Sample NEET Chemistry Vol 2 Study Materials from SURA'S Main Books 2018 Click Here : SURA'S NEET Books 2018 Target NEET Chemistry Volume-II Detailed Theory and Exhaustive MCQAs Venkatesan EDITION 2018 SURA COLLEGE OF COMPETITION Chennai Tirunelveli Ernakulam E 117 Vol II Thiruvananthapuram Bengalooru SURA'S Complete NEET Chemistry Vol - 2 Study Materials 2018 Click Here - http://bit.ly/2hl8PXI www.surabooks.com www.Padasalai.Net www.TrbTnpsc.com http://www.trbtnpsc.com/2017/09/neet-exam-study-materials-download-tamil-english-medium.html www.Padasalai.Net
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Sample NEET Chemistry Vol 2 Study Materials from SURA'S Main Books 2018Click Here : SURA'S NEET Books 2018
TargetNEET
ChemistryVolume-II
Detailed Theory andExhaustive
MCQAs
Venkatesan
EDITION2018
SURA COLLEGE OF COMPETITIONChennai Tirunelveli Ernakulam
E 117 Vol II Thiruvananthapuram Bengalooru
SURA'S Complete NEET Chemistry Vol - 2 Study Materials 2018
Sample NEET Chemistry Vol 2 Study Materials from SURA'S Main Books 2018Click Here : SURA'S NEET Books 2018
NEET – National Eligibility cum Entrance Test
INTRODUCTIONThe Medical Council of India (MCI) has restored the National Eligibility cum
Entrance Test (NEET) to select the aspiring candidates, who are seeking higher
education opportunities in Medical(MBBS) and Dental(BDS) Colleges/Universities across
the country. This book with its extensive and accurate question bank and answers will
enable students to understand the concept followed in the test thoroughly and enhance
their scores.
TEST PATTERN
1. Number of Questions/ Subjects : The question paper will consistof a total of 180 Multiple choicequestions with 45 questions fromPhysics and Chemistry each and90 questions from Biology.
2. Scoring Pattern : 4 marks will be awarded for eachcorrect answer And 1 mark willbe deducted for each incorrectAnswer. A maximum of 720 markshas been set as the upper limit.
3. Duration and Mode : The test duration will be 3 hoursin Pen & Paper Mode.
4. Languages : The test will be conducted in10 (TEN) languages.
5. Core Syllabus : The Medical Council of India(MCI) Recommends the followingsyllabus for NEET for Admissionto MBBS/BDS courses afterreviewing Various State BoardSyllabi and those of CBSE & NCERT.
SURA'S Complete NEET Chemistry Vol - 2 Study Materials 2018
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2. LIQUID SOLUTIONIntroductionSolutions are homogenous mixtures of two or more substances in a single phase. Most of solutions can beconsidered as having a majority ingredient called a solvent and one more minority ingredients called solutes. Forthe sake of simplicity in this unit, we shall consider only binary solutions. Here each component may be in solid,liquid or in gaseous state and, therefore, several types of possible solutions are summarized in the following table:
Different Types of Solutions
Types of Solutions Common Example
Gaseous Solutions
Gas in gas a mixture of oxygen and nitrogen gases.
Liquid in gas chloroform vapours mixed with nitrogen gas.
Solid in gas camphor
Liquid Solutions
Gas in liquid oxygen dissolved in water
Liquid in liquid ethanol dissolved in water
Solid in liquid sucrose dissolved in water
Solid Solutions
Gas in solid solutions of hydrogen in palladium
Liquid in solid Amalgam of mercury with sodium
Solid in solid copper dissolved in gold
Concentration Units
The concentration of a solute is the amount of solute dissolved in a given quantity of solvent or solution. The
quantity of solvent or solution can be expressed in terms of volume or in terms of mass or molar mass. Thus there
are several ways of expressing the concentration of a solution.
(a) Molarity (M): Moles of solute present in one litre solution.
M no. of moles of solute volume of solution in litre
(b) Molality (m): Moles of solute present in one kilogram of solvent.
M no. of moles of solute mass of solvent in kg
(c) Normality (N): No. of equivalents present in one litre solution.
N no. of equvalents of solute volume of solution in litre
(d) Mole fraction: The mole fraction of a component substance A(XA) in a solution is defined as the moles of component substance divided by the total moles of solution.X
A moles of substance A
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5. SURFACE CHEMISTRYINTRODUCTION
Surface chemistry is the branch of chemistry, which deals with the study of phenomenon occurring at the surface
separating the two bulk phases. These two bulk phases can be pure compounds or solutions.
ADSORPTION
The phenomenon of attracting and retaining the molecules of the substance on the surface of a liquid or a solid
resulting into a higher concentration of molecules on the surface is called adsorption. The substance thus adsorbed
on the surface is called the adsorbate and the substance on which it is adsorbed is called adsorbent. The reverse
process, i.e. removal of the adsorbed substance from the surface is called desorption (which can be brought about
by heating or reducing the pressure). The adsorption of gases on the surface of metals is called occlusion.
Difference between adsorption and absorption:
Adsorption AbsorptionIt is a surface phenomenon, i.e. it occurs only at It is a bulk phenomenon, i.e. occurs throughoutthe surface of the adsorbent. the body of the material.
In this phenomenon the concentration on the In this phenomenon, the concentration is samesurface of adsorbent is different from that in the throughout the material.bulk.
Positive and negative adsorption
When the concentration of the adsorbate is more on the surface of the adsorbent than in the bulk, it is called
positive adsorption. If the concentration of the adsorbate is less, relative to its concentration in the bulk, it is called
negative adsorption.
TYPES OF ADSORPTION
An experimental study of the adsorption of various types on solids shows that there are two main types of ad-sorption. Physical adsorption & chemical adsorption.PHYSICAL ADSORPTION & CHEMICAL ADSORPTION
Difference between physical adsorption and chemisorption
Physical Adsorption Chemisorption1. The forces operating in these cases are 1. The forces operating in these cases are
weak van der Waal’s forces. similar to those of a chemical bond.
2. The heats of adsorption are low, i.e. about 2. The heats of adsorption are high, i.e.20−40 kJmol−1. about 40 – 400 kJmol−1
3. The process is reversible, i.e. desorption 3. The process is irreversible.
of the gas occurs by increasing the tem-
perature or decreasing the pressure.
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8. d- AND f- BLOCK ELEMENTS
INTRODUCTION
Definition and Electronic Configuration of Atoms
The elements lying between s and p-block elements of the periodic table are collectively known as transitional
elements (T.E.’s): These elements either in their atomic state or in any of their common oxidation state have partly
filled (n–1)d orbitals of (n–1)th main shell and as such these are called d-block elements.
The valence shell configurations of these elements can be represented by (n–1)d1−10 .ns 0, 1, 2 . The configurationsclearly show that strictly, according to the definition of d-block elements, Cu, Ag and Au should be excluded from
d-block elements, since these elements, both in their atomic state [with configuration (n–1)d10 ns1 ] and in their +1
oxidation state [with configuration (n–1)d10 ns2− ] do not have partly filled (n–1) d-orbitals. Similiarly Zn, Cd and
Hg which, both in their atomic state (n −1)d10 ns2 and in +2 oxidation [(n–1)d10] do not contain partly filled (n–1)
d orbitals, should also be excluded from d–block elements. Similar is the case with Pd atom with configuration
4d105s0. Yet, in order to maintain a rational classification of elements, these elements (viz Cu, Ag, Au, Zn, Cd, Hg
and Pd) are also generally studied with d-block elements.
Studied with d-block elements are classified into four series viz 3d, 4d, 5d and 6d series corresponding to the filling
of 3d, 4d, 5d and 6d orbitals of (n–1)th main shell. Each of 3d, 4d and 5d series has ten elements while 6d series
has at present only one element viz Ac89 whose valence shell configuration is 6d1 7s2.
Irregularities in Configurations
The irregularities in the observed configurations of Cr (3d5 4s1), Cu (3d10 4s1), Pd (4d105s0), Ag (4d10 5s1) and Au
(5d106s1) are explained on the basis of the concept that half-filled and completely filled d-orbitals are relatively morestable than other d-orbitals.
On the basis of the above concept it is, however, not easy to explain the irregularities found in the observed
electronic configurations of the atoms of other elements, since one has to consider the net effect of so many other
factors such as (i) nuclear attraction (ii) shielding of one electron by several other electrons (iii) inter – electronic
repulsion (iv) the exchange-energy forces etc. All these factors play on important part together in determining the
final stability of an electronic configuration of an atom.
The properties of transition elements of any given period are not so much different from one another as those ofthe same period of non-transition elements. The reason of this fact lies in the electronic configuration of transition
elements. We know that electronic configurations of transition elements is invariably (n–1)d1–10 ns1 or 2 which
indicates that (i) the electronic configurations of transition elements differ from one another only in the number ofelectrons in d orbitals in the (n–1)th shell and (ii) the number of electrons in the outermost shell, ns, is invariably 1
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12. ALDEHYDES AND KETONES
INTRODUCTION
Both aldehydes & ketones contain carbonyl group as their functional group.
Structure of carbonyl group
Both aldehydes & ketones have carbonyl group as the functional group. The carbonyl carbon is sp2 hybridised & it uses sp2 hybrid orbitals to form 3σ bonds, one with oxygen atom & remaining 2 with two other atoms or groups (R or H). All these 3σ bonds lie in same plane at the angle of 120.
σ −bondC O
The unhybridized p – orbital of carbonyl carbon form π - bond with oxygen atom
by sidewise overlapping with half filled p – orbital of oxygen atom.
Since carbon & oxygen have different values of electronegativity, the bond be- π −bond
tween carbon & oxygen is polar. Infact electron density around the oxygen atom Orbital picture of carbonyl groupis increased which causes the development of partial positive charge (δ+) on
carbon & δ− on oxygen.Thus the carbonyl carbon is an electrophilic & carbonyl oxygen is nucleophilic centre.
Illustration 1:
Give the IUPAC name for
(i) CH3CHO
(ii)
CH CHO
Solution: (i) Ethanal
(ii) 2, 2 – diphenyl ethanal
Illustration 2:
Write structure of the following compounds:
(i) 3-phenyl propenal
(ii) 1, 5 – pentanedial
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Sol. (i) Out of all these compounds methyl formate does not undergo H-bonding therefore, its boiling pointis the lowest.
(ii) Amongst the remaining three compounds intramolecular H-bonding is most extensive in acetamide,followed by acetic acid and least in propan-1-ol. Therefore, their boiling points decrease in the sameorder i.e. acetamide > acetic acid > propan-1-ol. Thus, the overall increasing order of their boilingpoints is methyl formate < propan-1-ol < acetic acid < acetamide.
Prob 4. O
SOCl2 H2/Pd HCN H3OH3C C OH A
BaSO4B C D E
Sol. O O OH
A = H3C B = H3CC Cl C H O C = H3CC CN
H
OHH3C CH
C
O
D = H3CE =
C COOHO
CCH CH3
H
O
Prob 5. A dicarboxylic acid (A), C4H6O4, gave a compound (B), C6H10O4 upon treatment with excess of metha-nol
and a trace of H2SO4. Subsequent treatment of (B) with LiAlH4 followed by usual work up gave C, C4H10O2.
Heating of A yielded D, C4H4O3. Assign structures to A, B, C and D.
Sol. O
H2C COOH H2C OCH3 CH2CH2OHA =
C
C =B =
H2C COOH H2CC
OCH3 CH2CH2OH
OO
D = H2C CO
H2C C
O
SURA'S Complete NEET Chemistry Vol - 2 Study Materials 2018
(ii) Benzoic acid, 4-nitrobenzoic acid, 3, 4-dinitrobenzoic acid, 4-methoxybenzoic acid.
Sol: (i) We know that +I, effect decreases while I effect increases the acid strength of carboxylic acids. Since +I
effect of isopropyl group is more that that of propyl group, therefore, (CH3)2CHCOOH is a weaker
acid than CH3CH2CH2COOH.
Further since I effect decreases with distance, therefore, CH3CH2CH(Br)COOH is a stronger
acid than CH3CH(Br)CH2COOH. Thus, the overall acid strength increases in the order:
CH3
H3C CH COOH< CH3 H2C CH2 COOH
< H3C CH CH2 COOH< H3C CH2 CH COOH
Br Br
(ii) Since electron donating groups decrease the acid strength, therefore, 4 – methoxybenzoic acid
is a weaker acid than benzoic acid.
Further since electron – withdrawing groups increase the acid strength, therefore, both 4 –nitrobenzoic acid and 3, 4 – dinitrobenzoic acids are stronger acids than benzoic acid. Further
due to presence of an addition NO2 at m – position w.r.t COOH group, 3, 4 – dinitrobenzoic
acid is a little stronger acid than 4 – nitrobenzoic acid. Thus the overall acid strength increasesin the order:
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4. Which of the following compounds are aromatic?
(A) Pyridine (B) Pyridiazine
(C) Thiophene (D) Pyrrole
Ans. A,B,C
5. On treatment with a clear solution of CrO3 in dilute H2SO4, an aliphatic alcohol gives a greenish opaquesolution within 2-3 seconds. The alcohol can be
(A) CH3CH2OH (B) CH3
H3C CH CH3CH
OH
åå 781 åå
SURA'S Complete NEET Chemistry Vol - 2 Study Materials 2018