Air University Entry 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 Air University Entry Test, not a summary of it.

1. 1

   Fundamental Concepts

   3 topics

   • Atomic structure
   • Stoichiometry and the mole concept
   • Isotopes and atomic mass
2. 2

   Chemical Bonding

   3 topics

   • Ionic and covalent bonding
   • Hybridization and molecular geometry
   • Intermolecular forces
3. 3

   States of Matter

   3 topics

   • Gases and gas laws
   • Liquids
   • Solids and crystal structures
4. 4

   Physical Chemistry

   5 topics

   • Thermochemistry
   • Chemical equilibrium
   • Reaction kinetics
   • Electrochemistry
   • Acids, bases and salts
5. 5

   Periodicity and Inorganic Chemistry

   3 topics

   • Periodic table and properties
   • s and p block elements
   • Transition elements
6. 6

   Organic Chemistry

   4 topics

   • Hydrocarbons
   • Functional groups
   • Common reactions and mechanisms
   • Macromolecules and biochemistry

Chemistry flashcards for Air University Entry Test

21 of 64 cards from the Chemistry deck — real questions with worked answers.

1. What are the three subatomic particles, and what are their relative charges?

   Proton (+1), electron (-1), and neutron (0, neutral). Protons and neutrons sit in the nucleus; electrons occupy orbitals around it.

2. What do the atomic number (Z) and mass number (A) of an atom represent?

   Atomic number Z = number of protons. Mass number A = number of protons + neutrons. Number of neutrons = A - Z.

3. State the order of filling of atomic subshells according to the (n+l) Aufbau rule.

   1s, 2s, 2p, 3s, 3p, 4s, 3d, 4p, 5s, 4d, 5p, 6s, 4f, 5d, 6p, 7s — lower (n+l) fills first, and for equal (n+l) the lower n fills first.

4. State the Pauli exclusion principle.

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

5. State Hund's rule of maximum multiplicity.

   Electrons fill degenerate orbitals singly with parallel spins before any orbital is doubly occupied, minimizing electron-electron repulsion.

6. What are the maximum numbers of electrons in the s, p, d, and f subshells?

   s = 2, p = 6, d = 10, f = 14. The maximum in a shell of principal quantum number n is 2n^2.

7. What is the value of Avogadro's number, and what does it count?

   6.022 x 10^23 particles per mole — it is the number of atoms, molecules, ions, or other entities in one mole of a substance.

8. Define one mole.

   The amount of substance containing exactly 6.022 x 10^23 elementary entities (Avogadro's number). The mass of one mole in grams equals the substance's molar mass.

9. What formula relates number of moles to mass and molar mass?

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

10. What formula relates number of moles to the number of particles?

    moles (n) = number of particles / Avogadro's number (6.022 x 10^23). So number of particles = n x 6.022 x 10^23.

11. What is the molar volume of an ideal gas at STP?

    22.4 L per mole at standard temperature and pressure (0 degrees C / 273.15 K and 1 atm).

12. Distinguish between empirical formula and molecular formula.

    Empirical formula gives the simplest whole-number ratio of atoms (e.g., CH2O). Molecular formula gives the actual number of each atom (e.g., C6H12O6 = (CH2O)6).

13. What is a limiting reactant?

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

14. How do you calculate percentage yield?

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

15. Define isotopes.

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

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

    It is the weighted average of isotopic masses: Ar = sum of (isotopic mass x fractional abundance) for all isotopes.

17. Chlorine has isotopes Cl-35 (75%) and Cl-37 (25%). What is its relative atomic mass?

    (35 x 0.75) + (37 x 0.25) = 26.25 + 9.25 = 35.5.

18. What instrument is used to determine isotopic masses and abundances?

    The mass spectrometer, which ionizes atoms, deflects ions in a magnetic field by their mass-to-charge ratio, and detects their relative abundances.

19. What is the difference between ionic and covalent bonding?

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

20. Define electronegativity and state its general periodic trend.

    Electronegativity is the tendency of an atom to attract a shared (bonding) electron pair. It increases across a period (left to right) and decreases down a group; fluorine is the most electronegative element.

21. How does electronegativity difference classify a bond as ionic, polar covalent, or non-polar covalent?

    Difference > ~1.7 is largely ionic; ~0.4 to 1.7 is polar covalent; < ~0.4 is non-polar covalent.

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