and titration calculations: stoichiometry and the limiting reagent Concentration, solubility and titration calculations: titration calculations and estimating a titre Gas volumes and the ideal gas equation Yield, atom economy and experimental uncertainty: concepts of atom economy and percentage yield Yield, atom economy and experimental uncertainty: how to estimate the percentage error

Bonding

Topic overview Ionic bonds and covalent bonds: ionic bonding in terms of ion formation Ionic bonds and covalent bonds: covalent bonding and forces Electronegativity, polarity and in-between bonds: concepts of electronegativity and bond polarity Electronegativity, polarity and in-between bonds: forces Forces between molecules Hydrogen bonding Shapes of molecules and ions: VSEPR principle and its use Shapes of molecules and ions: bond angles associated with linear

Solid Structures

Topic overview Ionic crystals: sodium chloride and caesium chloride Giant covalent structures: diamond and graphite Simple molecular solids: iodine and ice Metals and the electron sea Using structure to explain physical properties

The Periodic Table

Topic overview How the Periodic Table is organised Oxidation and reduction as electron transfer Trends across periods and down groups Group 2: reactions, trends and the reasons behind them — reactions with oxygen, water and dilute acid Group 2: reactions, trends and the reasons behind them — trends down the group Group 2: reactions, trends and the reasons behind them — thermal stability of the carbonates Group 2: reactions, trends and the reasons behind them — oxides and hydroxides Identifying ions, making salts and gravimetric analysis: identifying cations with sodium hydroxide Identifying ions, making salts and gravimetric analysis: preparing a soluble salt from an acid Group 7: the halogens — physical properties and the trend in volatility Group 7: the halogens — reactions of the halogens with metals Group 7: the halogens — displacement reactions and the trend Group 7: the halogens — halide ions as reducing agents, uses of chlorine and the chlorate equilibrium

Simple Equilibria and Acid-Base Reactions

Topic overview Reversible reactions and dynamic equilibrium Le Chatelier's principle and shifting the position of equilibrium The equilibrium constant Kc Acids, bases, salts and neutralisation pH, strong acids and weak acids Acid-base titrations and their calculations

Thermochemistry

Topic overview Enthalpy changes and their definitions Calculating enthalpy changes from experimental measurements Determining enthalpy changes in the laboratory Hess's law and energy cycles Average bond enthalpies

Rates of Reaction

Topic overview Collision theory and the conditions that change rate Measuring rate and relating it to concentration Energy profiles and activation energy Temperature and the Boltzmann distribution Catalysts and how they work Following reactions in the laboratory

The Wider Impact of Chemistry

Topic overview Social and economic consequences of chemical manufacture and energy supply Environmental consequences of chemical processes and energy production Green chemistry and sustainable practice

Organic Compounds

Topic overview Drawing and reading organic structures Naming organic compounds Chain length, functional groups and physical properties Structural isomerism Electrophiles, nucleophiles, radicals and bond fission

Hydrocarbons

Topic overview Alkane bonding, combustion and fossil fuels: combustion reaction of alkanes and benefits Alkane bonding, combustion and fossil fuels: combustion calculations and acid rain Radical substitution of alkanes The C=C bond and why alkenes are reactive E–Z isomerism in alkenes Electrophilic addition, Markovnikov's rule and testing for alkenes: mechanism of electrophilic addition Electrophilic addition, Markovnikov's rule and testing for alkenes: Markovnikov's rule and the bromine water test Electrophilic addition, Markovnikov's rule and testing for alkenes: testing for a C=C bond Hydrogenation and addition polymers: conditions required Hydrogenation and addition polymers: nature of addition polymerisation

Halogenoalkanes

Topic overview Nucleophilic substitution by hydroxide ions Elimination to form alkenes Reactivity of the carbon–halogen bond and the silver nitrate test Uses of halogenoalkanes, CFCs and the ozone layer: uses of halogenoalkanes and CFCs Uses of halogenoalkanes, CFCs and the ozone layer: radical mechanism Uses of halogenoalkanes, CFCs and the ozone layer: replacements for CFCs Heating under reflux in the laboratory

Alcohols and Carboxylic Acids

Topic overview Two routes to ethanol: hydration and fermentation — hydration of ethene Two routes to ethanol: hydration and fermentation — fermentation Two routes to ethanol: hydration and fermentation — comparing the two routes on rate Classifying alcohols and dehydrating them Oxidising alcohols to aldehydes, ketones and acids Chemical tests for alcohols and carboxylic acids Carboxylic acids, bases and salts Making an ester and separating it by distillation: esterification Making an ester and separating it by distillation: carrying out the preparation Making an ester and separating it by distillation: separating and purifying Making an ester and separating it by distillation: yield

Instrumental Analysis

Topic overview Reading a mass spectrum Infrared spectra and functional groups NMR spectra and atomic environments Putting the three techniques together

Redox and Standard Electrode Potential

Topic overview Electron transfer and oxidation numbers Half-equations, half-cells and cell diagrams The hydrogen electrode and standard electrode potentials Cell EMF and the feasibility of reactions The hydrogen fuel cell

Redox Reactions

Topic overview Building ion–electron half-equations Combining half-equations into full equations Copper, iodide and thiosulfate Carrying out and calculating a redox titration: procedure for a manganate titration Carrying out and calculating a redox titration: redox titration calculations

Chemistry of the P-Block

Topic overview Amphoteric behaviour of aluminium and lead Stability of oxidation states down Groups 3, 4 and 5: increasing stability of the inert pair cations Stability of oxidation states down Groups 3, 4 and 5: change in relative stability Valence shells that break the octet rule: how some Group 3 elements can form compounds Valence shells that break the octet rule: structure and bonding in Al2Cl6 and formation Boron nitride: two structures, two sets of properties Group 4 oxides and chlorides, and lead in solution: structure Group 4 oxides and chlorides, and lead in solution: hydrolysis of the Group 4 chlorides Group 4 oxides and chlorides, and lead in solution: chloride hydrolysis and lead(II) precipitates Group 4 oxides and chlorides, and lead in solution: distinguishing lead from silver ions Chlorine, chlorate and the sodium halides: chlorine with water and with cold and hot alkali Chlorine, chlorate and the sodium halides: bleaching and bactericidal action of Cl2 Chlorine, chlorate and the sodium halides: differences in behaviour of NaCl

Chemistry of the D-Block Transition Metals

Topic overview Variable oxidation states and the colours of their solutions: how the d-block elements attain various Variable oxidation states and the colours of their solutions: most important oxidation states of Cr Complex ions: ligands, coordination number and shape Why transition metal complexes are coloured Ligand exchange and changes in coordination number Transition metals as catalysts: why transition metals Transition metals as catalysts: variable oxidation state Transition metals as catalysts: heterogeneous catalysis Transition metals as catalysts: surface area Transition metal ions with aqueous hydroxide

Chemical Kinetics

Topic overview Following a reaction by sampling and quenching Finding the order of a reaction from experimental results The rate equation and the rate constant Rate-determining steps and reaction mechanisms Temperature, catalysts and the Arrhenius equation

Enthalpy Changes for Solids and Solutions

Topic overview Defining the enthalpy changes Born-Haber cycles for ionic compounds Dissolving: lattice breaking against hydration What the enthalpy of formation says about stability

Entropy and Feasibility of Reactions

Topic overview Entropy as the freedom of particles Comparing entropy across states and reactions Calculating entropy changes Gibbs free energy change Feasibility, temperature and spontaneous endothermic change

Equilibrium Constants

Topic overview Writing equilibrium constant expressions and deriving their units Calculating Kc and equilibrium amounts Partial pressures and Kp calculations Temperature, magnitude and the position of equilibrium

Acid-Base Equilibria

Topic overview Proton transfer and conjugate pairs Strong and weak acids: Ka and pKa Water, Kw and the pH scale pH calculations for acids and alkalis: how to use pH pH calculations for acids and alkalis: strong bases, dilution and mixtures Buffers: how they hold pH steady and why they matter Titrations: curve shapes, salt pH and choosing an indicator — pH curve shapes for strong and weak acids and bases Titrations: curve shapes, salt pH and choosing an indicator Titrations: curve shapes, salt pH and choosing an indicator — how an indicator works and choosing one Titrations: curve shapes, salt pH and choosing an indicator — using a pH probe

Stereoisomerism

Topic overview Structural isomerism and stereoisomerism compared E‒Z isomerism and the priority rules Chiral centres, enantiomers and racemic mixtures Optical activity and plane-polarised light

Aromaticity

Topic overview Benzene: shape, bonding and delocalisation Aromatic stability and resistance to addition Electrophilic substitution: nitration, halogenation and alkylation How ring and substituent affect each other

Alcohols and Phenols

Topic overview Making primary and secondary alcohols Reactions of primary and secondary alcohols Phenol: acidity and characteristic reactions Recognising a phenol

Aldehydes and Ketones

Topic overview Making aldehydes and ketones from alcohols Distinguishing aldehydes from ketones Reduction of carbonyl compounds with NaBH₄ Nucleophilic addition of hydrogen cyanide 2,4-dinitrophenylhydrazine as a test for a carbonyl group The triiodomethane test

Carboxylic Acids and Their Derivatives

Topic overview Comparing the acidity of carboxylic acids, phenols, alcohols and water Making carboxylic acids by oxidation Reduction and decarboxylation of carboxylic acids: reduction of carboxylic acids using LiAlH₄ Reduction and decarboxylation of carboxylic acids: decarboxylation of carboxylic acids Esters and acid chlorides Turning acids and halogenoalkanes into amides and nitriles Hydrolysis and reduction of nitriles and amides

Amines

Topic overview Preparing aliphatic and aromatic amines The basicity of amines Ethanoylation of primary amines Primary amines and cold nitric(III) acid Coupling reactions and azo dyes: coupling of benzenediazonium salts with phenols Coupling reactions and azo dyes: role of the —N=N— chromophore in azo dyes The origin of colour

Amino Acids, Peptides and Proteins

Topic overview Structure and classification of α-amino acids Zwitterions, amphoteric character and physical properties Peptide links: dipeptides, polypeptides and proteins Levels of protein structure and the bonds that hold them Proteins at work: enzymes and biological function

Organic Synthesis and Analysis

Topic overview Planning a synthesis as a sequence of reactions Working up a preparation: separation and purification Melting temperature as a test of purity Addition and condensation polymerisation: polyesters and polyamides Polymers: hydrolysis, properties and identifying repeat units High-resolution ¹H NMR and the elucidation of structure: low- and high-resolution proton NMR High-resolution ¹H NMR and the elucidation of structure: chemical shift, TMS, solvents and D₂O exchange High-resolution ¹H NMR and the elucidation of structure: combining mass spectra and NMR to identify compounds High-resolution ¹H NMR and the elucidation of structure: combining NMR with mass spectrometry Chromatography and the composition of mixtures

Practical Skills and Techniques

Topic overview Measuring mass, volume, time and temperature Standard solutions and titration technique Indicators and acid–base titration curves Heating, refluxing, distilling and purifying: Heating Heating, refluxing, distilling and purifying: purifying Melting temperature, chromatography and pH measurement Electrochemical cells, rate methods and working safely: Electrochemical cells Electrochemical cells, rate methods and working safely: rate methods and working safely

Planning, Analysis and Evaluation

Topic overview Planning an investigation and controlling variables Recording observations and presenting data Graphs, gradients and processing data Errors, uncertainty, accuracy and precision Evaluating a method and suggesting improvements Research and referencing

Core Experiments and Their Chemistry

Topic overview Gravimetric and acid–base analysis Enthalpy and rate experiments: Enthalpy Enthalpy and rate experiments: rate experiments Redox titrations and electrochemical cells Equilibrium constants and following a titration with a pH probe Organic synthesis, separation and identification: Organic synthesis Organic synthesis, separation and identification: identification tests and chromatography

Mathematical Skills in Chemistry

Topic overview Units, standard form and proportion in chemical calculation: volume, equilibrium, rate and energy units Units, standard form and proportion in chemical calculation: standard form Units, standard form and proportion in chemical calculation: proportion Units, standard form and proportion in chemical calculation: checking answers, buffers, rate constants and units Significant figures, means and uncertainty in experimental data: significant figures in multiplication Significant figures, means and uncertainty in experimental data: relative atomic mass as a weighted mean Significant figures, means and uncertainty in experimental data: absolute and percentage uncertainty Symbols, rearranging equations and logarithms: chemical symbols and what each one asserts Symbols, rearranging equations and logarithms: rearranging an equation Symbols, rearranging equations and logarithms: substituting into equations for Kc, enthalpy and pH Symbols, rearranging equations and logarithms: logarithms, the Arrhenius equation and rearranging formulae Graphs: plotting, gradients, intercepts and tangents — reading a spectrum Graphs: plotting, gradients, intercepts and tangents — reaction order from data and plotting good graphs Graphs: plotting, gradients, intercepts and tangents — Arrhenius plots, zero-order graphs and tangents Graphs: plotting, gradients, intercepts and tangents — initial rates from tangents and interpreting graphs Shape, symmetry and three-dimensional structure: Shape Shape, symmetry and three-dimensional structure: symmetry

Chemistry of the P-Block

13 subtopics
37 things to know
A2 Unit 3

What Chemistry of the P-Block covers

Chemistry of the P-Block is examined on A2 Unit 3 of WJEC Chemistry, Physical and Inorganic Chemistry. 168 recall questions across 13 subtopics.

Where it is assessed

A2 Unit 3

Physical and Inorganic Chemistry.

Check the WJEC specification ↗

The 13 subtopics

Each one has its own page.

What you need to know

Answer each one before you reveal it.

Your recallNot started

Numbers

Sodium hydroxide solution is added dropwise, and then in large excess, to aluminium sulfate solution. Describe what is seen at each stage.

Key term

How could you distinguish between separate solutions of aluminium nitrate and lead(II) nitrate?

Key term

Magnesium hydroxide and aluminium hydroxide are both white precipitates. State a simple test that tells them apart and explain the result.

Numbers

State the most stable oxidation state of thallium in Group 3, and contrast it with aluminium.

Key term

Explain why carbon and silicon show only the +4 state in their common compounds.

Numbers

Tin(II) chloride solution turns iron(III) solution from yellow to pale green. Write the ionic equation and explain what this shows about tin.

Key term

Carbon monoxide reduces iron(III) oxide in the blast furnace. Write the equation and give the oxidation number change for each element that changes.

Key term

Why is carbon monoxide such a useful reducing agent?

Key term

Lead(IV) oxide is warmed with concentrated hydrochloric acid. Write the equation and describe what is seen.

Key term

Sulfur hexafluoride has an expanded octet. State the number of valence electrons around sulfur, the shape and the bond angle.

Process

Why does aluminium chloride dimerise, how is each aluminium bonded in Al₂Cl₆, and how do the bridging bonds compare with the terminal ones?

Key term

Ammonia and boron trifluoride combine to form a white solid. Explain how the bond between them is formed.

Key term

Identify the donor and the acceptor in the compound NH₃.BF₃ and explain your choice.

Key term

Boron nitride has the empirical formula BN. Why are its structures so similar to those of carbon?

Key term

Why is hexagonal boron nitride a good high-temperature lubricant?

Key term

Describe the structure and bonding in carbon dioxide.

Key term

Why is carbon dioxide a gas at room temperature while silicon dioxide is a solid melting above 1600 °C?

Key term

Carbon dioxide contains polar bonds but is a non-polar molecule. Explain.

Key term

Write an equation for the reaction of silicon tetrachloride with water and describe the observations.

Process

State and explain the trend in bonding shown by the Group 4 chlorides CCl₄, SiCl₄ and PbCl₂.

Key term

A student is given three unlabelled samples, one of each of CCl₄, SiCl₄ and PbCl₂. Describe how adding water would identify each.

Key term

Both CCl₄ and SiCl₄ are liquids of similar structure. Why can the difference in their reactions with water not be explained by bond polarity alone?

Process

Why is silicon tetrachloride, with a boiling temperature of 58 °C, so much more volatile than lead(II) chloride, which melts at about 500 °C?

Key term

Explain why tetrachloromethane can be used as a solvent for non-polar substances while lead(II) chloride cannot dissolve in it.

Key term

Explain how you could use sodium hydroxide solution and potassium iodide solution together to confirm the presence of lead(II) ions in a colourless solution.

Key term

A student adds sodium hydroxide solution slowly to a lead(II) salt solution and reports no precipitate at all. Suggest what went wrong.

Key term

Both the chloride and the iodide of lead(II) are insoluble. Why does the colour of the precipitate differ so markedly?

Key term

Give the ionic equation for chlorine reacting with cold dilute alkali and show that it is a disproportionation.

Numbers

What is seen when chlorine gas is bubbled into cold dilute sodium hydroxide solution?

Key term

Balance the ionic equation for chlorine with cold alkali and confirm the charge balance.

Process

Why is a bleaching action always an oxidation when chlorine-based bleaches are used?

Evaluation

Why does bleach lose its strength if the bottle is left open or stored in a warm place?

Key term

Explain why chlorate(I) is used to bleach paper pulp rather than a coloured pigment being simply washed out.

Key term

In the reaction between sodium bromide and concentrated sulfuric acid, state the oxidation number changes and identify the oxidising and reducing agents.

Key term

Describe the observations when concentrated sulfuric acid is added to solid sodium iodide.

Key term

Write equations for the three redox reactions in which hydrogen iodide reduces concentrated sulfuric acid.

Key term

Give the shape of chlorine trifluoride and the number of electrons around the chlorine atom.

Take Chemistry of the P-Block further

The same content, four other ways.

Commonly confused

Pairs that lose marks when they are blurred together.

Hexagonal boron nitride vs Cubic boron nitride
Hexagonal boron nitride: the layered, soft, lubricating form analogous to graphite. Cubic boron nitride: the tetrahedral, extremely hard form analogous to diamond.
An amphoteric oxide vs A basic oxide
An amphoteric oxide: an oxide that reacts with both acids and bases. A basic oxide: an oxide that reacts with acids only.

Questions from this topic

Each one with the model answer underneath.

1
What does it mean to call a substance amphoteric?
Model answer
An amphoteric substance reacts with both acids and bases. It behaves as a base towards an acid and as an acid towards a base, so it dissolves in both.
2
Aluminium foil dissolves in warm dilute hydrochloric acid. Write the ionic equation and state what is seen.
Model answer
2Al(s) + 6H⁺(aq) → 2Al³⁺(aq) + 3H₂(g). The grey metal dissolves with steady effervescence of a colourless gas, leaving a colourless solution.
3
Why does aluminium also dissolve in hot aqueous sodium hydroxide, and what is the aluminium-containing product?
Model answer
Aluminium is amphoteric, so it is attacked by strong alkali as well as by acid: 2Al(s) + 2OH⁻(aq) + 6H₂O(l) → 2[Al(OH)₄]⁻(aq) + 3H₂(g). The product is the colourless tetrahydroxoaluminate(III) ion, and hydrogen is given off.
4
Sodium hydroxide solution is added dropwise, and then in large excess, to aluminium sulfate solution. Describe what is seen at each stage.
Model answer
A white gelatinous precipitate of aluminium hydroxide forms first: Al³⁺(aq) + 3OH⁻(aq) → Al(OH)₃(s). In excess alkali the precipitate redissolves to give a colourless solution: Al(OH)₃(s) + OH⁻(aq) → [Al(OH)₄]⁻(aq).
5
Write the equation for aluminium hydroxide dissolving in dilute nitric acid.
Model answer
Al(OH)₃(s) + 3H⁺(aq) → Al³⁺(aq) + 3H₂O(l). The white precipitate dissolves to give a colourless solution.
6
Explain why aluminium hydroxide is described as amphoteric.
Model answer
It dissolves in acid by accepting protons to give Al³⁺(aq), acting as a base, and it dissolves in alkali by accepting a hydroxide ion to give [Al(OH)₄]⁻, acting as an acid. Because it reacts in both ways it is amphoteric.

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Chemistry of the P-Block revision questions

What does Chemistry of the P-Block cover in WJEC A-Level Chemistry?: 13 subtopics: amphoteric behaviour of aluminium and lead, stability of oxidation states down groups 3, 4 and 5: increasing stability of the inert pair cations, stability of oxidation states down groups 3, 4 and 5: change in relative stability, valence shells that break the octet rule: how some group 3 elements can form compounds, valence shells that break the octet rule: structure and bonding in al2cl6 and formation, boron nitride: two structures, two sets of properties, group 4 oxides and chlorides, and lead in solution: structure, group 4 oxides and chlorides, and lead in solution: hydrolysis of the group 4 chlorides, group 4 oxides and chlorides, and lead in solution: chloride hydrolysis and lead(ii) precipitates, group 4 oxides and chlorides, and lead in solution: distinguishing lead from silver ions, chlorine, chlorate and the sodium halides: chlorine with water and with cold and hot alkali, chlorine, chlorate and the sodium halides: bleaching and bactericidal action of cl2 and chlorine, chlorate and the sodium halides: differences in behaviour of nacl. Each one has its own page with questions and model answers.
How is Chemistry of the P-Block organised?: By the WJEC 1410QS specification, subtopic by subtopic, so it matches the order you are taught it in.

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