AMUEEE 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 AMUEEE, not a summary of it.

1. 1

   Some Basic Concepts of Chemistry

   2 topics

   • Laws of chemical combination
   • Atomic and molecular masses
2. 2

   Structure of Atom

   2 topics

   • Bohr’s model and its limitations
   • Concepts of shells and subshells
3. 3

   Chemical Bonding and Molecular Structure

   2 topics

   • Valence electrons
   • Ionic bond and covalent bond
4. 4

   States of Matter: Gases and Liquids

   2 topics

   • Three states of matter
   • Ideal gas equation
5. 5

   Thermodynamics

   2 topics

   • First law of thermodynamics
   • Second law of thermodynamics

Chemistry flashcards for AMUEEE

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

1. State the mole concept: what is one mole and what is the value of Avogadro's number?

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

2. Define molarity (M) and give its formula.

   Molarity is the number of moles of solute per litre of solution. M = moles of solute / volume of solution in litres.

3. Distinguish molarity from molality.

   Molarity = moles of solute per litre of solution (temperature-dependent). Molality = moles of solute per kilogram of solvent (temperature-independent).

4. State the law of conservation of mass and the law of definite proportions.

   Conservation of mass: mass is neither created nor destroyed in a chemical reaction. Definite proportions: a given compound always contains the same elements in the same fixed mass ratio.

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

   Molecular formula = n x empirical formula, where n = molecular mass / empirical formula mass. The empirical formula gives the simplest whole-number ratio of atoms.

6. Give the de Broglie equation relating wavelength to momentum.

   lambda = h / p = h / (mv), where h is Planck's constant, m is mass and v is velocity.

7. State Heisenberg's uncertainty principle as an equation.

   Delta x . Delta p >= h / 4pi. The position and momentum of a particle cannot both be known with arbitrary precision simultaneously.

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

   Principal (n) = shell/energy; Azimuthal (l) = subshell/shape; Magnetic (m_l) = orbital orientation; Spin (m_s) = electron spin (+1/2 or -1/2).

9. State Hund's rule of maximum multiplicity.

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

10. 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.

11. Give the energy of an electron in the nth Bohr orbit of hydrogen.

    E_n = -13.6 / n^2 eV per atom (negative, increasing toward zero as n increases).

12. State 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 = temperature in kelvin.

13. State Boyle's law, Charles's law and Gay-Lussac's law.

    Boyle's: PV = constant at constant T. Charles's: V/T = constant at constant P. Gay-Lussac's: P/T = constant at constant V.

14. State Dalton's law of partial pressures.

    The total pressure of a mixture of non-reacting gases equals the sum of their partial pressures: P_total = P1 + P2 + P3 + ...

15. What are the two correction terms in the van der Waals equation for real gases?

    Pressure correction a/V^2 (for intermolecular attraction) and volume correction b (for finite molecular volume): (P + an^2/V^2)(V - nb) = nRT.

16. State the first law of thermodynamics as an equation.

    Delta U = q + w, where Delta U is change in internal energy, q is heat added to the system, and w is work done on the system.

17. Define enthalpy and give its relation to internal energy.

    Enthalpy H = U + PV. At constant pressure, Delta H = q_p (heat exchanged) and Delta H = Delta U + Delta(PV).

18. State Hess's law of constant heat summation.

    The total enthalpy change of a reaction is the same whether it occurs in one step or several steps, because enthalpy is a state function.

19. Give the Gibbs free energy equation and the spontaneity criterion.

    Delta G = Delta H - T.Delta S. A process is spontaneous when Delta G < 0, at equilibrium when Delta G = 0, non-spontaneous when Delta G > 0.

20. State the second law of thermodynamics in terms of entropy.

    The total entropy of an isolated system (universe) always increases for a spontaneous process: Delta S_universe > 0.

21. State Le Chatelier's principle.

    If a system at equilibrium is disturbed by a change in concentration, pressure or temperature, the equilibrium shifts to counteract the change and re-establish equilibrium.

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