National MDCAT Chemistry Syllabus

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 National MDCAT, not a summary of it.

1. 1

   Fundamental Concepts and Atomic Structure

   4 topics

   • Stoichiometry and Mole Concept
   • Atomic Theory and Subatomic Particles
   • Hydrogen Spectrum
   • Quantum Numbers and Shapes of Orbitals
2. 2

   Gases

   3 topics

   • Gas Laws
   • Kinetic Molecular Theory
   • Ideal and Real Gases
3. 3

   Liquids and Solids

   3 topics

   • Properties of Liquids
   • Types of Solids
   • Crystal Lattice and Differences
4. 4

   Chemical Equilibrium

   3 topics

   • Equilibrium Constant
   • Le Chatelier's Principle
   • Applications of Equilibrium
5. 5

   Reaction Kinetics

   3 topics

   • Rate of Reaction
   • Rate Law and Order of Reaction
   • Factors Affecting Reaction Rate
6. 6

   Thermochemistry and Energetics

   3 topics

   • Internal Energy and Enthalpy
   • Hess's Law
   • Energetics of Chemical Reactions
7. 7

   Electrochemistry

   3 topics

   • Oxidation-Reduction Reactions
   • Electrochemical Cells
   • Electrode Potential
8. 8

   Chemical Bonding

   4 topics

   • Types of Bonds
   • VSEPR Theory
   • Dipole Moment
   • Hybridization
9. 9

   s- and p-Block Elements

   3 topics

   • s-Block Elements
   • p-Block Elements
   • Periodic Trends
10. 10

    Transition Elements

    3 topics

    • Electronic Structure
    • Properties of Transition Metals
    • Coordination Compounds
11. 11

    Fundamental Principles of Organic Chemistry

    3 topics

    • Classification of Organic Compounds
    • Functional Groups
    • Isomerism
12. 12

    Chemistry of Hydrocarbons

    4 topics

    • Alkanes
    • Alkenes
    • Alkynes
    • Chemistry of Benzene
13. 13

    Alkyl Halides

    3 topics

    • Nomenclature and Preparation
    • Substitution vs Elimination Reactions
    • Reaction Mechanisms
14. 14

    Alcohols and Phenols

    3 topics

    • Reactivity of Alcohols
    • Reactivity of Phenols
    • Electrophilic Aromatic Substitution
15. 15

    Aldehydes and Ketones

    2 topics

    • Structure and Comparison
    • Chemistry and Reactions
16. 16

    Carboxylic Acids

    2 topics

    • Structure and Acidity
    • Reactions and Reactivity
17. 17

    Macromolecules

    3 topics

    • Polymers
    • Proteins and Carbohydrates
    • Biological Macromolecules
18. 18

    Industrial Chemistry

    2 topics

    • Dyes and Their Uses
    • Industrial Processes

Chemistry flashcards for National MDCAT

21 of 60 cards from the Chemistry deck — real questions with worked answers.

1. Define one mole and state the value of Avogadro's number.

   A mole is the amount of substance containing as many elementary entities as there are atoms in exactly 12 g of carbon-12. Avogadro's number = 6.022 x 10^23 entities per mole.

2. What is the formula relating number of moles (n) to mass and molar mass?

   n = mass (g) / molar mass (g/mol).

3. In Stoichiometry, what is a limiting reactant?

   The reactant that is completely consumed first in a reaction, thereby limiting the amount of product formed. The other reactant(s) are in excess.

4. How do you calculate the volume of any ideal gas at STP given the number of moles?

   Volume = n x 22.414 L, since one mole of any ideal gas occupies 22.414 dm^3 (litres) at STP (0 C, 1 atm).

5. What is the difference between empirical formula and molecular formula?

   The empirical formula gives the simplest whole-number ratio of atoms; the molecular formula gives the actual number of each type of atom. Molecular formula = (empirical formula) x n, where n = molar mass / empirical formula mass.

6. State the principle of the law of conservation of mass as used in stoichiometry.

   Mass is neither created nor destroyed in a chemical reaction; the total mass of reactants equals the total mass of products, which is why chemical equations are balanced.

7. How is percentage yield calculated?

   Percentage yield = (actual yield / theoretical yield) x 100.

8. State the postulates of Dalton's atomic theory.

   Matter is made of indivisible atoms; atoms of an element are identical in mass and properties; atoms of different elements differ; atoms combine in simple whole-number ratios to form compounds; atoms are neither created nor destroyed in reactions.

9. Give the relative charge and relative mass of the proton, neutron, and electron.

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

10. Who discovered the electron, proton, and neutron respectively?

    Electron: J.J. Thomson (cathode rays). Proton: E. Goldstein discovered canal/positive rays; Rutherford identified the proton. Neutron: James Chadwick.

11. What do the atomic number (Z) and mass number (A) represent?

    Atomic number Z = number of protons (= number of electrons in a neutral atom). Mass number A = number of protons + number of neutrons.

12. What are isotopes? Give an example.

    Isotopes are atoms of the same element with the same atomic number but different mass numbers (different numbers of neutrons), e.g., carbon-12 and carbon-14.

13. What was the key conclusion of Rutherford's gold foil (alpha-scattering) experiment?

    Most of the atom is empty space, and the positive charge and nearly all the mass are concentrated in a tiny dense central nucleus, around which electrons revolve.

14. How is the wavelength of spectral lines in the hydrogen spectrum calculated?

    Using the Rydberg equation: 1/lambda = R_H (1/n1^2 - 1/n2^2), where R_H = 1.097 x 10^7 m^-1, and n2 > n1.

15. Name the spectral series of the hydrogen atom and the region in which each appears.

    Lyman (ultraviolet, n1=1), Balmer (visible, n1=2), Paschen (infrared, n1=3), Brackett (infrared, n1=4), Pfund (infrared, n1=5).

16. Why is the hydrogen emission spectrum a line spectrum rather than continuous?

    Because electrons occupy only certain quantized energy levels; an electron emits a photon of a definite energy (and wavelength) only when it jumps between two discrete levels, giving discrete lines.

17. According to Bohr's model, what happens when an electron jumps from a higher to a lower energy level?

    It emits a photon whose energy equals the difference between the two levels: E = E2 - E1 = h x nu, producing an emission spectral line.

18. What is the significance of the principal quantum number (n)?

    It indicates the main energy level/shell and the size of the orbital. n = 1, 2, 3...; larger n means higher energy and greater average distance from the nucleus.

19. What does the azimuthal (angular momentum) quantum number (l) describe, and what values can it take?

    It describes the subshell and the shape of the orbital. For a given n, l ranges from 0 to (n-1): l=0 (s), 1 (p), 2 (d), 3 (f).

20. What does the magnetic quantum number (m) specify, and what values can it take?

    It specifies the orientation of an orbital in space. For a given l, m ranges from -l to +l including 0, giving (2l+1) orbitals per subshell.

21. What are the two possible values of the spin quantum number (s) and what do they represent?

    +1/2 and -1/2, representing the two opposite directions of electron spin (clockwise and anticlockwise).

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