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KEAM Physical and Inorganic Chemistry Syllabus

The Physical and Inorganic Chemistry syllabus for KEAM in full: 5 chapters, 18 topics and 50 sub-topics, every one listed below, plus 51 Physical and Inorganic Chemistry flashcards with answers.

5Chapters

18Topics

50Sub-topics

51Flashcards

Physical and Inorganic Chemistry syllabus: all 5 chapters

Expand any chapter to see its topics and sub-topics.

Basic Concepts and Atomic Structure
3 topics
- Some Basic Concepts of Chemistry
  - Mole concept and molar mass
  - Stoichiometry and limiting reagent
  - Empirical and molecular formulae
- Structure of Atom
  - Bohr model and atomic spectra
  - Quantum numbers and orbitals
  - Electronic configuration and Hund's rule
- Classification of Elements and Periodicity
  - Modern periodic law and trends
  - Ionization enthalpy, electronegativity, atomic radius
Chemical Bonding and States of Matter
3 topics
- Chemical Bonding and Molecular Structure
  - Ionic and covalent bonding
  - VSEPR theory and hybridisation
  - Molecular orbital theory and hydrogen bonding
- States of Matter
  - Gas laws and ideal gas equation
  - Kinetic molecular theory
  - Real gases and van der Waals equation
- The Solid State
  - Crystal lattices and unit cells
  - Packing efficiency and density
  - Defects and electrical/magnetic properties
Physical Chemistry: Energetics and Dynamics
4 topics
- Thermodynamics
  - First law, enthalpy and Hess's law
  - Entropy and Gibbs free energy
  - Spontaneity criteria
- Equilibrium
  - Law of mass action and Kc, Kp
  - Le Chatelier's principle
  - Ionic equilibrium, pH and buffers
- Chemical Kinetics
  - Rate law and order of reaction
  - Integrated rate equations
  - Arrhenius equation and collision theory
- Solutions
  - Concentration terms and Raoult's law
  - Colligative properties
  - Van't Hoff factor and abnormal molar mass
Electrochemistry and Redox
3 topics
- Redox Reactions
  - Oxidation number and balancing
  - Redox titrations
- Electrochemistry
  - Galvanic cells and electrode potential
  - Nernst equation and EMF
  - Conductance and electrolysis
- Surface Chemistry
  - Adsorption and catalysis
  - Colloids and emulsions
Inorganic Chemistry of Elements
5 topics
- Hydrogen and s-Block Elements
  - Hydrogen, water and hydrides
  - Alkali metals and their compounds
  - Alkaline earth metals
- The p-Block Elements
  - Group 13 to 18 trends
  - Compounds of boron, carbon and nitrogen
  - Oxygen, halogen and noble gas chemistry
- The d- and f-Block Elements
  - Transition metal properties and oxidation states
  - Lanthanoids and actinoids
- Coordination Compounds
  - Werner's theory and nomenclature
  - Isomerism in coordination compounds
  - Valence bond and crystal field theory
- Metallurgy and Environmental Chemistry
  - Principles of isolation of metals
  - Thermodynamic and electrochemical principles
  - Environmental pollution

KEAM Physical and Inorganic Chemistry flashcards — 51 questions with answers

State the law of conservation of mass.
Matter can neither be created nor destroyed in a chemical reaction; the total mass of reactants equals the total mass of products.
What is the difference between molarity (M) and molality (m)?
Molarity = moles of solute per litre of solution (temperature-dependent). Molality = moles of solute per kilogram of solvent (temperature-independent).
What is the value of Avogadro's number, and what does it represent?
6.022 x 10^23; the number of particles (atoms, molecules, ions) in one mole of a substance.
Define limiting reagent.
The reactant that is completely consumed first in a reaction, thereby determining the maximum amount of product formed.
Give the de Broglie equation relating wavelength to momentum.
lambda = h / (mv) = h / p, where h is Planck's constant, m is mass, and v is velocity.
State Heisenberg's uncertainty principle as an equation.
Delta-x . Delta-p >= h / (4*pi); position and momentum cannot both be measured exactly at the same time.
What do the four quantum numbers n, l, m, and s represent?
n = principal (shell/energy), l = azimuthal (subshell/shape), m = magnetic (orbital orientation), s = spin (+1/2 or -1/2).
State the Aufbau principle.
Electrons fill orbitals in order of increasing energy, lowest energy orbital first (following the n+l rule).
State Hund's rule of maximum multiplicity.
Electrons occupy degenerate orbitals singly with parallel spins before any orbital is doubly occupied.
What is Pauli's 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.
How does atomic radius vary across a period and down a group?
It decreases across a period (left to right) due to increasing nuclear charge, and increases down a group due to added shells.
Define ionization enthalpy and state its trend in the periodic table.
Energy required to remove the most loosely bound electron from a gaseous atom. It increases across a period and decreases down a group.
Which element has the highest electronegativity, and on what scale?
Fluorine, with a value of 4.0 on the Pauling scale.
State the basis of the modern periodic law.
Physical and chemical properties of elements are a periodic function of their atomic numbers.
What is the shape and hybridization of methane (CH4)?
Tetrahedral shape with sp3 hybridization and a bond angle of 109.5 degrees.
According to VSEPR theory, what shape does a molecule with 3 bond pairs and 1 lone pair (e.g. NH3) adopt?
Trigonal pyramidal (bond angle ~107 degrees).
What is the difference between a sigma bond and a pi bond?
A sigma bond forms by head-on (axial) overlap of orbitals and is stronger; a pi bond forms by sideways (lateral) overlap and is weaker.
State the bond order formula in molecular orbital theory.
Bond order = (number of bonding electrons - number of antibonding electrons) / 2.
Why is O2 paramagnetic according to MO theory?
It has two unpaired electrons in its pi-antibonding (pi*) molecular orbitals.
State the ideal gas equation and define each term.
PV = nRT, where P = pressure, V = volume, n = moles, R = gas constant, T = temperature in Kelvin.

Show the other 31 Physical and Inorganic Chemistry flashcards

State Boyle's law and Charles's law.
Boyle's law: at constant T, V is inversely proportional to P. Charles's law: at constant P, V is directly proportional to absolute T.
State Dalton's law of partial pressures.
The total pressure of a mixture of non-reacting gases equals the sum of the partial pressures of the individual gases.
What are the seven types of crystal systems?
Cubic, tetragonal, orthorhombic, monoclinic, triclinic, hexagonal, and rhombohedral (trigonal).
What is the packing efficiency and coordination number of an FCC unit cell?
Packing efficiency = 74%; coordination number = 12.
What is the difference between Schottky and Frenkel defects?
Schottky: equal numbers of cations and anions are missing (decreases density). Frenkel: an ion is displaced to an interstitial site (density unchanged).
State the first law of thermodynamics.
Delta-U = q + w; energy of an isolated system is constant (energy can be transferred as heat or work but not created or destroyed).
Define enthalpy (H) and write its relation to internal energy.
H = U + PV; enthalpy is the heat content of a system at constant pressure.
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, depending only on initial and final states.
Write the Gibbs free energy equation and the condition for spontaneity.
Delta-G = Delta-H - T*Delta-S; a process is spontaneous when Delta-G is negative.
State Le Chatelier's principle.
When a system at equilibrium is disturbed (change in concentration, pressure, or temperature), it shifts to counteract the change and re-establish equilibrium.
Write the relationship between Kp and Kc.
Kp = Kc(RT)^(delta-n), where delta-n = moles of gaseous products - moles of gaseous reactants.
What is the ionic product of water (Kw) at 25 degrees C?
Kw = [H+][OH-] = 1.0 x 10^-14 mol^2/L^2.
State the Henderson-Hasselbalch equation for an acidic buffer.
pH = pKa + log([salt]/[acid]).
What is the difference between order and molecularity of a reaction?
Order is experimentally determined (sum of exponents in rate law) and can be fractional/zero; molecularity is the number of reacting species in an elementary step and is always a whole number.
Write the integrated rate law and half-life for a first-order reaction.
k = (2.303/t) log([A0]/[A]); half-life t(1/2) = 0.693/k (independent of initial concentration).
State the Arrhenius equation.
k = A*e^(-Ea/RT), where A is the frequency factor, Ea is activation energy, R is the gas constant, and T is temperature.
State Raoult's law for a solution of a non-volatile solute.
The relative lowering of vapour pressure equals the mole fraction of the solute: (P0 - P)/P0 = x(solute).
What are colligative properties? Name them.
Properties depending only on the number of solute particles, not their nature: relative lowering of vapour pressure, elevation of boiling point, depression of freezing point, and osmotic pressure.
Write the formula for osmotic pressure.
pi = CRT = (n/V)RT, where C is molar concentration, R is the gas constant, and T is temperature.
Define oxidation and reduction in terms of electron transfer.
Oxidation is loss of electrons (increase in oxidation number); reduction is gain of electrons (decrease in oxidation number).
State the Nernst equation for an electrode at 298 K.
E = E0 - (0.0591/n) log Q, where n is the number of electrons transferred and Q is the reaction quotient.
State Faraday's first law of electrolysis.
The mass of substance deposited at an electrode is directly proportional to the quantity of electric charge passed (m proportional to Q = It).
How does molar conductivity vary with dilution for strong and weak electrolytes?
It increases with dilution for both; for strong electrolytes the increase is small, while for weak electrolytes it increases sharply near infinite dilution due to greater dissociation.
What is the difference between physisorption and chemisorption?
Physisorption involves weak van der Waals forces (reversible, low enthalpy); chemisorption involves chemical bonds (irreversible, high enthalpy, specific).
Why are arsenic-doped (group 15) silicon crystals n-type and boron-doped (group 13) ones p-type?
Group 15 dopants add extra electrons giving n-type; group 13 dopants create electron holes giving p-type semiconductors.
Why does the s-block element's reactivity increase down the group?
Atomic size increases and ionization enthalpy decreases down the group, so the outer s-electron(s) are lost more easily, increasing reactivity.
What is the diagonal relationship, with one example pair?
Similarity in properties between an element and the element diagonally below-right in the next group, e.g. Lithium and Magnesium.
Why does the d- and f-block show variable oxidation states?
Because the energies of (n-1)d and ns orbitals are close, allowing both to participate in bonding, giving multiple stable oxidation states.
State Werner's coordination theory definitions of primary and secondary valencies.
Primary valency = ionizable oxidation state satisfied by negative ions; secondary valency = non-ionizable coordination number satisfied by ligands.
What is the IUPAC name of the [Cu(NH3)4]2+ ion's ligand and the geometry of [Ni(CN)4]2-?
The ligand NH3 is named ammine; [Ni(CN)4]2- is square planar (dsp2 hybridization).
Name the metallurgical processes: removing gangue using a frothing agent, and reducing oxide ore with carbon.
Concentration by froth flotation; reduction by smelting (carbon reduction in a blast furnace).

KEAM Physical and Inorganic Chemistry FAQ

What is in the KEAM Physical and Inorganic Chemistry syllabus?

KEAM Physical and Inorganic Chemistry is split into 5 chapters: Basic Concepts and Atomic Structure, Chemical Bonding and States of Matter, Physical Chemistry: Energetics and Dynamics, Electrochemistry and Redox and Inorganic Chemistry of Elements. Together they contain 18 topics and 50 sub-topics.

How many chapters are in KEAM Physical and Inorganic Chemistry?

5 chapters, containing 18 topics and 50 sub-topics. The largest chapter is Inorganic Chemistry of Elements, with 5 topics.

Are there flashcards for KEAM Physical and Inorganic Chemistry?

Yes — a 51-card Physical and Inorganic Chemistry deck, printed in full in the flashcards section of this page and available in the Examius app with spaced repetition. The free plan covers one exam of your choice, including its flashcards; Examius Pro, a one-time purchase, unlocks every other exam and deck.