Class XI CBSE Chemistry Model Paper


Class – XI

Time – 3 Hrs. Marks – 70


General Instructions :

i) All questions are compulsory.

ii) Q. s 1 to 8 carry 1 makes each. Answer them in one word or in about on sentence.

iii) Q. s 9 to 18 carry 2 marks each. Answer these in about 30 words each.

iv) Q. s 19 to 27 carry 3 marks each. Answer these in about 40 words each.

v) Q. s 28 to 30 are long answer questions carrying 5 marks each.

vi) Use long table if necessary, use of calculator is not permitted.


1. Write IUPAC name of the following compound : 1


2. Write down the formula of the monomer of silicone. 1

3. What would be the effect of increasing pressure on the equilibrium. 1

PCl5 (g) = Pcl3 (g) + Cl2 (g) ?

4. What is the oxidation number of oxygen in Na2O2 ? 1

5. What would be the sign of S for the process 2H (g) à H2 (g) ? 1

6. What is compressibility factor of a gas ? 1

7. Configuration of ion M+2 is Is2 2s2 2p5 what is configuration of atom M? 1

8. How many oxygen atoms would be there in 1 mole of H2SO4 ?

9. clip_image004 a) What is the hybridization of each carbon in CH3 – CH2 ? 1

b) What is the function of AlCl3 (anhyd) in Friedel Crafts reaction ? 1

10. How N and S are detected when present in an organic compound together ? (Reaction only) 2


Which is the electrophillic centre in CH3Br and why ?

11. Why lithium does not form a superoxide but potassium does ? 2


Why BeSO4 is water soluble but BaSO4 is not ?

12. Balance the following redox feaction by ion 2

Electron method :

Cr2 O7-2 + Fe+2 à Fe+3 + Cr+3 in acidic medium.

13. a) What is the change in internal energy in a process in which 700J of heat is absorbed and 450J of work is done by the system ?

b) Define a spontaneous process in terms of Gibbs energy. 1

14. Show by MO concept which one out of O2 and O2+ would be more stable. 2


Explain all the orbital overlaps in a molecule of ethene (C2H4) by drawing a sutitable diagram.

15. Calculate the mass of (NH4)2 S required to prepare 200 ml of O.1 molar aqueous solution.

(N = 14, H = 1, S = 32)

16. a) Write down the IUPAC name and symbol of the element with at no 119. 1

b) Why Cl has more negative electron gain enthalpy then F in group 17 ? 1

17. Arrange the species : F, O-2, N-3, Mg + 2, Al + 3 and Na+ in the increasing order of ionic radii and give reason. 2

Chemistry Syllabus for AIPMT 2011


Unit : 1 Some basic concepts in Chemistry

Importance of Chemistry, physical quantities and their measurement in Chemistry, SI Units, uncertainty in measurements and use of significant figures, Unit and dimensional analysis, Matter and its nature,laws of chemical combinations, atomic, and molecular, masses mole concept, molar masses, percentage composition and molecular formula, chemical stoichiometry.

Unit : 2 States of matter

Three states of matter, gaseous state, gas laws (Boyle’s Law and Charles Law), Avogadro’s Law, Grahams’Law of diffusion, Dalton’s law of partial pressure, ideal gas equation, Kinetic theory of gases, real gases and deviation from ideal behaviour, van der Waals’ equation, liquefaction of gases and critical points, Intermolecular forces; liquids and solids.

Unit : 3 Atomic structure

Earlier atomic models (Thomson’s and Rutherford) , emission spectrum of hydrogen atom, Bohr’s model, of hydrogen atom, Limitations of Bohr’s model, dual nature of matter and radiation, Heisenberg uncertainty principle, quantum mechanical model of atom (quantum designation of atomic orbitals and electron energy in terms of principal, angular momentum and magnetic quantum numbers), electronic spin and spin quantum numbers, Pauli’s exclusion principle, general idea of screening (constants) of outer electrons by inner electrons in an atom, Aufbau principle, Hund’s rule, atomic orbitals and their pictorial representation, electronic configurations of elements.

Unit : 4 Classification of elements and periodicity in properties

Need and genesis of classification of elements (from Doebereiner to Mendeleev), Modern periodic law and present form of periodic table, Nomenclature of elements with atomic number > 100, electronic configurations of elements and periodic table, electronic configuration and types of elements and s, p, d and f blocks, periodic trends in properties of elements (atomic size, ionization enthalpy, electron gain enthalpy, valence/ oxidation states and chemical reactivity).

Unit : 5 Chemical energetics

Some basic concepts in thermodynamics, first law of thermodynamics, heat capacity, measurement ofDU and DH, calorimetry, standard enthalpy changes, thermochemical equations, enthalpy changes during phase transformations, Hess’s Law, standard enthalpies of formation, bond enthalpies and calculations based on them.

Unit : 6 Chemical bonding

Kossel -Lewis approach to chemical bond formation, ionic bonds, covalent bonds, polarity of bonds and concept of electronegativity, valence shell electron pair repulsion (VSEPR) theory , shapes of simple molecules, valence bond theory, hybridization involving s, p and d orbitals and shapes of molecules sand p bonds; Molecular orbital theory involving homounclear diatomic molecules; Hydrogen-bonding.

Unit : 7 Equilibrium

Equilibrium in physical and chemical processes

Equilibrium in physical and chemical processes, dynamic equilibrium, law of chemical equilibrium and equilibrium constant, homogeneous equilibrium, heterogenous equilibrium, application of equilibrium constants, Relationship between reaction quotient Q, equilibrium constant, K and Gibbs’ energy G; factors affecting equilibrium-Le Chateliar’s principle.

Ionic equilibrium

Acids, Bases and Salts and their ionization, weak and strong electrolytes degree of ionization and ionization constants, concept of pH, ionic product of water, buffer solution, common ion effect, solubility of sparingly soluble salts and solubility products.

Unit : 8 Redox reactions