Inter (Part-I) Faisalabad Board 2016
Chemistry
Part I (Objective Type)
Time Allowed: 20 Minutes 
Max. Marks: 17

Note: You have four choices for each objective type question as A, B, C and D. The choice which you think is correct; fill that circle in front of that question number. Use marker or pen to fill the circles. Cutting or filling two or more circles will result in zero mark in that question.

Question #1
Circle the correct option i.e. A/B/C/D. Each part carries one mark.

• Orbitals having same energy are called:

(a) Hybrid orbitals
(b) Degenerate orbitals
(c) Valence orbitals
(d) Pure orbitals

• The element which has maximum number of unpaired electron is:

(a) Cr₂4
(b) Ca₂0
(c) Fe₂6
(d) Cu₂

• The highest value of lattice energy which one of these ionic compound has:

(a) NaI
(b) NaF
(c) NaBr
(d) NaCl

• Acetone and chloroform are soluble in each other due to:

(a) Intermolecular hydrogen bonding
(b) Ion dipole interaction
(c) Instantaneous dipole
(d) London dispersion forces

• The sum of mole fraction of gases in a mixture of gases is:

(a) Always more than
(b) Always less than
(c) May be less or more than
(d) Always

• The pair of gases which does not obey Dalton's law of partial pressure under normal condition is:

(a) H₂ and O₂
(b) H₂ and He
(c) NH₃ and HC1
(d) He and Ne

• The comparative rates at which the solutes move in paper chromatography, depend on:

(a) Rf values of solutes
(b) The size of paper
(c) Size of chromatographic tank used
(d) Temperature of the experiment

• The largest number of molecules are present in:

(a) 5.4g of N₂O₅
(b) 2.8g of CO
(c) 4.8g of C₂H₅OH
(d) 3.6g of H₂O

• Which is not a molecular ion?

(a) He 
(b) CH
(c) NH
(d) CO⁺

• The order of decomposition of nitrogen pentoxide is:

(a) First order 
(b) Second order
(c) Third order
(d) Zero order

• Stronger the oxidizing agent, greater is the:

(a) Oxidation potential
(b) Reduction potential
(c) Redox potential
(d) E.M.F of cell

• 18g glucose is dissolved in 90g of water. The relative lowering of vapour pressure is:

(a) 1.51
(b) 5.1
(c) 6
(d) 5

• Which aqueous solution has highest pH?

(a) 0.1M NaOH
(b) 0.1M H₂ SO₄
(c) 0.1M HCE
(d) 0.2M HNO₃

• An excess of aqueous silver nitrate is added to aqueous barium chloride and precipitate is removed by filtration. What are the main ions in the filtrate?

(b) Ag⁺ ,Ba⁺² & NO₃
(d) Ba⁺² , NO; Sio^-
(a) Al & NO; only
(c) Ba⁺² & NO; only

• The pressure of oxygen inside the bomb calorimeter is:

(a) 100 atm
(b) 50 atm
(c) 25 atm
(d) 20 atm

• The hybridization in ammonia molecule is:

(a) dsp²
(b) sp²
(c) spa
(d) sp

• Which hydrogen halide has the highest percentage of ionic character?

(a) HF
(b) HCl
(c) HBr
(d) HI

Inter (Part-I) Faisalabad Board 2016
Chemistry
Part I (Subjective)
Time Allowed: 2.10 Hours
Max. Marks: 83

Section I

2. Attempt any EIGHT short questions. (8 x 2 = 16)

• Define molecular ion with two examples.
• N₂ and CO have same number of electrons, protons and neutrons. Explain.
• Why actual yield is less than theoretic yield?
• How discoloration of undesirable colors is done for crystals in Crystallization?
• Define chromatography. Give its two uses.
• Convert 37°C into °F. (vii) Define absolute zero.
• Real gases show non ideal behavior due to two assumption of KMT. Explain.
• How value of lc of a reaction helps to predict the direction of a reversible reaction?
• What is the effect of change of pressure on given reaction? N₂(g) + 3H₂(g) 2NH₃(g)
• What is critical solution temperature? Give the critical solution temperature of phenol water system.
• One mole solution of urea is more dilute as compared to its one molar solution. Why?

3. Attempt any EIGHT short questions. (8 x 2 = 16)

• Define dipole-dipole forces with example.
• Define evaporation and name the factors which effect evaporation.
• Define transition temperature with example.
• Why diamond is hard and an electrically insulator?
• Write four properties of positive rays.
• State Aufbau's principle and Hund's rule.
• Why the potential energy of bounded electron has negative value?
• Write down the nuclear reactions involved in the conversion of Cu^- into Zn⁺
• Define molality and give its mathematical formula.
• Define the electrochemical series.
• Why Na and K can displace hydrogen from acids but Pt, Pd and Cu cannot?
• What is the difference between conduction through metals and molten electrolysis?

4. Attempt any SIX short questions. (6 x 2 = 12)

• Bond distance is the compromise distance between atoms. Justify it.
• What is the bond order? Give one example.
• Draw molecular orbital picture of N₂ molecule and also calculate its bond order.
• The dipole moment of CO₂ is zero but that of CO is 0.12 D. Give reason.
• What is non spontaneous reaction? Give two examples.
• Define standard enthalpy of neutralization. Give an example.
• Define activation energy and activated complex.
• What is zero order reaction? Give one example.
• Write two characteristics of a catalyst.

SECTION-II:

Attempt any THREE questions. (8 x 3=24)

Question #5
(a) When limestone (CaCO₃) is roasted, quicklime (CaO) is produced according to the following equation. The actual yield of CaO is 2.5kg, when 4.5kg of limestone is roasted. What is the percentage yield of this reaction? CaCO₃ (,) CaO(g) + CO) (at. mass of Ca = 40, C = 12, 0 = 16)
(b) Explain covalent solids with their properties.

Question #6
(a) State Graham's law of diffusion of gases and give its experimental verification.
(b) Give postulates of Bohr's atomic model.

Question #7
(a) Define hybridization of atomic orbital’s. Also discuss the Hybridization of carbon in Ethene molecule (CH = CH₂).
(b) Explain bomb calorimetric method for the measurement of Enthalpy of a reaction.

Question #8
(a) Calculate the pH of a buffer solution in which 0.11 molar CH₃COONa and 0.09 molar acetic acid solutions are present. Ka for CH3COOH is 1.85 x10-5 .
(b) Describe the construction and working of electrolytic cell.

Question #9
(a) Describe the measurement of depression of freezing point by using Beckmann's freezing point apparatus.
(b) Describe the electrolysis of fused NaCl salts and aqueous solutions of NaCl salts.