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12th Chemistry – Vol.2 Study Material
8. IONIC EQUILIBRIUM
1. Define Arrhenius concept:-
The substance dissociate to give Hydrogen ion in water is called acid.
Example: 𝐻𝐶𝑙 𝐻2𝑂
⇌𝐻+(𝑎𝑞) + 𝐶𝑙−
The substance dissociate to give hydroxyl ion in water is called base.
𝑁𝑎𝑂𝐻 𝐻2𝑂
⇌𝑁𝑎+ + 𝑂𝐻−
2. Write Limitation of Arrhenius concept
* Does not explain the behavior of acid base in non aqueous solution (acetone)
* Does not explain about basicity of substance like 𝑁𝐻3 (no hydroxyl group)
3. Write about Lowry – Bronsted theory (Proton theory)
The substance has a tendency to donate the proton to another substance.
𝐻𝐶𝑙 + 𝐻2𝑂 ⇌ 𝐻3𝑂+ + 𝐶𝑙−
The substance has tendency to accept the proton to from another substance write
𝐻2𝑂 + 𝑁𝐻3 ⇌ 𝑁𝐻4+ + 𝑂𝐻−
4. Write Limitation of Lowry – Bronsted theory
𝐵𝐹3, 𝐴𝑙𝐶𝑙3 etc donot, donate the proton but they are consider as acids.
5. Write about Lewis concept.
The species – accept the electron pair – acid
The species – donate the electron pair – base
Bage : NH3 Base BF3
6. Ionisation of water.
* The pure water itself has little tendency to dissociate.
* One water molecule donates a proton to an another water molecules.
𝑂𝐻 − 𝐻 + 𝐻2𝑂 ⇌ 𝐻3𝑂+ + 𝑂𝐻
acid 1 base 2 acid 2 base 1
7. Define 𝑷𝑯 and 𝑷𝑶𝑯of a solution.
* 𝑃𝐻 of a solution is defined as the negative logarithm of base 10 of the molar concentration of
the hydronium ions present in the solution.
𝑷𝑯 = −𝑙𝑜𝑔10[𝐻3𝑂+]
* Similarly, pOH can also be defined as follows
𝑃𝑂𝐻 = −𝑙𝑜𝑔10[𝑂𝐻−]
8. Ostwald dilution law
∝=𝑁𝑢𝑚𝑏𝑒𝑟 𝑜𝑓 𝑚𝑜𝑙𝑒𝑠 𝑑𝑖𝑠𝑠𝑜𝑐𝑖𝑎𝑡𝑒𝑑
𝑇𝑜𝑡𝑎𝑙 𝑛𝑢𝑚𝑏𝑒𝑟 𝑜𝑓 𝑚𝑜𝑙𝑒𝑠
When dilution increases, the degree of dissociation of weak electrolyte increases.
9. What is common ion effect.
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The dissociation of weak acid is reduced by adding salt of weak acid is called common ion effect.
𝐶𝐻3𝐶𝑂𝑂𝐻 ⇌ 𝐻+ + 𝐶𝐻3𝐶𝑂𝑂− -NV-
𝐶𝐻3𝐶𝑂𝑂𝑁𝑎 ⟶ 𝑁𝑎+ + 𝐶𝐻3𝐶𝑂𝑂−
here the dissociation reduced by common ion 𝐶𝐻3𝐶𝑂𝑂−
10. Define Buffer Solution.
Buffer solution resists drastic changes in its PH upon addition small quantities of acids (or) bases. It is also
called buffer action.
Example: 𝐶𝐻3𝐶𝑂𝑂𝐻 and 𝐶𝐻3𝐶𝑂𝑂𝑁𝑎
What types of Buffer Solution.
Acidic Buffer : 𝐶𝐻3𝐶𝑂𝑂𝐻 and 𝐶𝐻3𝐶𝑂𝑂𝑁𝑎
Basic Buffer : 𝑁𝐻4𝑂𝐻 and 𝑁𝐻4𝐶𝑙
11. Define Buffer index and Define Buffer Capacity.
Quantitative measure of the Buffer Capacity.
It is defined as the number of gram equivalents of acid (or) base added to 1 lit of the buffer solution to change
its PH by units.
𝛽 =𝑑𝐵
𝑑(𝑃𝐻)
12. Write the Henderson – Hasselbalch equation.
* For acid buffer
𝑷𝑯 = 𝑷𝑲𝒂 − 𝒍𝒐𝒈
[𝒔𝒂𝒍𝒕]
[𝒂𝒄𝒊𝒅]
* For basic buffer
𝑷𝑶𝑯 = 𝑷𝑲𝒃 + 𝒍𝒐𝒈
[𝒔𝒂𝒍𝒕]
[𝒃𝒂𝒔𝒆]
13. Define Molar solubility.
* Solubility can be calculated from the molar solubility i.e., the maximum number of moles of
solute that can be dissolved in one litre of the solution.
14. Salt hydrolysis.
Acid + Base Salt + Water
The above reaction is called neutralization.
Salt completely dissociate in aqueous solution to give their constituent ions.
In certain cases the cation (or) both react with water and the reaction is called salt hydrolysis.
15. Define Solubility Product.
* The solubility product of a compound is defined as the product of the molar concentration of
the constituent ions, each raised to the power of its stoichiometric co – efficient in a balanced
equilibrium equation.
𝐾𝑠𝑝 = [𝑋𝑛+]𝑚[𝑌𝑚−]𝑛
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-NV-
UNIT - 9
ELECTRO CHEMISTRY
1. Define Resistivity
The resistance of an electrolyte confined between to electrodes having unit cross sectional area and
are separated by unit distance. Unit of resistivity of (Ω m)
2. Define specific conductance
The conductance of cube of an electrolytic solution of unit dimensions
SI unit Sm-1
3. Define molar conductivity
Conductivity cell in which the electrode are separated by 1m and having Vm3 of electrolyte solution
which contains 1mole of electrolyte. The conductance of such system is called the molar conductance.
⋀m = K x V
4. Define equivalent conductance (^)
The conductance of ‘V’ m3 of electrolytic solution containing one gram equivalent of electrolyte in a
conductivity cell in which the electrode are one metre apart.
5. What are factors affecting electrolytic conductance
* Interionic attraction
* Dielectric constant
* Viscosity
* Temperature
6. Define galvanic cell (Voltaic cell) and electrolytic cell
Galvanic Cell Electrolytic cell
* Spontaneous chemical reaction Non – Spontaneous chemical reaction
* Chemical energy to electrical energy Electrical energy into chemical energy
7. Faraday’s first law
The mass of the substance (m) liberated at an electrode during electrolysis is directly proportional to
θ the quantity of change θ passed through the cell
m 𝛼 Q
m = ZIt
Q = It
8. Define specific resistance
It is resistance in ohms which meter cube of material offers to passage of electricity through it unit –
ohm meter.
9. Define electrochemical equivalent
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The amount of a substance deposited (or) liberated at the electrode by charge 1 columb
-NV-
10. State Faraday’s second law
When the same quantity of electricity passes through solution of different electrolyte, the amounts of
the substances liberated at the electrode are directly proportional to their chemical equivalents
M Ni α 𝑍 Ni, m Cu α 𝑍 cu and mCo α 𝑍 co
𝑚𝑁𝑖
𝑍𝑛𝑖 =
𝑚𝐶𝑢
𝑍𝐶𝑢 =
𝑚𝐶𝑜
𝑍𝐶𝑜
11. What is intercalation?
Li+ ions move from cathode to anode where they become embedded on the porous graphite electrode
12. Fuel cell
* The galvanic cell in which energy of combustion of fuels
* Fuels is directly converted into electrical energy is called fuel cell
13. Define corrosion
* Metal is oxidized by oxygen in the presence of moisture
* This redox process which causes the deterioration of metal is called corrosion
14. What is galvanizing?
* Coating of one metal with another metal such as Zn
* Zn stronger oxidising agent than the iron
* Hence it can be more easily corroded than Iron i.e: istead of Iron Zn is oxidized.
15. What is cathodic protection?
* Unlike galvanising the entire surface of the metal to protected need not be covered with protecting
metal.
* Instead metal such as Mg (or) Zn which is corroded more easilythan iron can be used as a
sacrificial Anode
* Iron is protected, but Mg (or) Zn is corroded
16. Define passivation
* The metal is treated with strong oxidizing agent such as con HNO3
* As a result a protective oxide layer is formed on the surface of the metal
17. What is alloy formation?
The oxidizing tendency of iron can be reduced by forming its alloy with other more anodic metals
Example: Stainless steel – an alloy of Fe and Cr.
18. What is electrochemical series?
The standard aqueous electrode potential at 298K various metal – metal ion electrode are arranged in
the decreasing order of their standard reduction potential value. This series is called electrochemical series.
Higher Eo value higher e- accept tendency.
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-NV-
19. State Kohlrausch’s law
Kohlrausch’s law states that, “at infinite dilution where in the ionisation of all electrolytes is
complete, each ion migrates independently and contributes a definite value to the total equivalent
conductance of the electrolyte.
λ∞ = AlCl3 = 1/3 λ∞ Al3+ + λ∞ Cl-
20. Define – Specific and equivalent conductance. How are they related?
Specific conductance (k) is define as the conductance of one metre cube of an electrolyte solution
K = 1/R. l/a
Equivalent conductance (λc) is defined as the conductance of an electrolyte solution containing one
gram equivalent of the electrolyte.
The equivalent conductance is equal to the product of specific conductance (K) of the solution and
the volume of the solution that contains 1gm equivalent of the electrolyte.
λ𝑐 = k x V, λ𝑐 = 𝑘×10−3
𝐶
unit of λ𝑐 = mol.m2. gram equiv-1
21. Define Faraday
Faraday is defined as the quantity of electricity required to liberate one gram equivalent of a
substance and it is equal to 96,495 coulombs. It is denoted by the symbol ‘F’.
1 faraday = 96,495 coulombs = 1 mole electron
22. What are the types of changes in the cathode and anode in electrolytic and electrochemical cells?
Eletcrolytic Cell Electrochemical cell
1. At cathode, the positively
charged ions reduced.
Cathodes are positively charged electrodes and
positive ions get reduced by electrons coming from
the anode
2. At anode, the negatively charged ions
get oxidized.
Anodes are negatively charged electrodes and
oxidation take place on it. Due to chemical reaction
electrons will be released to this electrode.
23. What are the two types of cell?
(i) Electrolytic Cell: It is the cell in which electrical energy is used to bring about chemical
reaction at the electrode.
(ii) Electro chemical cell: It is the cell in which chemical energy is used to bring about electrical
energy in the form of emf.
24. What is single electrode potential?
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An electro chemical cell consists of two half cells, with an open circuit, the metal electrode in each
half cell transfers its ions into solution. Thus an individual electrode develops a potential with respect to the
solution. The potential of a single electrode in a half cell is called single electrode potential. -NV-
25. How to predict the feasibility of a cell reaction?
The feasibility of a redox reaction can be predicted with the help of the electrochemical series. The
net emf of the cell reaction Eocell can be calculated from the expression.
EoCell = Eo
Cathode - Eoanode
In general, if EoCell = +ive, the reaction is feasible
EoCell = -ive, the reaction is not feasible
26. Write the Nernst equation
E = Eo – 2.303 𝑅𝑇
𝑛𝐹 log K
Eo = Standard electrode potential. R = Gas Constant
T = Temperature in Kelvin, K = Equilibrium constant
n = No. of electrons transferred in the half cell reaction
27. What is meant by emf of the cell?
The emf of the cell is the difference in the potentials of the cathode and the anode in contact with the
suitable electrolyte at the electrode. The driving force that sends the electrons through the circuit is called
emf of the cell.
28. What is cell diagram? Give one example
A cell diagram is an abbreviated symbolic representation of an electrochemical cell. A cell consists
of two half cells. Each half cell is made of a metal electrode in contact with metal ion in solution.
Example: Zn | Zn2+ || Cu2+ | Cu
Anode half cell Cathode half cell
29. Write a note abut standard Hydrogen electrode (SHE)
1. The standard hydrogen half cell (or) standard hydrogen electrode (SHE), is selected for coupling
with the unknown half cell.
2. It consists of a platinium electrode immersed in a 1M solution of H+ ions maintained at 25oC
3. Hydrogen gas at one atmosphere enters the glass hood and bubbles over the platinum electrode.
The hydrogen gas at the platinum electrode passes into solution, forming H+ ions and electrons.
4. The emf of the SHE is zero volts, So, SHE can be used as a standard for other electrodes.
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-NV-
UNIT – 10
SURFACE CHEMISTRY
1. Write any three difference between physisorption and chemisorptions.
Chemisorption Physisorption
* It is very slow - It is instantaneous
* Occurs at fixed site active centres - Occurs at all sides
* Heat of adsorption high - Heat of adsorption low
* Moholayer former - Multilayer formed
2. What are factors affecting the adsorption
(i) Nature of adsorbent
(ii) Nature of adsorbate
(iii) Pressure
(iv) Concentration at given temperature
3. Define adsorbtion isobar
When amount of adsorbtion is plotted temperature at constant P adsorbtion isobar.
4. Freundlinch isotherm.
𝑙𝑜𝑔𝑥
𝑚= 𝑙𝑜𝑔𝑘 +
1
𝑛log 𝑝
P, k and n are constant
M – amount of adsorbent
X – amount of adsorbate
5. Limitation of freundlinch isotherm
* Purely emprical
* Valid over a limitted pressure range
* Value of constant K, n also vary with T
* No theoritical explanation given
6. Define catalyst (and) catalysis.
* A substance which alters the rate of Chemical reaction.
* Without itself undergoing chemical change
* This phenomenon is known as catalysis.
7. Define positive and negative catalysis.
* Positive catalysis: The rate of reaction increased by catalyst.
* Negative catalysis: The rate of reaction decreased by catalyst.
8. Define homogenous and heterogeneous catalyst homogeneous catalyst.
The reactant, product and catalyst are present in the same phase.
𝑆𝑂2 + 𝑂2 𝑁𝑂(𝑔) 2𝑆𝑂3(𝑔)
Heterogeneous Catalyst:- The reactant, product and catalyst are different phase.
𝑆𝑂2(𝑔)+ 02(𝑔)
𝑃𝑡(𝑠) 2𝑆𝑂3(𝑔)
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-NV-
9. Write any three characteristic of catalyst.
* Needed in very small quantity.
* Catalyst doesnot change nature of product.
* Specific in Nature.
* Doesnot initiate reaction only increase the speed of reaction.
10. Define promoters with example.
* The substance increase the activity of catalyst.
Example:- Manufacture of Ammonia Iron act as catalyst.
The molybdenum increase the activity of Iron.
11. Define catalytic poison.
* The substance decrease (or) destroy the activity of catalyst.
Example:- Manufacture of 𝑆𝑂3 pt act as catalyst.
𝐴𝑆2𝑂3 destroy the activity of pt.
12. Define auto catalyst.
* In chemical reaction one of the product act as catalyst.
𝐶𝐻3𝐶𝑂𝑂𝐶2𝐻5 + 𝐻2𝑂 → 𝐶𝐻3𝐶𝑂𝑂𝐻 + 𝐶2𝐻5𝑂𝐻
Ester + 𝐻2𝑂 → acetic acid + Ethyl alcohol
* Acetic acid act as a catalyst.
13. Define Enzyme Catalysis.
* Enzyme are protein molecule
* Enzyme increase speed of Biochemical reaction
Example:- Urea urease Ammonia + Carbon dioxide
𝐻2𝑁 − 𝐶𝑜 − 𝑁𝐻2 + 𝐻2𝑂 → 2𝑁𝐻3 + 𝐶𝑂2
14. Special characteristics Enzyme catalyfied reaction.
* Effective and efficient conversion
* Highly specific in nature.
* Rate of reaction maximum at optimum temperature.
15. Define hydrosols (or) aquasols and alcosol, Benzosol.
* If the dispersion medium is water the colloids are referred as hydrosols (or) aquasols.
* If the dispersion medium is alcohol the colloids are referred as alcosol.
* If the dispersion medium is Benzene the colloids referred as Benzosol.
16. Difference between reversible and irreversible sol.
Reversible Sol Irreversible Sol
* Lyophillic colloids (or) Sol - Lyophobic colloids (or) Sol
* They have definite attractive force - No attractive force
* More stable - Less stable
* Not easily precipitate - Easily precipitated
17. Define peptisation and peptising (or) dispersing agent.
* By addition of suitable electrolyte the precipitated particles can be brought into colloidal state.
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* The process is called peptisation. -NV-
* The added electrolyte is called peptising (or) dispersing agent.
AgCl HCl – electrolyte
Precipitate Colloid
18. Define coagulation.
* The colloidal solution due to their different methods of preparation may contain impurities
* If they are not removed, they may destablise and precipitate the colloidal solution.
19. Write about dialysis.
* Seperation of electrolyte from colloids by using semipermeable membrane.
* Colloidal solution is taken in a bad madeup of semipermeable membrane.
* It is suspended in a trough of flowing water.
* Electrolytes diffuse out of the membrane and they are carried away by water
20. Write about electro dialysis.
* The presence of electric field increases the speed of removal of electrolyte from colloidal solution.
* The colloidal solution containing an electrolyte as impurity.
* The colloidal placed between two dialysing membranes enclosed into two compartments filled with water.
* When current is passed, the impurities with pass into water compartment and get removed periodically.
Advantage: * This process is faster than dialysis.
* The rate of diffusion of electrolyte is increased by application of electricity.
21. Ultra filteration:-
* The pores of ordinary filter papers permit the passage of colloidal solutions.
* In ultrafiltrations, the membranes are madeby using collodion, cellophane (or) visiking.
* When a colloidal solution is filtered using such a filter, colloidal particles are seperated on the filter the
impurities are removed as washing.
* The separation of sol particles from electrolyte by filteration through an ultrafilter is called ultrafiltration.
* Collodion is 4% solution of nitro cellulose in mixture of alcohol and water.
22. Define Tyndall effect (Optical property).
* When the light passes through colloidal solution it scattered in all direction.
* The scattering of light by colloidal particles are called Tyndall effect.
23. Brownian movement (Kinetic Property)
* The pollen grains suspended in water it is viewed by ultra microscope.
* Showed random, zigzag ceaseless motion.
* The colloidal sol particles are continuously bombard with the molecules of the dispersion medium.
* Hence they follow zigzag, random, movement.
24. Uses of Brownian movement.
* Used to calculate the Avogadro number.
* Understand the stability of colloids.
* To confim the kinetic theory.
* The T increase the movement molecules are increases.
25. Write about Electrical property. (Helmholtz double layer)
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* The surface of colloidal particle adsorbs one type of ion due to preferential adsorption. -NV-
* This layer attracts the oppositely charged ions in the medium hence at the boundary separating the two
electrical double layers are setup.
* This is called Helmholtz electrical double layer.
26. Define Electrophoresis (or) Cataphoresis.
* The migration of sol particles under the influence of electric field is called electrophoresis.
* When the electric potential is applied across two platinum electrode dipped in the hydrophillic sol.
* The dispersed particles move toward one (or) other electrode.
* If the sol particles migrate to the cathode then they posses positive (+) charges.
* If the sol particles migrate to the anode then they have negative (-) charges.
* We can find out charge of sol particles by direction of migration of sol particle.
Use:- Detect the charge of sol particles.
27. Electro Osmosis:-
* A sol is electrically neutral.
* Hence the medium carries an equal but opposite charge to that of dispersed particle.
* When sol particles are prevented from moving, under the influence of electric field.
* The medium moves in a direction opposite to that of sol particles.
* The movement of dispension medium under the influence of electric potential is called electro osmosis.
28. Define flocculation value:
* Used to determine precipitation power of electrolyte is the minimum concentration (millimoles / lit) required
to cause precipitation of a sol in 2 hours.
* This value is called flocculation value.
* The smaller flocculation value greater will be precipitation.
29. Define gold number.
* The number of milligrams of hydrophilic colloid that will just prevent the precipitation of 10ml gold sol on
the addition of 1 ml of 10% Nacl solution.
* Smaller the gold value greater protective power.
30. Define Emulsion and types of emulsion.
* It is colloidal solution.
* In which a liquid is dispersed in an another liquid.
Types o/w and w/o
31. Define emulsification and Deemulsification.
* The process of preparation of emulsion by dispersal of one liquid in another liquid is called Emulsification.
* Emulsion can be separated into two separated into two separate layers.
* This process is called deemulsification.
32. Write about mechanical dispersion
* Using colloid mill, solid is ground to colloidal dimension.
* The colloid mill consist of two metal plates rotating in opposite direction at very high speed.
* Nearly 7000 revolution / minutes.
* Required size of colloidal particles are prepared by adjusting the distance between two plates.
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* By this method ink, graphites are prepared. -NV-
UNIT – 14
BIO - MOLECULES 1. Why the carbohydrate is optically active
* The carbohydrate have one (or) move chiral carbon atom.
2. Give the preparation of glucose.
𝐶12𝐻12𝑂11 + 𝐻2𝑂 → 𝐶6𝐻12𝑂6 + 𝐶6𝐻12𝑂6
3. What is anomer?
* The conversion of achiral addehyde into chiral.
* It will make two possibility of two isomers.
* These two isomers differ only in the configuration of 𝐶1 carbon.
4. What is mutarotaion.
* When pure for of any one sugars is dissolved in water.
* Slow inter conversion of ∝ −𝐷 glucose and 𝛽 − 𝐷 glucose via open chain form occurs until the
equilibrium is established give the specific rotation + 53°.
* This phenomenone is called mutarotaion.
5. Epimers and Epimerisation.
* Sugar differing in configuration at an asymmetric centre is know as epimers.
* The conversion of one epimer to another epimer by enzyme (epimerase)
it is called Epimerisation.
6. What is meant glycosidic linkage.
In disaccharides two munosaccharide’s are linked by oxide linkage called glycosidic linkage.
7. Why the lactose is reducing sugar.
In the lactose the aldehyde carbon is not involved in the glycosidic bond hence it retains its reducing
property and is called reducing sugar.
8. Why Human cannot use the cellulose as food?
Because of our digestive system donot contain the necessary enzymes (glycosidases (or) cellulases)
that can hydrolyse the cellulose.
9. What is Isoelectric point.
* At a specific PH the net charge of amino acid is neutral.
* This PH is called isoelectric point.
* Above the isoelectric point aminoacid negatively charged
* Below the isoelectric point aminoacid positively charge
10. What is zwitter ion.
In aqueous solution the proton transfer from carboxyl group to the amino group of aminoacid.
* Amino group and carboxyl group has opposite charges.
* So this molecule is neutral.
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* This amphoteric behavior called Zwitter ion. -NV-
11. What is difference between 𝟏° and 𝟐° structure protein.
Primary Structure Secondary Structure
Amino acids are linked by pepdide chain In pepdide chain are linked by C = O and NH group
Small changes alter the over all structure
and function of protein
Pepdide high regular shapes (substructure)
12. What is Denaturation.
* The process of losing its higher order structure without losing primary structure.
13. Define enzyme.
* All the Biological reaction catalysed by special proteins called enzyme
* The rate of reaction order 105.
14. Write any 3 Biological importance of glucose
* Protective coating for aquatic organism
* Act as emulsifier
* Energy reserves
15. What is vitamins
* Small organic compounds
* Cannot be synthesized our body
* Esential for certain function
* It must be obtained through diet
16. Give the classification of vitamins.
Classified based on the solubility
17. Define chromosome and Nucleic acid.
* The inherent character of each and every species is transferred from one generation to next
generation.
* These transformation done by some particles present in nucleous of the cell. These are called
chromosomes.
* These are made up of protein is called Nucleic acid.
18. What are Basic structural components of nucleic acid
* Polynucleotide
1) Nitrogeneous base
2) Pentose sugar
Fat Soluble Vitamins Water Soluble Vitamins
Do not dissolved in water Readily soluble in water
It can be stored in fatty tissues and liver It can’t be stored
Example : A, D, E, K etc Example : Vitamin B (B1, B2, B3 etc)
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3) Phosphate group -NV-
19. Define Nucleoside and Nucleotide
* The molecule without phosphate group is called nucleoside.
* The addition of phosphoric acid molecules to nucleoside is called nucleotide
Sugar + base Nucleoside
Nucleoside + Phosphate Nucleotide
nNucleotide Polynucleotide (nucleic acid)
20. What are linkage found in DNA helix
a) Hydrogen bonding between complementary base pairs
b) Base – stacking interactions
21. What are the types of RNA
(i) r RNA (ii) m RNA (iii) t RNA
22. What are difference between DNA and RNA.
23. What is electrophoresis.
* The extracted DNA is cut at specific points along the stand with restriction of enzymes
* It gives DNA fragments varying length
* Separate the fragment based on their size
24. Define blotting
* The gel containing the DNA fragment is then transferred to nylon sheet is called blotting
25. What are biological function of nucleic acid
(i) Energy carriers
(ii) Components of Co-enzyme
(iii) Chemical messanger
26. Define the hormones type.
* It is organic substance
* Secretted by tissue
* It limits the blood stream and induces physiological response in other tissues
27. What are types of Hormones with examples
a) Endocrine hormones (insulin)
b) Para crine hormones (interleukin 1)
c) Auto crine hormones (interleukin-2)
DNA RNA
* Deoxyribose sugar Ribose sugar
* Double standard molecule Single standard molecule
* Life time high Life time low
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-NV-
UNIT - 15
CHEMISTRY IN EVERYDAY LIFE
1. Define drug:-
* A drug is a substance that is used to modify or explore physiological systems or pathological states
for the benefit of the recipient.
* It is used for the purpose of diagnosis, prevention, cure/relief of a disease.
2. Define Medicine & Chemotherapy:-
* The drug which interacts with macromolecular targets such as proteins to produce a therapeutic
and useful biological response is called medicine.
* The specific treatment of a disease using medicine is known as chemotherapy.
3. Define Antibiotics with examples:-
* The medicines that have the ability to kill the pathogenic bacteria are grouped as antibiotics.
* Example : Amoxicillin
4. What is Competitive Inhibitors :-
* When a drug molecule and substrate has a similar geometry (shape).
* It can also bind to the enzyme and inhibit its activity.
* In other words, the drug acts as an inhibitor to the enzyme catalyst.
* These type of inhibitors are often called competitive inhibitors.
5. What allosteric inhibitors:-
* In certain enzymes, the inhibitor molecule binds to a different binding site, which is
commonly referred to as allosteric site
* It causes a change in its active site geometry (shape).
* As a result, the substrate cannot bind to the enzyme.
* This type of inhibitors are called allosteric inhibitors.
6. Define antagonists:-
* If we want to block a message, a drug that binds to the receptor site.
* Inhibit its natural function. Such drugs are called antagonists.
7. Define agonists:-
* There are drugs which mimic the natural messenger by switching on the receptor.
* These type of drugs are called agonists and are used when there is lack of chemical messenger.
8. How will you avoid sleep:-
* When adenosine binds to the adenosine receptors, it induces sleepiness.
* On the other hand, the antagonist drug caffeine binds to the adenosine receptor and makes it
inactive.
* This results in the reduced sleepiness (wakefulness).
-NV-
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9. Define Tranquilizers & Mode of actions and its uses:-
* They are neurologically active drugs.
* Acts on the central nervous system by blocking the neurotransmitter dopamine in the brain
Uses :- Treatment of stress, depression, sleep disorders.
10. Define Analgesics with examples . (Non – narcotic)
* Analgesics reduce the pain without causing impairment of consciousness.
* They alleviate pain by reducing local inflammatory responses
Uses :- Used for short-term pain relief headache, muscle strain.
11. Define Antipyretics with examples :-
* These drugs have used to reducing body temperature.
* Preventing platelet coagulation. Due to this property, aspirin used to prevention of heart attacks.
Example : aspirin.
12. Define Anaesthetics with example:-
* It causes loss of sensation, without losing consciousness.
Uses :- They are often used during minor surgical procedures.
13. What is General anaesthetics
* The substance used for reversible loss of consciousness by affecting central nervous system
Uses :- Major surgical procedures.
14. Define Antacids and mode of action and it uses:-
* Neutralize the acid in the stomach that causes acidity.
Examples : Sodium bicarbonate, calcium bicarbonate,
Uses :- To relieve symptoms such as burning sensation.
15. Define Antiseptics with example:-
* Stop or slow down the growth of microorganisms – Applied to living tissue
Example : Hydrogen peroxide
16. Define Disinfectants with example :-
Stop or slow down the growth of microorganisms – Generally used on inanimate objects
Examples : - Hydrogen peroxide.
17. Define Antifertility drugs with example:-
* These synthetic hormones that suppresses ovulation/ fertilisation.
Example :-
Synthetic oestrogen - Menstranol
Synthetic Progesterone – Norethindrone
Uses :- Used in birth control pills.
18. What is food additive with example:
* The substances added to improve the quality of food are called food additives.
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* It enhance the nutritive, sensory and practical value of the food. -NV-
* They also increase the shelf life of food.
19. What are the Advantages of food additives:
* Uses of preservatives reduce the product spoilage and increase the shelf-life of food
* Addition of vitamins and minerals reduces the mall nutrient
* Flavouring agents enhance the aroma of the food
* Antioxidants prevent the formation of potentially toxic oxidation products of lipids.
20. What is Preservatives:
* Preservatives are capable of inhibiting, retarding or arresting the process of fermentation,
acidification or other decomposition of food by growth of microorganisms.
Example:- Organic acids such as benzoic acid.
21. Define Antioxidants with example :
* Antioxidants are substances which retard the oxidative deteriorations of food.
* Food containing fats and oils is easily oxidised and turn rancid.
* It prevent by chemical BHT, BHA are added as food additives.
22. What is Sugar Substituents with example:-
* Compounds are used like sugars (glucose, sucrose) for sweetening, they are metabolised without
the influence of insulin are called sugar substituents. Eg. Sorbitol, Mannitol.
23. What is Artificial sweetening agents with example:-
* Synthetic compounds which imprint a sweet sensation.
* Possess no or negligible nutritional value are called artificial sweeteners.
Example : - Saccharin.
24. Define Soaps:
* Soaps are made from animal fats or vegetable oils.
* They contain glyceryl esters of long chain fatty acids.
* When the glycerides are heated with a solution of sodium hydroxide they become soap and
glycerol.
25. What is Total fatty matter:
* The quality of a soap is described in terms of TFM value.
* It is defined as the total amount of fatty matter that can be separated from a sample after splitting
with mineral acids.,
* Higher the TFM quantity in the soap better is its quality.
* As per BIS standards, Grade-1 soaps should have 76% minimum TFM, while Grade-2 and 3 must
have 70 and 60% , minimum respectively.
26. Define Micelles:-
* When the soap is added to an oily or greasy part of the cloth, the hydrocarbon part of the soap
dissolve in the grease, leaving the negatively charged carboxylate end exposed on the grease surface.
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* At the same time the negatively charged carboxylate groups are strongly attracted by water, thus
leading to the formation of small droplets called micelles
27. Define Addition polymers:-
* Formed by polymerization of monomers without the elimination of byproduct.
Example :- polyethylene, PVC, teflon.
28. Define Condensation Polymer :-
* It formed by the condensation of two or more monomers with the elimination of simple molecules
like H2O, NH3, etc.,
Example :- Nylon-66, polyester
29. Define Co-polymers and example :-
* A polymer containing two or more different kinds of monomer units is called a copolymer.
* For example, styrene + butadiene SBR rubber(Buna-S)
30. What is vulcanization :-
* The physical properties of rubber can be altered by controlling the amount of sulphur is called
vulcanization.
* In sulphur rubber, 1 to 3% sulphur is soft and stretchy.
* In sulphur 3 to 10% sulphur harder and flexible.
(If you find any correction consult your Chemistry Staff)
N. VELLAICHAMY M.Sc., B.Ed., P.G. Asst. in Chemistry,
Sri Venkateshwara Vidhyalayaa Higher
Secondary School,
Sri Vaishnavi Devi Nagar,
Thasampalayam – 638 476,
Gobi (Tk), Erode (Dt).
Mobil No. 96292 66853 (WhatsApp)
70104 31615
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Thasampalayam, Polavakkalipalayam (Po), Gobi – 638 476.
=====================================================================================
HIGHER SECONDAY SECOND YEAR
VOLUME – II
UNIT 8 - IONIC EQUILIBRIUM
UNIT 9 - ELECTRO CHEMISTRY
UNIT 10 - SURFACE CHEMISTRY
UNIT 14 - BIOMOLECULES
UNIT 15 - CHEMISTRY IN EVERYDAY LIFE
N. VELLAICHAMY M.Sc., B.Ed., P.G. Asst. in Chemistry,
Sri Venkateshwara Vidhyalayaa Higher
Secondary School,
Sri Vaishnavi Devi Nagar,
Thasampalayam – 638 476,
Gobi (Tk), Erode (Dt).
Mobil No. 96292 66853 (WhatsApp)
70104 31615
Chemistry states the more energy you put into a bond the harder it is to break.
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