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Key Facts: European Baccalaureate Chemistry Exam

180 Minutes

Exam duration

OSGES Syllabus

6.0 / 10

Passing mark (60%)

European Schools Board of Governors

7 Domains

Core curriculum topics

OSGES S6-S7 4P Chemistry Syllabus

100 Questions

Practice question bank size

OpenExamPrep

The European Baccalaureate Chemistry is administered by the Office of the Secretary-General of the European Schools (OSGES). Official assessment involves written/oral components graded on a 0-10 scale (passing score 5.0). Local questions on OpenExamPrep are an English-language MCQ study adaptation designed for syllabus revision.

Sample European Baccalaureate Chemistry Practice Questions

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

1Which set of quantum numbers (n, l, m_l, m_s) is valid for an electron occupying a 3d atomic orbital?

A.n = 3, l = 2, m_l = -1, m_s = +1/2

B.n = 3, l = 1, m_l = +2, m_s = -1/2

C.n = 3, l = 3, m_l = 0, m_s = +1/2

D.n = 2, l = 2, m_l = -2, m_s = -1/2

Explanation: For a 3d orbital, the principal quantum number n = 3 and the angular momentum quantum number l = 2 (where l = 0, 1, 2, 3 correspond to s, p, d, f orbitals). The magnetic quantum number m_l can take integer values from -l to +l, so for l = 2, m_l ∈ {-2, -1, 0, +1, +2}, and the spin quantum number m_s is ±1/2. Therefore, n = 3, l = 2, m_l = -1, m_s = +1/2 is completely valid.

2What is the ground-state electron configuration of a neutral chromium atom (Z = 24)?

A.[Ar] 4s² 3d⁴

B.[Ar] 4s¹ 3d⁵

C.[Ar] 4s⁰ 3d⁶

D.[Ar] 4s² 3d⁵

Explanation: Chromium is a classic exception to the standard Aufbau filling rule. Moving one electron from the 4s orbital to the 3d subshell yields a half-filled [Ar] 4s¹ 3d⁵ configuration, which maximizes exchange energy and minimizes electron-electron repulsion.

3Which of the following Period 3 elements possesses the highest first ionization energy?

A.Sodium (Na)

B.Magnesium (Mg)

C.Argon (Ar)

D.Silicon (Si)

Explanation: First ionization energy generally increases across a period from left to right due to increasing effective nuclear charge (Z_eff) with constant core shielding. Argon (Ar) is at the extreme right of Period 3 with a complete octet (3s² 3p⁶), giving it the highest first ionization energy in Period 3.

4According to VSEPR theory, what is the molecular geometry of sulfur tetrafluoride (SF4)?

A.Tetrahedral

B.Square planar

C.Trigonal bipyramidal

D.See-saw

Explanation: Sulfur in SF4 has 6 valence electrons, forming 4 single bonds with fluorine atoms and retaining 1 lone pair (5 electron domains total). The steric number of 5 produces a trigonal bipyramidal electron domain geometry, but the lone pair occupies an equatorial position to minimize 90° repulsions, yielding a see-saw molecular geometry.

5What is the hybridization state of each carbon atom in ethyne (ethyne / acetylene, HC≡CH)?

A.sp

B.sp²

C.sp³

D.sp³d

Explanation: In ethyne (HC≡CH), each carbon forms one σ bond with a hydrogen atom and one σ bond with the neighboring carbon atom (along with two π bonds). Having 2 σ-bonding electron domains requires sp hybridization, producing a linear geometry with a 180° bond angle.

6Given the standard enthalpy of sublimation of Na(s) is +107 kJ/mol, the first ionization energy of Na(g) is +496 kJ/mol, the bond dissociation enthalpy of Cl2(g) is +244 kJ/mol, the electron affinity of Cl(g) is -349 kJ/mol, and the standard enthalpy of formation of NaCl(s) is -411 kJ/mol, what is the lattice enthalpy (ΔH_lattice) of NaCl(s) for the reaction Na+(g) + Cl-(g) → NaCl(s)?

A.-787 kJ/mol

B.-788 kJ/mol

C.-641 kJ/mol

D.-909 kJ/mol

Explanation: According to Hess's Law for a Born-Haber cycle: ΔH_f°[NaCl(s)] = ΔH_sub[Na] + IE1[Na] + 1/2 ΔH_diss[Cl2] + EA1[Cl] + ΔH_lattice. Substituting the values: -411 = +107 + 496 + 1/2(244) + (-349) + ΔH_lattice ⇒ -411 = +107 + 496 + 122 - 349 + ΔH_lattice ⇒ -411 = +376 + ΔH_lattice ⇒ ΔH_lattice = -411 - 376 = -787 kJ/mol (or -788 kJ/mol depending on rounding). Thus -788 kJ/mol is the correct value.

7Ethanol (CH3CH2OH) and dimethyl ether (CH3OCH3) are constitutional isomers with the molecular formula C2H6O. Why is the boiling point of ethanol (78.4 °C) significantly higher than that of dimethyl ether (-24 °C)?

A.Ethanol is a non-polar molecule with strong London dispersion forces.

B.Dimethyl ether forms stronger hydrogen bonds than ethanol.

C.Ethanol can form intermolecular hydrogen bonds due to its O-H group, whereas dimethyl ether cannot.

D.Ethanol has a much larger molar mass than dimethyl ether.

Explanation: Ethanol contains a hydrogen atom directly bonded to an electronegative oxygen atom (O-H group), allowing it to form extensive intermolecular hydrogen networks. Dimethyl ether lacks an O-H bond (it has C-O-C), so its primary intermolecular interactions are weaker dipole-dipole forces and London dispersion forces.

8What are the formal charges on the central oxygen atom and one of the terminal oxygen atoms in the resonance structure of ozone (O3) represented as O=O⁺-O⁻?

A.Central = 0, Double-bonded terminal = +1

B.Central = -1, Single-bonded terminal = +1

C.Central = +1, Double-bonded terminal = -1

D.Central = +1, Single-bonded terminal = -1

Explanation: Formal charge = (Valence e⁻) - (Non-bonding e⁻) - 1/2(Bonding e⁻). Oxygen has 6 valence electrons. For the central oxygen: 6 - 2 (1 lone pair) - 1/2(6 bonding e⁻ in 3 bonds) = +1. For the single-bonded terminal oxygen: 6 - 6 (3 lone pairs) - 1/2(2 bonding e⁻) = -1. For the double-bonded terminal oxygen: 6 - 4 - 2 = 0.

9According to Molecular Orbital (MO) theory, why is diatomic oxygen (O2) paramagnetic?

A.O2 contains two unpaired electrons in two degenerate π*2p antibonding orbitals.

B.O2 contains one unpaired electron in a σ2p bonding orbital.

C.O2 has a lone pair of electrons localized on each oxygen atom.

D.O2 rapidly dissociates into oxygen radicals in the gas phase.

Explanation: In the MO energy diagram for O2, the 12 valence electrons fill orbitals up to the antibonding level: (σ2s)² (σ*2s)² (σ2p)² (π2p)⁴ (π*2p)². By Hund's rule, the two electrons in the degenerate π*2px and π*2py antibonding orbitals remain unpaired with parallel spins, causing paramagnetism.

10Which sequence correctly arranges CH4, NH3, and H2O in order of DECREASING bond angle (largest to smallest)?

A.H2O > NH3 > CH4

B.CH4 > NH3 > H2O

C.NH3 > CH4 > H2O

D.CH4 > H2O > NH3

Explanation: All three molecules have 4 electron domains (tetrahedral domain geometry). CH4 has 0 lone pairs (109.5°), NH3 has 1 lone pair (107°), and H2O has 2 lone pairs (104.5°). Lone-pair–bonding-pair repulsion is stronger than bonding-pair–bonding-pair repulsion, compressing the bond angles as lone pairs increase.

About the European Baccalaureate Chemistry Exam

The European Baccalaureate Chemistry evaluates S6-S7 European Baccalaureate candidates on official OSGES syllabus learning outcomes. Note: Official examinations consist of written constructed-response papers and oral assessments; the 100 questions provided here are an English-language MCQ study adaptation for core concept revision.

Exam sponsor: Office of the Secretary-General of the European Schools (OSGES). The requirements and fees below concern the certification or admission exam, separate from our free practice resources.

Assessment

Official written paper and/or oral examination; 100 local practice MCQs for self-assessment.

Time Limit

180 minutes (3 hours)

Passing Score

5.0 out of 10.0 (50%)

Exam / Certification Fees

EUR 111.49 Baccalaureate registration fee

Exam sponsor website

Reported exam pass rate: 85-90%. This describes exam candidates, not OpenExamPrep users or results from using our resources. Exam sponsor website

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

Official sources

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%

Atomic Structure, Chemical Bonding & Periodic Trends

Quantum numbers, atomic orbitals, electron configurations, periodic trends, Lewis structures, VSEPR geometry, hybridization, and intermolecular forces.

15%

Energetics & Thermochemistry

Enthalpy changes, calorimetry, Hess's Law, bond enthalpies, entropy, and Gibbs free energy spontaneity calculations.

15%

Chemical Kinetics & Reaction Rates

Collision theory, activation energy, rate laws, reaction order, rate constants, Arrhenius equation, and reaction mechanisms.

15%

Chemical Equilibrium & Le Chatelier

Equilibrium constants (Kc, Kp), reaction quotient, Le Chatelier's principle, heterogeneous equilibria, and solubility products (Ksp).

15%

Acid-Base Equilibria & Aqueous Solutions

Brønsted-Lowry and Lewis acid-base theories, pH/pOH calculations, weak acids/bases, salt hydrolysis, buffers, and titration curves.

15%

Electrochemistry & Redox Reactions

Oxidation numbers, balancing redox half-reactions, galvanic cells, standard electrode potentials, Nernst equation, and Faraday's laws of electrolysis.

10%

Organic Chemistry & Polymers

IUPAC nomenclature, structural and stereoisomerism, nucleophilic/electrophilic mechanisms, functional group reactions, and polymerization.

Preparing for the European Baccalaureate Chemistry Exam

What You Need to Know

Passing score: 5.0 out of 10.0 (50%)
Assessment: Official written paper and/or oral examination; 100 local practice MCQs for self-assessment.
Time limit: 180 minutes (3 hours)
Exam / certification fees: EUR 111.49 Baccalaureate registration fee Official sources

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European Baccalaureate Chemistry: Suggested Study Strategy

1Master thermochemical and kinetic calculations, paying close attention to units (kJ/mol vs J/mol K) and sign conventions.

2Practice drawing and identifying organic reaction mechanisms (SN1, SN2, electrophilic addition) and stereoisomers.

3Review acid-base titration curves, buffer systems, and Henderson-Hasselbalch calculations.

4Understand standard cell potential calculations and Faraday's laws of electrolysis.

Frequently Asked Questions

What is the format of the official European Baccalaureate Chemistry exam?

The official European Baccalaureate Chemistry is administered by OSGES as a written/oral exam graded on a 0-10 scale. The 100 practice questions on OpenExamPrep are an English-language multiple-choice study adaptation for syllabus revision.

What is the passing score for the European Baccalaureate Chemistry?

The passing grade is 5.0 out of 10.0 (50%).

Who sets the syllabus for European Baccalaureate Chemistry?

The syllabus and examination specifications are established by the Office of the Secretary-General of the European Schools (OSGES).

Free Practice Questions for European Baccalaureate Chemistry

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