InstaQB - Edit Syllabus

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Basic Concepts of Chemistry and Chemical Calculations

<ul>
	<li>explain the importance of chemistry in different spheres of life.</li>
	<li> classify different substances into elements, compounds and mixtures.</li>
	<li> define atomic mass and molecular mass.</li>
	<li> define the amount of substance using SI unit 'mole'.</li>
	<li> describe Avogadro number.</li>
	<li> explain the relationship among mass, moles and number of atoms (or) molecules and perform calculations relating to the conversions.</li>
	<li> define equivalent mass and calculate equivalent mass of acid, base and oxidising/reducing agents.</li>
	<li> deduce empirical and molecular formula of a compound from experimental data.</li>
	<li> solve numerical problems based on stoichiometric calculations.</li>
	<li> identify the limiting reagent and calculate the amount of reactants and products in a reaction.</li>
	<li> define the terms oxidation, reduction, oxidant and reductant.</li>
	<li>predict the oxidation states of elements in various compounds.</li>
	<li>explain the process involved in a redox reaction and describe the electron transfer process.</li>
	<li> classify redox reactions into different types.</li>
	<li> formulate a balanced redox reaction from two half-reactions.</li>
</ul>

Quantum Mechanical Model of Atom

<ul>
	<li>Recognise various atomic models</li>
	<li> Explain the dual behaviour of matter</li>
	<li> Derive de Broglie equation and solve numerical problems</li>
	<li> Explain Heisenberg’s uncertainty principle and solve related problems</li>
	<li> Appreciate the signifi cance of quantum numbers</li>
	<li> Summarise important features of quantum mechanical model of atom</li>
	<li> Draw the shapes of various atomic orbitals</li>
	<li> Explain the Aufb au principle</li>
	<li> Describe Hund's rule and Pauli’s exclusion principle</li>
	<li>Apply the relevant rules for fi lling electrons in atoms and write the electronic confi guration of various atoms</li>
</ul>

Periodic Classification Of Elements

<ul>
	<li>recognise the development of the periodic table</li>
	<li> explain the work of Mosley's and modern periodic law</li>
	<li> outline the concept of grouping elements</li>
	<li> name the elements with atomic number greater than 100 using IUPAC nomenclature</li>
	<li> classify the elements into s, p, d and f blocks</li>
	<li> recognise the periodic trends and describe qualitatively the variation in periodic properties such as atomic radius, ionisation energy etc.</li>
	<li> explain the anomalies in the expected trend in the periodic properties</li>
	<li>calculate the effective nuclear charge using Slater's rule</li>
	<li> calculate the ionic radius using Pauling's method</li>
	<li> predict the probable position for a given element in the periodic table</li>
	<li> explain the anomalous properties of second period elements and the diagonal relationship</li>
</ul>

Hydrogen

<ul>
	<li>Justify the position of hydrogen in the periodic table</li>
	<li>Recognise the different isotopes of hydrogen</li>
	<li> Explain the methods of preparation of hydrogen.</li>
	<li> Explain the properties of hydrogen</li>
	<li> Appraise the uses of hydrogen</li>
	<li> Differentiate various types of hydrides</li>
	<li> Translate the knowledge of structure of water for explaining its physical and chemical properties</li>
	<li> Differentiate hard and soft water and select the suitable method for water softening.</li>
	<li> Recognise heavy water and explain its properties.</li>
	<li> Explain the preparation and properties of hydrogen peroxide</li>
	<li> List the uses of hydrogen peroxide</li>
</ul>

Alkali and Alkaline Earth Metals

<ul>
	<li>Explain the properties of alkali metals and alkaline earth metals</li>
	<li> Recognise the anomalous properties of Li and Be</li>
	<li> List the uses of alkali metals and alkaline earth metals</li>
	<li> Describe the general characteristics of compounds of alkali metals and alkaline earth metals</li>
	<li>Appreciate the biological importance of sodium and potassium, Magnesium and Calcium</li>
	<li> Explain the preparation, properties and uses of calcium oxide, calcium hydroxide, gypsum and plaster of paris.</li>
</ul>

Gaseous State

<ul>
	<li>State the laws governing an ideal gas</li>
	<li> Demonstrate gas laws in various real life situations</li>
	<li> Derive ideal gas equation and perform calculations using it.</li>
	<li> State the deviations from ideal behavior</li>
	<li> Derive van der Waals equation.</li>
	<li> Define Graham's law of diffusion</li>
	<li> Define compressibility factor</li>
	<li> Explain critical phenomena</li>
	<li> Derive critical constants in terms of van der Waal's constants</li>
	<li> Explain Andrew's isotherms of carbon dioxide</li>
	<li> Describe Joule – Thomson effect and liquefaction of gases.</li>
</ul>

Thermodynamics

<ul>
	<li>distinguish between the system and surroundings</li>
	<li> define closed, open and isolated systems</li>
	<li> distinguish between state and path functions</li>
	<li> describe the relation between internal energy, work and heat</li>
	<li> state four laws of thermodynamics</li>
	<li> correlate internal energy change (ΔU) and enthalpy change (ΔH)and their measurement.</li>
	<li> calculate enthalpy changes for various types of reactions</li>
	<li> apply Hess’s law to calculate lattice energy of crystals</li>
	<li>define spontaneous and non spontaneous processes</li>
	<li> establish the relationship between thermodynamic state functions enthalpy (H), entropy (S) and Gibbs free energy (G)</li>
	<li> list the factors that determines spontaneity of the process</li>
	<li>establish the link between ΔG and spontaneity, and the relationship between ΔG0 and equilibrium constant</li>
</ul>