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🇵🇰 AKU MBBS Admission Test · subject

AKU MBBS Admission Test Chemistry Syllabus

Every chapter and topic of Chemistry examined in AKU MBBS Admission Test — 9 chapters, 28 topics, plus 67 flashcards written against it.

9Chapters
28Topics
0Sub-topics
~20hEst. first pass
23%Of AKU MBBS Admission Test
67Flashcards

Chemistry syllabus — full chapter and topic list

Expand any chapter to see its topics and sub-topics. This is the whole examinable outline for Chemistry in AKU MBBS Admission Test, not a summary of it.

  1. Atomic Structure

     3 topics
    • Subatomic Particles and Isotopes
    • Electronic Configuration
    • Periodic Trends

  2. Chemical Bonding

     4 topics
    • Ionic and Covalent Bonding
    • Molecular Geometry and VSEPR
    • Hybridization
    • Intermolecular Forces

  3. States of Matter

     2 topics
    • Gas Laws
    • Liquids and Solids

  4. Chemical Equilibrium

     4 topics
    • Equilibrium Constant
    • Le Chatelier's Principle
    • Acids, Bases and pH
    • Solubility Product

  5. Thermochemistry and Energetics

     2 topics
    • Enthalpy and Hess's Law
    • Entropy and Gibbs Free Energy

  6. Chemical Kinetics

     3 topics
    • Rate of Reaction and Rate Laws
    • Factors Affecting Reaction Rate
    • Catalysis

  7. Electrochemistry

     3 topics
    • Redox Reactions and Oxidation Numbers
    • Galvanic and Electrolytic Cells
    • Electrode Potentials

  8. Organic Chemistry

     4 topics
    • Hydrocarbons
    • Functional Groups and Reactions
    • Isomerism
    • Reaction Mechanisms

  9. Biochemistry

     3 topics
    • Carbohydrates, Lipids and Proteins
    • Nucleic Acids
    • Metabolism Basics

Chemistry flashcards for AKU MBBS Admission Test

21 of 67 cards from the Chemistry deck — real questions with worked answers.

  1. What are the relative charges and masses of the three subatomic particles?

    Proton: charge +1, mass ~1 amu. Neutron: charge 0, mass ~1 amu. Electron: charge -1, mass ~1/1836 amu (negligible).

  2. Define atomic number (Z) and mass number (A).

    Atomic number (Z) = number of protons in the nucleus (defines the element). Mass number (A) = number of protons + number of neutrons.

  3. What are isotopes?

    Atoms of the same element with the same number of protons (same Z) but different numbers of neutrons, giving different mass numbers.

  4. How is the relative atomic mass of an element calculated from its isotopes?

    Relative atomic mass = Σ (isotopic mass × fractional abundance), i.e. the weighted average of all isotope masses by their natural abundances.

  5. State the four quantum numbers and what each describes.

    Principal (n): energy level/shell size. Azimuthal (l): subshell shape (s,p,d,f). Magnetic (m_l): orbital orientation. Spin (m_s): electron spin (+1/2 or -1/2).

  6. State the Aufbau principle, Pauli exclusion principle, and Hund's rule.

    Aufbau: fill lowest-energy orbitals first. Pauli: no two electrons in an atom have identical quantum numbers (max 2 per orbital, opposite spins). Hund: orbitals in a subshell fill singly with parallel spins before pairing.

  7. What is the maximum number of electrons in s, p, d, and f subshells?

    s = 2, p = 6, d = 10, f = 14 electrons.

  8. Write the ground-state electronic configuration of chromium (Z=24) and explain the anomaly.

    [Ar] 3d5 4s1. A half-filled 3d5 with 4s1 is more stable than [Ar]3d4 4s2 due to the extra stability of a half-filled d-subshell.

  9. Why is the electron configuration of copper (Z=29) [Ar]3d10 4s1 rather than [Ar]3d9 4s2?

    A completely filled 3d10 subshell gives extra stability, so one 4s electron shifts into 3d to achieve a fully filled d-subshell.

  10. Define first ionization energy.

    The minimum energy required to remove one mole of electrons (the outermost) from one mole of gaseous atoms to form one mole of gaseous +1 ions.

  11. How does atomic radius vary across a period and down a group?

    Decreases across a period (increasing nuclear charge pulls electrons in). Increases down a group (additional shells and greater shielding).

  12. How does first ionization energy vary across a period and down a group?

    Generally increases across a period (greater nuclear charge, smaller radius). Decreases down a group (electrons farther from nucleus, more shielding).

  13. How does electronegativity vary across a period and down a group?

    Increases across a period (greater nuclear charge, smaller atom). Decreases down a group (larger atom, more shielding). Fluorine is the most electronegative element.

  14. What is the trend in metallic vs non-metallic character across a period?

    Metallic character decreases and non-metallic character increases from left to right across a period; metallic character increases down a group.

  15. Differentiate between ionic and covalent bonding.

    Ionic bonding: electrostatic attraction between oppositely charged ions formed by electron transfer (typically metal + non-metal). Covalent bonding: sharing of electron pairs between atoms (typically non-metal + non-metal).

  16. What is a coordinate (dative covalent) bond? Give an example.

    A covalent bond in which both shared electrons come from the same atom. Example: NH4+ (the N lone pair bonds to H+) or H3O+.

  17. Compare typical properties of ionic vs covalent (molecular) compounds.

    Ionic: high melting/boiling points, conduct when molten/dissolved, often water-soluble, hard/brittle. Molecular covalent: low melting/boiling points, generally non-conductive, often insoluble in water.

  18. What does bond polarity depend on, and when is a bond nonpolar covalent, polar covalent, or ionic?

    Depends on the electronegativity difference (ΔEN). ΔEN ≈ 0 (<0.4): nonpolar covalent; ~0.4-1.7: polar covalent; >1.7: largely ionic.

  19. State the main postulate of VSEPR theory.

    Electron pairs (bonding and lone) around a central atom arrange themselves as far apart as possible to minimize repulsion, determining molecular geometry. Repulsion order: lone-lone > lone-bond > bond-bond.

  20. Give the electron-pair geometry and bond angle for 2, 3, and 4 electron domains.

    2 domains: linear, 180°. 3 domains: trigonal planar, 120°. 4 domains: tetrahedral, 109.5°.

  21. What are the shapes and bond angles of water (H2O) and ammonia (NH3)?

    H2O: bent/angular, ~104.5° (2 lone pairs). NH3: trigonal pyramidal, ~107° (1 lone pair). Both based on tetrahedral electron geometry.

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Planning Chemistry for AKU MBBS Admission Test

Chemistry is about 23% of the AKU MBBS Admission Test syllabus by topic count — 28 of 122 topics, spread over 9 chapters. At roughly 45 minutes per topic plus 12 minutes per sub-topic, a first pass runs to about 20 hours.

The heaviest chapters are Chemical Bonding (4 topics), Chemical Equilibrium (4 topics), Organic Chemistry (4 topics) . Front-load those while your energy is high; the short chapters are better revision filler later.

Work top-down: read the chapter, then tick topics off individually rather than marking the whole chapter done. Sub-topics are where silent gaps hide.

Chemistry (AKU MBBS Admission Test) FAQ

What is in the AKU MBBS Admission Test Chemistry syllabus?

Chemistry is split into 9 chapters — Atomic Structure, Chemical Bonding, States of Matter, Chemical Equilibrium, Thermochemistry and Energetics and Chemical Kinetics, and 3 more, containing 28 topics and 0 sub-topics in total.

How is Chemistry structured in the AKU MBBS Admission Test syllabus?

9 chapters. Chemistry accounts for about 23% of the topics in the whole AKU MBBS Admission Test syllabus (28 of 122).

How long should I spend on Chemistry for AKU MBBS Admission Test?

Budget around 20 hours for a first pass through Chemistry — about 45 minutes per topic plus 12 minutes per sub-topic across its 28 topics. Add revision cycles on top.

Are there flashcards for AKU MBBS Admission Test Chemistry?

Yes — a 67-card Chemistry deck. Sample cards are printed on this page, and the full deck is free in the Examius app with spaced repetition scheduling.