Every student wants to take admission in Top Engineering Colleges like Indian Institute of Technology (IITs), National Institutes of Technology (NITs), Indian Institute of Information Technology (IIITs) and other Government Funded Technical Institutes (GFTIs). To take admission in these reputed colleges students will have to crack JEE Examination 2018. It is one of the toughest entrance examinations of India. It is a two phase examination i.e., JEE Main and JEE Advanced. After qualifying JEE Main Examination students have to appear for JEE Advanced Examination. JEE Advanced Examination consists of two papers i.e., Paper 1 and Paper 2 with 54 questions in each paper. There are only few months left for JEE Advanced Examination 2018. The most important thing to boost the preparation of all aspirants is the latest syllabus. In this article, we bring to you the latest syllabus of Chemistry for JEE Advanced Examination 2018. This will give you the detailed information about all the topics of Chemistry like Atomic structure and chemical bonding, Gaseous and liquid states, Chemical equilibrium and so on.
1. General topics:
Concept of atoms and molecules; Dalton’s atomic theory; Mole concept; Chemical formulae; Balanced chemical equations; Calculations (based on mole concept) involving common oxidation-reduction, neutralisation, and displacement reactions; Concentration in terms of mole fraction, molarity, molality and normality
2. Gaseous and liquid states:
Absolute scale of temperature, ideal gas equation; Deviation from ideality, van der Waals equation; Kinetic theory of gases, average, root mean square and most probable velocities and their relation with temperature; Law of partial pressures; Vapour pressure; Diffusion of gases
3. Atomic structure and chemical bonding:
Bohr model, spectrum of hydrogen atom, quantum numbers; Wave-particle duality, de Broglie hypothesis; Uncertainty principle; Qualitative quantum mechanical picture of hydrogen atom, shapes of s, p and d orbitals; Electronic configurations of elements (up to atomic number 36); Aufbau principle; Pauli’s exclusion principle and Hund’s rule; Orbital overlap and covalent bond; Hybridisation involving s, p and d orbitals only; Orbital energy diagrams for homonuclear diatomic species, Hydrogen bond; Polarity in molecules, dipole moment (qualitative aspects only); VSEPR model and shapes of molecules (linear, angular, triangular, square planar, pyramidal, square pyramidal, trigonal bipyramidal, tetrahedral and octahedral)
First law of thermodynamics; Internal energy, work and heat, pressure-volume work; Enthalpy, Hess’s law; Heat of reaction, fusion and vapourization; Second law of thermodynamics; Entropy; Free energy; Criterion of spontaneity
Law of mass action; Equilibrium constant, Le Chatelier’s principle (effect of concentration, temperature and pressure); Significance of ΔG and ΔG0 in chemical equilibrium; Solubility product, common ion effect, pH and buffer solutions; Acids and bases (Bronsted and Lewis concepts); Hydrolysis of salts.