This document provides an introduction to the B.Sc. Part I Semester II chemistry syllabus from Shri Shivaji Science College in Amravati, India. It outlines the six units that will be covered: inorganic chemistry (units I-II), organic chemistry (units III-IV), and physical chemistry (units V-VI). Each unit is briefly described, including topics like polarisation, covalent bonding, acids and bases (unit I), p-block elements, noble gases, and non-aqueous solvents (unit II). Contact information is provided for questions.

1. Shri Shivaji Science College, Amravati
Department of Chemistry
Presents
Introduction of B.Sc. Part – I
Semester - II
University Chemistry Syllabus

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4. By Dr. Pramod R. Padole
Organic
Chemistry
Inorganic
Chemistry
Physical
Chemistry
Chemistry
First Second Third

5. B.Sc. First Year
Semester – II
Chemistry Paper
Unit-VI
Unit-I
Unit-II
Unit-III
Unit-IV
Unit-V

6. B.Sc. Sem - II
(Effective from session 2016-17)
Inorganic
Chemistry
Unit-I
Organic Physical
Unit-II
Unit-III Unit-IV Unit-V Unit-VI

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Inorganic Chemistry
A) Polarisation
B) Covalent bonding
C) Acids & Bases
Unit - I

8. Unit – I
A] Polarisation:
Effect of
polarization
on nature
of bond.
Polarisation
-
Definition,
polarising
power,
polarizability
First Second Third Fourth
Its
applications
Fajan’s
rules of
polarisation

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Unit-I B) Covalent bonding:
1
Directional
nature of
covalent bond.
2
Hybridisation,
Types of
hybridisation
3
To explain
geometries
of NH4+ ion,
PCl5 ,
SF6
and IF7

10. 3. Hard and soft acids and bases
2. Lux-Flood concept of acids and bases
1. Acids and Bases-
Theory of solvent systems
4. Pearsons HSAB or SHAB principle with
important applications.
C) Acids & Bases:

11. Inorganic Chemistry
Unit - II
A) p-block elements
B) Noble gases
C) Non-aqueous solvents

12. Periodic Table

13. Unit II
Unit-II A] P-Block Elements:
(CFT):
• Comparative study of
16th and 17th group elements with
reference to electronic configuration,
ionization energy and oxidation
states.
 Oxidising properties of halogens
with reference to oxidation potential.
 Interhalogen compounds,
structure and bondings.
 Introduction to fluorocarbons.
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Unit-II B) Noble Gases:
Inertness
of noble
gases
Noble
Gases
Compounds of
noble gases
only structure
and bonding in
XeF2 , XeF4, XeF6,
XeO3 and XeO4

15. Unit-II
C) Non-aqueous Solvents:
Requirements of a good solvent.
Water as an universal solvent.
1
Physical properties of solvents namely liquid
range, dielectric constant, dipole moment,
heat of vaporisation and solubility behaviour
2
Classification of solvents:
1) Acid base, 2) Precipitation, 3) Redox,
4) Solvolysis and 5) Complexation reactions
in liquid ammonia.
3
Merits and demerits
of liquid ammonia as a solvent.
4

16. Organic Chemistry
Unit - III Unit - IV

17. Organic Chemisrtry
Unit-III
A) Alkenyl Halides:
B) Aryl Halides:
C) Alcohols:

18. III A) Alkenyl Halides:
Synthesis
of
allyl
chloride
from
propylene
Synthesis
of
vinyl
chloride
from
acetylene
1 2 3 4
Comparison
of
Reactivity
of vinyl &
allyl
chloride
Reactions
of both
with
aqueous
&
alcoholic
KOH

19. III B) Aryl Halides:
First
Synthesis Chlorobenzene
from benzene, phenol and
benzene diazonium chloride
Second
Synthesis of Benzyl chloride
from toluene and benzyl
alcohol
Third
Reactions of both with aqueous
KOH, NH3 and sodium ethoxide,
Comparison of reactivity of
chlorobenzene and benzyl chloride.
Fourth Benzyne intermediate
mechanism

20. 3. Trihydric alcohols: Glycerol:
Preparation from propylene,
Chemical Reactions with Na, HCl, PCl5 , HNO3 and KHSO4.
2. Chemical Reactions:
with Na, PCl5 , CH3COOH, ZnCl2 , conc. H2SO4 and
dehydration with heat
1. Dihydric alcohols:
Ethylene glycol- Preparation from ethylene,
ethylene chloride and ethylene oxide,
4. Pinacol- pinacolone rearrangement
(mechanism).
C) Alcohols:

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Unit-IV
B) Ethers C) Epoxides
A) Phenol

22. Unit IV- Aromatic Hydrocarbons
Phenols: Methods of formations
a) from aniline & b) from cumene.
Acidic character of Phenol,
Reaction of Phenols-
a) Carboxylation (Kolb’s reaction),
b) Fries Rearrangement, c) Claisen Rearrengement and
d) Reimer – Tiemann reaction.
A
Ethers: Diethyl ether: Preparation by Williamson’s
synthesis and continuous etherification process,
Chemical Reactions with cold and hot HI
B
Epoxides: Synthesis of ethylene oxide from ethylene
and styrene oxide from styrene.
Ring opening reactions of both catalysed by acid and alkali
C

23. Physical Chemistry
Physical
Properties
and
Molecular Structure
Unit- V Unit- VI
Chemical
Kinetics:

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Unit-V) Physical Properties and
Molecular Structure:
A)
Electrical
Properties:
Unit-V
B)
Magnetic
Properties:

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Unit – V A) Electrical Properties:
 Polar and non-polar molecules. Dipole moment.
 Induced polarization and orientation polarization.
Clausius Mossotti equation (only qualitative
treatment).
Measurement of dipole moment by temperature
and refractivity methods.
Applications of dipole moment for the
determination of molecular structure.
i.e. percentage ionic character of covalent bonding,
molecular geometry, cis-trans isomers, ortho, meta and
para isomers of a disubstituted benzene.

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Unit-V B) Magnetic Properties:
 Paramagnetic and diamagnetic substances, origin
of paramagnetism, diamagnetism, ferromagnetism
and antiferromagnetism.
 Volume, specific, mass and molar susceptibility.
Relationship between molar magnetic
susceptibility and magnetic moment.
 Relationship between magnetic moment and
number of unpaired electrons.
 Gouy’s balance method for determination of
magnetic susceptibility.
 Application of magnetic moment in the
determination of molecular structure.
 Numericals

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Physical Chemistry
A]
Gaseous
State :
Unit - VI
B]
Phase Rule:

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Physical Chemistry
Explanation of Important Terms
Derivation of Rate Equation
Determination of order of a reaction
Unit - VI

29. Explanation of Important Terms
Explanation of terms like
 Rate of reaction, order of a
reaction and molecularity.
 Definition with one example of
zero, first and second order
reaction.
 Half life period of a reaction
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Derivation of Rate Equation
 Derivation of rate equation for first and second order
reaction with equal initial concentration and different
initial concentration of a reactant.
 Characteristics of first and second order reaction.
 Examples of first and second order reaction and their
kinetics study with modified rate equation viz. the
reactions (i) decomposition of H2O2 , (ii) reaction
between K2S2O8 and KI, (iii) hydrolysis of methyl
acetate catalyzed by acid, (iv) saponification of ethyl
acetate by NaOH and (v) inversion of cane sugar.

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Determination of order of a reaction:
 Determination of order of a reaction by:
(1) Integration,
(2) Graphical,
(3) Equifractional change,
(4) vant Hoff’s differential method and
(5) Ostwald’s isolation method.
 Effect of temperature on reaction rates.
 Arrhenius equation, activation energy and
its determination using Arrhenius equation.
 Numericals

32. Dr. Pramod R. Padole
Professor
Department of Chemistry
Shri Shivaji Science College, Amravati
Mobile: 9422158188
Email: pramodpadole@gmail.com

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