IAT 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 IAT, not a summary of it.

1. 1

   Some Basic Concepts of Chemistry

   3 topics

   • Mole Concept
   • Laws of Chemical Combination
   • Stoichiometry
2. 2

   Structure of Atom

   2 topics

   • Atomic Models
   • Quantum Mechanical Model of Atom
3. 3

   Classification of Elements and Periodicity in Properties

   2 topics

   • Modern Periodic Table
   • Periodic Trends
4. 4

   Chemical Bonding and Molecular Structure

   3 topics

   • Ionic Bond
   • Covalent Bond
   • Molecular Orbital Theory
5. 5

   States of Matter: Gases and Liquids

   2 topics

   • Gas Laws
   • Kinetic Theory of Gases
6. 6

   Thermodynamics

   3 topics

   • First Law of Thermodynamics
   • Enthalpy
   • Entropy
7. 7

   Equilibrium

   2 topics

   • Equilibrium in Physical and Chemical Processes
   • Ionic Equilibrium
8. 8

   Redox Reactions

   2 topics

   • Oxidation and Reduction
   • Electrochemical Cells
9. 9

   Hydrogen

   2 topics

   • Properties of Hydrogen
   • Hydrides
10. 10

    s-Block Elements

    2 topics

    • Group 1 Elements
    • Group 2 Elements
11. 11

    Some p-Block Elements

    2 topics

    • Group 13 Elements
    • Group 14 Elements
12. 12

    Organic Chemistry - Some Basic Principles and Techniques

    3 topics

    • Classification of Organic Compounds
    • Nomenclature
    • Isomerism
13. 13

    Hydrocarbons

    4 topics

    • Alkanes
    • Alkenes
    • Alkynes
    • Aromatic Hydrocarbons
14. 14

    Environmental Chemistry

    1 topic

    • Environmental Pollution

Chemistry flashcards for IAT

21 of 61 cards from the Chemistry deck — real questions with worked answers.

1. What is the mole concept, and how many entities are in one mole (Avogadro's number)?

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

2. How is the number of moles calculated from mass and from number of particles?

   Moles (n) = given mass / molar mass = number of particles / 6.022 x 10^23. For gases at STP, n = volume / 22.4 L.

3. State the Law of Conservation of Mass.

   In a chemical reaction, matter is neither created nor destroyed; the total mass of reactants equals the total mass of products.

4. State the Law of Definite (Constant) Proportions and the Law of Multiple Proportions.

   Definite Proportions: a given compound always contains the same elements in the same fixed mass ratio. Multiple Proportions: when two elements form more than one compound, the masses of one element combining with a fixed mass of the other are in small whole-number ratios.

5. In stoichiometry, what is the limiting reagent and how does it control product yield?

   The limiting reagent is the reactant completely consumed first; it limits the amount of product formed. The other reactants are in excess. Product amounts are calculated from the moles of the limiting reagent using the balanced equation's mole ratios.

6. Define empirical formula and molecular formula, and give their relationship.

   Empirical formula shows the simplest whole-number ratio of atoms; molecular formula shows the actual number of atoms in a molecule. Molecular formula = n x empirical formula, where n = molar mass / empirical formula mass.

7. What were the main postulates of Dalton's atomic theory?

   Matter consists of indivisible atoms; atoms of an element are identical in mass and properties; atoms of different elements differ; compounds form from atoms combining in fixed whole-number ratios; atoms are rearranged (not created/destroyed) in reactions.

8. What did Rutherford's gold foil experiment conclude about atomic structure?

   The atom has a tiny, dense, positively charged nucleus containing most of its mass, with electrons surrounding it; the atom is mostly empty space (most alpha particles passed straight through).

9. What is the main limitation of Bohr's model of the atom?

   It explained the hydrogen spectrum but failed for multi-electron atoms, could not explain fine spectral splitting (Zeeman/Stark effects), and violated the Heisenberg uncertainty principle by assuming fixed orbits with defined position and momentum.

10. State the Heisenberg Uncertainty Principle.

    It is impossible to simultaneously determine the exact position and momentum of an electron. Mathematically, Δx · Δp ≥ h/4π.

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

    Principal (n): shell/energy & size. Azimuthal (l): subshell/shape (0=s,1=p,2=d,3=f). Magnetic (m_l): orbital orientation (-l to +l). Spin (m_s): electron spin (+1/2 or -1/2).

12. State the Aufbau principle, Pauli exclusion principle, and Hund's rule.

    Aufbau: electrons fill lowest-energy orbitals first. Pauli: no two electrons in an atom have all four quantum numbers identical (an orbital holds max 2 electrons with opposite spins). Hund: degenerate orbitals are each singly filled before pairing, all with parallel spins.

13. On what basis is the modern periodic table arranged, and what is the modern periodic law?

    Elements are arranged in order of increasing atomic number. Modern periodic law: the physical and chemical properties of elements are periodic functions of their atomic numbers.

14. What are the s, p, d, and f blocks in the periodic table?

    s-block: groups 1-2 (last electron in s). p-block: groups 13-18 (last electron in p). d-block: groups 3-12, transition metals (d orbitals filling). f-block: lanthanides and actinides (f orbitals filling).

15. How do atomic radius and ionization enthalpy vary across a period and down a group?

    Across a period (left to right): atomic radius decreases, ionization enthalpy increases. Down a group: atomic radius increases, ionization enthalpy decreases.

16. How do electronegativity and metallic character vary across a period and down a group?

    Across a period: electronegativity increases, metallic character decreases. Down a group: electronegativity decreases, metallic character increases.

17. What is an ionic bond, and name a key factor favoring its formation.

    An ionic bond is the electrostatic force of attraction between oppositely charged ions formed by complete transfer of electrons from a metal to a non-metal. It is favored by low ionization energy of the metal, high electron affinity of the non-metal, and high lattice energy.

18. What is lattice enthalpy, and how does it relate to ionic compound stability?

    Lattice enthalpy is the energy released when one mole of an ionic solid forms from its gaseous ions. Higher lattice enthalpy (favored by higher ionic charge and smaller ionic size) means a more stable, harder, higher-melting ionic compound.

19. What is a covalent bond, and how do sigma and pi bonds differ?

    A covalent bond forms by sharing electron pairs between atoms. A sigma (σ) bond forms by head-on (axial) overlap of orbitals and is stronger; a pi (π) bond forms by sideways (lateral) overlap and is weaker. A single bond is one σ; a double bond is one σ + one π.

20. What does VSEPR theory predict, and what shapes correspond to 2, 3, and 4 bonding pairs?

    VSEPR predicts molecular geometry by minimizing repulsion between electron pairs around the central atom. 2 pairs = linear (180°), 3 = trigonal planar (120°), 4 = tetrahedral (109.5°).

21. In Molecular Orbital Theory, how is bond order calculated and what does it indicate?

    Bond order = (number of bonding electrons − number of antibonding electrons) / 2. A higher bond order means a stronger, shorter bond; bond order of zero means the molecule does not exist.

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