Pharm-D Admission Test 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 Pharm-D Admission Test, not a summary of it.

1. 1

   Atomic Structure

   4 topics

   • Fundamental Particles and Atomic Models
   • Quantum Numbers and Orbitals
   • Electronic Configuration
   • Periodic Table and Periodicity
2. 2

   Chemical Bonding

   4 topics

   • Ionic and Covalent Bonding
   • Hybridization and Molecular Geometry
   • Hydrogen Bonding and Intermolecular Forces
   • Bond Energy and Polarity
3. 3

   States of Matter

   3 topics

   • Gaseous State
   • Liquid State
   • Solid State and Crystal Lattice
4. 4

   Thermochemistry and Energetics

   3 topics

   • Enthalpy and Heat of Reaction
   • Hess's Law
   • Internal Energy and First Law
5. 5

   Chemical Equilibrium

   4 topics

   • Law of Mass Action
   • Le Chatelier's Principle
   • Solubility Product
   • Common Ion Effect
6. 6

   Acids, Bases and Salts

   3 topics

   • Acid-Base Theories
   • pH and Buffers
   • Salt Hydrolysis
7. 7

   Chemical Kinetics

   3 topics

   • Rate of Reaction
   • Order and Molecularity
   • Factors Affecting Reaction Rate
8. 8

   Electrochemistry

   3 topics

   • Oxidation and Reduction
   • Electrochemical Cells
   • Electrolysis and Electrode Potential
9. 9

   Fundamentals of Organic Chemistry

   3 topics

   • Classification and Nomenclature
   • Isomerism
   • Reaction Mechanisms and Intermediates
10. 10

    Hydrocarbons

    3 topics

    • Alkanes
    • Alkenes and Alkynes
    • Aromatic Hydrocarbons and Benzene
11. 11

    Organic Functional Groups

    5 topics

    • Alkyl Halides
    • Alcohols, Phenols and Ethers
    • Aldehydes and Ketones
    • Carboxylic Acids and Derivatives
    • Amines
12. 12

    Biochemistry and Industrial Chemistry

    3 topics

    • Carbohydrates, Proteins and Lipids
    • Vitamins, Enzymes and Hormones
    • Environmental and Industrial Chemistry

Chemistry flashcards for Pharm-D Admission Test

21 of 65 cards from the Chemistry deck — real questions with worked answers.

1. What are the three fundamental subatomic particles, and what is the charge and relative mass of each?

   Proton (charge +1, mass 1 amu), neutron (charge 0, mass 1 amu), and electron (charge -1, mass ~1/1836 amu).

2. What did Rutherford's gold-foil (alpha-scattering) experiment establish about atomic structure?

   It showed the atom has a tiny, dense, positively charged nucleus containing most of the mass, with electrons occupying the largely empty space around it.

3. State the main postulate of Bohr's atomic model regarding electron energy.

   Electrons revolve in fixed circular orbits (energy levels) of quantized energy without radiating energy; they absorb or emit energy only when jumping between orbits.

4. In Bohr's model, what is the expression for the angular momentum of an electron in an allowed orbit?

   mvr = nh/2pi, where n is the principal quantum number (n = 1, 2, 3...) and h is Planck's constant.

5. What is the defining limitation of Bohr's model that the quantum mechanical model overcomes?

   Bohr's model only works for hydrogen-like (single-electron) species and cannot explain spectra of multi-electron atoms, fine spectral lines, or the wave nature of electrons; the quantum model uses orbitals and probability instead of fixed orbits.

6. What does the principal quantum number (n) describe, and what values can it take?

   It describes the main energy level/shell and the average size and energy of an orbital; n = 1, 2, 3,... (positive integers).

7. What does the azimuthal (angular momentum) quantum number (l) describe, and what is its range of values?

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

8. What does the magnetic quantum number (m) describe, and what values can it take for a given l?

   It describes the orientation of the orbital in space; m ranges from -l to +l, including 0 (i.e., 2l+1 values).

9. What does the spin quantum number (s) represent and what are its possible values?

   It represents the spin orientation of the electron; values are +1/2 and -1/2.

10. How many orbitals and how many electrons can the s, p, d, and f subshells hold?

    s: 1 orbital, 2 electrons; p: 3 orbitals, 6 electrons; d: 5 orbitals, 10 electrons; f: 7 orbitals, 14 electrons.

11. State the Aufbau principle for electronic configuration.

    Electrons fill orbitals in order of increasing energy, lowest energy orbitals first (following the n+l rule).

12. State the Pauli exclusion principle.

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

13. State Hund's rule of maximum multiplicity.

    Electrons occupy degenerate (equal-energy) orbitals singly with parallel spins before any orbital is doubly occupied.

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

    [Ar] 3d5 4s1. A half-filled 3d subshell plus half-filled 4s gives extra stability, so one 4s electron shifts to 3d.

15. Write the ground-state electronic configuration of copper (Z = 29) and explain the anomaly.

    [Ar] 3d10 4s1. A completely filled 3d10 subshell is more stable, so one 4s electron shifts to 3d.

16. What is the (n+l) rule for the order of orbital filling?

    Orbitals fill in order of increasing (n+l); if two orbitals have equal (n+l), the one with lower n fills first. E.g., 4s (n+l=4) fills before 3d (n+l=5).

17. On what basis are elements arranged in the modern periodic table, and what is the modern periodic law?

    They are arranged by increasing atomic number; the modern periodic law states that the properties of elements are a periodic function of their atomic numbers.

18. How does atomic radius change across a period and down a group, and why?

    It decreases across a period (increasing nuclear charge pulls electrons closer) and increases down a group (new shells are added).

19. Define ionization energy and describe its trend across a period and down a group.

    Ionization energy is the energy required to remove the most loosely bound electron from a gaseous atom. It increases across a period and decreases down a group.

20. Define electron affinity and describe its general periodic trend.

    Electron affinity is the energy released when an electron is added to a gaseous atom. It generally increases (becomes more negative) across a period and decreases down a group.

21. Define electronegativity and identify the most electronegative element.

    Electronegativity is the tendency of an atom to attract a shared (bonding) pair of electrons toward itself. Fluorine is the most electronegative element.

See more Chemistry flashcards →

Planning Chemistry for Pharm-D Admission Test

Chemistry (Pharm-D Admission Test) FAQ