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ASSIGNMENTS FOR CLASS-XI

SCIENCE STREAM

ENGLISH

Chapter : The Portrait of a Lady

Q1. Compare the routine of the grandmother in the city with that of it in the village.

Q2. How did Khushwant Singh portray his grandfather in the lesson.

Q3. Describe the happiest half hour of the day for the grandmother.

Q4. What was the turning point in the relationship of the author and the grandmother?

Q5. Describe the grandmother’s behavior towards the animals.

Q6. How did the grandmother spend her time in the city?

Q7. What was the author’s routine in the village?

Q8. How did the sparrows show their love for the grandmother?

Q9. How did the grandmother express her happiness when the author returned from abroad?

Q10. Was the author’s grandmother a religious lady? Discuss.

Chapter: The Summer of the Beautiful White Horse

Q1. Which tribe did Aram and Mourad belong to? What was its speciality

Q2. What did the two boys long for since their childhood?

Q3. What did Aram see one morning that surprised him?

Q4. Who was John Byro? What was the cause of his sufferings?

Q5. What were the special character traits of uncle Khosrove?

Q6. Describe the conversation between uncle Khosrove and John Byro.

Q7. How did Aram convince himself to ride the stolen horse?

Q8. What thoughts came to Aram’s mind when he saw Mourad sitting on a beautiful white horse?

Q9. Why did the boys return the horse

Q10. Make a comparison between Khosrove and Mourad.

Chapter : A Photograph

Q1. Describe the three girls as they pose for the photograph. The snapshot

Q2. Why would the poet’s mother laugh at the snapshot?

Q3. What are the losses of the poet’s mother and the poet?

Q4. What is the meaning of the word ‘circumstance’ in the poem?

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Q5. Comment on the tone of the poem.

Q6. What is the significance of the ‘cardboard frame’

Q7. What is silenced and how has it silenced the poet

Q8. ‘Each photograph is a memory.’ Justify the statement.

Q9. What has the camera captured?

Q10. What has not changed over the years? Does this suggest something to you?

BIOLOGY

Chapter-1: THE LIVING WORLD

1. What are the various features of living organisms?

2. What is meant by Binomial Nomenclature? Who introduced it?

3. What are the various guidelines to be followed for naming of an organism?

4. Define; Classification, Taxonomy, Identification, Systematics and Taxon.

5. Define Taxonomic Hierarchy. What are the various levels in taxonomic hierarchy?

6. Define Species.

7. Write the systematic position of Man, Housefly, Mango and Wheat.

8. What are the various taxomical aids used for understanding the principles of

Taxonomy?

9. Write short notes on Herbarium, Botanical gardens, Museum, Zoological parks & Key.

10. Expand: ICBN, ICZN.

11. Name the publication of Linnaeus.

CHAPTER – 2: BIOLOGICAL CLASSIFICATION

1. What are the two kingdoms in two kingdom classification? Why it is inadequate?

2. Who proposed five kingdom system of classification? What were the main criteria

taken for classifying organisms into five kingdoms?

3. Write the characteristic features of kingdom Monera.

4. How bacteria are classified based on their shape?

5. Differentiate photosynthetic autotrophs from Chemosynthetic autotrophs.

6. Write a note on Archaebacteria.

7. What are Eubacteria? Give their features.

8. What are Heterocysts? Where they are found?

9. Which are the smallest bacteria?

10. Write the economic importance of bacteria. (Mention both benefits and harms).

11. Write the salient features of kingdom Protista.

12. Write a note on chrysophytes, Dianoflagellates, Euglenoids, Slime moulds and Protozoans.

13. Write the general features of kingdom fungi.

14. What are lichen &mycorrhiza? Explain how both algae and fungi are benefited in

Lichen.

15. Write the economic importance of various fungi.

COMPUTER SCIENCE

Q1. Define the following terms : Variable, Comment, Fundamental Data type, Constant

Q2. Briefly explain Errors with type.

Q3. Differentiate between

(a) ‘a’ and “a” (b) if - else if and switch

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Q4. Write a C++ program to covert a given number into years, weeks & days.

Q5. School library charges the fine, according to the following criteria :

For first 5 days - Rs. 2 per day

For next 10 days - Rs. 5 per day

Beyond 15 days - Rs. 10 per day

Q6. Write a C++ program to find roots of quadratic equation.

Q6. Evaluate z = ++x + x++ if x=10 initially.

Q7. What is the result : a>=b && (a + b) >a, if a=3, b=0

Assignments (LOOPS)

Q1. Rewrite the following fragment:

a) Using do while and for loop. int i = 1; //actual loop

int sum = 0; // int sum is 0 in start

while ( sum < 10000 ) { // the condition sum = sum + i; // the sum

i++;

}

b) Using do while and for loop. intdsum = 0;

while ( n > 0) {

dsum += n % 10; n /=10;

}

c) Using while and for loop. do {

sum = sum + i;

System.out.println(sum); i++;

} while(i <= 7);

d) Using while and do while loop. for (d = 0; n != 0; d++)

{

n /= 10; }

System.out.println(d);

e) Using do while and for loop.

int volume = 25; intbarrelSize = 200;

while(volume <barrelSize) {

System.out.println ("The barrel is not full."); volume = volume +25;

}

f) Using while and do while loop.

for(int speed = 10; speed => 1; time = time - 1) { System.out.println ("You are traveling at a speed of " + speed +

" miles per hour.");

}

g) Using while and do while loop.

for(intmult = 10; mult<=30; mult = mult + 1 { i = 7;

i = i * mult;

System.out.println("i is " +i); }

h) Using while and for loop.

intndx = 0; do {

if(whatever) {

doSomething(); }

ndx++;

} while(ndx< limit);

i) Using while and for loop. int n=1;

double x=0,s=0;

do{ s=10/n*n;

x=x+s;

n++;

}while(s>0); System.out.println("the value of x is "+x);

j) Using while and do while loop. for ( i = 0 ; i <num ; i++ )

{

if ( i >num / 2 ) continue ; // Jumps to update, i++

System.out.println( "Here I am!" ) ;

}

k) Using do while and for loop.

int count = 1; while (count < 11) {

System.out.println("Count is: " + count);

count++;

l) Using while and do while loop.

i=2; do{

System.out.println(i);

I+=2;

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} }while(i<51);

JoptionPane.showmessageDialouge(null,”Thank You”);

m) Using do while and for loop.

i=100;

while(i<=50)

System.out.println(i--); JoptionPane.showmessageDialouge(null,”Thank

You”);

n) Using do while and for loop.

int j=1,s=0;

while(j<10){

System.out.println(j+ “+”); s=s+j;

j=j+j%3;

} System.out.println(“=” + s);

Q2. Predict the output of following code fragments:

a) int b=0; do{

int a=2;

b++; System.out.println(a++);

}

while(b!=3);

b) int i = 1, j = 10; do

{

if(i > j) {

break;

}

j--; } while (++i < 5);

System.out.println("i = " + i + " and j = " + j);

c) for (int z=0; z < 3; z++) {

switch (z)

{

case x: System.out.print("0 "); case x-1: System.out.print("1 ");

case x-2: System.out.print("2 ");

} }

d) int x=4; int j = 1;

switch (x)

{

case l: j++; case 2: j++;

case 3: j++;

case 4: j++; case 5: j++;

default: j++;

}

return j + x;

e) int i = 1, j = 0;

switch(i)

{ case 2: j += 6;

case 4: j += 1;

default: j += 2;

case 0: j += 4; }

System.out.println("j = " + j);

f) for(int i = 0; i < 3; i++)

{

switch(i) {

case 0: break;

case 1: System.out.print("one ");

case 2: System.out.print("two "); case 3: System.out.print("three ");

}

} System.out.println("done");

g) booleanbool = true;

if(bool = false)

{ System.out.println("a");

}

else if(bool {

System.out.println("b");

}

h) int i=1,j=0,n=0;

while(i<4)

{ for(j=1 ; j <=i ; j++)

n+=1;

} i=i+1;

}

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else if(!bool)

{ System.out.println("c");

}

else {

System.out.println("d");

}

i) int j=1,s=0; while(j<10)

{

System.out.ptinln(j+”+”); s= s + j;

j= j + j%3;

}

System.out.println(“=” + s);

j) what will be the values of variables ‘P’ and ‘Q’ int P,Q=0;

for(P=1 ; P<=4 ; P++)

{ Q+=P;

Q--;

}

k) for (int i=12 ; i>5 ; i-=12 )

{

System.out.println(i); }

l) int i, sum=0;

for ( i=10,sum=5 ; sum<15 ; i++ )

{ sum +=i;

}

System.out.println(sum);

m) int j=1,s=0; while(j<10)

{

s= s + j;

i+=3; }

System.out.println(“=” + s);

n) intx,y; x=5;

y=1;

while(x>0)

{ x=x-1;

y=y*x;

System.out.ptinln(y); }

o) int c=0,i=2;

while(i<10) {

c=++i - i * 2

} System.out.println(“c=” + c + “i=” +i);

p) int i=0,x=0;

do {

if(i%5==0)

{ x++;

System.out.println(x+ “ ”);

} ++i;

}while(i<20);

System.out.println(“\n”+x);

q) for(int i=10; i>6; i=i-2) System.out.println(i); r) for(int i= -5; i< -8; i--) System.out.println(i+1);

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Mathematics

Chapter – Sets

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Chapter – Trigonometric Functions

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21.

22.

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21. 22.

CHEMISTRY

Chapter No.1

Matter In Our Surrounding

Q1. State whether the following statement is true or false:

Milk is a pure substance. Q2. Name three mixtures found in nature.

Q3. Which of the following is a mixture?

Salt, Air, Water, Alum, Sugar. Q4. Name one metal and one non-metal which exist as liquids at room temperature.

Q5. Name a metal which is soft and a non-metal which is hard.

Q6. Name a non-metal which is good conductor of electricity.

Q7. Name a liquid which can be classified as a pure substance and conducts electricity. Q8. Name one solid, one liquid and one gaseous non-metal.

Q9. Name the property:

(a) Which allows metals to be hammered into thins sheets. (b) Which enables metals to be drawn into wires?

Q10. Which type of elements, metals or non-metals, show the property of brittleness?

Q11. What is meant by saying that metals are malleable and ductile? Q12. What is meant by saying that non-metals are brittle?

Q13. What is meant by saying that metals are sonorous?

Q14. What is meant by saying that metals are lustrous?

Q15. What is the general name of the materials which contains at least two pure substances and shows the properties of their constituents?

Q16. “The properties of the product are different from those of the constituents”. State whether this statement best describes an

element, a compound and one mixture. Q17. Name one element, one compound and one mixture.

Q18. What name is given to those elements which are neither good conductors of electricity like copper nor insulators like sulphur?

Q19. Fill in the following blanks with suitable words: (a) An element is made up of only one kind of ________.

(b) Brine is _______ whereas alcohol is a____________.

(c) Brass is an alloy which is considered a ___________.

(d) The three important metalloids are ______, _______ and ________. (e) The elements which are sonorous are called_______.

Q20. Classify the following into elements and compounds

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(i) H2O (ii) He (iii) Cl2 (iv) CO (v) Co (vi) Iron (vii) Iron sulphide (viii) Sulphur (ix) Chalk (x) Washing soda (xi) Sodium (xii) Carbon (xiii) Urea.

Chapter No.1

Chemical Reactions and Equations

Q1. Translate the following into balanced chemical equation.

a) Chlorine reacts with oxygen to form chlorine heptaoxide.

b) Lead nitrate reacts with sulphuric acid to form a precipitate of lead sulphate and nitric acid.

c) Chlorine gas burns in hydrogen gas to give hydrogen chloride. d) Hydrogen sulphide burns in air to give water and sulphur dioxide.

e) Potassium permanganate on heating gives potassium manganate, manganese dioxide and oxygen.

f) Magnesium reacts with steam to form magnesium hydroxide and hydrogen gas. g) Barium chloride reacts with aluminiumsulphate to give aluminium chloride and a precipitate of Barium sulphate

h) A solution of potassium chloride when mixed with silver nitrate solution, an insoluble white substance is formed.

i) A Solution of lead nitrate and potassium iodide are mixed in a test tube.

j) A metal in the form of ribbon burns with a dazzling White flame and changes into white powder. k) Magnesium burns in the presence of nitrogen to form magnesium nitride.

l) Phosphorous burns in oxygen to give phosphorous pentoxide

m) Carbon disulphide burns in air to give carbon dioxide and sulphur dioxide. n) Aluminium metal replaces iron from ferric oxide giving aluminium oxide and iron.

o) Barium chloride reacts with zinc sulphate to give zinc chloride and barium sulphate.

Q2. Balance the following equations using Algebric method.

a) Na + O2 → Na2O b) H2O2 → H2O + O2

c) Mg(OH)2 + HCl → MgCl2 + H2O

d) Fe + O2 → Fe2O3 e) Al(OH)3 → Al2O3 + H2O

f) NH3 + CuO → Cu + N2 + H2O

g) Al2(SO4)3 + NaOH → Al(OH)3 + Na2SO4

h) HNO3 + Ca(OH)2 → Ca(NO3)2 + H2O i) NaOH + H2SO4 → Na2SO4 + H2O

j) BaCl2 + H2SO4 → BaSO4 + HCl

k) NH3 → N2 + H2 l) C + CO2 → CO

m) Zn + HCl → ZnCl2 + H2

n) MnO2 + HCl → MnCl2 + Cl2 + H2O

o) Fe(s) + H2O(g) → Fe3O4(s) + H2(g) p) CO(g) + H2 → CH3OH(l)

q) Cu + O2 → CuO

r) Fe2O3(s) + Al(s) → Al2O3(s) + Fe(s)

Q3. (a) Give one example of a chemical reaction. (b) State two characteristics of the chemical reaction which takes place when dilute sulphuric acid is poured over zinc granules.

(c)Give two characteristics of the chemical reaction which occurs on adding potassium iodide solution to lead nitrate solution.

Q4. (a) What is a chemical equation? Explain with the help of an example.

(b) Giving examples, state the difference between balanced and imbalanced chemical equations.

Q5. When hydrogen is passed over copper oxide, copper and steam are formed. Write a balanced equation for this reaction and

state which of the chemicals are :

(i) Elements (ii) compounds (iii) reactants

(iv) Products (v) metals (vi) non-metals

Q6. (a) What are the various ways in which a chemical equation can be made more informative? Give examplesto illustrate your

answer. (b) Write balanced chemical equation from the following information:

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An aqueous calcium hydroxide solution (lime water) reacts with carbon dioxide gas to produce a solid calcium carbonate precipitate and water.

Q7. (a) What is a balanced chemical equation? Why should chemical equations be balanced?

(b) Aluminium burns in chlorine to form aluminium chloride (A1C13). Write a balanced chemical equation for this reaction.

Chapter No.2

Acids, Bases and Salt

Q1. (a) What is an indicator? Name three common indicators. (b) Name the acid-base indicator extracted from lichen. (c) What colour does the turmeric paper turn when put in an alkaline solution?

Q2. What is an olfactory indicator? Name two olfactory indicators. What is the effect of adding sodium hydroxide solution to these olfactory indicators?

Q3. (a) What happens when an acid reacts with a metal? Give chemical equation of the reaction involved. (b) Which gas is usually liberated when an acid reacts with a metal? How will you test for the presence of this gas?

Q4. While diluting an acid, why is it recommended that the acid should be added to water and not water to the acid? Q5. What happens when an acid reacts with a metal hydrogencarbonate? Write equation of the reaction which takes place. Q6. (a) What happens when dilute hydrochloric acid is added to sodium carbonate? Write a balanced chemical

Equation of the reaction involved.

(b) Which gas is liberated when dilute hydrochloric acid reacts with sodium carbonate? How will you test for the presence of this gas?

Q7. What happens when an acid reacts with a base? Explain by taking the example of hydrochloric acid and sodium hydroxide. Give equation of the chemical reaction which takes place. What is the special name of such a reaction?

Q8. What happens when an acid reacts with a metal oxide? Explain with the help of an example. Write a balanced equation for the reaction involved.

Q9. (a) What are organic acids and mineral acids? (b) Give two examples each of organic acids and mineral acids. (c) State some of the uses of mineral acids in industry.

Q10. What is meant by strong acids and weak acids? Classify the following into strong acids and weak acids : HC1, CH3COOH, H2SO4, HNO3, H2CO3, H2SO3

Q11. Why do HC1, H2S04, HN03, etc., show acidic character in aqueous solutions while solutions of compounds like C6H1206 (glucose) and C2H5 OH (alcohol) do not show acidic character?

Q12. What is a neutralisation reaction? Explain with an example. Give the chemical equation of the reaction which takes place. Q13. Why should curd and other sour foodstuffs (like lemon juice, etc.) not be kept in metal containers (such as copper and brass

vessels)? Q14. (a) What is produced if an acid is added to a base?

(b) Why does dry HC1 gas not change the colour of dry litmus paper? (c) What colour does phenolphthalein indicator turn when added to an alkali (such as sodium hydroxide) ?(a) Why do acids not

show acidic behaviour in the absence of water? (b) Why does an aqueous solution of an acid conduct electricity? (c) Why does distilled water not conduct electricity whereas rain water does?

Chapter No.1

Some Basic Concept Chemistry

Q1. Calculate the mass fraction of ethyl alcohol and water in a solution containing 9.2 g of alcohol in 18.0 g of water.

Q2. The mole fraction of benzene in a solution in toluene is 0.50. Calculate the mass percentage of benzene in the solution.

Q3. The concentration of H2SO4 in a bottle labeled “conc. Sulphuric acid” is 18 M. the solution has a density of 1.84 g cm-3. What

is the mass percentage of H2SO4 in this solution.

Q4. The density of a 3 M Na2S2O3 (sodium thiosulphate) solution is 1.25 g cm-3. Calculate the mass percentage of sodium

thiosulphate.

Q5. A solution contains 20% CH3OH, 30% C2H5OH and rest is water (by mass). Calculate mole fraction of each component.

Q6. A solution of glucose (C12H22O11) is 10% w/w. calculate the mole fraction of glucose.

Q7. Calculate the mole fraction of 2.5 g of ethanoic acid (CH3COOH) in 75 g of benzene.

Q8. Calculate the mole fraction of ethylene glycol (CH2OH2)2 and water in a solution containing 20% of (CH2OH2)2 by mass.

Q9. A solution contains 25% H2O, 25% C2H5OH and 50% acetic acid by mass. Calculate mole fraction of each component.

Q10. What is the mole fraction of a solute in 2.5 m aqueous solution?

Q11. Molarity of H2SO4 is 0.8 and its density is 1,06 g/cm3.What will be its concentration in terms of mole fraction ?

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Q12. Calculate the mole fraction of the solute in aqueous solution containing 3.0 g of urea (NH2CONH2) per 250 g of water.

Q13. The concentration of H2SO4 in a bottle labeled “conc. Sulphuric acid” is 18 M. the solution has a density of 1.84 g cm-3. What

is the mole fraction of H2SO4 in this solution?

Q14. 9 g of NaOH is contained in one deciliter of a solution. Calculate the mole fraction of NaOH.

Q15. The percentage composition by mass of a solution is 45% X, 15% Y, 40% Z. Calculate the mole fraction of each component

of the solution (Molecular mass of X=18, Y=60, Z=60).

Q16. Calculate the mole fraction of ethyl alcohol and water in a solution containing 9.2 g of alcohol in 18.0 g of water.

Q17. A sugar syrup of mass 214.2 g contains 34.2 g of sugar (C12H22O11). Calculate mole fraction of the sugar in the syrup.

Q18. Calculate the mole fraction of ethanol and water in a sample of rectified spirit which contains 95% of ethanol by weight.

Q19. The density of a 3 M Na2S2O3 (sodium thiosulphate) solution is 1.25 g cm-3. Calculate the mole fraction of sodium

thiosulphate.

Q20. An aqueous solution of sodium chloride is marked 10% (w/w) of the bottle. The density of the solution is 1.071 g ml -1. What

is the mole fraction of each component in solution?

Chapter No.2

Structure of an Atom

Q1. Calculate the number of protons, neutrons and electrons (a) 𝐵𝑟3580 (b) 𝐴𝑙3+13

27 (c) 𝑂2−8

15 (d) 𝑁3−7

14 (e) 𝐶𝑙1735 .

Q2. Find out the atomic number, mass number, number of protons, electrons and neutrons present in the element with the

notation U92238 .

Q3. The nuclear radius is of the order of 10−13cm while atomic radius is of the order 10−8 cm. Assuming the nucleus and the

atom to be spherical, what fraction of the atomic volume is occupied by the nucleus?

Q4. Complete the following table:

Q5. The number of electrons, protons and neutrons in a species are equal to 18, 16 and 16 respectively. Assign the proper symbol to the species.

Q6. Neutron can be found in all atomic nuclei except in one case. Which is this atomic nucleus and what does it consist of ?

Q7. Calculate the percentage of higher isotope of neon which has atomic mass 20.2 and the isotopes have the mass numbers 20

and 22.

Particle Mass No. Atomic No. Protons Neutrons Electrons

Nitrogen atom — — — 7 7

Calcium ion — 20 — 20 —

Oxygen atom 16 8 — — —

Bromide ion — — — 45 36

Sodium atom — 11 — 12 —

Aluminium ion 27 — — — 10

Chloride ion — — — 18 18

Phosphorus atom 31 — 15 — —

Cuprous ion — — — 35 28

Sodium ion 23 — 11 — —

Bromine — — — 35 45

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Q8. Naturally occurring boron consists of two isotopes whose atomic weights are 10.01 and 11.01 the atomic weight of natural

boron is 10.81. Calculate the percentage of each isotope in natural boron.

Q9. How many nucleons are present in an atom of Nobelium, No102254 ? How many electrons are present in the atom? How many

nucleons may be considered as neutrons?

Q10. Calculate (a) wave number and (b) frequency of yellow radiations having wavelength of 5800 Å.

Q11. The VividhBharati station of All India Radio, Delhi broadcasts at a frequency of 1368 kHz (kilohertz). Calculate the wavelength of the electromagnetic radiation emitted by the transmitter. Which part of the electromagnetic spectrum does it

belong to?

Q12. The wavelength range of the visible spectrum extends from violet (400 nm) to red (750 nm). Express these wavelengths in

frequencies (Hz) (1 nm = 10-9 m) Q13. Calculate the frequency of infrared radiations having wavelength, 3 × 106 nm.

Q14. Calculate the range of frequencies of visible light from 3800 - 7600 Å.

Q15. How long would it take a radio wave of frequency, 6×103 sec-1 to travel from Mars to the Earth, a distance of 8 × 107 km? Q16. Calculate the wave number of radiations having a frequency of 4 × 1014 Hz.

Q17. A particular radio station broadcasts at a frequency of 1120 kHz (kilohertz). Another radio station broadcasts at a frequency

of 98.7 MHz (Megahertz). What are the wavelengths of the radiations from each station? Q18. Calculate the frequency and energy of a photon of radiation having wavelength 6000 Å.

Q19. Calculate the energy of a mole of photons of radiations whose frequency is 5×1014 Hz?

Q20. A 100 watt bulb emits monochromatic light of wavelength 400 nm. Calculate the number of photons emitted per second by

the bulb.

Chapter No 11.

Coordination Compound

Q1. Explain with examples the following : (i) complex ion (ii) coordination compound (iii) ligand (iv) coordination number (v) oxidation state.

Q2. How does a complex ion differ from a double salt?

Q3. What is meant by unidentate and bidentate ligands? Illustrate with examples.

Q4. Write what you know about the following with respect to coordination compounds. Illustrate each with one example. (i) ionisation isomerism (ii) linkage isomerism (iii) geometrical isomerism (iv) optical isomerism (v) coordination isomerism.

Q5. Define cis and trans isomerism. Draw the cis and trans isomers of [Co (NH3)4C12]+ ion.

Q6. Explain with a suitable example, the geometrical isomerism exhibited by coordination compounds.

Q7. Illustrate with an example each of the following : (i) Linkage isomerism (ii) Optical isomerism.

Q8. Draw all the possible isomers (structural and stereoisomeric) having the composition CrBr2Cl(NH3)4.

Q9. Mention the geometrical shapes of the complexes involving the following hybrid orbitals :

(i) sp3 (ii) dsp2 (iii) d2sp3 Give an example of each of the above.

Q10. How would you account for the following ? [Ni(CO)4] has tetrahedral geometry while [Pt(NH3)2Cl2] is square planar.

Q11. Explain the structure of [Ni(CO)4] with the help of valence bond theory.

Q12. Write a note on stability of coordination compounds in solution.

Q13. Explain how the nature of the ligand affects the stability of a complex ion.

Q14. Name two properties of the central metal ion which enable it to form stable complex entities.

Q15. Giving a suitable example, describe the importance of the formation of complex compounds in (i) the estimation of hardness of water (ii) the extraction of a particular metal from its natural source.

Q16. Mention at least three applications of organometallic compounds.

Q17. Give three different methods for the preparation of coordination compounds, giving one example of each.

Q18. Give an example of each of the following : (i) Outer orbital octahedral complex (ii) Tetrahedral complex (iii) Inner orbital

octahedral complex

Q19. Define organometallic compounds giving examples.

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Q20. How are the organometallic compounds classified?

Chapter No.1

Solid State

Q1. A compound formed by elements A and B has a cubic structure in which A atoms are at the corners of the cube and B atoms are

at the face centers. Derive the formula of the compound.

Q2. A cubic solid is made up of two elements X and Y. Atoms X are present at the corners of the cube and atoms Y at the body

centre. What is the formula of the compound? What are the Coordination numbers of X and Y?

Q3. A compound formed by elements X and Y crystallizes in the cubic structure where X atoms are at the corners of the cube and Y

atoms are at the alternate face centers. What is the formula of the compound?

Q4. If three elements P, Q and R crystallize in a cubic solid lattice with P atoms at the corners, Q atoms at the cube centre and R

atoms at the centre of the faces of the cube, then write the formula of the compound.

Q5. Three elements A, B and C crystallize into a cubic solid lattice. Atoms A occupy the corners, B atoms the cube corners and

atoms C the edges. The formula of the compound is

(a) ABC (b) ABC2

(c) ABC3 (d) ABC4

Q6. A compound made up of elements A and B crystallizes in the cubic structure. Atoms A are present on the corners as well as

face centers whereas atoms B are present on the edge centers as well as body centre. What is the formula of the compound?

Draw the structure of its unit cell.

Q7. Write the coordination number of each ion in the following crystals:

(i) NaCl (ii) CsCl (iii) ZnS (iv) Na2O (v) CaF2

Q8. A solid substance AB has a rock salt geometry. What is the coordination number of A and B? How many atoms of A and B are

present in the unit cell?

Q9. MgO has the structure of NaCl and TlCl has the structure of CsCl. What are the coordination numbers of the ions in MgO and

TlCl?

Q10. What is the coordination number of each sphere in cubic close packing of spheres in three dimensions?

Q11. What is the coordination no of HCP and CCP?

Q12. What is the coordination number of octahedral void?

Q13. A compound consisting of the monovalent ions A+, B− crystallizes in the body - centred cubic lattice.(i) What is the formula

of the compound ? (ii) If one of A+ ions from the corner is replaced by a monovalent ion C+, what would be the simplest

formula of the resulting compound?

Q14. The unit cell of the binary alloy composed of A and B metals has a ccp structure with A atoms occupying the corners and B

atoms occupying Centres of each face of the cube. If during the crystallization of this alloy in the unit cell, two A atoms are

missed, the overall composition per unit cell is

(a) AB6 (b) AB4

(c) AB8 (d) A6B24

Q15. An ionic compound made up of atoms A and B has a face-centred cubic arrangement in which atoms A are at the corners and

atoms B are at the face-centres. If one of the atoms is mission from the corner, what is the simplest formula of the compound?

Q16. The intermetallic compound LiAg crystallizes in cubic lattice in which both lithium and silver have coordination number of

eight. The crystal class is

(a) Simple cubic (b) Body centred cubic

(c) Face-centred cubic (d) None of these

Q17. In a solid AB having the NaCl structure A atoms occupy the corners of the cubic unit cell. If all the face centred atoms along

one of the axes are removed, then the resultant stoichiometry of the solid is

(a) AB2 (b) A2B

(c) A4B3 (d) A3B4

Q18. In a crystalline solid, anions B are arranged in a cubic close packing. CationsA are equally distributed between octahedral and

tetrahedral voids. If all the octahedral voids are occupied, what is the formula of the solid?

Q19. In an ionic compound, the anions (N) form cubic close type of packing while the cations (M) occupy one third of the

tetrahedral voids. Deduce the empirical formula of the compound and the coordination number of (M) ions.

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Q20. In corundum, oxide ions are arranged in hexagonal close packing and aluminium ions occupy two-third of the octahedral

voids. What is the formula of corrundum?

Chapter No.2

Solution

Q1. To what type of solution an alloy belongs? What helps in existence of aquatic life ?

Q2. Explain the terms ‘Mass fraction’ and ‘Mole fraction’ ?

Q3. Which out of molality, molarity and mole fraction of a solution will remain unchanged on raising the temperature and why ? Q4. State Henry’s law correlating the pressure of a gas and its solubility in a solvent and mention two applications for the law.

Q5. Discuss the effect of temperature on the solubility of solids in liquids.

Q6. What are ‘solubility curves’? Describe them briefly.

Q7. How can you justify the observation that the vapour pressure of solution of a non-volatile solute in a given solvent is less than that of the pure solvent ? Also state the law concerning this observation.

Q8. State Raoult’s law. Derive its mathematical expression for a solution of a non-volatile solute in a volatile solven.

Q9. State Raoult’s Law for solution containing (i) volatile solutes (ii) non-volatile solutes. Q10. Define vapour pressure of a liquid. What happens to the vapour pressure when (a) a volatile solute dissolves in the liquid and

(b) the dissolved solute is non-volatile.

Q11. Show that the relative lowering of vapour pressure for a solution is equal to the mole fraction of the solute when solvent alone

is volatile. Q12. Draw a suitable labelled diagram to express the relationship for ideal solution of A and B between vapour pressure and mole

fractions of components at constant temperature.

Q13. What are ideal solutions ? Explain non-ideal solutions showing negative deviation with diagram. Q14. Distinguish between ideal and non-ideal solutions.

Q15. What are the characteristics of an ideal solution? Why do solutions behave ideally only at low

Concentration? Q16. State Raoult’s law. Using the law, how would you distinguish between ideal and non-ideal solutions?

Q17. What is Raoult’s law? State the factors responsible for deviations from this law. Illustrate deviations with suitable examples.

Q18. What are ideal and non-ideal solutions? Give reasons for the formation of such solutions. Give

one example in each case. Q19. What type of deviation (positive or negative) from ideal behaviour will be shown by the solution of cyclohexane and

ethanol? Give suitable reason.

Q20. Miscible liquid pairs often show negative or positive deviation from Raoult’s law. What is the reason for such deviations? Give one example of each type of liquid pairs.

Chapter No.3

Electrochemistry

Q1. What is electrolysis? Discuss its mechanism by taking the electrolysis of lead bromide as an example.

Q2. What is one faraday ? How is its value calculated in Coulombs?

Q3. Define electrochemical equivalent. How is it related to the equivalent weight of the element?

Q4. On the basis of electrolytic conduction, how are the electrolytes classified?

Q5. Distinguish between strong electrolyte and weak electrolyte.

Q6. List the points of difference between metallic conductors and electrolytic conductors ?

Q7. What do you understand by the term ‘conductance’ ? What are its units?

Q8. Why is it necessary to platinize the electrodes of a conductivity cell before it is used for conductance measurement?

Q9. What is cell constant? How is it determined? Q10. What is conductivity water? Q11. How is molar conductivity related to the concentration of an electrolyte? How will you explain a weak and a strong

electrolyte based on their conductivity values?

Q12. With the help of a graph explain why it is not possible to determine Λ0 for a weak electrolyte by extrapolating the

concentration-molar conductance curve as for strong electrolyes. Q13. What is the effect of dilution on specific conductivity and equivalent conductivity? Explain briefly giving reasons.

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Q14. How does molar conductivity vary with concentration for (i) weak electrolyte (ii) strong electrolyte ? Give reasons for these variations.

Q15. Why is it not possible to determine Λ0for a weak electrolyte? Explain. Q16. Define Kohlrausch’s law. How can it be used to find the degree of dissociation of a weak electrolyte? Q17. How is the molar conductivity of a weak electrolyte at infinite dilution determined ? Q18. Define molar conductivity. Express the relationship between degree of dissociation of an electrolyte and its molar

conductivities. Q19. What is a Galvanic cell ? Give the symbolic representation of the Daniell cell? Q20. What is difference between Galvanic cell (Electrochemical cell) and Electrolytic cell ?