CLASS XI CHEMISTRY HOLIDAY HOME WORK 2016

WRITING CHEMICAL FORMULAE

1. Give the formulae of the following radicals

a. bicarbonate

b. hydrogen sulphate

c. nitrate

d. phosphate

e.ammonium ion

f. lead ion

g. silver ion

h. nitrite

i. carbonate

j. magnesium ion

2. Write all the possible formulae of the compounds in the above question and write their names?

3. Convert the following into equations and balance them;

a. magnesium ribbon burns in air to give magnesium oxide

b. lead nitrate on heating decomposes to give lead oxide, nitrogen dioxide and oxygen

c. ethane burns in oxygen to evolve carbon di oxide gas and water vapour

d. iron displaces copper sulphate solution to give ferrous sulphate and copper

e. aqueous barium chloride react with aqueous sodium sulphate to give aqueous sodium choloride and precipitate of barium sulphate.

f. hydrogen sulphide gas combines with sulphur di oxide gas to give water and sulphur.

4. Calculate the molar masses of the following:

a. aluminium chloride

b. potassiumcarbonate

c. bariumsulphate

d.ammoniumhydrogencarbonate

e. butane

f.ethanoic acid

g. ethanol

h. calcium phosphate

i. lithiumbromide

j. sodiumoxide.

5. Calculate the number moles in

a. 0.56 mg of iron

b. 3.55 g chlorine

c. 3.01 x 10 23 atoms of helium

d. 0.32 g oxygen

e. 1.06 mg sodium carbonate

6. round of the following to three significant figures

a. 23.456

b.0.01238

c.15483

d.1.546487

e.01.157962

f.0.0045738

g.1.000456

h.456721.

7. Express the above in scientific notation?

8. Define

a. amu

b. gram molar mass

9. State the following laws

a. Gay Lussac's of combining volumes

b. Avagadro's law

c. Law of definite proportions

d. Law of multiple proportion

10. Give multiples for the following pico, femto, giga , tera, mega, nano , deci, deca, milli.

 

CLASS XII HOLIDAY HOME WORK 2016 chapter CO-ORDINATION COMPOUNDS

CO-ORDINATION COMPOUNDS

1.Write the name and draw the structure of each of the following complex compounds:

a. [Co(NH3)4(H2O)2]Cl3

b. [pt(NH3)4[NiCl4]

2. Illustrate the following with an example each (i) linkage isomerism (ii) co-ordination isomerism (iii) outer orbital complex (iv) bidentate ligand (v) ambident ligand.

3.why is [NiCl4]-2 parmagnetic?

4. Explain how the two complexes of nickel [Ni(CN)4]-2 and [Ni(CO)4] have different structures but do not differ in their magnetic behaviour?

5. Compare the following complexes w.r.t their shape, magnetic behaviour and the hybrid orbitals involved: a. [CoF4]-2 

b. [Cr(H2O)2(C2O4)2]- 

c. [Ni(CO)4]

6.three geometrical isomers are possible for [Co(en)(H2O)2(NH3)2]+2. Draw molecular structures of these three isomers and indicate which one of them is chiral?

why is CO a stronger ligand than Cl-?

7. name the following complexes:

a. [Pt(NH3)4Cl2]Cl2

b. K3[CrF6]

c.[CoCl2(en)2]Cl

d.[Co(en)3]+3

e.[Cr(NH3)5(NCS)][ZnCl4]

f.[Pt(NH2CH3)(NH3)2]Cl

g.K4[Mn(CN)6]

8. Explain crystal field splitting in an octahedral complex?

9. Square

planar complexes of MX2L2 type with co-ordination number 4 exhibit geometrical isomerism, where as tetrahedral complexes with similar co-ordination number do not . Why?
10.State reason for the following:
a. CO is a stronger complexing reagent than NH3.
b. Nickel (II) does not form low spin octahedral complexes.
c. the pi complexes are known for transition metals only.
d. Co+2 is easily oxidised to Co+3 in the presence of strong field ligand
11. Name the following co-ordination entities and draw the structures of their stereo isomers:
a. [Co(en)2Cl]+
b.[Cr(C2O4)3]-3
c.[Co(NH3)3Cl3]

CLASS XII CHEMISTRY HOLIDAY HOME WORK chapter HALO ALKANES AND HALO ARENES

HALO ALKANES AND HALO ARENES

1. What is meant by chirality of a compound? Give an example.

2. Which of the following is easily hydrolysed by KOH and why? CH3CHClCH2CH3 or CH3CH2CH2Cl 

3. Write a chemical test to distinguish between chlorobenzene and benzyl chloride and between chloroform and carbon tetra chloride?

4. Why n\methyl chloride is more easily hydrolysed than chlorobenzene?

5.Which compound in the following couples will react faster towards SN2 displacement and why ?

(a) 1.bromopentane or 2-bromopentane, (b) 1-bromo-2-methylbutane or 2-bromo-2-methylbutane.

6.give one use each of DDT and Iodoform?

7. Draw the structure of the folloeing compounds: 4-bromo-3-methylpet-2-ene , 4-ter.butyl-3-iodoheptane, 1-chloro-4-ethylcyclohexane, 1-chloro-2,2-dimethylpropane.

8. How do you distinguish between SN1 and SN2 reaction  mechanisms? Give one example each.

9. Suggest a possible reason for the following observatins:

a. the order of reactivity of haloalkanes is RI>RCl> RBr.

b. neopentyl chloride does not follow SN2 mahanism.

c. haloalkanes easily dissolve in organic solvents.

10. What is known as racemic mixture? Give an example.

11. Complete the following reactions:

a. C6H5N2Cl + H3PO2 + H2O---------------

b. cyclohexanol + SOCl2-----------------

c. 1-methylcyclohexene + HI--------------

12. Although chlorine is an electron withdrawing group , yet it is ortho-para directing in electrophilic substitution reactins of aromatic compounds. Expain?

CLASS XII CHEMISTRY HOLIDAY HOME WORK 2016 chapter SOLUTIONS

SOLUTIONS

1.An antifreeze solution is prepared from 222.6 g of ethylene glycol C2H4(OH)2 and 200 g of water. calculate the molality of the solution. If density of this solution is 1.072 g/mL what will be the molarity of the solution?

2. A 0.1539 molal aqueous solution of cane sugar ( mol.mass =342 g/mol) has a freezing point of 271 K while the freezing point of pure water is 273.15 K. What will be the freezing point of an aqueous solution of 5 g gluose( mol.mass= 180 g/mol) per 100 g of solution?

3. The vapour pressure of water is 12.3 k.Pa at 300 K. Calculate the vapour pressure of a one molal solution of a non-volatile , non-ionic solute in water?

4. State Raoult's law for solutions of volatile liquids. Taking suitable examples explain the meaning of positive and negative deviation from Raoult's law?

5. Define the term osmotic pressure. Describe how molecular mass of a substance can be determined by a method based on measurement of osmotic pressure?

6. State the co-relating the osmotic pressure of a gas and its solubility in a liquid. State an application of this law?

7. Calculate the temperature at which a solution containing 54 gof glucose in 250 g of water will freeze.(kf for water = 1.86 K kg/mol).

8. A solution containing 8 g of a substance in 100 g diethyl ether boils at 36.86 degree celsius , where as pure ether boils at 35.6 degree celsius. Determine the molecular mass of the solute? (kb for ether = 2.02 Kkg/mol)?

9.(a) State how vapour pressure of a solvent is affected when a non-volatile solute is dissolved in it? (b) 5% solution (by mass) of cane sugar in water has freezing point of 271 K. Calculate the freezing point of 5% glucose (by mass) solution in water. Freezing point of pure water is 273.15 K. (molar mass o cane sugar =342 g/mol, glucose =180 g/mol)?

10.Calculate freezing point depression expected for 0.0711 m aqueous solution of Na2SO4. If this solution actually freezes at -0.320 degree celsius, what would be the value of van't Hoff factor?( kf = 1.86 C kg/mol).

11. 15 g of an unknown moleular substance was dissolved in 450 g of water. The resulting solution freezes at -0.34 degree celsius. What is the molar mass of the substance?( kf=1.86 K kg/mol).

12. 0.1 mole acetic acid was dissolved in 1 kg of benzene. Depression in freezing point of benzene was determined to be 0.256 K. What conclusion can you draw about the state of solute in solution? 9 kf of benzene = 5.12 K kg/mol).

13.define the following: mole fraction, van't Hoff factor, ideal solution, isotonic solutions, ebullioscopic constant.

14. A 0.561 m solution of unknown electrolyte depress the freezing point of water by 2.93 degree celsius. What is van't Hoff factor for this electrolyte. kf = 1.86 C kg/mol?

15. An aqueous solution containing 12.48 g barium chloride in 1 kg water bolis at 373.0832 K, calculate the degree of dissociation of barium chloride in water, molar mass of it =208.34 g/mol, kb= 0.52 Kkg/mol?