PracticeVideosBlogFlashcardsEspañol
All Practice Exams

Free Practice Questions for Érettségi Chemistry

Exam-style questions and explanations by OpenExamPrep.

✓ No registration✓ No credit card
100+ Questions
100% Free

Loading practice questions...

Same family resources

Explore More Hungary Érettségi Secondary School Leaving Examinations (Oktatási Hivatal)

Continue into nearby exams from the same family. Each card keeps practice questions, study guides, flashcards, videos, and articles in one place.

Hungary Érettségi — Biology

Practice Questions

Hungary Érettségi — English Language

Practice Questions

Hungary Érettségi — Film Culture and Media Studies

Practice Questions

Hungary Érettségi — Geography

Practice Questions

Hungary Érettségi — History

Practice Questions

Hungary Érettségi — Hungarian Language and Literature

Practice Questions
Exam Review

Key Facts: Érettségi Chemistry Exam

Codified under Hungarian Government Decree 100/1997. (VI. 13.) Korm. rendelet 3. melléklet 1.2.16 and NAT 2020.

Administered nationwide by the Oktatási Hivatal (Educational Authority) during the May–June and October–November exam sessions.

Középszint written exam duration: 150 minutes (100 points); oral exam: 15 minutes (50 points).

Emelt szint written exam duration: 240 minutes (100 points); oral exam: 20 minutes with practical lab evaluation (50 points).

Passing threshold is 25% overall, with a strict sub-minimum of 12% required in both the written and oral sections.

Grading differs by level: grade 5 begins at 80% for középszint and 60% for emelt szint; both require 25% overall and at least 12% in each required part.

Chemistry can be relevant to medical, pharmaceutical, and engineering programmes, whose current admission requirements must be checked individually.

Permitted aids in the written examination include non-programmable scientific calculators and the officially supplied periodic table.

The Hungarian Érettségi Chemistry examination is a current school-leaving subject offered at középszint and emelt szint. It combines theory, observations, equations, experiments, and quantitative calculations in a 150- or 240-minute written paper followed by an oral component.

Sample Érettségi Chemistry Practice Questions

Try these sample questions to review concepts for the Érettségi Chemistry exam. Each question includes a detailed explanation. Start the interactive quiz above for the full 100+ question experience with AI tutoring.

1A neutral chromium atom contains 24 electrons. Which configuration represents its observed ground state?
A.[Ar] 3d⁴ 4s²
B.[Ar] 3d⁵ 4s¹
C.[Ar] 3d⁶ 4s⁰
D.[Ar] 3d³ 4s² 4p¹
Explanation: Chromium has the ground-state configuration [Ar] 3d⁵ 4s¹ rather than the simple Aufbau prediction [Ar] 3d⁴ 4s². The actual ordering reflects the close energies of the 3d and 4s orbitals together with electron-electron and exchange interactions that favour the observed half-filled 3d subshell.
2What is the maximum number of electrons that can occupy the 4d subshell of an atom?
A.6
B.10
C.14
D.18
Explanation: For any d subshell, the azimuthal (angular momentum) quantum number is l = 2. The magnetic quantum number m_l can take 2l + 1 values: -2, -1, 0, +1, +2, meaning there are 5 individual d orbitals. By the Pauli exclusion principle, each orbital holds a maximum of 2 electrons with opposite spins (m_s = +1/2, -1/2). Therefore, the subshell accommodates at most 5 × 2 = 10 electrons.
3Why is the first ionization energy of nitrogen (Z = 7, 1402 kJ/mol) higher than that of oxygen (Z = 8, 1314 kJ/mol), despite oxygen having a higher nuclear charge?
A.Oxygen has a larger atomic radius than nitrogen, making its valence electrons easier to remove.
B.Nitrogen has a stable half-filled 2p³ subshell, whereas removing an electron from oxygen's 2p⁴ subshell relieves inter-electronic repulsion in the doubly occupied orbital.
C.Oxygen has greater core electron shielding than nitrogen, reducing effective nuclear charge.
D.The valence electron of nitrogen is removed from the 2s subshell rather than the 2p subshell.
Explanation: Nitrogen has the valence configuration 2s² 2p³, where each of the three 2p orbitals is singly occupied with parallel spins (Hund's rule), conferring high exchange stability. Oxygen has the configuration 2s² 2p⁴, in which one 2p orbital contains a paired pair of electrons. The electrostatic repulsion between the two electrons sharing that orbital raises their energy, lowering the energy needed to remove one electron compared to nitrogen.
4The ions O²⁻, F⁻, Na⁺, and Mg²⁺ each have ten electrons. Which option orders them from largest to smallest ionic radius?
A.Mg²⁺ > Na⁺ > F⁻ > O²⁻
B.O²⁻ > F⁻ > Na⁺ > Mg²⁺
C.Na⁺ > Mg²⁺ > O²⁻ > F⁻
D.F⁻ > O²⁻ > Mg²⁺ > Na⁺
Explanation: All four species (O²⁻, F⁻, Na⁺, Mg²⁺) are isoelectronic with neon (10 electrons: 1s² 2s² 2p⁶). In an isoelectronic series, ionic radius decreases as the atomic number (nuclear charge Z) increases. O²⁻ has Z = 8, F⁻ has Z = 9, Na⁺ has Z = 11, and Mg²⁺ has Z = 12. Mg²⁺ exerts the greatest electrostatic attraction on the 10 electrons, pulling them closest to the nucleus, while O²⁻ has the lowest nuclear charge, resulting in the largest radius: O²⁻ > F⁻ > Na⁺ > Mg²⁺.
5Why does carbon dioxide (CO₂) have a zero dipole moment (non-polar) while sulfur dioxide (SO₂) has a permanent dipole moment (polar), given that both contain polar bonds?
A.The electronegativity difference between C and O is zero, whereas S and O differ in electronegativity.
B.CO₂ is a linear molecule (180°) whose bond dipole vectors cancel, whereas SO₂ has a bent molecular geometry due to a lone pair on the sulfur atom.
C.CO₂ forms giant covalent networks, whereas SO₂ forms discrete molecules.
D.Carbon forms single bonds with oxygen, while sulfur forms double bonds.
Explanation: In CO₂, the central carbon has two bonding regions and zero lone pairs, giving a linear geometry (O=C=O, 180°). The two equal C=O bond dipole vectors point in exactly opposite directions and cancel vectorially, resulting in a net dipole moment μ = 0. In SO₂, sulfur has two bonding regions and one lone pair (AX₂E), producing a bent geometry (bond angle ~119°). The S=O bond dipoles do not cancel, giving a permanent molecular dipole moment.
6According to VSEPR theory, what is the molecular geometry and approximate bond angle of the ammonia (NH₃) molecule?
A.Trigonal planar, 120°
B.Tetrahedral, 109.5°
C.Trigonal pyramidal, ~107°
D.T-shaped, ~90°
Explanation: In NH₃, the central nitrogen atom is surrounded by four electron pairs (three N-H single bonding pairs and one non-bonding lone pair), defining an AX₃E steric system with tetrahedral electron geometry. Because lone pair-bonding pair repulsions are stronger than bonding pair-bonding pair repulsions, the lone pair compresses the H-N-H bond angles from the ideal tetrahedral angle of 109.5° down to approximately 107.3°, giving a trigonal pyramidal molecular shape.
7In ethyne, HC≡CH, each carbon forms two sigma-bond directions and participates in two pi bonds. What is the hybridization of each carbon?
A.sp³
B.sp²
C.sp
D.dsp²
Explanation: In ethyne (H-C≡C-H), each carbon atom forms one single σ-bond to hydrogen and one σ-bond to the other carbon atom, comprising two σ-bonding domains and zero lone pairs. This linear arrangement (180° bond angle) requires sp hybridization. The two unhybridized 2p orbitals on each carbon atom overlap laterally at 90° angles to form the two mutually perpendicular π-bonds of the triple bond.
8Ethanol (CH₃CH₂OH) has a boiling point of +78 °C, whereas its constitutional isomer dimethyl ether (CH₃OCH₃) boils at -24 °C. What accounts for this large difference?
A.Ethanol has a much higher molar mass than dimethyl ether.
B.Ethanol molecules form strong intermolecular hydrogen bonds via their -OH groups, whereas dimethyl ether molecules only interact through weaker dipole-dipole and dispersion forces.
C.Dimethyl ether possesses a higher dipole moment than ethanol, causing destructive interference.
D.Ethanol forms a giant covalent lattice in the liquid state.
Explanation: Ethanol and dimethyl ether are constitutional isomers sharing the identical molecular formula C₂H₆O (M = 46.07 g/mol). Ethanol contains a highly polarized O-H bond, allowing its molecules to form extensive intermolecular hydrogen bonds. Dimethyl ether lacks hydrogen atoms bonded directly to electronegative atoms (all hydrogens are bonded to carbon); its molecules interact only via weaker dipole-dipole interactions and London dispersion forces, requiring far less thermal energy to vaporize.
9Magnesium oxide (MgO) has a melting point of 2852 °C, while sodium chloride (NaCl) melts at 801 °C. Which factor primarily explains this difference in lattice energy?
A.Magnesium has a higher electronegativity than sodium.
B.The ionic charges in MgO are +2 and -2, whereas in NaCl they are +1 and -1, quadrupling the electrostatic attraction according to Coulomb's law.
C.MgO forms a covalent network lattice, whereas NaCl forms an ionic crystal.
D.The sodium cation is smaller than the magnesium cation.
Explanation: Lattice energy (U) is directly proportional to the product of ionic charges (|z₊ × z₋|) and inversely proportional to the sum of ionic radii (r₊ + r₋) according to the Born-Landé equation. In MgO, the charge product is |(+2) × (-2)| = 4, compared to |(+1) × (-1)| = 1 in NaCl. Furthermore, Mg²⁺ (72 pm) is smaller than Na⁺ (102 pm) and O²⁻ (140 pm) is smaller than Cl⁻ (181 pm), resulting in a shorter internuclear distance. The 4-fold higher charge product and smaller interionic distance yield a lattice energy for MgO (~3791 kJ/mol) nearly five times greater than that of NaCl (~787 kJ/mol).
10Which macroscopic property of metals is directly explained by the presence of a 'sea' of delocalized valence electrons?
A.Brittleness under mechanical stress
B.High electrical and thermal conductivity
C.Low boiling points compared to non-metals
D.Inability to conduct electricity in the liquid state
Explanation: In metallic bonding, positive metal cations occupy fixed lattice positions surrounded by delocalized valence electrons that are free to move throughout the entire crystal. When an electric potential difference is applied, these mobile electrons drift toward the positive terminal, resulting in high electrical conductivity. Similarly, kinetic energy is rapidly transferred via electron collisions, yielding high thermal conductivity. The non-directional nature of the bonding also allows atomic layers to slide without shattering (malleability and ductility).

About the Érettségi Chemistry Exam

Kémia is a current elective Hungarian Érettségi subject at középszint and emelt szint. The requirements span general, inorganic, organic, environmental, and everyday chemistry, with equations, experiments, observations, data, and quantitative calculations. Középszint is a 150-minute written paper followed by a 15-minute oral; emelt szint is a 240-minute written paper followed by a 20-minute oral. The oral includes theoretical and experimental or practical work. These 100 English MCQs are independent concept and calculation review, not an official format simulation and not a substitute for laboratory, constructed-response, or oral preparation.

Exam sponsor: Oktatási Hivatal (Educational Authority, Hungary). The requirements and fees below concern the certification or admission exam, separate from our free practice resources.

Assessment

Question count not published by the exam provider

Time Limit

150 minutes written + 15-minute oral (középszint); 240 minutes written + 20-minute oral (emelt szint)

Passing Score

At least 25% overall and at least 12% in both the written and oral parts. Középszint grades: 25–39% = 2, 40–59% = 3, 60–79% = 4, 80–100% = 5. Emelt szint grades: 25–32% = 2, 33–46% = 3, 47–59% = 4, 60–100% = 5.

Exam / Certification Fees

Free for qualifying students taking examinations toward their first school-leaving certificate, including the first remedial or replacement examination before receiving it. For fee-paying 2026 entries, the per-subject fee is HUF 48,000 at középszint and HUF 81,000 at emelt szint.

Exam sponsor website

Fees, eligibility, and exam policies can change. Confirm them with the exam sponsor before applying or paying.

Our practice resources: topics covered

We aim to reflect publicly available exam outlines and topic information in our study resources. Coverage, format, and difficulty may differ from the actual exam, and we cannot guarantee that every detail is accurate or current. Confirm exam requirements, fees, and policies with the official exam sponsor.

15%

General Chemistry & Chemical Bonding

Atomic orbitals, electron configuration principles (Aufbau, Pauli, Hund), periodic trends in ionization energy and electronegativity, ionic lattices, covalent bonding types (sigma, pi), VSEPR molecular geometry, and intermolecular interactions.

12%

Reaction Kinetics & Equilibrium

Reaction rates, collision theory, catalyst modes of action, reversible equilibria, equilibrium constant expressions (Kc, Kp), Le Chatelier's principle under pressure, temperature, and concentration shifts.

16%

Acid-Base & Redox Chemistry

Brønsted-Lowry acid-base theory, pH/pOH calculations for strong and weak electrolytes, Ka and Kb relationships, buffer action, oxidation numbers, balancing redox reactions, galvanic cell EMF, and molten/aqueous electrolysis.

17%

Stoichiometry & Solution Chemistry

Calculations with amount of substance (mole), molar volume of gases, mass percent (m/m%), molarity (mol/dm³), solubility curves, precipitation reactions, gas law stoichiometric problems, and multi-component reaction mixture analysis.

15%

Inorganic Chemistry of Non-Metals & Metals

Physical and chemical properties of s-block, p-block, and d-block elements; synthesis and reactions of halogens, chalcogens, nitrogen group, and carbon group compounds; metallic reactivity, corrosion, passivity, and complex formation.

15%

Organic Chemistry & Functional Groups

Nomenclature and isomerism (constitutional, stereoisomers); reaction mechanisms of alkanes, alkenes, alkynes, and aromatics; nucleophilic substitutions; chemistry of alcohols, aldehydes, ketones, carboxylic acids, esters, and addition/condensation polymers.

10%

Biochemistry & Environmental Chemistry

Structure and reactions of carbohydrates (mono-, di-, polysaccharides), amino acids, zwitterions, peptide linkages, primary-quaternary protein structure, lipids, nucleic acids, atmospheric chemistry, greenhouse effect, and water treatment.

Preparing for the Érettségi Chemistry Exam

What You Need to Know

  • Passing score: At least 25% overall and at least 12% in both the written and oral parts. Középszint grades: 25–39% = 2, 40–59% = 3, 60–79% = 4, 80–100% = 5. Emelt szint grades: 25–32% = 2, 33–46% = 3, 47–59% = 4, 60–100% = 5.
  • Assessment: Question count not published by the exam provider
  • Time limit: 150 minutes written + 15-minute oral (középszint); 240 minutes written + 20-minute oral (emelt szint)
  • Exam / certification fees: Free for qualifying students taking examinations toward their first school-leaving certificate, including the first remedial or replacement examination before receiving it. For fee-paying 2026 entries, the per-subject fee is HUF 48,000 at középszint and HUF 81,000 at emelt szint. Official sources

Using Our Practice Resources

  • Work through all 100 available questions
  • Review every answer and explanation
  • Track weak areas and revisit them
  • Use our AI tutor for tough concepts

Érettségi Chemistry: Suggested Study Strategy

1Master the 'tabellás' (equilibrium table / stoichiometric table) method for solving ICE (Initial, Change, Equilibrium) problems, which are central to multi-step quantitative tasks on Hungarian papers.
2Thoroughly memorize periodic trends, oxidation state rules, and solubility rules for common salts and hydroxides in aqueous media.
3Practice full written balancing of complex redox reactions in acidic and basic solutions using the ion-electron (half-reaction) or oxidation number change methods.
4Work extensively with past papers downloadable freely from oktatas.hu going back to 2005; pay careful attention to the official marking guides (javítási-értékelési útmutató).
5Focus intensely on organic reaction types: Markovnikov addition to alkenes, electrophilic aromatic substitution on benzene and toluene, nucleophilic addition to carbonyls, and esterification equilibria.
6Learn laboratory test reactions and diagnostic visual indicators: silver mirror (Tollens) test, Fehling's test, biuret test, xanthoproteic reaction, flame tests of alkali/alkaline earth cations, and halogen displacement reactions.
7Manage your time strictly: on the written exam, allocate adequate time (at least 90–120 minutes on emelt) to the extended calculation problems, which carry significant points and require zero arithmetic errors.

Frequently Asked Questions

What is the legal framework governing the Hungarian Chemistry Érettségi?

The examination is codified under 100/1997. (VI. 13.) Korm. rendelet 3. melléklet 1.2.16 and adheres to the National Core Curriculum (Nemzeti Alaptanterv — NAT 2020) and the corresponding Kerettanterv (Framework Curriculum) issued by the Hungarian Ministry of Education.

Why is the emelt szint (advanced level) chemistry exam so important in Hungary?

Chemistry is commonly relevant to medicine, pharmacy, chemical engineering, and related programmes, but each institution and programme sets its current subject and scoring requirements. Candidates should verify the current Felvi programme entry rather than assuming a universal requirement or point award.

What is the difference in structure between középszint and emelt szint chemistry?

Középszint consists of a 150-minute written examination (100 points) plus a 15-minute oral (50 points). Emelt szint has a 240-minute written paper (100 points) and a 20-minute oral (50 points). Both levels assess theory, observations, equations, and calculations; the oral requirements include experimental or practical work.

What are the passing criteria and grading boundaries for Chemistry Érettségi?

Candidates need at least 25% overall and at least 12% in both the written and oral parts. Középszint grades are 25–39% = 2, 40–59% = 3, 60–79% = 4, and 80–100% = 5. Emelt szint grades are 25–32% = 2, 33–46% = 3, 47–59% = 4, and 60–100% = 5.

Are calculators and periodic tables allowed during the examination?

Yes. Non-programmable scientific calculators that cannot store text or transmit data are permitted. An official periodic table (Periódusos rendszer) with standard relative atomic masses is supplied as part of the official examination booklet.

What mathematical and problem-solving skills are tested in the calculation section?

Stoichiometry is a defining feature of the Hungarian exam. Candidates must solve multi-component gas mixtures, titration back-calculations, solubility and crystallisation changes upon cooling/evaporation, electrochemical Faradaic yields, equilibrium conversions (equilibrium tables with quadratic equations), and organic combustion analyses.

How are these practice questions related to the official exam?

This is an independent English-language, four-option study bank covering relevant Chemistry concepts and calculations. It is not an official translation, blueprint replica, or format simulation and does not substitute for experimental, constructed-response, or oral preparation.