COMSATS NTS-based Test Chemistry (NAT-IE / NAT-IM) Syllabus

Chemistry (NAT-IE / NAT-IM) syllabus — full chapter and topic list

Expand any chapter to see its topics and sub-topics. This is the whole examinable outline for Chemistry (NAT-IE / NAT-IM) in COMSATS NTS-based Test, not a summary of it.

1. 1

   Physical Chemistry

   5 topics

   • Atomic Structure
   • Chemical Bonding
   • States of Matter
   • Chemical Equilibrium
   • Thermochemistry
2. 2

   Inorganic Chemistry

   3 topics

   • Periodic Table and Periodicity
   • s and p Block Elements
   • Transition Elements
3. 3

   Organic Chemistry

   3 topics

   • Hydrocarbons
   • Functional Groups
   • Reaction Mechanisms
4. 4

   Analytical and Applied Chemistry

   3 topics

   • Stoichiometry and Mole Concept
   • Acids, Bases and Salts
   • Electrochemistry

Chemistry (NAT-IE / NAT-IM) flashcards for COMSATS NTS-based Test

25 of 52 cards from the Chemistry (NAT-IE / NAT-IM) deck — real questions with worked answers.

1. What are the three subatomic particles, and what is the relative charge and approximate mass (in amu) of each?

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

2. State the maximum number of electrons a shell can hold using the formula in terms of the principal quantum number n.

   2n2. So shell 1 holds 2, shell 2 holds 8, shell 3 holds 18, shell 4 holds 32.

3. What are the four quantum numbers and what does each describe?

   Principal (n) - shell/energy & size; Azimuthal (l) - subshell/shape; Magnetic (m) - orbital orientation; Spin (s) - electron spin (+1/2 or -1/2).

4. State the maximum number of electrons each subshell (s, p, d, f) can hold.

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

5. State Hund's rule of maximum multiplicity.

   Electrons fill degenerate orbitals singly with parallel spins first, before any orbital is doubly occupied.

6. 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.

7. State the Aufbau principle and give the filling order up to 4s.

   Electrons fill orbitals from lowest to highest energy: 1s, 2s, 2p, 3s, 3p, 4s, 3d, 4p...

8. What are isotopes? Give an example.

   Atoms of the same element with the same number of protons (atomic number) but different numbers of neutrons (mass number), e.g. C-12, C-13, C-14.

9. How are mass number (A) and atomic number (Z) defined, and how do you find the number of neutrons?

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

10. Define ionic, covalent, and metallic bonding.

    Ionic = transfer of electrons forming oppositely charged ions; covalent = sharing of electron pairs; metallic = lattice of cations in a sea of delocalized electrons.

11. Distinguish between a sigma (sigma) bond and a pi (pi) bond.

    Sigma bond forms by head-on (axial) overlap of orbitals and is stronger; pi bond forms by sideways (lateral) overlap of p orbitals and is weaker. A single bond is 1 sigma; double = 1 sigma + 1 pi; triple = 1 sigma + 2 pi.

12. According to VSEPR theory, what are the shapes and bond angles for 2, 3, and 4 electron pairs (no lone pairs)?

    2 = linear (180 degrees), 3 = trigonal planar (120 degrees), 4 = tetrahedral (109.5 degrees).

13. Why is the H2O molecule bent (~104.5 degrees) rather than linear?

    Oxygen has two bonding pairs and two lone pairs; lone pair-bond pair repulsion compresses the angle below the tetrahedral 109.5 degrees, giving a bent shape.

14. What is the hybridization of carbon in methane, ethene, and ethyne?

    Methane (CH4) = sp3; ethene (C2H4) = sp2; ethyne (C2H2) = sp.

15. Define electronegativity and state the trend across a period and down a group.

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

16. What determines whether a covalent bond is polar or nonpolar?

    The electronegativity difference between the two atoms. A difference greater than 0 but typically below ~1.7 gives a polar covalent bond; zero gives nonpolar; large differences (>~1.7) give ionic character.

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

    A covalent bond in which both shared electrons come from the same atom, e.g. formation of the ammonium ion NH4+ from NH3 and H+.

18. List the three types of intermolecular forces in order of increasing strength.

    London dispersion forces < dipole-dipole forces < hydrogen bonding.

19. State the postulates of the kinetic molecular theory of gases (any three).

    Gas particles are in constant random motion; their volume is negligible vs container volume; collisions are perfectly elastic (no energy lost); average kinetic energy is proportional to absolute temperature; no intermolecular forces.

20. State Boyle's law and its mathematical form.

    At constant temperature, the volume of a fixed gas mass is inversely proportional to its pressure: PV = constant, or P1V1 = P2V2.

21. State Charles's law and its mathematical form.

    At constant pressure, the volume of a fixed gas mass is directly proportional to its absolute temperature: V/T = constant, or V1/T1 = V2/T2.

22. Write the ideal gas equation and define each term.

    PV = nRT, where P = pressure, V = volume, n = moles, R = gas constant (8.314 J/mol/K), T = absolute temperature in kelvin.

23. State Avogadro's law.

    Equal volumes of all gases at the same temperature and pressure contain equal numbers of molecules; volume is directly proportional to number of moles (V proportional to n).

24. Define the dynamic equilibrium of a reversible reaction.

    A state where the forward and reverse reaction rates are equal, so the concentrations of reactants and products remain constant over time (though both reactions continue).

25. State Le Chatelier's principle.

    If a system at equilibrium is disturbed by a change in concentration, pressure, or temperature, the equilibrium shifts in the direction that counteracts the change.

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