Federal Public Service Commission (FPSC) Competitive Examination for Recruitment to BPS-17 Posts under the Federal Government
Time Allowed: 3 Hours
MAXIMUM MARKS: 100 Marks
CHEMISTRY, PAPER-I
PART-II
Attempt FIVE questions in all, Including Questions No.1 which is COMPULSORY, All questions carry EQUAL marks.
Q. No. 2. (a) What are zeolites and how can they be synthesized? Give some important applications of zeolites. (07) (b) Explain the significance of the quantum mechanical wave function. Also enlist properties of a well-behaved wave function. (07) (c) Write some important chemical properties of Cl₂. Also give its general and industrial applications. (06)
Q. No. 3. (a) How are human activities in urban areas responsible for air pollution? What measures should be taken to minimize air pollution? (07) (b) With suitable examples, differentiate between internal energy change and enthalpy change. Under what conditions do the two quantities have almost the same value? (07) (c) Explain the dissociation of weak acids. How can the dissociation constant be determined using conductance measurements? (06)
Q. No. 4. (a) Many transition element complexes (TECs) exhibit their characteristic spectra in the visible region. Give a detailed account of factors which affect or modify the spectra of the TECs. (07) (b) Explain the synthesis of cement; also draw a flow-chart diagram to show the significant steps. (07) (c) Explain the significance of the Gibbs expression. How can the ΔG value be utilized to predict the occurrence of a chemical reaction? (06)
Q. No. 5. (a) How does silver exist in nature? What shapes of compounds are formed by Ag(I) with different ligands? (07) (b) Elaborate on the common and different features of H₂ and H₂⁺ molecules according to the pertinent molecular orbital theory. (07) (c) Enlist different oxyacids of N and P. Also explain differences in their behavior. (06)
Q. No. 6. (a) Derive Schrödinger’s wave equation for a particle of mass ‘m’ confined in a one-dimensional box of length ‘l’. Also give a relationship for the zero-point energy. (07) (b) Define the 2nd law of thermodynamics. How can the entropy change become an indicator for the spontaneity of a process? (07) (c) How can the shapes of transition element complexes (TECs) be explained on the basis of some typical hybridization by the central ion? (06)
Q. No. 7. (a) Describe the functioning of a typical Fuel Cell (FC). What is the role of membrane equilibria in the FC? (07) (b) What is the origin of magnetic properties in the complexes of transition elements? Give some factors on which magnetic properties may depend. (07) (c) With suitable examples of multi-electron atoms, elaborate on the Aufbau principle in the light of Pauli’s exclusion principle and Hund’s rule. (06)
Q. No. 8. (a) ‘Debye-Hückel theory (D-HT) works under limiting conditions’. Elaborate the statement with examples. Also give the significance of D-HT. (07) (b) What are transition elements? Give a generalized account of the physical and chemical characteristics of transition elements. (07) (c) With the electrochemical reactions that take place at the two electrodes, describe the ‘electrolysis of aqueous solutions’. (06)
CHEMISTRY, PAPER-II
Attempt FIVE questions in all, Including Questions No.1 which is COMPULSORY, All questions carry EQUAL marks.
PART-II
Q. No. 2. Define the following terms: (2 x 10 = 20) (a) Catalytic cracking (b) Catalytic reforming (c) Fermentation (d) Alkylation (e) Antibiotics (f) Plastic (g) Surfactant (h) Unit operation (i) Unit Process (j) Emulsion polymerization
Q. No. 3. (a) Explain the following with suitable examples: (2 x 7 = 14) (a) Partition Coefficient (b) Surface tension (c) Viscosity (d) Colloidal solution (e) Emulsions (f) Nanoparticles (g) Baeyer’s strain theory (b) Give one example (with structure) of each of the following: (2 x 3 = 06) (a) s – sp hybridization (b) sp² – sp² hybridization (c) sp – sp² hybridization
Q. No. 4. (a) What do you mean by Chemiluminescence? Explain with examples. (07) (b) Arrange the following functional groups in decreasing order of stability of carbocations: (05) (CH₃)₃C⁺, CH₃⁺, CH₃CH₂⁺, (CH₃)₂CH⁺, CH₂=CH–CH₂⁺, C₆H₅CH₂⁺ (c) Explain the following terms: (05) (a) Standard solution (b) Molar solution (c) Molal solution (d) Formal Solution (e) Normal solution (d) How many grams of KOH are in 600 mL of 0.450 M KOH solution? (03)
Q. No. 5. Give one representative example of each of the following reactions. Give the complete equation and label it: (2 x 10 = 20) (a) Wittig reaction (b) Oxidation of 1° and 2° alcohols (c) Friedel-Crafts alkylation (d) Hydration of Alkenes (e) Glycol cleavage (f) Ozonolysis (g) Tollen’s test (h) Propagation reaction (i) S_N1 reaction (j) Condensation polymerization
Q. No. 6. (a) What are wetting agents and for what purpose are they used? (10) (b) Describe briefly the alternatives used instead of the hydrogenation of vegetable oils for the formation of vegetable Ghee. (05) (c) Give a laboratory test to differentiate between unsaturated and saturated molecules. (05)
Q. No. 7. (a) What approaches are followed to rule out keto-enol tautomerism? Draw the tautomerism exhibited by acetone and acetoacetic ester. (10) (b) Explain the industrial preparation of Gels. Explain their use in medicine and cosmetics. (10)
Q. No. 8. (a) Draw the structures of the following molecules: (10) (a) Cyclohex-3-en-1-one (b) Cyclohexanecarbaldehyde (c) Hexadecane (d) 3-methyl-1-butene (e) 4-bromo-3-methyl-1-butene (f) 4-ethenylcyclohexanol (g) 2-methyl-3-buten-1-ol (h) 6-ethyl-1-methylcyclohexene (i) 2-amino-3-phenylpropanoic acid (j) 2-formyl-4-oxocyclohexanecarboxylic acid (b) Name the structural configurations provided above according to the IUPAC/common system of nomenclature. (10)
