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 MDCAT, not a summary of it.

1. 1

   Fundamental Concepts

   3 topics

   • Atomic Structure
   • Chemical Bonding
   • Mole Concept
2. 2

   States of Matter

   3 topics

   • Gases
   • Liquids
   • Solids
3. 3

   Thermodynamics

   3 topics

   • First Law of Thermodynamics
   • Second Law of Thermodynamics
   • Heat of Reaction
4. 4

   Chemical Equilibrium

   3 topics

   • Dynamic Nature of Equilibrium
   • Le Chatelier's Principle
   • Acids and Bases
5. 5

   Organic Chemistry

   3 topics

   • Introduction to Organic Chemistry
   • Hydrocarbons
   • Functional Groups

Chemistry flashcards for MDCAT

21 of 51 cards from the Chemistry deck — real questions with worked answers.

1. What are the relative charge and mass of a proton, neutron, and electron?

   Proton: charge $+1$, mass $\approx 1\,\text{amu}$. Neutron: charge $0$, mass $\approx 1\,\text{amu}$. Electron: charge $-1$, mass $\approx \frac{1}{1836}\,\text{amu}$ (negligible).

2. State the relationship between atomic number $Z$, mass number $A$, and number of neutrons.

   $Z$ = number of protons; $A$ = protons + neutrons; number of neutrons $= A - Z$.

3. What is the maximum number of electrons that a shell with principal quantum number $n$ can hold?

   $2n^{2}$ electrons.

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

   Principal ($n$): size/energy of shell. Azimuthal ($l$): subshell/shape ($0$–$(n-1)$). Magnetic ($m_l$): orbital orientation ($-l$ to $+l$). Spin ($m_s$): electron spin, $\pm\frac{1}{2}$.

5. State the Pauli Exclusion Principle.

   No two electrons in an atom can have the same set of all four quantum numbers; each orbital holds a maximum of two electrons with opposite spins.

6. State Hund's rule of maximum multiplicity.

   Electrons occupy degenerate (equal-energy) orbitals singly with parallel spins before pairing up.

7. Give the shapes and maximum electron capacities of the $s$, $p$, $d$, and $f$ subshells.

   $s$: spherical, $2\,e^{-}$; $p$: dumb-bell, $6\,e^{-}$; $d$: $10\,e^{-}$; $f$: $14\,e^{-}$.

8. What is an ionic (electrovalent) bond and how does it form?

   An electrostatic force of attraction between oppositely charged ions formed by the complete transfer of electrons from a metal to a non-metal, e.g. $\ce{Na+ + Cl- -> NaCl}$.

9. What is a covalent bond and how does it differ from a coordinate covalent (dative) bond?

   A covalent bond is a shared electron pair where each atom contributes one electron; in a coordinate covalent bond both shared electrons come from a single atom (the donor).

10. Compare sigma ($\sigma$) and pi ($\pi$) bonds.

    $\sigma$ bonds form by head-on (axial) overlap and are stronger; $\pi$ bonds form by sideways (lateral) overlap of $p$-orbitals and are weaker. A single bond is $1\sigma$; a double bond is $1\sigma + 1\pi$; a triple bond is $1\sigma + 2\pi$.

11. Predict the geometry and bond angle for $sp$, $sp^{2}$, and $sp^{3}$ hybridization.

    $sp$: linear, $180^{\circ}$; $sp^{2}$: trigonal planar, $120^{\circ}$; $sp^{3}$: tetrahedral, $109.5^{\circ}$.

12. What is a hydrogen bond and give one consequence of it?

    A dipole-dipole attraction between an H atom bonded to a highly electronegative atom ($\ce{F, O, N}$) and a lone pair on another such atom. It accounts for the anomalously high boiling point of water.

13. Define the mole and give the value of Avogadro's number.

    A mole is the amount of substance containing as many particles as there are atoms in $12\,\text{g}$ of $\ce{^{12}C}$. Avogadro's number $N_A = 6.022\times10^{23}\ \text{mol}^{-1}$.

14. Write the formula relating number of moles $n$ to mass and molar mass.

    $$n = \frac{\text{mass (g)}}{\text{molar mass (g mol}^{-1})}$$

15. What volume does one mole of an ideal gas occupy at STP?

    $22.4\ \text{dm}^{3}$ (litres) at STP ($0\,^{\circ}\text{C}$, $1\,\text{atm}$).

16. How do you calculate the number of particles from the number of moles $n$?

    $$\text{number of particles} = n \times N_A = n \times 6.022\times10^{23}$$

17. State Boyle's law and its equation.

    At constant temperature, the volume of a fixed mass of gas is inversely proportional to its pressure: $$PV = \text{constant} \quad\text{or}\quad P_1V_1 = P_2V_2$$

18. State Charles's law and its equation.

    At constant pressure, the volume of a fixed mass of gas is directly proportional to its absolute temperature: $$\frac{V}{T} = \text{constant} \quad\text{or}\quad \frac{V_1}{T_1} = \frac{V_2}{T_2}$$

19. Write the ideal gas equation and identify all terms.

    $$PV = nRT$$ where $P$ = pressure, $V$ = volume, $n$ = moles, $R$ = gas constant ($8.314\ \text{J mol}^{-1}\text{K}^{-1}$), $T$ = absolute temperature.

20. State Dalton's law of partial pressures.

    The total pressure of a non-reacting gas mixture equals the sum of the partial pressures of the component gases: $$P_{\text{total}} = P_1 + P_2 + P_3 + \dots$$

21. State Graham's law of diffusion.

    The rate of diffusion of a gas is inversely proportional to the square root of its density (or molar mass): $$\frac{r_1}{r_2} = \sqrt{\frac{M_2}{M_1}}$$

See more Chemistry flashcards →

Planning Chemistry for MDCAT

Chemistry (MDCAT) FAQ