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PHYSICAL SCIENCE
Preparation Tips
Important Questions
th
Class
Important Bits
2
10th Special
Physical Science
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Physical Science.. Success path
Prepared by:
A.V. Sudhakar,
Senior Faculty
1. HEAT
1.
2.
3.
4.
5.
6.
7.
8.
9.
10.
11.
12.
13.
14.
Latent heat of fusion for ice is ____.
S.I Unit of specific heat is ____.
Specific heat ____.
Latent heat of vaporization of water is
____.
The process of converting solid into liquid
is called ____.
The amount of a water vapour present in
air is called____.
_____ is the reverse process of evaporation.
Evaporation is a ____ phenomenon.
Conservation of steam into liquid is called
____.
The water droplets condensed on cold surfaces is called ____.
1 Calorie = ____ joule
The temperature of a steel rod is 330K. Its
temperature ºC is ____.
____ is used as a coolant.
Rate of evaporation depends on ____,
____, ____.
1)80 cal / gm;
ANSWERS
2) J Kg-1k-1;
3)  S =  Q   ;
 m∆T  

4) 540 cal/gm; 5) melting;
6) Humidity;
7) condensation;
8) cooling;
9) condensation;
10) Dew;
11) 4.186;
12) 57ºc;
13) Water;
14) Surface Area,Humidity, Temperature;
IMPORTANT QUESTIONS
1 Mark
1. Convert 30ºC into Kelven Scale?
A. K = C+273; T = 30+273=303k
2. What is latent heat of vapourization?
A. The heat energy required to change 1 gm
of liquid to gas at constant temperature is
called latent heat of vapourization.
3. Why do we sweat while doing a work?
A. When we work our bodies produce heat.
As a result the temperature of the skin
becomes higher and water in the sweat
glands start evaporating. This evaporation
cools the body.
4. What is humidity?
A. The amount of water vapour present in air
is called humidity.
5. What are the factors affecting rate of
evaporation?
A. Surface area, temperature and amount of
water vapour already present in the surrounding air.
6. A desert is very hot in the day and very
cool at night why?
A. Because low specific heat capacity air
above earth heated up quickly in the day
and cooled quickly at night.
7. Why does ice floats on water?
A. When water converts into ice its volume
increases so density decreases. Hence density of ice is less than water so ice floats
on water.
8. What is the effect of pressure on melting
point of ice?
A. With increase in pressure the melting
point of ice reduces.
9. What is the major difference between boiling and evaporation?
A. Evaporation is the surface phenomenon
while boiling is a bulk phenomenon.
10. What is the value of latent heat of fusion
of ice?
A. 80 cal/gm
2 Marks
1. Explain why dogs pant during hot summerdays using the concept of evaporation?
2. Why do we get dew on the surface of a
cold soft drink bottle kept in open air?
3. Write the differences between evaporation
and boiling?
4. What happens to the water when wet
clothes dry?
5. What happens, when water is kept in a
refrigerator?
4 Marks
1. Your teacher made an experiment that
shows the information of dew and frost.
Explain how you show they effect on the
rate of evaporation?
2. Define evaporation. Explain what are the
affecting factors of evaporation and how
they effect on the rate of evaporation?
3. Determine the specific heat of solid experimentally?
4. How do you appreciate the role of the
higher specific heat of water in stabilizing
atmospheric temperature during winter
and summer seasons?
7. Which metal is used in the manufacture of
Diwali crackers?
A. Magnesium.
8. Which gas is used in the chips like Lays
and Kurkure’s?
A. Nitrogen gas
9. Write the formula of rust?
A. Fe2O3.XH2O
10. Which type of reaction involved when silver bromide is exposed to sunlight?
A. Photo chemical reaction.
2. CHEMICAL REACTIONS
AND EQUATIONS
1. ____ chemical reaction is involved in the
corrosion of iron.
2. ____ reaction involved when silver chloride is exposed to sunlight.
3. Rancidity is an ____ reaction.
4. The decomposition of vegetables into
compost is an examples of ____ reaction.
5. By painting we can prevent ____.
6. Chemical formula of rust is ____.
7. Stainless steel is a mixture of Iron with
____and chromium.
8. Respiration is a ____reaction.
9. Examples of Antioxidants are ____.
10. CuO +H2 → Cu+H2O is ____ reaction.
ANSWERS
1)Oxidation; 2) Photo chemical reaction;
3) oxidation; 4) oxidation (or) fermentation; 5) corrosion; 6) Fe2O3.XH2O;
7) Carbon, nickel; 8) exothermic;
9) Vitamin C and E; 10) Redox reaction.
IMPORTANT QUESTIONS
1 Mark
1. State important uses of decomposition
reaction?
A. Extract metals from their compounds &
digestion of food.
2. What happens when silver chloride
exposed to sunlight?
A. 2 AgCl →2Ag+Cl2↑
3. Why photosynthesis reaction considered
as endothermic reaction?
A. During photosynthesis plants absorb heat
from sunlight so photosynthesis reaction
is example for endothermic reaction.
4. What is antioxidant?
A. The substance which is used to prevent
oxidation are called antioxidants.
5. Why do we apply paint on iron articles?
A. To prevent corrosion.
6. Give any two examples of double displacement reactions?
A. (i) BaCl2+Na2SO4→2NaCl+BaSO4
(ii) 2KI+Pb(NO3)2→ PbI2+2KNO3
2 Marks
1. What do you mean by corrosion? How can
you prevent it?
2. Why does respiration reaction considered
as exothermic reaction? Explain?
3. A shiny brown coloured ‘X’ on heating in
air becomes black colour. Can u predict
the element ‘X’ and the black colour substance formed? How do you support your
predictions?
4. What is meant by precipitation reaction?
Give example?
4 Marks
1. Take two beakers and prepare lead nitrate
aqueous solution and Potassium iodide
aqueous solutions. What are the colours of
solutions. Now mix them in another
beaker. What happens? What type of
chemical reaction it is? What are products
obtained?
2. Latha take some quantity of powder of a
substance in a test tube. Heated it with
spirit lamp. A gas was liberated. She send
the gas into another test tube. The colour
of solution in the second test tube turned
into milk white?
1) Which substance was heated
2) Whic gas is liberated
3) What was the solution taken in second
test tube
4) Which type of chemical reactions
involved the experiment
3. Balance the following chemical equations
including the physical states?
a) C6H12O6 →C2H5OH + CO2
b) Fe+O2 →Fe2O3
c) NH3+Cl2→N2H4+NH4Cl
d) Na+H2O→NaOH+H2
4. Give some daily life oxidation Reactions?
Sir C.V. Raman
explained the phenomenon of light scattering in
gases and liquids. He found
experimentally that the frequency of scattered light by the
liquids is greater than
the frequency of
incident light. This
is called Raman
Effect.
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3. REFLECTION OF LIGHT
BY DIFFERENT SURFACES
1. We get a diminished image with a concave
mirror when the object is placed ____.
2. The drivers mirror used in automobiles is
____.
3. The distance between pole and focus is
____.
4. Mirror formula is ____.
5. Light chooser the path which takes the
least time to travel. This is called____
principle.
6. The geometric centre of the mirror is
____.
7. A concave mirror can form a ____.
8. Convex and concave mirrors are known
collectively as ____.
9. Virtual image cannot be received on a
____.
10. ____ mirrors are used in head lights of
vehicles.
ANSWERS
1) beyond C; 2) convex; 3) Focal length;
4)  1 = 1 + 1  ;
 f
u
v
10th Special
ENT specialist?
A. Concave mirrors
9. Preetham saw his face in the cars mirror
and found that his image is small. Which
type of mirror is that?
A. Convex mirror.
10. Which principle is used in the law of
reflection?
A. Fermat principle.
2 Marks
1. How do you find the focal length of a concave mirror?
2. Write the rules for sign convention of
spherical mirrors?
3. Explain the process of making a solar
cooker/heater (or) Make a solar heater/
cooker and explain the process of making.
4. How do you appreciate the role of spherical mirrors in daily life? (or) What are the
applications of spherical mirrors in daily
life?
5. Write any two uses of convex and concave
mirrors in our daily life?
6. Why does an image suffer lateral inversion?
5) Fermat; 6) pole;
7) real (or) virtual image; 8) Spherical
mirror; 9) screen; 10) concave.
IMPORTANT QUESTIONS
1 Mark
1. State Fermat’s principle?
A. It states that the light selects the path
which takes the least time to travel. It is
also applicable to reflection of light.
2. Which objects at your home act as spherical mirrors?
A. Cooking vessels, sink, spoons.
4 Marks
1. How do you support your answer to
“When light gets reflected from a surface,
it selects the path that takes the least
time”?
2. What is magnification? Derive the formula for magnification of spherical mirrors?
3. Write the experimental method in verification laws of reflection in plane mirrors?
4. Write the experimental method to measures the distances of object and image
using concave mirror? And write the table
for observations?
4. ACIDS, BASES AND SALTS
3. Which type of mirrors are used in head
light of vehicles?
A. Concave mirrors are used in the head
lights of vehicles.
4. Why does our image appear thin or
bulged?
A. Due to converging (or) diverging of light
rays from the mirror.
5. Write the mirror formula?
 1 1 1
= +  ƒ: focal length, u : object
 f u v
A. 
distance, v = image distance
6. Which mirrors are used in saloons and
sweets shops?
A. Plane mirrors
7. Which principle involved in the working
of periscope?
A. Principle of reflection of light.
8. Which mirrors are used by dentists and
1. The colour of Methyl orange indicator in
acidic medium is____.
2. The colour of phenophalein indicator in
Basic medium is ____.
3. ____ medicine is used for treating indigestion.
4. Bleaching powder is represented by formula ____.
5. The acid forms in stomach is ____.
6. Many salts absorb water from atmosphere
this property is called ____.
7. If pH of rain water is less than 5.6 it is
called____.
8. Water soluble bases are known as ____.
9. Formula of plaster of Paris____.
10. ____is derived from tomato and turns blue
litmus to red.
ANSWERS
1)Red; 2) pink; 3) Antacid; 4) CaOCl2;
5) HCl; 6) Crystallisation; 7) Acid rain;
8) Alkali; 9) CaSO4.½H2O; 10) Tartaric
acid.
IMPORTANT QUESTIONS
1 Mark
1. Why does distilled water not conduct electricity.
A. Distilled water does not conduct electricity due to no ions present in distilled water.
2. Give two examples of neutralization
3
Physical Science
reaction.
A. NaOH+HCl →NaCl+H2O
NaOH+CH3COOH →CH3COONa+H2O
3. What is acid rain?
A. When pH of rain water is less than 5.6, it is
called acid rain.
4. Plaster of Paris should be stored in a moisture proof container. Explain.
A. The Plastic of Paris should be stored in the
moisture proof container as it absorbs water from moisture and turns in to Gypsum.
5. What are Amphoteric oxides.
A. Oxides capable of showing properties for
both acids & bases.
6. Which substance is used for making
chalks and fire proof material.
A. Plaster of Paris.
7. Give any two examples of olfactory indicatiors.
A. Vanilla essence & clove oil.
8. Write the formula of baking soda & washing soda.
A. Baking soda : NaHCO3
Washing Soda : Na2CO3.10H2O
9. Which acid derived from lemon and turn
blue litmus in Red.
A. Citric acid.
10. Define universal pH indicator.
A. A mixture of several indicator is called
universal pH indicator.
11. Define alkalis.
A. Bases which are soluble in water are
called alkalis.
12. Which substance used to control the stomach pain causes due to indigestion.
A. Antacid.
3. Acids produce ions only in aqueous solution? Justify your answer with an activity.
4. Write any 4 uses of (a) Washing soda
(b) Baking soda.
5. REFRACTION OF LIGHT
AT PLANE SURFACES
1.
2.
3.
4.
Speed of light in vacuum is ____.
Mirage is an example of ____.
____is the basic principle of optical fibre.
The unit of refractive index is ____.
5. The angle of refraction for critical angles
is ____.
6. The critical angle of diamond is ____.
7. Refractive index of glass is 3/2. Then the
speed of light in glass is ____.
8. n1sin i=n2sin r is called ____.
9. A lemon kept in a glass of water appears to
be ____
10. Refractive index of water is ____.
ANSWERS
m/sec; 2) Total internal reflec1)
tion; 3) Total internal reflection; 4) No
units; 5) 90º; 6) 24.4º; 7) 2×108 m/sec;
8) Snell’s law; 9) Bigger ;10) 1.33.
3×108
IMPORTANT QUESTIONS
2 Marks
1. What happens when an acid or base is
mixed with water?
2. Why does distilled water not conduct electricity where rain water does?
3. Plaster of paris should be stored in a moisture proof container explain why?
4. Fresh milk has a pH of 6. How does the pH
change as it turns to curd? Explain your
answer?
5. What is baking powder? How does it
make the cake soft and spongy?
4 Marks
1. Write the formulae for the following salts.
(a) Sodium sulphate (b) Ammonium chloride. Identify the acids and bases for
which the above salts are obtained also
write chemical equations for the reactions
between such acids and bases which type
of chemical reactions they are?
2. Compounds such as alcohols and glucose
contain hydrogen but are not categorized
as acids. Describe an activity to prove it.
1 Mark
1. What is optically denser medium?
A. The medium in which speed of light is less
is called optically denser medium.
2. Determine the refractive index of benzene
if the critical angle of it is 42º?
A. Critical angle of benzene (C) = 42º
n=
1
1
=
= 1.51
sin C sin 42 0
3. What is lateral shift?
A. Side wise shift when a ray of light is inci-
Niels
Henrik David
Bohr was a Danish
physicist who made foundational contributions to understanding atomic structure and
quantum theory, for which he
received the Nobel Prize
in physics in 1922.
Bohr was also a
philosopher and
a promoter.
4
4.
A.
5.
A.
6.
dent obliquely on a parallel sided glass
slab.
Name the colour of light for which critical
angle is minimum?
Violet.
What are applications of total internal
reflection?
Formation of mirages, brilliance of diamond, working of optical fibre.
Find the critical angle for a material of
refractive index √2?
9. The power of convex lens is____.
10. The ray from the distant object, falling on
the convex lens pass through____.
1
1
⇒ SinC =
= C = 450
µ
2
When is angle of incidence is equal to the
angle of refraction?
When light travels perpendicular to surface it will not undergo any refraction. So
angle of incidence is equal to angle of
refraction.
What is the principle involved in the optical fibre?
Total internal reflection.
Define shift?
The perpendicular distance between the
emergent and incident rays which are parallel is called shift.
Is the refractive index for a given pair of
medium depend on the angle of incidence?
No. It is independent of the angle of incidence.
6) Focal length; 7) +½; 8) away;
9) positive; 10) focal point.
A. SinC =
7.
A.
8.
A.
9.
A.
10.
A.
10th Special
2 Marks
1. Why is it difficult to shoot a fish swimming in water?
2. Take a bright metal ball and make it black
with soot in a candle flame. Immerse it in
water. How does it appear and why?
3. How do you appreciate the role of Fermat
principle in drawing ray diagrams.
4. What is the angle of deviation produced
by a glass slab? Explain with ray diagram?
4 Marks
1. Derive the Snell’s formula from Fermat
principle? (or) Derive the formula in relation with angle of incidence and angle of
refraction?
2. What is meant by Total internal reflection
and derive the relation between critical
angle and total internal reflection?
3. Explain the experiment that showing the
relation between angle of incidence and
angle of refraction through the figure?
4. Explain the experiment that showing the
determination of position and nature of
image formed by a glass slab through the
figure?
6. REFRACTION OF LIGHT
AT CURVED SURFACES
1. S.I Unit of the power of a lens is____.
2. The power of a concave lens is____.
3. Focal length of a convex lens is ____
when it is kept in water.
4. Lens formula is given by____.
5. Lens maker formula is ____.
6. The distance between the principle focus
and optical centre of the lens is ____.
7. The power of a convex lens of focal length
50 cm= ____Dioptre.
8. When a ray of light passes from denser to
rarer medium it bends____to the normal.
ANSWERS
1) dioptre; 2) negative; 3) increases;
 1 1 1
= − ;
 f v u
4) 
1
 1
1 
= (n − 1) −
  ;
f
R
R

1
2 

5) 
IMPORTANT QUESTIONS
1 Mark
1. Define focal point?
A. The rays coming from the sun parallel to
the principal axis of concave mirror converge to a point. This point is called Focus
or focal point.
2. Give two uses of a convex lens?
A. (i) used in projectors
(ii) Cameras
3. Do only convex lens converge?
A. No, a concave mirror also converge.
4. What is positive lens?
A. Convex lens.
5. Define principal axis?
A. The line joining the centre of curvature
and the pole is called principal axis.
6. Write the lens formula?
1 1 1 
A.  − = 
v u f 
7. Write the lens makers formula?
A.
1
1
1
= (n − 1)  − 
f
R
R
2
 1
8. Which lens will form both real and virtual
images?
A. Plane mirror.
9. What is negative lens?
A. Concave lens.
10. Draw the plane-concave mirror?
A.
2 Marks
1. Preethi tells Sushant that the double convex lens behaves like a convergent lens.
But Sushant knows that Preethi assertion
is wrong and corrected Preethi by asking
some questions. What are the questions
asked by Sushant?
2. Draw a ray diagram for the following
Physical Science
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positions and explain the nature and position of image i) Object is placed at C2
ii) Object is placed between F2 and optic
centre P?
3. A plane convex lens whose n=1.5 has a
curved surface of radius 15cm what is its
focal length? Why do you see a diminished image? How could this happen?
4. Write the steps involved in sign convention used in lenses?
4 Marks
1. Derive the formula of image formation in
refraction at curved surfaces?
2. Derive the lens formula?
3. Derive the lens maker’s formula?
4. Write the experimental method and apparatus required in finding out the image formation using convex lens?
7. HUMAN EYE AND
COLOURFUL WORLD
1. The value of least distance of distinct
vision is about____.
2. The distance between the eyes lens and
retina is about____.
3. The maximum focal length of the eye lens
is about____.
4. Myopia can be corrected by using ____
lens.
5. Hyper metropia can be corrected by using
____ lens.
6. Angle of vision for a healthy human is
____.
7. The process of adjusting focal length is
called ____.
8. ____explained the phenomenon of scattering of light in gages and liquids.
9. The human eye forms the image of an
object____.
10. The splitting of white light into different
colour____is called____.
ANSWERS
1) 25 cms; 2) 2.5 cms; 3) 2.27 cms;
4) biconcave; 5) biconvex; 6) 600;
7) accommodation; 8) Sir. C.V. Raman;
9) retina; 10) VIBGYOR, dispersion.
IMPORTANT QUESTIONS
1 Mark
1. What are rods?
A. Rods are the receptors which identify the
colour.
2. What is retina?
A. The retina is delicate membrane, which
acts as a screen, the eye lens formula a real
and inverted image of an object on the
retina.
3. What are cones?
A. Cones are the receptors identify the intensity of light.
4. Which colour is best for school buses?
A. Yellow (or) Orange.
5. What is an optic nerve?
A. Optic nerve is nerve which transmit the
light signals to the brain.
6. What type of lens used to correct myopia?
A. Bi concave.
7. State the role of ciliary muscles in accommodation?
A. It can adjust the focal length of the eye
lens.
8. What is the function of pupil in human
eye?
A. It allows the light falling on iris.
9. Write the formula of refractive index of
the prism?
 A+D 
Sin 

 2 
A. µ =
A
Sin
2
10. Name the molecules responsible for blue
sky?
A. Nitrogen & oxygen molecules.
2 Marks
1. How do you appreciate the working of
“iris”?
2. Have you seen a rainbow in the sky after
rain? How is it formed?
3. Why the red signal is used for danger signals?
4. Why does the sky sometimes appear
white?
5. Glass is known to be transparent material
but ground glass is opaque and white in
colour why?
6. A person is viewing an extended objects if
a converging lens is placed in front of his
eye, will he feel that the size of object has
increased. Why?
4 Marks
1. Derive the formula for refractive index of
a prism?
2. Write the different characteristics of red
colour and violet colours in dispersion of
light?
3. Explain briefly the reasons for the blue of
the sky?
4. Write the experimental procedure of finding the refractive index of a prism?
5. Explain the formation of rainbow with the
help of water drop diagram?
Max
Karl Ernst Ludwig
Plank was a German theoretical physicist who originated quantum theory, which won
him the Nobel Prize in Physics in
1918. Plank made many contributions
to theoretical physics, but his fame
rests primarily on his role an originator of the quantum theory?
This theory revolutionized
human understanding
of atomic and subatomic processes.
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8. STRUCTURE OF ATOM
1. The electronic configuration of cu(29)
____.
2. Elliptical orbits are introduced by____.
3. The subshell of the orbital for l = 1 is
____.
4. ____is a group of wavelength.
5. Splitting of spectral lines due to magnetic
field is called____.
6. Splitting of spectral lines in the presence
of electric field is called____.
7. Stationary orbits are introduced by ____.
8. The electronic configurations of Cr is
____.
9. The elements in which outermost orbitals
are completely filled are called____.
10. Short notation of electron configuration is
____.
ANSWERS
1) [(Ar)4s13d10]; 2) sommerfeld; 3) p;
4) spectrum; 5) Zeeman effect; 6) stark
effect; 7) Niels Bohr; 8) [Ar]4s13d5;
9) inert gas;10) nlx.
10th Special
9. Write the electronic configuration of
chromium?
A. 1s22s22p63s23p64s13d5
10. What is the shape of d-orbital?
A. Double dumbell.
2 Marks
1. Rainbow is an example for continuous
spectrum explain? or Define continuous
spectrum? Explain with one example?
2. How many elliptical orbits are added by
sommerfeld in third bohr’s orbit? What
was the purpose of adding these elliptical
orbits?
3. Which rule is violated in the electronic
configuration 1S0 2s2 2p4? (or) The following electronic configuration does not
support the Aufbau principle Why 1S0 2s2
2p4?
4. Write the four quantum numbers for the
differentiating electrons of sodium atom?
(or) Write the four quantum for the
valence electron of sodium (Na) atom?
5. Write the four quantum numbers for 1S1
electron. (or) Write the four quantum
numbers for hydrogen atom?
Physical Science
IMPORTANT QUESTIONS
1 Mark
1. What are lanthanoids?
A. Elements from 58Ce to 71Lu are called
Lanthanoids.
2. Write the name of the element family of
16 group?
A. Chalcogen family.
3. State Mendeleeff's periodic law?
A. The physical and chemical properties of
the elements are the periodic functions of
the their atomic weights.
z
y (Spherical)
A.
4 Marks
1. What are the postulates of Bohr atomic
model? Write the defects on it?
2. In an atom the number of electrons in N.
Shell is equal to the number of electrons in
K and L and M shells. Answer the following questions?
(i) Which is the outer most shell?
(ii) How many electrons are there in its
outermost shell.
(iii)What is the atomic number.
(iv) Write the electronic configuration of
the elements.
3. How many elliptical orbits are added by
sommerfeld in third Bohr’s orbit? What
was the purpose of adding these elliptical
orbits?
4. Explain the significance of three quantum
numbers in predicting the positions of an
electron in an atom?
x
7. Who proposed principle quantum number?
A. Niel’s Bohr.
8. What is Zeeman effect?
A. Splitting of spectral lines in presence of
magnetic field is called Zeeman effect.
9. CLASSIFICATION OF
ELEMENTS
THE PERIODIC TABLE
1.
2.
3.
4.
5.
6.
7.
8.
9.
10.
11.
12.
d block elements are also called ____.
Electro negativity is assigned by ____.
Father of periodic table____.
Atomic radius is measured in ____units.
Inner transition elements are____block
elements.
II a group elements are called____.
Noble gases belongs to ____ group of
periodic table.
Group IA is called____family.
____is the most electronegative element.
Gallium is named by Mendeleeff as ____.
VIIA group elements are called ____.
____is the least electronegative element.
ANSWERS
1) Transition elements; 2) Pauling;
3) Mendeleeff; 4) Aº; 5) f block; 6) Alkali
earth metal; 7) 18th; 8) Alkali metal;
9) fluorine; 10) Eka aluminium;
11) Haloge-ns; 12) cesium.
the advantage of this kind of classifications?
2. What is a periodic property? How do the
following properties change in a group
and period? Explain?
(a) Atomic radius
(b) Ionization energy
(c) Electron affinity
(d) Electronegativity
3. What is Ionization energy? Explain the
factors affect the ionization energy?
4. What are the limitations of Mendeleeff’s
periodic table. How could the modern
periodic table over come the limitations of
Mendeleev’s table.
10. CHEMICAL BONDING
1. Ionic compounds dissolved in ____ solvents.
2. Example for polar solvents is ____.
3. The shape of BeCl2 is ____.
4. Electro positivity is also called as ____.
5. Valence bond theory was proposed by
____.
6. The shape of NH3 is ____.
7. 1 nanometer ____Meter
8. Examples of Triple bond molecules ____.
9. General electronic configuration of Noble
gas____.
10. The noble element which is exception of
octet rule____.
IMPORTANT QUESTIONS
1 Mark
1. Give the relation between c, υ and λ?
A. c = υλ
2. Write the four quantum numbers for the
differentiating electron of sodium (Na)?
A. n = 3, l = 0, m = 0, s = +½.or -½
3. What is the value of planks constant?
A. 6.625×10-27 erg sec (or) 6.625×10-34 Js
4. What is spectrum?
A. A group of frequencies (or) wave length is
called spectrum.
5. Define Pauli exclusion principle?
A. No two electrons can have same four
quantum numbers.
6. Draw the shape of s-orbital?
5
4.
A.
5.
A.
What is the unit of ionization energy?
ev (or) K cal / mole (or) KJ/mole.
What are actinoids?
Elements from 90Th to 103Lr are called
Actinoids.
6. Write the formula proposal by Milliken to
measure electronegativity?
A. E.N =
I .E + E . A
2
7. Give any two examples of Dobereiner’s
traids?
A. Li, Na, K
S, Se,Te
8. Write the electronic configuration of
Transition elements?
A. ns2np6(n−1)d1−10
9. Write the Nobel gas elements?
A. He, Ne, Ar, Kr, Xe, Rn
10. Who is the father of periodic table?
A. Mendeleeff.
2 Marks
1. Name two elements that you would expect
to have chemical properties similar to Mg.
What is the basis for your choice?
2. An element has atomic number 19. Where
would you expect this element in the periodic table and why?
3. Explain New Lands concept of octaves?
4. Second ionization energy of an element is
higher than its first ionization energy
why?
5. All alkali metals are solids but hydrogen is
a gas with di atomic molecules. Do you
justify the inclusion of Hydrogen in first
group with alkali metals?
6. Why Mendeleeff had to leave certain
blank spaces in his periodic table? What is
your explanation for this?
4 Marks
1. Explain how the elements are classified
into s, p, d, f in the Periodic table and give
ANSWERS
1) polar; 2) H2O; 3) Linear; 4) Metallic
character;
5)
Linus
Pauling;
6) Pyramidal; 7) 10-9; 8) N2,C2H2;
9) ns2np6; 10) Helium
IMPORTANT QUESTIONS
1 Mark
1. General electronic configuration of noble
gases?
A. ns2np6
2. What is the shape of Ammonia?
A. Pyramidal.
3. Give example for double bonded molecule?
A. O2, C2H4
4. Bond angle present in H2O molecule?
A. 104º. 311
5. Who proposed valance bond theory?
A. Linus Pauling.
6. Expand VSEPRT?
A. Valence – shell- electron – pair-repulsionTheory.
7. Examples of non-pair solvents?
A. CCl4, C6H6, CS2
8. Write the Lewis dot structure of Ar?
A.
9. Examples of triple bond molecules?
Hans
Christian Oersted
was one of the leading
scientist of the 19th century,
played a crucial role in understanding electromagnetism. The
unit of magnetic field strength is
named Oersted in his honour.
Oersted was made a foreign
member of the Royal
Swedish Academy of
Sciences in 1822.
6
A. N2, C2H2, HCN
10. Example of FCC molecule?
A. NaCl
2 Marks
1. Predict the reasons for low melting point
of covalent compounds when compared
with ionic compound?
2. Draw simple diagrams to show how electrons are arranged in the following covalent molecules?
a) Calcium oxide [CaO]
b) Water [H2O]
c) Chlorine [Cl2]
3. Draw the simple diagrams to show how
electrons are arranged in the following
covalent molecules?
a) Ammonia (NH3)
b) Methane (CH4)
4. Represent the lewis dot structure for the
following?
He, Kr, Ne, Xe, Ar, Rn.
5. Represent each of the following atoms
using lewis notation?
a) Berylium
b) Calcium
c) Lithium
4 Marks
1. Explain what type bond is formed in
AlCl3?
2. Explain VSEPRT theory?
3. What is hybridization? Explain the formation of the following molecules using
hybridization?
(b)BF3
(a) BeCl2
4. Explain Lew’s approach to chemical
bonding?
11. ELECTRIC CURRENT
1. The Kilowatt hour is the unit of ____
2. The S.I Unit of potential difference is
____.
3. Units of resistance____.
4. The surface of earth is taken to be at ____
potential.
5. Kirchoff’s loop law is based on the conservation of____.
6. Voltmeter is always connected in____ in a
circuit.
7. Units of specific resistant ____.
8. A thick wire has a ____ resistance than a
thin wire.
9. S.I unit of electric power is____.
10. 1 KWH = ____Jouls.
ANSWERS
1) Electric energy; 2) Volt; 3) Ohm;
4) Zero; 5) energy; 6) parallel; 7) Ohmmeter; 8) less; 9)watt; 10) 36×105.
10th Special
ν
6
=I =
= 0.4amp
R
15
What do you mean by short circuit?
A sudden flow of a very large circuit due
to direct current of live and neutral wire is
called short circuit.
What is the shape of V-I shape for a metallic wire?
A straight line passing through origin.
A. I =
5.
A.
6.
A.
V
I
7. Draw the symbol of Resistor?
A.
8. Define Resistivity?
A. Resistivity of the material is the resistance
per unit length of a unit cross section of
the material.
9. Define ohmic conductors?
A. The materials which obeys ohm’s law are
called ohmic conductors.
10. Write the ohm’s law?
A. V=IR
2 Marks
1. What do you mean by electric shock?
Explain how it takes place?
2. Why do we use fuses in household circuits?
3. Why should we connect the electric appliances in parallel to household circuit?
4. Explain the working of multimeter?
5. Define ohmic and non- ohmic conductors
with examples?
4 Marks
1. State Ohm’s law. Suggest an experiment
to verify it and explain the procedure?
2. What are the factors one which the resistance of conductor depends? Give the corresponding relation?
3. Derive the equation for resultant resistance of resistors in series combination?
4. Three resistors connect as shown in figure
derive the equation for resultant resistance?
12. ELECTROMAGNETISM
1. The S.I unit of magnetic field is____.
2. Faraday’s law of induction is the consequence of____.
Physical Science
3. The device used for producing electric
current is called ____.
4. Unit of magnetic flux____.
5. A metallic wire carrying an electric current is associated with it’s a____.
6. A current that flows in the same direction
is____.
7. The current that reverses its direction is
____current.
8. An electric motor is a device that converts
____ energy into ____ energy.
9. Name the long wire wound in close
packed helix____.
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13. PRINCIPLES OF
METALLURGY
1. The impurity present in the ore is called as
____.
2. Galena is an ore of____.
3. The purpose of smelting an ore is to ____
It.
4. The formula of rust ____.
5. Smelting is carried out in____furnace.
ANSWERS
1) Tesla; 2) law of conservation of energy; 3) Generator; 4) Weber.; 5) magnetic
field; 6) direct; 7) alternate; 8) electric,
Mechanical; 9) solenoid
IMPORTANT QUESTIONS
1 Mark
1. Which field has both strength and direction are constant?
A. Uniform magnetic field.
2. Name the long wire wound in a close
packed helix?
A. Solenoid
3. What is the unit of magnetic flux density?
A. Weber /mt2 (or) Tesla.
4. List two sources of magnetic fields?
A. Magnet, moving charges, electric current
5. What is Induced current?
A. The current produced by moving a straight
line in a magnetic field is called induced
current.
6. What is Induced EMF?
A. The EMF produced by moving a straight
line in a magnetic field is called induced
EMF.
7. What are the imaginary lines that helps us
to understand the nature of the field?
A. Magnetic lines.
8. What is the flux through unit area perpendicular other field?
A. Flux density (or) Magnetic induction
9. What happens when a coil without current
is made to rotate as a magnetic field?
A. Electricity is generated.
10. Mention two uses of solenoid?
A. It is used in electric bells, fans and motors.
2 Marks
1. How do you appreciate the variation
between magnetic field and electricity that
changed the life style of mankind?
2. Give a few application of Faraday’s law of
induction in daily life?
3. Which of the various methods of current
generation protects nature well. Give
examples to support your answer?
6. The new substance added to ore to remove
gangue is called____.
7. Aluminium is used as a reducing agent in
____ process.
8. Roasting is carried out in____furnace.
9. ____ are least reactive elements.
10. Sulphide ores are concentrated by ____
process.
11. The formula of Bauxite ____.
12. Name the pyro chemical process in which
ore is heated in the absence of air____.
ANSWERS
1) Gangue; 2) pb; 3) Reduce;
4) Fe2O3XH2O; 5) Blast; 6) flux;
7) Thermite; 8) Reverberatory; 9) Au, Ag;
10) froth floatation; 11) Al2O3.2H2O;
12) calcination.
IMPORTANT QUESTIONS
1 Mark
1. What is poling?
A. The method of removing impurities either
for gases (or) liquids get them oxidized
and form slag over surface of molten
metal is called poling.
2. What is thermite process?
A. The exothermic reaction in which highly
reactive metals displaces low reactive
metals is used in thermite process.
3. Write the formula’s of Gypsum, plaster of
paris?
IMPORTANT QUESTIONS
1 Mark
1. What are the examples of non-ohmic conductors?
A. LED, Semiconductors.
2. Which material act as the best conductor?
A. Silver
3. How is power related to current and voltage?
A. P = V×I
4. A battery of 6v is applied across a resistance of 15Ω. Find the current flowing
through the circuit?
4 Marks
1. How can you verify that a current carrying
wire produces a magnetic field with the
help of experiment?
2. Write any four applications of faraday
laws of induction in daily life?
3. Explain different ways induced current in
a coils?
4. Explain the working of AC electric generator with a neat diagram?
5. Explain the working electric motor with
neat diagram?
Linus Pauling..
The world's one of the
greatest scientists and a
great humanist. He was
acknowledged as the most influential chemist. He is the only person ever to receive two
unshared Nobel Prizesfor Chemistry (1954)
and for Peace
(1962).
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A. Gypsum: CaSO4, 2H2O, Plaster of Paris :
CaSO4.½H2O
4. What is calcination?
A. Calcination is a pyrochemical process in
which the ore is heated in the absence of
air.
5. What is froth flotation?
A. The impurities of the ore is wetted by producing froth in water is called froth flotation.
6. Write the names of any two ores of Fe?
A. Hematite: Fe2O3 Magnetite : Fe3O4
7. What is corrosion?
A. Process of slowly coated with oxides (or)
other salts of the metal and forms thin layers.
8. Why is carbon not used for reducing aluminium from aluminium oxide?
A. The oxide of aluminium is very stable and
can be reduced by electrolytic process.
9. Mention two methods which produce very
pure metals?
A. Electrolytic reduction, smelting are two
methods which produce very pure metals.
10. Name two metals other than aluminium
which are obtained by electrolytic reduction?
A. Sodium and Magnesium.
2 Marks
1. Write short notes on froth floating
process?
2. Write any 4 examples of ores of sulphides?
3. Write a note on dressing of ore in metallurgy?
4. How do you extract the metals at the top
of the activities series?
5. What is difference between blast furnace
and reverberatory furnace?
10th Special
14. CARBON AND
ITS COMPOUNDS
1. Very dilute solution of ethanoic acid ____.
2. When sodium metal is dropped in
ethanol____ gas will be released.
3. Soaps are the alkali salts of____.
4. Number of single covalent bonds in
ammonia are____.
5. Sodium lauryl sulphate is an example of
____.
6. A sweet odour substance formed by the
reactor of an alcohol and a carboxylic and
is____.
7. The first number of homologous series
among alkynes is____.
8. Commercially available ethanol is known
as____.
9. The reactive part of the organic molecule
is called its ____group.
10. CnH2n is the general formula of ____.
11. Hydrocarbons having the general formula
CnH2n+2 are called____.
12. Carbon compounds containing double
bond and triple bonds are called ____.
13. Formula of Ethyl acetate ____.
14. ____catalyst used to in the hydrogenation
of oils.
15. Nano tubes are discovered by which scientist____.
ANSWERS
1) Vinegar; 2) Hydrogen; 3) Higher fatty
acids); 4) Three; 5) Synthetic detergent;
6) Ester; 7) C2H2; 8) rectified spirit; 9) functional; 10)Alkene; 11) Alkanes; 12)Unsaturated compounds;13) CH3COOC2H5;
14) Nickel; 15) Sumio Lijima.
IMPORTANT QUESTIONS
4 Marks
1. Write the short notes on each of the following.
(a) Distillation
(b) Poling
(c) Liquation
(d) Electrolysis.
2. Suggest an experiment to prove that the
presence of air and water are essential for
corrosion. Explain the procedure.
3. Write a note on dressing of ore in metallurgy.
4. What is thermite process? Mention its
application in daily life
1 Mark
1. Nano tubes are discovered by which scientist?
A. Sumio Lijima.
2. What we call a spherical aggregate of soap
molecule in the soap solution in water?
A. Micelle.
3. Which allotropic form of carbon has foot
ball like structure?
A. Buck minister fullerene.
4. Which allotropic form of carbon has layered structure?
Important diagrams (5 Marks)
4. Acids, Bases and Salts:
Draw a neat diagram showing and solution in water conducts electricity and also
label in the diagram.
1. Heat: Draw the diagram and label the
parts to prove that the rate of increase in
temprature depends on the nature of substance.
2. Chemical reactions and equations:
Draw a neat diagram of representing electrolysis of water.
3. Reflection of light by different surfaces:
Draw the ray diagram of reflection of light
in concave mirrors as an object place at.
a) Beyond the centre of curvature (beyond
C)
b) At centre of curvature.
c) In between focus point and centre of
curvature (between F-C).
d) At Focus point.
e) In between pole of the mirror and focus
point (between P-F)
6. Refraction of Light at Curved Surfaces:
1. Draw the ray diagrams when the incident ray passes through the curved surfaces.
a) Rarer medium to denser medium
b) Denser medium to rarer medium.
7. Human Eye and Colourful world: Draw
the structure of human eye and explain its
parts.
8. Structure of Atom:
1. Draw the shapes of s, p, d orbitals.
2. Draw the diagram of electromagnetic
waves and label the parts.
3. Draw the diagram of Moeller chart.
7
Physical Science
A. Graphite
5. What do we call the self linking property
of carbon?
A. Catenation
6. Name the carboxylic acid used as a preservative?
A. Acetic acid is the carboxylic acid used as
a preservative.
7. Name the product other than water formed
on burning of ethanol in air?
A. The product other than water formed on
burning of ethanol is carbondioxide.
8. What happens when a small piece of sodium is dropped into ethanol?
A. When a small piece of sodium is dropped
into ethanol bubbles of hydrogen gas is
produced.
9. What is meant by Rectified spirit?
A. 96% alcohol is called Rectified spirit.
10. What is the formula of Ethyl acetate?
A. CH3COOC2H5
2 Marks
1. Explain with the help of a chemical equation how an addition reaction is used in
vegetable ghee industry?
2. Name the product obtained when ethanol
is oxidized by either chromic Anhydride
(or) alkaline potassium permanganate?
3. Define homologous series of compounds
mention any two characteristics of homologous series?
4. Suggest a chemical test to distinguish
between ethanol and ethonoic acid and
explain procedure?
5. How do you appreciate the role of esters in
everyday life?
4 Marks
1. Write the characteristics of homologous
series of organic compounds?
2. Explain the cleaning action of soaps?
3. Distinguish between esterification and
saponification reaction of organic compounds?
4. Complete the following reactions?
a ) CH 3CH 2OH
conH 2 SO 4


→
Heat
b) CH3COOH+NaHCO3→
Sunlight
c ) CH 4 + Cl 2 
→
Ni
d ) CH 2 = CH 2 + H 2 
→
12. Electromagnetism:
1. Draw the diagram of AC electric generator and label its parts.
2. Draw the diagram of DC electric generator and label its parts.
3. Draw the diagram of electric motor and
label its parts.
4. Draw the diagram of magnetic field
lines when current passes through the
solenoid and label its parts.
13. Principles of Metallurgy:
1. Draw the diagram of magnetic seperator for enrichment of the ore and label
its parts.
2. Draw a neat diagram of reverberatory
furnace and label its parts.
3. Draw a neat diagram of Blast furnace
and label its parts.
4. Draw the diagram showing Froth
MATCHING
Column -I
a) Plaster of Paris
b) Gypsum
c) Bleaching
powder
d) Banking soda
e) Washing soda
Column - II
[d] a) CaOCl2
[e] b) NaHCO3
[a] c) NaCO3
[b] d) CaSO4 ½ H2O
[c] e) CaSO4. 2H2O
Molecule
1) CH4
2) NH3
3) H2O
4) CO2
5) Bcl3
[c]
[d]
[e]
[a]
[b]
Column -I
a) Bauxite
b) Cinnabar
c) Limestone
d) Epsom salt
e) Haematite
[f]
[e]
[d]
[c]
[a]
Bond angles
a) 180º
b) 120º
c) 190º 281
d) 107º
e) 104.5º
Column - II
a) Fe4O3
b) CaSO2.½H2O
c) MgSO4.7H2O
d) CaCO3
e) HgS
f) Al2O3.2H2O
Column -I
1) Alcohol
2) Aldehyde
3) Ketone
[c]
Column - II
O
||
−
C
−
a)
[d]
[a]
O
||
b) −C − OH
c) −OH
4) Carboxylic acid [b]
O
||
d) −C − H
5) Ester
O
||
e) −C − O −
Column -I
a) CH4
b) C2H4
c) C2H2
d) C3HCOOH
e) C3HCC2OH
[e]
[d]
[e]
[b]
[c]
[a]
Column - II
1) Ethanol
2) Ethyne
3) Ethanoic acid
4) Methane
5) Ethene
floatation and label its parts.
14. Carbon and its compounds:
1. Draw the diagrams of Diamond and
Graphite, label the parts.
2. Draw the electronic dot structure of
ethane molecule.
Wohler
Friedrich.. German
chemist who was a student of Berzelius. In attempting to prepare ammonium
cyanate from silver cyanide and
ammonium chloride, he accidentally synthesized urea in
1828. This was the first
organic synthesis,
and shattered the
vitalism theory.
8
10th Special
IMPORTANT CONCEPTS
The average kinetic energy of the molecules is directly proportional to the
obsolute temperature.
Boiling is the process in which the liquid
phase changes to gaseous phase at a constant temperature and constant pressure.
The process of escaping of molecules from
the surface of a liquid at any temperature is
called evaporation and it is a cooling
process.
A Chemical equation is said to be balanced,
when the number of atoms of each element
is same on both reactants side and products
side.
Acidic and basic solutions in water conduct
electricity because they produce hydrogen
ions and hydroxide ions respectively.
A neutral solution has a PH of 7, while an
acidic solution has a PH less than 7 and a
basic solution has a PH more than 7.
The angle of incidence, at which the light
ray travelling from denser to rarer medium
grazes the interface, is called the critical
angle for those media. Sin C=n2/n1, where
n1 is the refractive index of denser medium
and n2 is the refractive index of rarer medium. (n1> n2).
The process of re-emission of absorbed
light in all directions with different intensities by atoms or molecules, is called scattering of light.
The arrangment of electrons in shells, subshells and orbitals in an atom is called the
electron configuration.
Anomalies in arrangment of elements
based on increasing atomic mass could be
removed when the elements were arranged
in order of increasing atomic number, a
fundamental property of the element discovered by Moseley.
The force between any two atoms or a
group of atoms that results in the formation
of stable entity is called chemical bond.
In the formation of ionic bond the atoms of
electro positive elements lose their valence
electrons to atoms of electro negative ele-
ELECTRONIC CONFIGURATION
: 1s22s22p63s1
: 1s22s22p63s23p64s1
: 1s22s22p63s23p64s2
: 1s22s22p63s23p64s23d6
: 1s22s22p63s23p64s13d5
: 1s22s22p63s23p64s13d10
: 1s22s22p63s23p3
: 1s22s22p63s23p64s23d8
: 1s22s22p63s23p4
: 1s22s22p63s23p64s23d10
Sodium (11)
Potassium (19)
Calcium (20)
Iron (26)
Chromium (24)
Copper (29)
Phosphrous (15)
Nickel (28)
Sulphur (16)
Zinc (30)
ments so that both of them can attain octet
in their valence shell.
Electric potential difference between
points in an electric circuit is the work
done to move a unit positive charge from
one point to another.
Ohm's law is valid for metal conductors at
Faraday
Maxwell
J.J. Thomson
Rutherford
Einstein
Sommerfeld
Schrodinger
Maxplank
Neils Bohr
Ulenbeck & Goudsmith
Dobereiner
Sorensen
Newlands
Sumio Lijima
: Laws of electrolysis.
: Electron magnetic theory
: Watermelon model.
: Planetory Model
: Laws of mass equivalence
: Elliptical orbit model
: Wave equation
: Quantum theory
: Principle Quantum number
: Spin Quantum number
: Triad Theory
: pH Scale
: Octave theory
: Nanotubes
PERIODIC PROPERTIES OF
ELEMENTS
Atomic Property
Atomic size
Ionization Potential
Electron affinity
Electro negativity
Electro Positivity
Oxidation
Reduction
In groups
(from top
to bottom)
Increases
Decreases
Decreases
Decreases
Increases
Decreases
Increases
In period
(from Left –
Right)
Decreases
Increases
Increases
Increases
Decreases
Increases
Decreases
PHYSICAL CONSTANTS VALUES
Specific heat of lead
Specific heat of Mercury
Latent heat of fusion
Latent heat of Vaporization
Refractive Index of Diamond
Refractive Index of Benzene
Refractive Index of Quartz
: 0.031Cal/g-Cº;130 J/Kg - k
: 0.033Cal/g-Cº; 139 J/Kg – k
: 80 Cal / gm
: 540 Cal / gm
: 2.42
: 1.50
: 1.46
USES
: Determination of specific heat of substance.
Thermometer
: Determination of Temperature
Prism
: Observation of Angle of Dispersion.
: Observation of Acid – Base Strength.
pH paper
Bleaching powder : Used as decolorizing agent, oxidant, used
in preparation of chloroform, used in
chlorination process.
Baking Soda
: Manufacture of cakes, preparation of
Antacid, preparation of Anti septic.
Washing Soda
: Used in Glass, soap, paper industry
preparation of borax, used to removal of
hardness of water.
Galvanometer
: Determination of electric current.
Electric motor
: Convert the electric energy to mechanical
energy.
Dynamo
: Convert the mechanical energy to electric
energy
Blast furnace
: used to smelting process.
Voltmeter
: Determine the potential difference.
UNITS
Specific heat
Latent heat of fusion
Power of lens
Electric current
Specific resistivity
Electric energy
Atomic Radius
Ionization potential
Calorimeter
SCIENTISTS
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Physical Science
: cal/g.cº (or) J/Kg-k.
: Cal /gm (or) J/k.g
: dioptres
: Ampere
: Ohm-mt
: KWH
: Angstrom Unit (Aº)
: Electron Volt.
constant temperature. It is not applicable
for gaseous conductors and semiconductors.
Electric power is the product of potential
difference and the current. SI unit of power
is watt (W).
Magnetic flux density (B) is defined as the
ratio of flux passing through a plance perpendicular to field and the area of the
plane.
Physical methods adopted in dressing the
ore are: hand picking, washing, froth flotation, Magnetic separation etc.
Carbon forms a large variety of compounds. its tetravalency and the property of
catenation and ability to form four single
bonds, a double bond and two single
bonds, a triple bond and a single bond or
two double bonds makes carbon versatile
and brings one special branch in chemistry
for carbon compounds.
Carbon compounds with identical molecular formula but different structures are
called structural isomers.
CHEMICAL
SUBSTANCES FORMULAS
Substance
Bauxite
: Formula
: Al2O32H2O
Epsum salt
: MgSO47H2O
Sinnabar
Magnetite
: HgS
: Fe3O4
Galena
Carnalite
: PbS
: KClMgCl26H2O
Gypsum
: CaSO4 2H2O
Pyrotusite
: MnO2
Hypo
: Na2S2O32H2O
Bleaching powder
: CaOCl2
Plaster of Paris
: CaSO4½H2O
Ethanol
: C2H5OH
Ethyl Acetate
: CH3COOC2H5
Soap
: C17H35COONa
Zincite
Lime stone
: ZnO
: CaCO3
Horn silver
Zinc Blende
Rock Salt
Hematite
: AgCl
: ZnS
: NaCl
: Fe2O3
Different Solutions
pH Values
Solution
pH value
HCl
1
NaOH
13-14
Distilled water
7
Lemonjuice
2.5
Coffee
5
Carrot Juice
4
Soda Water
6
Tomato Juice
4.1
Saliva (before meal)
7.4
Saliva (after meal)
5.8