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100+ Free Higher Chemistry Practice Questions

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Which type of reaction joins amino acids together to form a peptide?

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2026 Statistics

Key Facts: Higher Chemistry Exam

A-D

Grading scale

Qualifications Scotland

100 + 20

Marks (paper + assignment)

SQA course specification

2h 30

Question paper duration

Qualifications Scotland

100

Free practice questions here

OpenExamPrep

Qualifications Scotland Higher Chemistry (course code C813 76) is graded A-D and assessed by a 2h30 question paper (100 marks: Section 1 multiple-choice + Section 2 extended-response) plus a 20-mark assignment. The 2026 specification covers rates, periodicity, bonding, organic chemistry, equilibria, redox and chemical analysis.

Sample Higher Chemistry Practice Questions

Try these sample questions to test your Higher Chemistry exam readiness. Each question includes a detailed explanation. Start the interactive quiz above for the full 100+ question experience with AI tutoring.

1According to collision theory, why does increasing temperature increase the rate of most chemical reactions?
A.More molecules have kinetic energy greater than or equal to the activation energy
B.The activation energy of the reaction decreases at higher temperature
C.The concentration of reactants increases with temperature
D.The frequency of collisions decreases but each collision releases more energy
Explanation: Raising temperature shifts the Maxwell-Boltzmann distribution so a larger fraction of molecules has kinetic energy at or above the activation energy (Ea). This greatly increases the proportion of successful collisions, which is the dominant effect on rate.
2On a Maxwell-Boltzmann energy distribution curve, what does the area under the curve to the right of the activation energy represent?
A.The number of molecules with energy greater than or equal to Ea
B.The total number of collisions per second
C.The activation energy of the reverse reaction
D.The enthalpy change of the reaction
Explanation: The Maxwell-Boltzmann distribution plots the number of molecules against kinetic energy. The area to the right of Ea represents the molecules that have at least the activation energy and are therefore capable of reacting on collision.
3How does a catalyst increase the rate of a chemical reaction?
A.It provides an alternative reaction pathway with a lower activation energy
B.It raises the average kinetic energy of the reactant molecules
C.It shifts the equilibrium position towards products
D.It increases the enthalpy change of the reaction
Explanation: A catalyst lowers the activation energy by offering an alternative route, so a larger proportion of molecules has enough energy to react at a given temperature. The catalyst is unchanged at the end and does not affect ΔH or the equilibrium position.
4Which statement best describes a heterogeneous catalyst?
A.It is in a different physical state from the reactants
B.It is in the same physical state as the reactants
C.It is always a transition metal in solution
D.It is consumed during the reaction and must be replaced
Explanation: A heterogeneous catalyst is in a different state from the reactants, typically a solid catalysing a gas or liquid-phase reaction (e.g. Fe in the Haber process). Reactants adsorb onto the surface, react, and products desorb.
5Enzymes are described as biological catalysts. Which feature explains why most enzymes are very specific?
A.Their active site has a complementary shape to one substrate
B.They lower the activation energy by a much greater amount than other catalysts
C.They contain transition metals at their active site
D.They are denatured by gentle heating
Explanation: An enzyme's active site has a specific three-dimensional shape complementary to its substrate. Only molecules that fit can bind, react, and leave as products, giving enzymes their high specificity.
6Why does the covalent radius generally decrease from left to right across a period of the periodic table?
A.Nuclear charge increases while electrons are added to the same shell
B.A new electron shell is added with each element
C.Shielding from inner electrons increases sharply
D.The number of neutrons decreases across the period
Explanation: Across a period the number of protons (nuclear charge) increases, but each added electron enters the same outer shell. Shielding from inner electrons stays roughly the same, so the effective nuclear charge pulls the outer electrons in more strongly and the atom contracts.
7Why does the first ionisation energy generally decrease down a group?
A.The outer electron is further from the nucleus and more shielded by inner electrons
B.Nuclear charge decreases down the group
C.The atoms have fewer protons further down the group
D.Electrons are removed from inner shells instead of outer shells
Explanation: Going down a group, the outermost electron is in a higher energy shell, so it is further from the nucleus and shielded by more inner electrons. Both effects weaken the nuclear attraction, so less energy is needed to remove it.
8The first four ionisation energies of an element are 738, 1451, 7733 and 10540 kJ/mol. To which group of the periodic table does the element most likely belong?
A.Group 2
B.Group 1
C.Group 3
D.Group 4
Explanation: There is a very large jump between the 2nd and 3rd ionisation energies (1451 to 7733). This shows that two electrons are easily removed before reaching a stable noble-gas core, so the element has 2 outer electrons and is in Group 2.
9On the Pauling electronegativity scale, which element is the most electronegative?
A.Fluorine
B.Oxygen
C.Chlorine
D.Nitrogen
Explanation: Fluorine has the highest Pauling electronegativity (4.0) because it is small, has a high nuclear charge, and an outer electron shell close to the nucleus. Electronegativity decreases down a group and (broadly) decreases from F across the period.
10A bond between two atoms with an electronegativity difference of 0.4 is best described as:
A.A polar covalent bond
B.A pure covalent bond
C.An ionic bond
D.A metallic bond
Explanation: An electronegativity difference around 0.4 indicates the bonded atoms share electrons unequally, giving a polar covalent bond. Differences close to 0 give pure covalent bonds; differences above about 1.7-2.0 produce essentially ionic bonds.

About the Higher Chemistry Exam

Higher Chemistry is a Scottish Credit and Qualifications Framework (SCQF) Level 6 course delivered by Qualifications Scotland (formerly SQA). It covers three areas — Chemical Changes and Structure, Nature's Chemistry, and Chemistry in Society — assessed through a 100-mark question paper and a 20-mark assignment.

Questions

100 scored questions

Time Limit

Question paper 2 hours 30 minutes; Assignment 1 hour 30 minutes

Passing Score

Grade C is the minimum pass (A, B, C); D awarded for near-pass

Exam Fee

Entry fees set by school/centre (typically around £12-£15 per subject) (Qualifications Scotland (formerly SQA))

Higher Chemistry Exam Content Outline

~11%

Controlling Rates of Reaction

Collision theory, activation energy, Maxwell-Boltzmann distribution, catalysts (heterogeneous/homogeneous/enzymes), rate-temperature and concentration relationships

~11%

Periodicity

Group and period trends in covalent radius, ionisation energy, electronegativity (Pauling scale); explaining trends in terms of nuclear charge, shielding and distance

~11%

Structure and Bonding

Bonding continuum (pure covalent to ionic), polar and non-polar molecules, London dispersion forces, permanent dipole-dipole, hydrogen bonding, viscosity, properties of water

~11%

Esters, Fats and Oils, Proteins

Esterification with concentrated sulfuric acid, hydrolysis, saturated vs unsaturated fats, iodine number, hydrogenation; amino acids, peptide bonds, primary structure, enzyme denaturation

~11%

Oxidation of Food and Soaps

Oxidation of primary/secondary/tertiary alcohols by acidified K2Cr2O7, Tollens' and Fehling's tests, antioxidants and free radicals; soap structure, hard water, emulsions, terpenes and skin care

~11%

Getting the Most from Reactants

Industrial process considerations (cost, energy, recyclability), atom economy, percentage yield, limiting reactant calculations, mole calculations from balanced equations

~11%

Equilibria and Chemical Energy

Le Chatelier's principle, equilibrium constant Kc, Haber and Contact processes; enthalpy of combustion, calorimetry (q = cmΔT), mean bond enthalpies, Hess's law calculations

~11%

Oxidising/Reducing Agents and Chemical Analysis

OIL RIG, electrochemical series, balanced ion-electron equations with H+ and H2O, EMF; volumetric titration calculations, paper and thin-layer chromatography (Rf), transition metals

How to Pass the Higher Chemistry Exam

What You Need to Know

  • Passing score: Grade C is the minimum pass (A, B, C); D awarded for near-pass
  • Exam length: 100 questions
  • Time limit: Question paper 2 hours 30 minutes; Assignment 1 hour 30 minutes
  • Exam fee: Entry fees set by school/centre (typically around £12-£15 per subject)

Keys to Passing

  • Complete 500+ practice questions
  • Score 80%+ consistently before scheduling
  • Focus on highest-weighted sections
  • Use our AI tutor for tough concepts

Higher Chemistry Study Tips from Top Performers

1Drill mole, concentration, percentage yield and atom economy calculations until the steps are automatic — they appear every year
2Memorise the colour changes for K2Cr2O7 (orange to green), Tollens' (silver mirror) and Fehling's (brick-red) — they recur in oxidation of alcohols questions
3Use past papers from the Qualifications Scotland archive and mark with official marking instructions to learn exam phrasing
4Build one-page summaries for each unit: bonding/IMFs, organic functional groups, redox/equilibria — Higher Chemistry rewards spaced revision

Frequently Asked Questions

What awarding body runs Higher Chemistry?

Higher Chemistry is delivered by Qualifications Scotland (formerly SQA). The course code is C813 76 and it sits at SCQF Level 6 within the Scottish qualifications framework.

How is Higher Chemistry assessed?

Assessment is a 100-mark question paper (Section 1 multiple-choice and Section 2 extended-response) lasting 2 hours 30 minutes, plus a 20-mark assignment researched by the candidate and written up under supervised conditions.

What grades are awarded for Higher Chemistry?

Grades A, B, C and D are awarded, with C as the minimum pass and D as a near-pass. The grade is calculated from the combined question paper and assignment mark out of 120.

When are Higher Chemistry exams sat?

The question paper is normally sat in the May diet of the SQA exam timetable, most often in S5. The assignment is completed earlier in the school year and submitted to Qualifications Scotland for external marking.