Bhavita20.02.2014eng--Physical Science Bit Bank

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PHYSICS

MEASUREMENT OFLENGTH

1. Smallest length that can be measured

accurately using any scale is called ____.

2. Screw gauge works on the principle of

____.

3. Screw gauge consists of ____ scale and

____ scale.

4. Pitch of the screw (P) = ____/ no. of com-

plete rotations made(n).

5. For a screw gauge, Least Count = ____.

6. If the zeroth division of the head scale is

below the index line of Pitch scale, the

error is said to be ____.

7. For a Positive zero error the correction is

____.

8. If the zeroth division of

the head scale is above

the index line of pitch

scale, the error is said to

be ____.

9. For a negative zero error, the correction is

____.

10. Diameter of a wire or thickness of an

object using screw gauge is ____.

11. The Head of a screw gauge is divided into

50 divisions if it advances1m.m.when

screw is turned through 2 rotations then

the pitch of the screw is ____.

12. If the zeroth division of head scale coin-

cides with the index line of pitch scale

then the screw gauge has no ____.

13. While measuring the diameter of a nail

using a screw gauge of L.C.0.01 mm,the

H.S.R.is 18 and P.S.R. is found to be 1.5mm, then the diameter of the nail = ____.

14. The distance traveled by the tip of a screw

for one complete rotation of its head is

called the ____.

15. The distance between two adjacent

threads of a screw is ____.

ANSWERS

1)Least count; 2) Screw in a nut; 3) Pitch,

Head; 4) Distance travelled by the screw

(x); 5) Pitch of the screw(p)/No.of Head

scale divisions(n); 6) Positive Zeroerror;

7) Negative; 8) Negative Zero Error; 9)

Positive;10)PSR+(HSR×L.C);11)0.5

m.m; 12) Zero Error; 13) 1.68 m.m.; 14)

Pitch of the screw; 15) Pitch of the screw;

IMPORTANT QUESTIONS

1 Mark

1. What is meant by Least count of a Screw

gauge?

2. On what principle does a Screw gauge

work?

4 Marks

1. Describe a method to find the diameter of

a wire using Screw gauge?

2. What are the Positive and Negative zero

errors of a Screw gauge? How are they

determined?

5 Marks

1. Draw a neat labeled diagram of Screw

Gauge?

2. Draw the diagrams showing a) No zero

error, b) Positive zero error, c) Negative

zero error of a screw gauge?

OUR UNIVERSEGRAVITATION

1. Geocentric theory was proposed by ____.

2. Heliocentric Theory was proposed by

____.

3. According to Heliocentric theory, the

____ is at the center of the universe.4. According to Ptolemic theory the ____ is

at the center of the universe.

5. The moon makes one revolution about the

earth in ____.

6. The distance of the moon from the earth is

about ____.

7. Every object in the universe attracts every

other object with a force called ____.

8. The value of Universal Gravitational con-

stant ____.

9. Gravitational constant is applicable ____.

10. The uniform acceleration produced in a

freely falling body due to gravitational

pull of the earth is known as ____.

11. Units of acceleration due to gravity, g; is

____.

12. The relation between G and g is ____.

13. Mass of the earth is ____.

14. Radius of the earth is ____.

15. Acceleration due to gravity is independent

of ____.

16. At a height equal to half the radius of

earth, acceleration due to gravity

approaches ____.

17. At the center of the earth, acceleration due

to gravity is ____.

18. The value of 'g' at the poles is ____.

19. The value of 'g' at the equator is ____.

20. The instrument used to measure small

changes in the value of 'g' at a given loca-

tion is called ____.

21. The quantity of matter contained in a body

is called the ____ of the body

22. The___of a body is the force with which it

is attracted by the earth towards its center.

ANSWERS

1) Ptolemy; 2) Copernicus; 3) Sun; 4)Earth; 5) 27.3 days.; 6) 3.85×105 k.m.; 7)

Gravitational force; 8) G=6.67x10-11 nm2

/kg2; 9) Every where in the universe .; 10)

Acceleration due to gravity; 11) m/sec2;

12)g=Gm/r2; 13)6×1024kg;14) 6.4×106m;

15) Mass; 16) Zero; 17) Zero; 18)

Maximum; 19) Minimum; 20) Gravity

meter; 21) Mass; 22) Weight

IMPORTANT QUESTIONS

1 Mark

1. What is Helio centric theory?

2. What is meant by Acceleration due to

gravity?

3. Define the weight of an object?

4. State Hook's law?

2 Marks

1. Mention the differences between Geocent-

ric theory and Heliocentric theory?

2. Derive a relation between acceleration due

to gravity(g) and Universal law of

Gravitation(G)?

3. Mention the differences between 'g' &'G'?

4. Mention the differences between mass and

weight of an object?

5. What are the factors influencing 'g'

KINEMATICS

1. The value of g for a freely falling body is

____.

2. The value of 'g' for a body thrown upward

is ____.

3. The maximum height reached by a body

thrown upward h = ____.

4. The maximum height reached by a body

thrown upward is directly proportional to

the ____.

5. Time taken by a vertically projected body

to reach its maximum height is called

____.

6. Time of ascent t1=____.

7. Time taken by a freely falling body to

touch the ground is ____.

8. The sum of time of ascent and time of

descent is called ____.

9. Time of flight T=____.

10. The time of ascent is equal to the ____ in

the case of bodies moving under gravity.

11. Time of flight is directly proportional to

its ____.

12. The initial velocity of a vertically project-

ed body ____.

13. A stone is thrown vertically upward with

an initial velocity 10m/sec. Then the max-

imum height reached by the body is ____.

14. A body is projected vertically upward with

a velocity 20m/sec. Then the maximum

height reached by the body is ____.

15. A stone is dropped from the top of a build-

ing is found to reach the ground in one

sec. The height of the building is ____.

ANSWERS

1) Positive; 2) negative; 3) h=u2 /2g; 4)Square of its initial velocity; 5) Time of

ascent; 6) u/g; 7) Time of descent; 8)

Time of flight; 9) 2u/g; 10) Time of

descent; 11) Initial velocity; 12) u=2gh;

13) 5m; 14) 20m; 15) 5m.

IMPORTANT QUESTIONS

1 Mark

1. What is the time of flight?

2. Find the velocity of a freely falling body

from a height of 20m when it touches the

ground? ( g = 10m/sec2)

2 Marks

1. Derive an expression to find the maximum

height reached by a vertically projected

body?

DYNAMICS

1. Circular motion is the simplest of

2. The direction of velocity of a bo

cuting circular motion will be ___

3. The angle described by a radius v

a particle on a rotating body in

interval of time is known as ____.

4. Angular displacement is measu

____.

5. The angle subtended by an arc length on a circle of unit radius is

as a ____.

6. The rate of angular displacem

defined as ____.

7. The units of angular velocity are _

8. The time taken by a body in unifo

cular motion to complete one revol

known as its ____.

9. In a uniform circular motion, the

constant.

10. The relation between linear veloc

angular velocity is ____.

11. The angular momentum possesse

particle in a circular motion is g

____.

12. The force acting on a body in mot

direction normal to the motion of

ticle at every point is called a ____

13. A particle executing uniform

motion undergoes a continuous ch

the direction of its velocity which

in an acceleration directed towa

centre of the circle called ____.

14. Centripetal acceleration ____.

15. The force which continuously de

particle from its straight

line path and makes it

along a circular path is

called ____.

16. ____ force acts towards

the centre of the circle.

17. Centripetal force ____.

18. An imaginary coordinate system wattached to a rotating or accelerate

where Newton's laws are not v

called ____.

19. Newton's laws are not valid in ___

20. An imaginary co-ordinate system w

either at rest or in uniform and

Newton's laws are valid is called _

21. Newton's laws are valid in ____.

22. The radially outward force on a b

uniform circular motion, observab

in a rotating frame of reference, i

____.

23. ____ force is known as fictious fo

24. A ____ is a machine used to separ

ticles of higher mass from those o

mass in a given mixture.

25. Banking angle ____.

ANSWERS

1) rotatory motion; 2) tangential t

circle; 3) angular displacement

Radians; 5) Radian; 6) angular velo

7) radians/sec; 8) Time Period; 9) an

velocity; 10) v=rω ; 11) L=mω r2; 12)

mal force; 13) centripetal accelera

14) a=v2 /r; 15) centripetal force

Centripetal; 17) F = mv2 /r (or) mω 2r

non inertial frame of reference; 19

inertial frame of reference; 20) an in

frame of reference; 21) inertial fram

reference; 22) centrifugal force; 23)

trifugal; 24) centrifuge; 25) Tan θ=v

Vý $Æý ‡$ÐéÆý ‡… l

íœ{ºÐ]lÇ l 20 l 2014 Physical Science Bit Bank

Prepared by:

A.Nagaraja Shekar,ZPHS, Chatakonda,

Khammam Dist.

Tips:

• While answering 4 marks ques-tions, the answer must be at least 8points.

• Differences must be written in tabularform

• Draw diagrams wherever necessary.(Diagram will carry 1 mark)


3/8

IMPORTANT QUESTIONS

1 Mark

1. What is the principle of launching a satel-

lite into an orbit?

2. What is a centripetal force?

3. Define Banking angle?

2 Marks

1. Distinguish between Rotatory motion and

Circular motion?

2. What is a centrifuge? How does it work?

3. Describe the working of a laundry drier?4. What is the necessity of Banking of roads?

5. What are the characteristics of Simple

Harmonic Motion?

6. Define Angular velocity? What are its

units?

4 Marks

1. Distinguish between Centripetal force and

Centrifugal force?

2. Derive an expression to find the Banking

angle?

ELECTRO MAGNETICSPECTRUM

1. ____ is a group of wave lengths or fre-

quencies.

2. All electro magnetic radiations are ____ in

nature.

3. Velocity of light in vacuum is ____.

4. The difference in the properties of differ-

ent types of electro magnetic radiations ar-

ise only from the difference in their ____.

5. ____is emitted when excited valence elec-

trons in atom jump back to their normal

state.

6. ____ radiations are used to take photo-

graphs of objects in darkness.

7. Mapping of the radio emissions from

extra-terrestrial sources is known as ____.

8. ____ radiations are produced by the tran-

sitions of electrons in atoms.

9. The wave length range of hard X- rays is

____.10. The wavelength range of soft X-rays is__.

11. Medical diagnosis

using X-rays is called

____.

12. Curing of diseases

using X-rays is called

____.

13. ____ radiations emitted when an excited

nucleus comes to its ground state.

ANSWERS

1)spectrum; 2) transverse; 3) 3×108m/

sec; 4) wave lengths or frequencies; 5)

visible spectrum; 6) infra red; 7) radio

astronomy.; 8) ultra violet; 9) 0.001Ao-

10Ao;10) 10Ao to 100 Ao.; 11) Radiogr-

aphy; 12) Radio theraphy.; 13) Gamma

IMPORTANT QUESTIONS

1 Mark

1. Draw the sketch of Electro magnetic

wave?

2. What is Radiography?

3. What is Radiotherapy?

4. What are the uses of hard X - rays?

2 Marks

1. What are the common features among all

electro magnetic radiations?

SOUND

1. Every body has its own frequency called

____.

2. Periodic vibrations of decreasing ampli-

tude are called ____.

3. When a body executes vibrations under

the action of an external periodic force,

then the vibrations are called ____.

4. If one of the two bodies of the same natu-

ral frequency is set into vibration, the

other body also vibrates with larger ampli-

tude under the influence of the first body.

This phenomenon is called ____.

5. Any two successive particles vibratingwith the same phase are separated by a

distance equal to ____.

6. Sets of____are formed in longitudinal

waves.

7. Sets of____are formed in transverse

waves.

8. On reflection form a rigid of fixed end, a

wave undergoes a phase change of ____.

9. In a stationary wave the points where the

particles undergo minimum displacement

are called ____.

10. In a stationary wave, the points where the

particles undergo maximum displacement

are called ____.

11. The distance between a node and its adja-

cent antinode is equal to ____.

12. Distance between two successive nodes or

antinodes is equal to ____.

13. A medium transmits a sound wave

through it by virtue of its ____.

14. Velocity of sound if the frequency of the

wave is ν and wavelength is λ is ____.

15. Velocity of sound in air according to res-

onating air columns experiment is ____.

16. If the distance between a node and its

adjacent antinode is 10 cm, then the wave-

length = ____ cm

17. If the distance between two successive

nodes of a stationary wave is 12 cm, then

the wavelength is ____ cm.

ANSWERS

1) natural frequency; 2) damped vibra-

tions; 3) forced vibrations; 4) resonance;

5) wave length (λ ); 6) compressions and

rarefactions; 7) crests and troughs; 8)

1800; 9) nodes; 10) anti nodes; 11)λ /4;

12) λ /2; 13) elasticity and inertia.14) v= ν λ 15) v=2n (l

2-l

1); 16) 40; 17) 24.

IMPORTANT QUESTIONS

1 Mark

1. What are damped vibrations?

2. Define Resonance?

3. Define Node and Antinode?

4. Draw the sketch of Stationary wave?

5. What is resonating air column?

2 Marks

1. Mention any two incidents of Resonance

phenomenon observed in your day to day

life?

4 Marks

1. Distinguish between progressive and sta-

tionary waves?

2. Describe an experiment to determine the

velocity of sound in air?

LIGHT

1. According to corpuscular theory, various

colours of light are supposed to be due to

____.

2. According to Huygens, waves transmit in

a medium called ____.

3. According to corpuscular theory, thevelocity of sound is more in ____.

4. According to Huygens, light propagates in

the form of ____.

5. The imaginary three dimensional surface

formed by the envelope of all those parti-

cles of medium which are vibrating in the

same phase is called ____.

6. Corpuscules are____by reflecting surface.

7. Corpuscules are____by refracting surface.

8. According to Huygen's the colours of light

are due to difference in ____.

9. The reflection and refraction of water

waves can be determined with the help of

____.

10. In a ripple tank bright bands represent

____ and dark bands are due to ____.

11. The velocity of water waves depends on

the ____ of water.

12. When two or more wave motions combine

in space at a time, ____ occurs.

13. When crest falls on crest or trough falls on

trough, the interference is called ____

interference.

14. The phase difference when constructive

superposition obtained between two

waves is ____.

15. When a crest falls on a trough or vice

versa, then the super position is said to be

____ super position.

16. The phase difference when destructive

superposition obtained between two

waves is ____.

17. The bending of a wave front from the orig-

inal direction of propagation when it

meets a small obstacle is called ____.

18. The science of measuring brightness or

relative luminous intensities of light emit-

ted by different sources using certain stan-dards and techniques is ____.

19. The amount of radiant energy flowing fr-

om a source of light per unit time is ____.

20. The unit of luminous flux is ____.

21. Unit of solid angle ____.

22. The total solid angle for a sphere is ____

Steredians.

23. Unit of luminous intensity ____.

24. The luminous flux emitted from a point

source of light per unit solid angle is

called ____.

25. The basic scientific principle behind a

laser was first put forward by ____.

26. LASER: ____.

27. Bandwidth of LASER is of the order____.

28. The spread of wavelengths about the

wavelengths of maximum inten

called ____.

ANSWERS

1) Difference in the size of corpusc

2) Ether; 3) Denser Medium; 4) W

5) Wave front; 6) Repelled; 7) Attra

8) Wavelengths; 9) Ripple Tank

Crests, Troughs; 11) Depth;

Interference; 13) Constructive; 14)

15) Destructive; 16) (2n+1)π; 17) Dction; 18) Visual Photometry; 19) Lu

ous Intensity; 20) Erg/sec or Lumen

Steredian; 22) 4π; 23) Candela;

Luminous Intensity; 25) Dr.Charles

Townes; 26) Light Amplificatio

Stimulated Emission of Radiation

10Ao; 28) Band Width.

IMPORTANT QUESTIONS

1 Mark

1. Expand LASER?

2. Define Diffraction?

3. What is interference?

4. Define 'Solid angle'?

2 Marks

1. What are the different theories

explain the nature of light?

2. What are the special properties of

light?

3. Mention the applications of LA

medicinal field?

4. Mention the applications of LA

industry?

5. What are the basic processes invo

the working of a LASER?

4 Marks

1. Give a comparison between N

Corpuscular theory and Huygen'

Theory of light?

2. Describe a ripple tank? How does

in understanding reflection and re

of light?

3. What are the applications of LASEin Science and Technology?

MAGNETISM

1. The limit of magnetization of a su

is called ____.

2. The poles in a magnet exists in

also called ____.

3. ____ is used to make electromagn

4. Ewings molecular theory failed to

the distinction between ____ an

substances.

5. The drawbacks of Ewings molecul

ry are explained by ____ theory.

6. The two poles in a magnet have th

ty to attract or repel another magne

called ____.7. The poles in a magnet have __

strength.

8. An elementary bar magnet is also

____.

9. The S.I unit of polestrength is ____

MKS system ____.

10. The ratio of magnetic force in a me

the magnetic force in free space i

____.

11. When a pole repels an identical p

mts. distance with a force of ____ i

unit pole strength.

12. Unit of µ 0

is ____ (S.I system)

13. The unit of magnetic flux is____.

14. The relation between units o

strength in M.K.S and S.I system


í œ{ºÐ] lÇ l 20 l 2014Physical Science4 Bit Bank

Tips:

• While answering the questionon experiment type, don't forget todraw the diagram & observation table

• While answering 5 marks diagram,proper depiction of parts is important.The diagram carries 3 marks andparts 2 marks. So try to identify atleast 4 important parts.


4/8

15. 1 Wb/m2 = ____ Gauss.

16. If a north pole of strength 'm' is placed at

a point where the magnetic induction is B

the force acting on it is given by ____.

17. The relation between absolute permeabili-

ty (µ 0) and relative permeability (µ

r) is µ

r=

____.

18. Relation between B and H is ____.

19. If m1=1A-m, m

2=m, then the pole strength

of any magnet ____.

20. The fundamental reason for magnetismlies in ____.

21. The value of µ 0

=____.

22. The absolute magnetic permeability of the

medium is denoted by ____.

23. The unit pole strength is defined as that

pole which repels an identical pole at 1

metre distance with a force of ____.

24. When magnetic flux (∅) is measured in

webers the unit of B is ____.

25. The strength of a magnetic field at a point

in C.G.S. units is defined as ____.

26. The units of H in C.G.S. system is ____.

27. The product of the pole strength and the

magnetic length of a magnet is called

____.

28. The S.I. units of magnetic moment are___.

29. The value of (B) on the axial line is ____

the value on the equatorial line for the

same distance.

30. The magnetic field induction (B) is ____

to the axis of the magnet.

ANSWERS

1) Magnetic Saturation; 2) Magnetic

Dipole; 3) Soft Iron; 4) Magnetic, Non

Magnetic; 5) Modern Electron; 6) Pole

Strength; 7) SAME; 8) Magnetic Dipole;

9) AMP-Metre, Weber; 10) Relative

Permeability; 11) 10-7N; 12) Hentry/

Metre; 13) Weber; 14) 1 Weber=µ 0

amp.m; 15)104; 16) F=m×B; 17) µ r=µ/µ

0;

18) B=µ 0

H; 19) F=K m/R2; 20)

Electricity; 21)4π×10-7

Henry/metre; 22)µ; 23) 10-7N; 24) Weber/meter2 or Tesla;

25) Intensity of Magnetic Field; 26)

Gauss; 27) Magnetic Moment; 28)

Ampere-meter2; 29) twice; 30) Parallel.

IMPORTANT QUESTIONS

1 Mark

1. Define Magnetic moment?

2. What are the Ferro mag-

netic substances?

3. Define magnetic field

induction?

2 Marks

1. State and explain Coulo-

mb's inverse square law of magnetism?

2. Define magnetic Susceptibility and mag-

netic permeability?3. Define a) Magnetic flux density b)

Magnetic field intensity?

4 Marks

1. What are the essential ideas of Ewing's

molecular theory of magnetism? What are

the reasons for its failure?

2. Compare the values of susceptibility and

permeability of Dia, Para, and Ferro mag-

netic substances?

3. Compare the properties of Dia, Para, and

Ferro magnetic substances?

5 Marks

1. Draw the arrangements of magnetic lines

of force when the magnetic North facing

towards Geographic North? Locate the

null points?

2. Draw the arrangement of magnetic lines

of force when the magnetic South facing

towards Geographic North? Locate the

null points?

ELECTRICITY

1. The net charge flowing through a cross

section of a conductor in unit time is

called ____.

2. Units of electric current ____.3. Coulomb/sec = ____.

4. Current is measured in Amperes using___.

5. Units of electrical Potential ____.

6. Electric potential ____.

7. Joule/Coulomb = ____.

8. The Potential Difference of an electrical

device or energy source is called its ____.

9. Units of electro motive force(e.m.f.) ____.

10. Volt meter is always connected in ____.

11. When negative terminal of a cell is con-

nected to the positive terminal of the next

cell, then the cells are said to be in ____.

12. When cells are connected in series more

____ will appear in the circuit.

13. Tap key is used to____and____the circuit.

14. When the cells of 1V, 1.5V, 2V are con-

nected in series then the resultant emf is

____.

15. When three cells of 1V, 1.5V, 2V, are con-

nected in parallel, then the resultant emf is

____.

16. If 90 coulombs charge passes through the

conductor for 5 minutes, then the current

in the conductor is ____.

17. Electric potential is measured using ____.

18. The electric property of a conductor which

opposes the free flow of current is called

____.

19. Any conductor used in a circuit to provide

resistance is called ____.

20. The reciprocal of resistance is called ____.

21. Units of resistance ____.

22. Ammeter is always connected in ____ in

an electrical circuit

23. According to Ohm's law the current (i) in

a conductor is directly proportional to the

____ between its ends.

24. Volt/Amp = ____.25. Conductors which obey ohm's law are

called ____.

26. Example of Ohmic conductors ____.

27. Conductors which do not obey ohm's law

are called ____.

28. Example of non ohmic conductors ____

and ____.

29. ____ is used to regulate the value of cur-

rent in a circuit

30. Voltage of house hold supply is ____.

31. For ohmic conductors, graph between cur-

rent and potential difference is ____.

32. For non ohmic conductors, the graph

between current and potential difference is

____.

33. The resistance of a conductor is directly

proportional to its ____.

34. The resistance of a conductor is inversely

proportional to its ____.

35. Resistance of an ohmic conductor increas-

es with the increase of ____.

36. The resistance of a specimen of unit length

and unit area of cross section is called___.

37. Units of conductivity are ____.

38. In ____ combination the same current

exists in all of them through a single path.

39. When resistances are connected in ____the total voltage is divided among them.

40. When resistances are connected in series

their equivalent resistance is equal to____.

41. The equivalent resistance is more than any

individual resistances when resistances

are connected in ____.

42. In a circuit resistors connected to common

terminals are said to be connected in ____.

43. In a ____ combination same potential dif-

ference exists across all of the resistors.

44. When resistances are connected in ____

the total current is divided among all the

resistors.

45. In a parallel combination of resistances,

the reciprocal of equivalent resistance is

equal to ____.

46. The effective resistance is less than that of

individual resistances if they are in ____

combination.

47. If two resistances R1

and R2

are connected

in parallel their effective resistance is___.

48. When two resistances of 6Ω and 12 Ω are

connected in series then the effective

resistance is ____.

49. When two resistances of 6Ω and 12Ω are

connected in parallel then the effective

resistance is ____.

50. Units of specific heat ____.

51. Units of electric power are ____.

52. In the formula Q = msθ , S is called ____.

ANSWERS

1) Current; 2) Ampere; 3) Ampere; 4)

Ammeter; 5) Volt; 6) V= W/Q; 7) Volt; 8)

Voltage; 9) Volt; 10) Parallel; 11) Series;

12) Potential difference; 13) Break ,

close; 14) 4.5v; 15) 2v; 16) 0.3A; 17) Volt

meter; 18) Resistance; 19) Resistor; 20)Conductance; 21) Ohm (Ω); 22) Series;

23) Potential difference; 24) Ohm; 25)

Ohmic conductors; 26) Metals; 27) Non

ohmic conductors; 28) Electrolytes , semi

conductors; 29) Rheostat; 30) 230v; 31)

Linear; 32) Curved line; 33) Length; 34)

Area of cross section; 35) Tempara-ture;

36) Specific resistance; 37) Mho/ meter;

38) Series; 39) Series; 40) The sum of

individual resistances; 41) Series; 42)

Parallel; 43) Parallel; 44) Parallel; 45)

The sum of reciprocals of the individual

resistances; 46) Parallel;47) R1R

2 /R

1+R

2;

48) 18Ω; 49) 4 Ω; 50) Cal/g oC; 51) Watt

or joule/sec; 52) Specific heat.

IMPORTANT QUESTION

1 Mark

1. What is Specific resistance?

2. State Lenz's law?

3. What is the difference between AC

and DC motor?

4. What is the principle of workin

Transformer?

5. What is electrolysis?

6. What is the use of iron

core in a transformer?7. State Ohm's law?

2 Marks

1. State the laws of Resistance?

2. State and explain Lenz's law?

3. State Faraday's laws of electrolysi

4. Differentiate between Step up an

down Transformers?

5. On what factors does the speed of

depend?

4 Marks

1. Derive R=R1

+ R2

+ ---- (or) Show

resultant resistance is equal to the

the individual resistances when t

connected in series?

2. Derive 1/R=1/R1+1/R

2+ ---- (or)

an expression to find the resultan

ance when two or more resistors a

nected in parallel?

3. Derive Q = i2Rt /J

4. Describe an experiment to ver

Ohm's law?

5. Describe an experiment to ver

Faraday's second law of eletrolysi

6. Explain the construction of a Tran

with a neat labeled diagram?

5 Marks

1. Draw a neat labeled diagram of

motor?

MODERN PHYSICS

1. Radius of nucleus is ____.

2. Mass of electron is ____ of the mparticle.

3. Rutherford's gold foil experimen

the discovery of ____.

4. Rutherford's model failed to exp

____ of atom.

5. Atom is electrically ____.

6. According to Bohr's model el

revolve in ____ orbits.

7. Bohr's quantum condition is ____

8. In ____ orbits electrons do not

energy.

9. ____ atomic model explained the

lines emitted by different elements

10. Neutron was discovered by ____.

11 Electrically neutron is ____.

12. Mass of proton is ____ times to t

of electron.13. Protons and neutrons together calle

14. The number of protons in an

defined as ____.

15. The mass of the atom is measured

called ____.

16. The amu is defined is ____ of the

the neutral carbon atom.

17. The total number of protons and n

in an atom is defined as ____.

18. Mass of proton = ____.

19. Mass of neutron = ____.

20. Velocity of light in vacuum (c) = _

21. Einstein's mass energy equival

____.

22. The magnitude of the mass def

measure of the ____ of nucleus.



Tips:

• Read the question paper thor-oughly for 2 or 3 times and identifythe well known questions and markthem with pencil.

• Don't use sketch pens / colours etc fordiagrams. Use only a quality pencil.

• Formula of the experiment mustbe in a box.


5/8

23. Binding energy = ____.

24. 1amu = ____.

25. 1Mev = ____.

26. Electron volt is a unit of ____.

27. Radioactivity was discovered by ____.

28. The rays which are deflected towards neg-

ative terminal are ____.

29. The rays which are deflected towards pos-

itive terminal are ____.

30. α particle is the doubly ionized ____atom.

31. The mass of α particle is ____ times themass of proton and its

charge is ____ times the

charge of proton.

32. Particles whose ioniz-

ing power is more are

____.

33. α particles have ____ penetrating power

when compared to β and γ radiations.

34. The speed ofα particle is ____.

35. β particles are the flow of ____.

ANSWERS

1) 2.4×10-15mts; 2) 1/1000; 3) Nucleus;

4) Stability; 5) Neutral; 6) Stationary; 7) I

=nh/2π; 8) Stationary; 9) Bohr's; 10)

Chadwik (1937); 11) Neutral; 12) 1836;

13) Nucleons; 14) Atomic Number; 15)

Atomic Mass Units (amu).; 16) 1/12th;

17) Atomic Mass Number or Mass

Number (A); 18) 1.0078amu.; 19) 1.0087

amu.; 20) 3×108m/sec.; 21) E=∆mc2; 22)

Stability; 23) Mass defect ×931.5 Mev.;

24)931.5×106 ev. (or) 931.5 Mev.; 25) 1.6

×10-12Joules.; 26) Energy; 27) A.H. Bec-

queral(1896); 28) α- rays.; 29) β- rays.;

30) Helium; 31) 4, 2; 32) α particles.; 33)

Small; 34) 107 m/sec.; 35) Electrons.

IMPORTANT QUESTIONS

1 Mark

1. What is the difference between Atomic

number and Atomic mass?

2. Define mass defect?3. What is binding energy?

4. What are the Isobars? Give examples?

5. What are Isotopes? Give examples?

6. What are Isotones? Give examples?

7. State law of radioactive disintegration?

2 Marks

1. What is the role of moderator in a Nuclear

reactor?

2. What are the uses of Radio isotopes in the

field of medicine?

3. What is artificial transmutation? Give an

example?

4 Marks

1. Compare the properties of α, β and γ radi-

ations?

2. What is the principle of Nuclear Reactor?

How the chain reaction does controlled ina nuclear reactor?

5 Marks

1. Draw a neat labeled diagram of Nuclear

Reactor?

ELECTRONICS

1. At 00K conduction band is completely

____.

2. At 00K valence band is completely ____.

3. Rubber is an ____.

4. The energy gap is highest in the case of

____.

5. When temperature of a semi conductor is

raised its energy gap ____.

6. The energy gap of an insulator is general-

ly more than ____.

7. The gap between conduction band and

valence band is known as ____ or ____.

8. In an insulator the concentration of free

electrons is nearly equal to ____.

9. In a conductor the concentration of free

electrons is nearly equal to ____.

10. The energy gap of a conductor is ____.

11. The energy gap of pure silicon at room

temperature is ____.

12. The energy gap of pure germanium atroom temperature is ____.

13. At 0K semi conductor behaves as an ___.

14. The conductance of a semi conductor

____ with the increase in temperature.

15. The absence of an electron in the valence

band of a semi conductor is called ____.

16. A group of closely spaced energy levels is

called an ____.

17. In an intrinsic semi conductor the number

of ____ is equal to the number of ____.

18. Doped or impure semi conductors are

called ____ semi conductors.

19. The process of introducing impurities in

small quantities into a material is called

____.

20. In a p type semiconductor the majority

carriers are ____ and the minority carriers

are ____.

21. If a small quantity of acceptor impurity is

added to the pure semiconductor then

____ type semi conductor is formed.

22. Trivalent impurities are also called ____.

23. Pentavalent impurities are called as ____.

24. If a small quantity of Donor impurity is

added to the pure semi conductor then

____ type semi conductor is formed.

25. In an n type semiconductor the majority

carriers are ____, and the minority carriers

are ____.

26. In a semiconductor the charge carriers are

____ and ____.

27. The combination of p type and n type semi

conductors results in the formation of

____.

28. The region close to p-n junction is deplet-

ed of mobile charge carriers and is called

____.

29. The p-n junction consisting of p type andn type semiconductors provided with two

terminals is called a ____.

30. The potential deference across the junc-

tion is called ____.

31. If the p side of a diode is connected to the

positive terminal of a battery then the

diode is said to be in ____.

32. If the n side of a diode is connected to the

positive terminal of a battery then the

diode is said to be in ____.

33. A diode offers ____ resistance in forward

bias condition.

34. A diode offers ____ resistance in reverse

bias condition.

35. Under ____ bias condition a diode con-

ducts.

36. Diode is used as ____.

37. ____ converts AC to DC.

38. A device which consist two p-n junctions

is called ____.

39. The three terminals of a transistor are

____.

40. The arrow mark in the symbol of transis-

tor indicates ____.

41. Transistor acts as ____.

42. In radio communication the range of carri-

er frequency is ____.

ANSWERS

1) Empty; 2) Saturated; 3) Insulator; 4)

Insulator; 5) Decreases.; 6) 3ev; 7)

Energy gap , forbidden gap; 8) 107 per

c.c; 9) 1028 per c.c; 10) 1 ev; 11) 1.1 ev;

12) 0.72 ev; 13) Insulator; 14) Increases;

15) Hole; 16) Energy band; 17) Electrons,

holes; 18) Extrinsic; 19) Doping; 20)

Holes, electrons; 21) P; 22) Acceptor

impurities; 23) Donar impurities; 24) n;

25) Electrons, holes; 26) Electrons, holes;

27) Junction; 28) Depletion region; 29) P-

n junction diode; 30) Potential barrier;

31) Forward bias; 32) Reverse bias; 33)

Less; 34) High; 35) Forward; 36)

Rectifier; 37) Rectifier; 38) Junction tran-

sistor; 39) Emitter, base, and collector;

40) Emitter; 41) Amplifier; 42) 300 KHz

to 30 MHz.

IMPORTANT QUESTIONS

1 Mark

1. Define Hole?

2. What is a Byte?

3. What is doping?

4. What is modulation?

5. What is a programme?

2 Marks

1. Draw the symbols of p-n-p and n-p-n tran-

sistors?

2. What are the differences between machine

language and high level language?

3. What are the hardware and software in a

computer?

4. What are the important uses of computer

in daily life?

5. Define intrinsic and extrinsic semi con-ductors?

4 Marks

1. Explain the formation

of p-type and n-type

semi conductors?

2. What are the properties

and uses of Junction Diode?

3. What are the properties and uses of junc-

tion transistor?

4. Explain the important steps involved in

Radio broadcasting?

5. Explain the important steps involved in

T.V. broadcasting?

6. Draw the block diagram of Computer and

explain the various components in it?

CHEMISTRY

ATOMIC STRUCTURE

1. First model of atom was proposed

2. Rutherford proposed the model o

based on his ____ experiment.

3. Rutherford's model of atom is also

as ____.

4. According to Rutherford, atoms a

in shape.5. Quantum theory of radiation is p

by ____.

6. According to Quantum theory elec

netic radiation is in the form of

called ____.

7. Quantum principle is ____.

8. In the formulae E = h ν 'h' is ____.

9. Planck based on his theory explai

radiation of ____.

10. Value of Planck's constant is ____

11. Bohr proposed a model of atom b

____.

12. According to Bohr's model, el

revolve in ____.

13. The energy of a stationary orbit w

near to the nucleus is ____.

14. Electron jumps from ____ energy

____ energy level.

15. When electron jumps form higher

level to lower energy level the dif

in the energy levels is radiated as _

16. Angular momentum of electron is

____.

17. In the formula mvr = nh /2π 'n' is

as ____.

18. Splitting of spectral lines in the p

of magnetic field is known as ____

19. Bohr's model is applicable only

atoms of ____.

20. Elliptical orbits are introduced by

21. The angular momentum of an

revolving in elliptical orbit is ____

22. Dual nature of electron was expla____.

23. De broglie explained ____ based

dual nature of electron.

24. Wave equation of electron was p

by ____.

25. Derivations of wave equation lead

26. Stationary orbits are denoted by __

27. Sub stationary orbits are also kn

____.

28. The number of sub stationary orbi

ent in a stationary orbit depends o

value.

29. Number of sub stationary orbits in

are ____.

30. Principle quantum number was p

by ____.

31. 'n' value of N shell is ____.32. The quantum number which gives

and energy of an orbit is ____.

33. No. of sub stationary orbit in a st

orbit is ____.

34. Azimuthal quantum number was p

by ____.

35. Azimuthal quantum number is also

as ____.

36. For a given value of n, the m

value of l is ____.

37. Shape of sub stationary shell can b

mined by using ____.

38. When l = 0, the shape of the orbit

39. Magnetic quantum number was p

by ____.

40. 'm' value depends on ____.



Tips:

• Practice all bits given at the endof each lesson.

• Important formulae, constants, units,important equations, names of scien-tists etc must be written at one place,so that the practice will be easier

• Follow previous papers at least forpast 5 years.


6/8

ANSWERS

1) J.J. thomson; 2)α-ray scattering; 3)

Planetary model or nuclear model; 4)

Spherical; 5) Max planck; 6) quanta; 7)

E=h ν; 8) Planck's constant; 9) Black

body; 10) 6.625×10-27 erg. Sec or 6.625×

10-34 joule. Sec; 11) Planck's quantum

theory; 12) Stationary orbits; 13) Less;

14) Higher, lower; 15) E2−E

1=h ν; 16)

Mvr=nh /2π; 17) Principal quantumnum-

ber; 18) Zeeman effect; 19) Single elec-tron; 20) Sommerfeld; 21) Mvr = kh/2π;

22) Louis de broglie; 23) Quantization of

angular momentum; 24) Erwin schro-

dinger; 25) Atomic orbitals; 26) Principle

quantum number; 27) Atomic orbitals;

28) 'n'; 29) 3; 30) Neils bohr; 31) 4; 32)

Principle quantum number; 33)n2; 34)

Sommerfeld; 35) Angular momentum

quantum number; 36) n-1; 37) l; 38)

Circular; 39) Lande; 40) '1'.

IMPORTANT QUESTIONS

1 Mark

1. Write the Planck's equation?

2. What is zeeman effect?

3. What is a stationary orbit?

4. What is a nodal plane?

5. Why an electron enters into 4s but not into

3d after filling up of 3p orbital?

6. State "Aufbau" principle?

7. State "pauli's" exclusion principle?

2 Marks

1. Define Electron affinity and Ionization

energy?

2. Write the electronic configurations of Cu,

and Zn.and Mg?

3. Draw the boundary diagrams of 's' and 'p'

orbitals?

4. Write a short note on Principle quantum

number?

4 Marks

1. What are the important features of

Rutherford's planetary model? Mention itsdefects?

2. State the postulates of Bohr's model of

atom? What are its defects?

3. Define ionization energy? What are the

factors influencing it?

4. State and explain "Aufbau" principle with

an example?

5. State and explain with one example the

"Hund's" rule of maximum multiplicity?

6. Explain the features of modern atomic

structure?

5 Marks

1. Draw the boundary surface diagrams of 'd'

orbitals?

CHEMICAL BONDING

1. Complete transfer of

one or more electrons

from one atom to anoth-

er result in the forma-

tion of ____ bond.

2. Sharing of two electrons

between two atoms causes ____ bond.

3. The filling up of valence orbital with 8

electrons is referred to as ____.

4. The distance between two atoms after

bond formation is called as ____.

5. ____ takes place by the atoms either by

losing or sharing electrons to achieve inert

gas configuration.

6. The ____ decides the strength of the

chemical bond.

7. The atom formed by s-s overlapping is

____.

8. The atoms formed by p-p overlapping are

____ etc.

9. The atoms formed by s-p overlapping are

____, etc.

10. The bond formed by end on overlapping is

____.

11. Strongest bond is ____ bond.

12. ____ bond can exist independently.

13. Examples for Sigma bond(σ) are ____ etc.14. The bond formed by side on overlap is

____.

15. Pie bond (π).is present only along with a

____.

16. Example for Pie bond(π) is ____.etc.

17. Single bonded atom consists only ____.

18. Double bond consists one ____ bond and

one ____.

19. Example for double bonded atoms ____

etc

20. Triple bond consists one ____ bond and

two ____.

21. Example for triple bonded atoms ____etc.

22. The bond formed by contribution of elec-

tron pair is called as ____bond.

23. Example for coordinate covalent bond is

____.

24. In NH3BF

3, electron donor is ____and

electron acceptor is ____.

25. All diatomic molecules are ____.

26. Shape of PCl3

is ____NSWERS

ANSWERS

1) ionic; 2) covalent; 3) octet configura-

tion.; 4) bond length.; 5) Bond formation;

6) extent of overlap; 7) Hydrogen (H2).;

8) F2, Cl

2, Br

2, O

2; 9) HCl, HBr, HI, H

2S,;

10) Sigma bond.(σ); 11) Sigma (σ); 12)

Sigma (σ); 13) H2, HCl, Cl

2, BF

3, BeF

2;

14) Pie bond (π).; 15) sigma bond (σ).;

16) Ethylene (c2H

4), CO

2, O

2, N

2; 17)

Sigma (σ) bond.; 18) Sigma (σ) ,Pie bond

(π); 19) O2,Co

2,C

2H

4etc; 20) Sigma (σ),

Pie bonds (π); 21) C2H

2, CaCl

2, HcN; 22)

Coordinate covalent; 23) NH3BF

3; 24)

NH3,BF

3.; 25) linear.; 26) Trigonal by

pyramidal.

IMPORTANT QUESTIONS

1 Mark

1. Write the names of two atoms having

pyramidal shape?

2. Draw the shape of Ammonia (NH3)?

3. Draw the shape of Water molecule (H2O)?

2 Marks

1. Mention the differences between σ and π

bonds?

2. What is the shape of PCl5

? Draw it?

3. Draw the shape of PCl3

molecule?

4 Marks

1. Discuss the types of overlaps that are pos-

sible with s and p orbitals?

2. Explain the formation of double bond?

3. Explain the formation of Triple bond?

4. Explain the formation of Coordinate cova-

lent bond?

CLASSIFICATION OFELEMENTS

1. The first classification of elements is

attempted by ____.

2. In a Doberiener triad, the atomic weight of

middle element is the ____ of atomic

weights of first and the third elements.3. Example for Doberiener triad ____.

4. Mendeleef's periodic table is based on the

____.

5. Mendeleef's periodic law states that the

properties of the elements are periodic

functions of the ____.

6. Gallium was named by ____.

7. Scandium was discovered by ____.

8. Modern periodic table is based on ____.

9. In the periodic table horizontal rows are

called ____.

10. In the periodic table vertical columns are

called ____.

11. In the long form periodic table there are

____ periods and ____groups.

12. The number of elements in the first period

is ____.

13. The number of elements in the second

period is ____.

14. The number of elements in the third peri-

od is ____

15. The number of elements in the fourth and

fifth periods are ____,____.

16. The number of elements in the sixth peri-

od is ____.

17. ____ period is incomplete.

18. Elements from atomic number 57 to 70 are

known as ____.

19. Elements form atomic number 89 to 102 is

known as ____.

20. Valence electronic configuration of inert

gas is ____.

21. Every period in the periodic table ends

with ____.

22. The elements with electronic configura-

tion ns1 and ns2 are known as ____ele-

ments.

23. The valence electronic configuration of p-block elements is from ____.

24. The distance between the centre of the

nucleous and the outer most orbital is

defined as ____.

25. The minimum energy required to remove

an electron from the outer most orbital of

an atom in the gaseous state is defined as

____.

26. The tendency of bonded atom to attract the

electron is defined as ____.

27. Electro negativity is measured in

____scale.

28. The ability to lose electron and become

positively charged ions is defined as ____.

29. Addition oxygen or removal of hydrogen

from a compound is defined as ____.

ANSWERS

1) Doberiener; 2) mean; 3) Li, Na,

atomic weight; 5) atomic weights; 6

Boisbaudran; 7) Nilson; 8) Atomic

ber; 9) Periods; 10) Groups; 11) 7, 16

2; 13) 8; 14) 8; 15) 18 , 18; 16) 32

7th; 18) lanthanoides; 19) Actinoide

ns2np6; 21) Inert gas; 22) s block

ns2np1 to ns2np5; 24) Atomic radius

Ionization Energy; 26) Electro negat

27) Linus Pauling Electro negativityElectro positivity; 29) Oxidation.

IMPORTANT QUESTION

1 Mark

1. State Mendeleef's periodic law?

2. Define Oxidation?

3. State modern periodic law?

4 Marks

1. How does the following properties

a period and a group?

a) Atomic radius b) Oxidat

Reduction d) Electro negativity e)

positivity and f) Ionization energy

2. What is Modern periodic law? Ex

main features?

ALKALINE EARTH MET

1. Alkaline earth Metals belon

____Group

2. Beryl [Be3

Al2

(Sio3)6] is the ore o

3. No.of water molecules in Epsum

____.

4. Chemical formulae for Epsum salt

5. Barite (BaSo4) is the ore of ____.

6. The metals present in D

(MgCo3CaCo

3) are ____.

7. Atomic size from Be to Ra ____.

8. From Be to Ra the Ionization

____.

9. From Be to Ra the

Electro Negativity

____.10. Alkaline Earth metals

react with water and

gives ____.

11. Beryllium doesn't react with ____

12. Alkaline Earth metals react with

and gives ____.

13. Beryllium doesn't react with

below ____ temperature.

14. The Alkaline earth metal which gi

oxides in addition to oxide when b

excess of air is ____.

15. The oxides of alkaline earth me

____in nature.

16. All alkaline earth metals except B

with H2

to form ____.

17. The reagent used to prepare BeH

BeCl2 is ____.18. All alkaline earth metals react wi

rine to form ____.

19. All alkaline earth halides are ____

Be.

20. BeCl2

is ____.

21. The alkaline earth chloride which

moisture and fumes in air is ____.

22. Alkaline earth metals are extrac

____.

23. While extracting Mg from MgCl2

_

added.

24. Addition of KCl and NaCl durin

trolytic extraction of Mg will lo

____ and increases the ____.

25. The cathode in the electrolyses of

is ____.



Tips:

• Practice bits in groups in theform of quiz etc.

• Matching is very important. For this,Light, Modern Physics, Electronics,

Atomic structure, Chemistry of carbon

compounds, etc are very important

chapters.


7/8

ANSWERS

1) IIA; 2) Beryllium; 3) 7; 4)

MgSo47H

2o; 5) Barium; 6) Magnesium

and calcium; 7) Increases; 8) Decreases;

9) Decreases; 10) H2

gas; 11) Water; 12)

Oxides; 13) 6000C; 14) Barium; 15) Ba-

sic; 16) Hydrides; 17) LiAlH4; 18) Chlor-

ides; 19) Ionic; 20) Covalent; 21) Becl2;

22) Electrolysis; 23) KCl and NaCl; 24)

Melting point , conductivity; 25) Iron pot.

IMPORTANT QUESTIONS

1 Mark

1. Why do we add KCl

and NaCl to MgCl2

dur-

ing Mg extraction?

4 Marks

1. Write the reactions of

alkaline earth metals with a) oxygen b)

Hydrogen c) water and d) chlorine ?

2. Describe a method of extraction of Mg

from its ore?

5 Mark

1. Draw a neat diagram showing the extrac-

tion of Magnesium from its ore?

SOLUTIONS1. In a solution the component which is taken

in relatively less quantity is called ____.

2. In a solution, the component which is

taken in relatively large quantity is called

____.

3. Solute+ solvent = ____.

4. If the solvent used is water, the resultant

solution is called ____solution.

5. The maximum amount of solute by weight

in grams dissolved in 100 g of solvent at

constant temperature is defined as ____.

6. Solubility depends on ____.

7. Common name of sodium thiosulphate is

____.

8. Chemical name of Hypo is ____

9. ____solution is unstable.10. Naphthalene is soluble in ____.

11. Polar solutes dissolve in ____solutions.

12. On increasing the temperature, the solubil-

ity of Nacl remains ____.

13. The solution of Co2

in water is called

____.

14. The amount of solute present in a solution

is known as ____.

15. The weight of solute present in 100g of

solution is called ____

16. W% = ____.

17. The volume of solute present in 100 ml of

solution is called ____.

18. The no. of moles of a solute present in one

litre of solution is defined as ____

19. Molarity (M) = ____.

20. Molarity of a solution depends on ____.21. The sum of the mole fractions of all con-

stituents present in the solution is equal to

____.

22. Gram molecular weight of Na2Co

3is

____.

23. Gram molecular weight of NaoH is ____.

24. The process of a molecule giving rise to

ions is called ____.

25. Solutions which ionize completely

(100%) are known as ____.

26. Solutions which ionize incompletely

( 7, then the solution is ____.

21. If pH = 7, then the solution is ____.

22. The concentration of H+ ions in a solution

whose pH = 8 is ____.

23. Example for strong acid is ____.

24. Example for weak acid is ____.

25. Example for strong base is ____.

26. Example for weak base is ____.

27. The heat liberated when one mole of acid

reacts with one mole of base is defined as

the ____.

28. The heat evolved when a strong acid

reacts with a strong base is equal to ____.

29. NaOH + HCl → NaCl + H2O + ____.

30. The body fluid whose pH > 7 is ____.

ANSWERS

1) non metallic; 2) Bases; 3) Acid; 4)

Red; 5) Salt and water; 6) Base; 7)

Yellow; 8) H+; 9) OH-; 10) Water; 11)

Equal; 12) Temperature; 13) Ionic

Product of water; 14) [H+]×[OH-]; 15)

1.0×10-14 mol.ion2 /lit2; 16) Sorensen; 17)

pH; 18) -log [H+]; 19) Acid; 20) Base; 21)

Neutral;22)10-8; 23) Hcl; 24) CH3COOH;

25) NaOH; 26) NH4OH; 27) Heat of

Neutralization; 28) 13.7 Kcal/mole; 29)

13.7 K. cal/mole; 30) blood.

IMPORTANT QUESTIONS

1 Mark

1. Define pH?2. What is the ionic product of water? What

is its value at 250C?

3. Define heat of neutralization?

4. Calculate the pH of 0.001M Hcl?

4 Marks

1. State Arrehenius theory of Acids and

Bases? What are its limitations?

2. Define Strong acid, Strong base, Weak

acid, and weak base and give examples?

CHEMISTRY OF CARBONCOMPOUNDS

1. Percentage of carbon in the earth crust is

____.

2. The occurrence of same element in two or

more different forms is known as _

3. The density of Diamond is ____.

4. The refractive index of diamond is

5. ____is used as glass cutter.

6. The C-C bond length in diamond i

7. The C-C bond angle in diamond is

8. The allotropy of carbon used as lu

is ____.

9. The density of graphite is ____.

10. Graphite contains carbon atoms i

rings.11. In graphite the C-C bond length is

12. In graphite the C-C bond angle is

13. Two successive graphite layers ar

rated by ____.

14. C60

contains ____ pentagonal rin

____ hexagonal rings of carbon.

15. C60

is a ____ like struc-

ture.

16. Co2

dissolves in water

and gives ____.

17. ____ is used as fire

extinguisher.

18. Solid carbon dioxide is called ___

19. The phenomenon in which atoms

element join together to form long

is known as ____.

20. Compounds having same molecu

mula but different structures are

____ and the phenomenon is ca

____.

21. The oldest coal is called ____.

22. The compounds containing exc

carbon and hydrogen are known as

23. Example of aromatic hydrocarbon

24. Saturated hydrocarbons are also kn

____.

25. General formula of alkanes is ____

26. If one hydrogen is removed from a

is called ____ group.

27. Alkanes undergo ____ reactions.

28. Formula for chloroform is ____.

29. L.P.G consists of ____.

30. The unsaturated hydrocarbons haleast one C = C are known as ____

31. The general formula of alkenes is

32. Alkenes are also known as ____.

33. Alkenes undergo ____ reactions.

ANSWERS

1) 0.3%; 2) allotropy; 3) 3.51 gm/c

2.41; 5) Diamond; 6) 1.54 A0; 7) 109

8) Graphite; 9) 2.25 gm/cc; 10) hex

nal; 11)1.42A0; 12) 1200; 13) 3.35 A0

12 , 20; 15) football; 16) Carbonic

17) Carbon dioxide; 18) dry ice

Catenation; 20) isomers, isomerism

anthracite; 22) hydrocarbons; 23) B

ene; 24) paraffins; 25) CnH

2n+2; 26) a

27) substitution; 28) CHCl3; 29) Bu

(C4H10); 30) Alkenes; 31) CnH2nolefins; 33) addition.

IMPORTANT QUESTION

1 Mark

1. What is Allotropy?

2. Define catenation?

3. What is polymerization?

4. What is isomerism?

5. What are the uses of Acetylene?

2 Marks

1. Draw the structure of Benzene?

2. Write the substitution reacti

Alkanes?

3. Differentiate between Alkane

Alkenes?

4. Mention the uses of CO2

?



Tips:

• Short and very short answertype questions must be very brief.

• Draw diagrams wherever necessary.• Long answer type questions must be

written point wise

• Highlight the key words in theanswer with highlighter or pencil.


8/8

4 Marks

1. Compare the structures of diamond and

graphite?

CARBOHYDRATES ANDPROTEINS

1. Sweetest sugar is ____.

2. Example for polysaccerides is ____.

3. Polyhydroxy aldehydes are ____.

4. Poly hydroxyl ketones are ____.5. Number of carbon atoms in Hectose are

____.

6. In Tollen's test, Glucose reduces ____.

7. Defacation is addition of ____.

8. Acidity in the sugar cane juice is removed

by adding ____.

9. The sugar content of molasses is ____.

10. The main by-product in sugar industry is

____.

11. The chief use of ethyl alcohol is as ____.

12. ____ is added to get absolute alcohol from

rectified spirit.

13. Consumption of denatured spirit causes

____.

14. Calorific value of Glucose is ____.

15 The dirty grey precipitate formed during

the preparation of Tollen's reagent is ____.

16. The spent cane is called ____.

17. ____ are used to separate the crystals of

sugar and liquid juices.

18. ____ is the micro organism used for fer-

mentation of molasses.

19. Sucrose is broken down

into ____during fer-

mentation.

20. Sucrose is broken down

into Glucose and fruc-

tose during fermenta-

tion by the enzyme ____.

21. ____ enzyme breaks Glucose.

22. The products obtained from glucose dur-

ing fermentation are ____.

23. ____ is the by-product of alcohol industry.24. ____ are building blocks of Proteins.

25. Number of essential amino acids are ____.

26. Polymeric compounds of amino acids are

____.

27. CO-NH bond is called ____.

28. ____. is the process of breaking down of

large molecules into small molecules by

the action of enzymes.

29. 96% alcohol is commercially called ____.

30. ____ is added to denatured spirit.

31. The precipitates formed by defecation,

carbonation, and sulphitation is called

____.

32. The result of Tollen's test is ____.

ANSWERS

1) Fructose; 2) Starch and cellulose; 3)Aldoses; 4) Ketoses; 5) 6; 6) Ag+ ion as

Ag metal; 7) Ca(OH)2; 8) Ca(OH)

2; 9)

50%; 10) molasses; 11) solvent; 12) CaO;

13) blindness; 14) 3.81 K.Cal/gm or 686

K.Cal/mole; 15) AgOH; 16) Bagasse; 17)

Centrifuge machines; 18) Yeast; 19) Glu-

cose and Fructose; 20) Invertase; 21) Zy-

mase; 22) Ethyl Alcohol & Co2; 23) Co

2;

24) Amino acids; 25) 9; 26) proteins; 27)

Peptide bond; 28) Fermentation; 29) rec-

tified spirit; 30)Pyridine; 31) press mud;

32) Silver mirror on the walls of test tube.

IMPORTANT QUESTIONS

1 Mark

1. Define calorific value?

2. What is defecation/

3. What is Sulphitation?

4. What is rectified spirit?

5. What is bagasse? How is it useful?

6. Give the classification of carbohydrates

based on hydrolysis?

2 Marks

1. Explain the formation of peptide bond?

2. What are the functions of proteins?

4 Marks

1. How is Tollen's reagent prepared? How isglucose tested with it?

2. How is Benedict's reagent prepared? How

is glucose tested with it?

3. Explain the various steps involved in man-

ufacturing of sugar from sugar cane?

4. How is alcohol manufactured industrially?

5 Marks

1. Draw the diagram showing the parts of

sugar industry?

2. Draw a chart showing alcohol manufac-

ture?

OILS AND FATS

1. The cation of soap useful for dry cleaning

is ____.

2. Shaving soap contains excess of ____.

3. The fatty acid obtained from cotton oil is

____.

4. The catalyst used in the hydrogenation of

oils is ____.

5. The chemical formula of soap is ____.

6. The catalyst used in soap manufacturing is

____.

7. Transparent soap contains ____.

8. Deodorant soap contains ____.

9. The formula of stearic acid is ____.

10. Oils are triestors of ____.

11. ____ improves preservation, taste and

odour of many oils.

12. Hydrolysis of oils and

fats in the presence of a

base is called ____.

13. The by product in the

preparation of soap is

____.

14. Sodium salt of ABS or FAS + builders =

____.15. Saturated fatty acids have high ____.

16. ____.removes the Ca2+ ions present in

hard water.

17. Detergents are useful even in hard water

because ____.

18. All soaps contain ____ water.

19. Fat exists in ____ state at room tempera-

ture.

20. ____ is a fat obtained by the catalytic

hydrogenation of vegetable oil.

21. The chemical formula of lauric acid is

____.

22. Chemically ____are sodium salts of alkyl

benzene sulphonates of fatty alcohol sul-

phates.

ANSWERS

1) Tri ethanol ammonium; 2) stearic acid;

3) oleic acid; 4) Ni; 5) C17

H33

COONa; 6)

Zinc oxide; 7) Glycerol; 8) 3,4,5,tri

bromo salicylanilide; 9)C17

H35

COOH;

10)Glycerol and fatty acids; 11)

Hydrogenation; 12) hydrogenation of

oils; 13) Glycerol; 14) soap; 15) melting

points; 16) Na3Po

4; 17) they react with

hard water but do not form precipitate;

18) 30% of; 19) solid; 20) Vanaspati(Dalda); 21) C

11H

23COOH; 22) deter-

gents.

IMPORTANT QUESTIONS

1 Mark

1. What is the hydrogenation of oils?

2. What is the use of hydrogenation of oils?

3. What is saponification?

4. What is a soap?

2 Marks

1. What are the industrial uses of oils?

4 Marks

1. How do you test the quality of soap?

2. How is soap industrially manufactured?

CHEMISTRY ANDINDUSTRY

1. The raw materials required for cement

manufacture are ____.

2. The temperature required in the manufac-

ture of cement is ____.

3. ____is added to powdered clinker cement.

4. Glass may be considered as ____.

5. The composition of cement is ____.

6. By chemical composition, glass is a mix-

ture of ____.

7. Raw materials used for glass manufacture

are ____.

8. The mixture of raw materials in the glass

manufacture is called ____.

9. Broken glass pieces are called ____.

10. Cullet helps in ____ of raw materials.

11. Heat required for glass manufacturing is

____.

12. The mixture of impurities floating on the

liquid glass is called ____.

13. Slow cooling of glass is called ____.14. Glass blowing is possible with ____glass.

15. Optical instruments are made with ____.

16. The raw materials required for manufac-

ture of ceramics are ____.

17. Simple pottery (Terra-cota) articles are

____.

18. Earthen ware is ____ pottery.

19. The polymeric organic substance is com-

monly known as ____.

20. ____ derived from amino acids are exam-

ples of condensation polymers.

21. ____ is the main constituent in natural

fibers.

22. Example of fibers from melt spinning is

____,____.

23. Cold creams are ____of oil and water.

24. Chemical composition of talc is __

25. First synthetic dye was prepared b

26. The ____ impart colour to the dye

27. The function of oxochrome is ___

28. Examples of chromophore ____.

29. Examples of oxochrome: ____.

30. A substance used in prevention, di

treatment or cure of a disease is

____.

31. Examples of Harmones : ____.

32. Drugs given to the patient in ore modified form are ____.

33. Petrol is a mixture of ____.

34. Chemicals obtained from petrol ar

35. Example of mixed fertilizer ____.

ANSWERS

1) Lime stone, Clay; 2) 17000

19000C; 3) Gypsum; 4) frozen liqu

super cooled liquid; 5) calcium silic

calcium aluminates; 6) Sodium sili

(Na2Sio

3), Calcium silicate (CaSio

3

Sand (4Sio2); 7) Soda ash (Na

2

Limestone (CaCo3), and Sand (4Sio

Batch; 9) cullet; 10) lowering of me

point; 11) 10000C; 12) glass gall

Annealing; 14) Pyrex or Borosilicate

quartz glass; 16) clay, felspar, and

17) porous; 18) glazed; 19) resins

Poly peptides; 21) Cellulose; 22) N

Dacron; 23) emulsions; 24) Magne

silicate; 25) William Henry Perkin

chromophor; 27) intensifies the colo

the dye and attaches the colour to the

28) -NO2,-NO,-N=N-,C=O,C=S; 2

OH,-COOH, -SO3H

2- NH

2, NHR,

30) drug; 31) Insulin, cortisone

Pharmaceuticals; 33) Hydrocarbons

Petrochemicals; 35) Nitrophosk.

IMPORTANT QUESTION

1 Mark

1. What is the use of adding cullet to

materials of glass?2. What are primary nutri-

ents?

3. What is the use of

Micronutrients?

4. What is annealing?

5. What is cracking?

2 Marks

1. Draw the structures of paracetam

aspirin?

2. What are the characteristics of

quality of face powder?

3. Write a short note on earthenware

4. Define a) Plastic b) Adhesive

4 Marks

1. What is a drug? What are the qua

an ideal drug?2. What is a drug? How are they clas

per therapeutic action?

3. Describe the manufacturing of cem

5 Marks

1. Draw a neat diagram of fraction

petroleum and label its parts?

2. Sketch the cement manufacture pl


íœ{ºÐ]lÇ l 20 l 2014 Physical Science 1Bit Bank

Tips:

• First attempt all 14 questions asper choice i.e. 2 marks questions-5,one mark questions -4, four marksquestions - 4, and one diagram (5marks).

• If time permits then answer addition-al questions.

• Try to avoid spelling mistakes.

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Bhavita20.02.2014eng--Physical Science Bit Bank