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100+ Free Schleswig-Holstein Abitur Chemistry Practice Questions

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2026 Statistics

Key Facts: Schleswig-Holstein Abitur Chemistry Exam

Since 2025

First Abiturprüfung year in which Chemie tasks are centrally selected from the IQB Gemeinsamer Abituraufgabenpool der Länder (Physik joined the same year; Biologie followed from 2026)

za.schleswig-holstein.de, Zentralabitur portal

255 / 300 min

Bearbeitungszeit at grundlegendem Anforderungsniveau / Profilfach (erhöhtes Anforderungsniveau), including Auswahlzeit

schullv.de Chemie-Abi 2026 Schleswig-Holstein

24.04.2026

Written Chemie (Profilfach) exam date in the 2026 main session

ZAB-Terminplan Abitur 2026 (Ministerium für Bildung SH), via salemkolleg.de and stark-verlag.de

4 -> 3 Aufgaben

Candidates receive four centrally set Aufgaben and select three to answer; at most one may carry a fachpraktischer Anteil

schullv.de Chemie-Abi 2026 Schleswig-Holstein

0-15 Punkte

Grading scale for each Prüfungsfach, from Note 1 (15-13 Punkte) to Note 6 (0 Punkte)

OAPVO §11, Schleswig-Holstein

200 / 100 Punkte

Minimum Gesamtqualifikation: 200+ from Block I and 100+ from Block II, out of 900 maximum

OAPVO §§31-33, Schleswig-Holstein

Free 100-question English-language MCQ study bank for Schleswig-Holstein Zentralabitur Chemie, weighted to the confirmed Basiskonzepte: organic chemistry/macromolecules (~28%), redox/electrochemistry (~20%), acid-base (~18%), equilibrium (~14%), reaction energetics/kinetics (~12%), and atomic structure/bonding (~8%). Official exam: German materialgebundene Klausur, centrally IQB-pool-set since Abitur 2025, 255 min (grundlegend) / 300 min (Profilfach), written date 24.04.2026. Not an official-format simulation; no fee for regular school candidates.

Sample Schleswig-Holstein Abitur Chemistry Practice Questions

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

1Which trend best describes the general change in electronegativity across Period 3 of the periodic table, from sodium (Na) to chlorine (Cl)?
A.It increases steadily from Na to Cl
B.It decreases steadily from Na to Cl
C.It stays essentially constant across the period
D.It increases then decreases in the middle of the period
Explanation: Across a period, nuclear charge increases while the number of inner shielding electron shells stays the same, so atoms pull bonding electrons more strongly. This makes electronegativity rise fairly steadily from the alkali metal to the halogen in the same period.
2What type of bonding forms when sodium reacts with chlorine to produce sodium chloride (NaCl)?
A.Ionic bonding, through the transfer of an electron from Na to Cl
B.Covalent bonding, through a shared pair of electrons
C.Metallic bonding, through delocalized electrons
D.Hydrogen bonding, through a shared hydrogen atom
Explanation: Sodium has low electronegativity and readily loses its single valence electron, while chlorine has high electronegativity and gains that electron to complete its octet. The resulting Na+ and Cl- ions are held together by electrostatic attraction, which is ionic bonding.
3Two nonmetal atoms form a bond with an electronegativity difference of about 0.5. What kind of bond do they most likely form?
A.A polar covalent bond, with partial charges but no full electron transfer
B.A nonpolar covalent bond with no charge separation at all
C.An ionic bond, with complete transfer of an electron
D.A metallic bond, with a shared sea of delocalized electrons
Explanation: A small but nonzero electronegativity difference means the shared electron pair spends more time near the more electronegative atom, creating partial positive and negative charges without a full electron transfer. This is the hallmark of a polar covalent bond.
4Water (H2O) has a much higher boiling point than hydrogen sulfide (H2S), even though sulfur is larger and more polarizable than oxygen. Which intermolecular force best explains this?
A.Hydrogen bonding between water molecules
B.Dipole-dipole forces alone, with no hydrogen bonding
C.London dispersion forces alone
D.Ionic bonding between neighboring water molecules
Explanation: Oxygen is small and highly electronegative, so the O-H bonds in water form strong hydrogen bonds between neighboring molecules. Hydrogen sulfide lacks this because sulfur is less electronegative and larger, so its S-H bonds cannot form comparably strong hydrogen bonds.
5Using the electron-pair repulsion (VSEPR) model, what molecular shape does ammonia (NH3) adopt, given that nitrogen has three bonding pairs and one lone pair?
A.Trigonal pyramidal
B.Tetrahedral
C.Trigonal planar
D.Linear
Explanation: The four electron domains (three bonding pairs and one lone pair) arrange themselves in a tetrahedral electron geometry to minimize repulsion, but molecular shape is described only by the positions of the atoms. With one corner occupied by a lone pair instead of an atom, the resulting shape of NH3 is trigonal pyramidal.
6Why are most metals malleable, meaning they can be hammered into sheets without breaking?
A.Delocalized electrons let layers of metal cations slide past each other while remaining bonded
B.Strong, fixed covalent bonds hold every atom rigidly in place
C.The ionic lattice cleaves cleanly along charged planes
D.Each atom is joined to its neighbors by a single, non-directional hydrogen bond
Explanation: In the electron-sea model of metallic bonding, positive metal ions are held together by a mobile sea of delocalized valence electrons rather than fixed, directional bonds. When a force is applied, layers of cations can slide into new positions while the delocalized electrons keep bonding them, so the metal deforms instead of shattering.
7Which combination of factors most increases the lattice energy of an ionic compound, according to Coulomb's law?
A.Smaller ionic radii and higher ionic charges
B.Larger ionic radii and higher ionic charges
C.Smaller ionic radii and lower ionic charges
D.Larger ionic radii and lower ionic charges
Explanation: Lattice energy is proportional to the product of the ionic charges and inversely proportional to the distance between ion centers, which is set by the sum of the ionic radii. Smaller ions pack closer together and higher charges increase the electrostatic attraction, so both factors together maximize lattice energy.
8An element belongs to Group 16 (VIA) of the periodic table, the same group as oxygen and sulfur. How many valence electrons does an atom of this element have?
A.6
B.4
C.8
D.2
Explanation: For main-group elements, the traditional A-group number directly gives the number of valence electrons. Group 16 elements such as oxygen and sulfur each have 6 valence electrons, which is why they typically form 2- ions or two covalent bonds to complete an octet.
9Which functional group is responsible for the acidic properties of ethanoic acid (acetic acid), CH3COOH?
A.The carboxyl group (-COOH)
B.The hydroxyl group (-OH) alone
C.The aldehyde group (-CHO)
D.The ester group (-COO-)
Explanation: The carboxyl group combines a carbonyl and a hydroxyl on the same carbon, and the resulting O-H bond is acidic because the conjugate base (the carboxylate ion) is resonance-stabilized. This is what makes ethanoic acid behave as a weak acid in water.
10What is the correct IUPAC name for CH3-CH2-CH2-OH?
A.Propan-1-ol
B.Propan-2-ol
C.Propanal
D.Propanoic acid
Explanation: The hydroxyl group is attached to the first (terminal) carbon of a three-carbon chain, so the compound is named propan-1-ol. The '-ol' suffix identifies it as an alcohol, and the locant '1' specifies the position of the hydroxyl group.

About the Schleswig-Holstein Abitur Chemistry Practice Questions

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