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TargetNEET
ChemistryVolume-II
Detailed Theory andExhaustive
MCQAs
Venkatesan
EDITION2018
SURA COLLEGE OF COMPETITIONChennai Tirunelveli Ernakulam
E 117 Vol II Thiruvananthapuram Bengalooru
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© PUBLISHERS
Target NEET - CHEMISTRY Vol-II
ISBN : 978-93-86485-44-1Code : E 117
[NO ONE IS PERMITTED TO COPY OR TRANSLATE IN ANY OTHER LANGUAGETHE CONTENTS OF THIS BOOK OR PART THEREOF IN ANY FORM WITHOUT THE WRITTEN PERMISSION
OF THE PUBLISHERS]
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E 117 Vol II
09 1
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CONTENTS
VOLUME - II
CHAPTER 1 : SOLID STATE................................................... 2 - 73
CHAPTER 2 : LIQUID SOLUTION............................................. 74 - 148
CHAPTER 3 : ELECTROCHEMISTRY.......................................... 149 - 233
CHAPTER 4 : CHEMICAL KINETICS AND NUCLEAR CHEMISTRY....... 234 - 329
CHAPTER 5 : SURFACE CHEMISTRY ....................................... 330 - 351
CHAPTER 6 : GENERAL PRINCIPLES AND PROCESSES OF ............. 352 - 364ISOLATION OF ELEMENTS
CHAPTER 7 : P - BLOCK ELEMENTS........................................ 365 - 414
CHAPTER 8 : D- AND F- BLOCK ELEMENTS.............................. 415 - 431
CHAPTER 9 : TRANSITION ELEMENTS & ................................. 432 - 515CO-ORDINATION COMPOUNDS
CHAPTER 10 : HALOALKANES AND HALOARENES......................... 516 - 577
CHAPTER 11 : ALCOHOL, ETHER & PHENOL.............................. 578- 681
CHAPTER 12 : ALDEHYDES AND KETONES................................. 682 - 796
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E 117 Vol II (iii)
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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.
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E117 Vol-II (iv)
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Sura’s NEET CHEMISTRY
1. SOLID STATEIntroductionA solid is defined as that form of matter which possesses rigidity and hence possesses a definite shape and a
definite volume. Unlike gases and liquids in which the molecules are free to move about and hence constitute fluid
state, in a solids the constituent particles are not free to move but oscillate about their fixed positions.
Classification of Solids
Solids are broadly classified into two types. Crystalline solids and amorphous solids.
A crystalline solid is a substance whose constituent particles possess regular orderly arrangement e.g. Sodium
chloride, sucrose, diamond etc. In other words a solid is said to be crystalline if its various constituent particulars
are arranged in a definite geometric pattern in three dimensional space so that there is short range as well as long
range order of constituent particles. However an amorphous solid is a substance whose constituent particles do not
possess a regular orderly arrangement e.g. glass, plastics, rubber, starch, and proteins. Though amorphous solids
do not possess long range regularity, in some cases they may possess small regions of orderly arrangement.
These crystalline parts of an otherwise amorphous solid are known as crystallites.
An amorphous solid does not posses a sharp melting point. It undergoes liquefication over a broad range of
temperature. The amorphous solid do not posses any characteristic heat of fusion. When an amorphous solid is cut
with the help of sharp edged knife it results in an irregular cut.
Amorphous substances are also, sometimes, referred to as super cooled liquids because they posses disorderly
arrangement like liquids. In fact many amorphous solids such as glass are capable flowing. Careful examination of
the window panes of very old houses reveals that the panes are thicker at the bottom than at the top because the
glass has flown under constant influence of gravity.
Distinction Between Crystalline and Amorphous Solids
Crystalline solids Amorphous solids
1. The internal arrangement of particles 1. The internal arrangement of particles
is regular so they possess definite and is irregular. Thus they do not have any
regular geometry. definite geometry.
2. They have sharp melting points. 2. They do not have sharp melting points.
3. There is regularity in the external form 3. There is no regularity in the external form
when crystals are formed. when amorphous solids are formed.
4. Crystalline solids give a regular cut when 4. Amorphous solids give irregular cut.
cut with a sharp – edged knife.
5. They have characteristic heat of fusion. 5. They do not have characteristic heat of
fusion.
6. Crystalline solids are rigid and their 6. Amorphous solid are not very rigid.
shape is not distorted by mild distorting These can be distorted by bending or
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forces. compressing forces.
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Sura’s NEET CHEMISTRY
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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total moles of solution
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Sura’s NEET CHEMISTRY
3. ELECTROCHEMISTRY – 1
INTRODUCTIONMost of the chemical reactions occurs in solutions. When a given substance is dissolved in the solvents like water.
In an ionic solutions the substance splits up into ions where as in molecular solution, the substance remains as
such. Both the solutions can be represented as
XY(s) aq XY(aq) X (aq) Y− (aq) (for ionic solution)
XY(s) aq XY(aq) (for molecular solution)
The substances are classified regarding this concept is;
1. Electrolytes and
2. Non-electrolytes
1. Electrolyte (conducting)
Those substance whose aqueous solution or molten form can conduct electricity.
They are further classified into
(A) Strong electrolyte: Those substance whose aqueous solution or molten form conduct electricity to a
greater extent. They almost completely ionised in water.
e.g. NaCl, H2SO4, HCl, NaOH, NH4Cl
Since strong electrolyte completely ionised in aqueous solution so their ionisation is represented as
HCl aq → H (aq) Cl − (aq)
(B) Weak electrolyte: Those substance whose aqueous solution or molten form conduct electricity to a lesser
extent. They do not completely ionised in water i.e. partly ionised. They behaves as poor conductor of
electricity.
e.g. when CH3COOH is dissolved in water, it ionised partly and an equilibrium is setup between the ions
and the unionised electrolyte.
CH3 COOH aq CH3COO− (aq) H (aq)
2. Non-electrolyte (non-conducting)
Those substance whose aqueous solution or molten form does not conduct electricity to any extent. They are
bad conductor of electricity.
e.g. aqueous solution of sugar, urea, etc. do not conduct electricity.
DEGREE OF IONISATION ‘α’
It may be defined as “fraction of total number of molecules which dissociates into ion”. It is represented by α.
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α Number of molecules dissociated as ions
Total number of molecules dissolved
Number of moles dissociatedTotal number of moles dissolved
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Sura’s NEET CHEMISTRY
4. CHEMICAL KINETICS AND NUCLEAR CHEMISTRY
INTRODUCTIONChemical Kinetics is the branch of science that deals with rate of reaction, factors affecting the rate of reaction and
reaction – mechanism.
Different reactions occur at different rate. In fact a chemical reaction involves redistribution of bonds –– breaking of
bond(s) in the reactant molecule(s) and making of bonds in the product molecule(s). The rate of a chemical
reaction actually depends upon the strength of the bond(s) and number of bonds to be broken during the reac-tion.
It takes longer time for the reactant molecules to acquire higher amount of energy which they do by colli-sion.
Hence reactions involving strong bond – breaking occur at relatively slower rate while those involving weak bond –
breaking occur at relatively faster rate. On the basis of rate, reactions are classified as.
Instantaneous or extremely fast reactions i.e. reactions with half-life of the order of fraction of second.
Extremely slow reactions i.e. reactions with half-life of the order of years.
Reactions of moderate or measurable rate.
Ionic reactions are instantaneous. If a drop of silver nitrate solution is added to a solution of the chloride salt of any
metal or solution of HCl, a white precipitate of silver chloride appears within twinkling of eye. This is because of the
fact that in aqueous solution an ionic compound exists as its constituent ions. No bond needs to be broken during
the reaction. Hence reaction takes no time to complete. The half life period of an ionic reac-tion is of the order of
10–10 s.
Na+ + Cl– + Ag+ + NO3− → AgCl↓ + Na+ + NO3
−
Free radicals being very unstable (reactive) due to the presence of unpaired electron, reactions involving free
radicals also occur instantaneously. Thus, the reactions, are instantaneous.CH3 + Cl2 → CH3Cl + Cl
CH3 + CH3 → H3C – CH3
Some molecular reactions involving reactant(s) containing odd electron completes within a fraction of second. The
speed of such reactions is attributable to the tendency of the odd electron molecule (paramagnetic in nature) to
transform into stable spin-paired molecule (diamagnetic) by dimerisation. An example of such reaction is the
dimerisation of nitrogen dioxide into nitrogen tetraoxide as mentioned below.NO2 + NO2 → N2O4
There are some molecular reactions which are known to be extremely slow. Their half-lives are of the order of
several years. Some examples of the type of reactions are as given below:
4 Fe xH2 O 3O2 → 2Fe2O3.xH2O
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[Cr(H2O)6]3+ + I– → [Cr(H2O)5I]2+ + H2O
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Sura’s NEET CHEMISTRY
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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4. It does not require any activation energy. 4. It requires activation energy.
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Sura’s NEET CHEMISTRY
6. GENERAL PRINCIPLESAND PROCESSES OF
ISOLATION OF ELEMENTSMetallurgy is the process of extracting metal in a pure state on large scale from its ore by physical or chemical
means.
Ore: It is a mineral from which a metal can be extracted profitably and conveniently.
All ores are minerals but all minerals are not ores.
Gangue/matrix: It is the impurity of sand and rocky materials present in the ore.
Occurrence of Metals: From a study of the activity series of metals it will be clear that certain metals due to their
inactive nature tend to exist in the free state, example: Ag, Au, Pt & Cu. The metals at the top of the activ-ity series
(K, Na, Mg etc) are so reactive that they are never found free in nature.
Most abundant metal is aluminum, next is iron.
Some important ores :
Oxide ores: Zincite ZnO
Bauxite Al2 O 3 .2H2 O
Corundum Al2 O3
Cuprite Cu 2 O
Haematite Fe 2 O3
Magnetite Fe 3 O4
Halide ores: Rock Salt NaCl
Horn Silver AgCl
Cryolite Na 3 AlF6
Fluorspar CaF2
Carnalite KCl, MgCl2 .6H2 O
Sulphide ores: Zinc blende ZnS
Galena PbS
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Cinnabar HgS
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Sura’s NEET CHEMISTRY
7. p - BLOCK ELEMENTS
INTRODUCTION
The right side of the periodic table having group number 13, 14, 15, 16, 17 and 18 are known as p – block
elements. These elements have 3, 4, 5, 6, 7 and 8 electrons in their outer most shell, respectively. The last electron
of these groups’ elements occupies the position in p – sub shell that is why are added as p – block elements. Their
general configuration is ns2np1-6.
NITROGEN FAMILY
The elements of groups 15 are nitrogen (N), phosphorous (P), arsenic (As), antimony (Sb) and bismuth (Bi). The
first two elements N and P are non – metal. The next two, arsenic and antimony are metalloids whereas the last
element, bismuth is a metal. The general electronic configuration of this group is ns2np3.
GENERAL TRENDS IN PHYSICAL PROPERTIES
Sr. No. Property Nitrogen Phospho- Arsenic Antimony Bismuthrus
1. Configuration [He]2s22p3 [Ne]3s23p3 [Ar]4s24p3 [Kr]5s25p3 [Xe]6s26p3
2. Common oxidation state −3, +3, +5 −3, +3, +5 +3, +5 +3, +5 +3
3. Atomic radius (pm) 70 110 120 140 150
4. First ionization energy (KJ/ 1012 1012 947 834 703mol)
5. Electronegativity 3.0 2.1 2.0 1.9 1.9
Illustration 5.
Name three allotropes of phosphorous? Which of the three is most reactive?
Solution: White or yellow, red and black. White phosphorus is most reactive.
Exercise - 1.
The range of the oxidation states shown by phosphorous is from
(A) −2 to 0 (B) 0 to +5
(C) −3 to +5 (D) 2 to +4
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Sura’s NEET CHEMISTRY
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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or 2.
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Sura’s NEET CHEMISTRY
9. CO-ORDINATIONCOMPOUNDS
INTRODUCTION(i) Co-ordination chemistry : is a branch of inorganic which deals with the study of co-ordination
compounds.
(ii) Addition or molecular compounds : When two or more stable compounds are allowed to combine
together in stoichiometric proportions, it results in the formation of crystalline substances called addition
compounds.
(iii) Addition compounds are classified into two types :
(a) Double salt
(b) Complex compounds
(iv) Double salt : Addition compounds which are quite stable in solid state but dissociate into ions in their
aqueous solution i.e. they give the test of all its constituent ions.
e.g. K2SO4.Al2(SO4)3.24H2O.
(v) Complex compounds : Addition compounds which are stable in solid state as well as in dissolved state.
They do not give the test of all its constituent ions e.g. K4[Fe(CN)6]
(vi) Complex ion : Metal atom which accepts the electron pair from ligands
(viii) Ligands : Species (neutral, negative, positive) which donate the electron pair to the central metal atom.
Depending upon the no. of donor sites, the ligands may be classified as:
Monodenate, bidentate, tridentate etc.
e.g. of monodentate: Cl − , Br − (negative ligands), H 2 O, NH3 (neutral ligand)
e.g. of bidentate : ( − CH 2 − NH 2 ) 2 and C 2 O42−
(ix) Ionisation sphere: Portion present outside the square bracket
Central Metal LigandIonisation
Sphereion
[Co(NH3)6]Cl3
Coordination
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Number
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Sura’s NEET CHEMISTRY
10. HALOALKANES ANDHALOARENES
INTRODUCTIONAlkyl halides or halo alkanes are compounds in which a halogen is bonded to an alkyl group. They have the
general formula RX (where R is alkyl group CnH2n+1) X is halogen atom.− H, X
RH → RX
alkane alkyl halide
Alkyl halides are classified as primary, secondary and tertiary alky halides depending on whether the halogen
atom is attached to a primary, secondary or tertiary carbon atom respectively.
For example
H
H3C C Cl
H
Chloro ethane (Primary)
CH3 CH3
H3C C Cl H3C C Cl
H CH3
2- Chloro propane (Secondary) 2- Chloro - 2 - methyl propane (tertiary)
Aromatic halogen compounds or halo arenes are the halogen compounds which contain atleast one aromatic
ring. Halogen derivatives of aromatic compounds are of two types.
1. Aryl halides
In this type of compounds, the halogen atom is directly linked to the carbon of benzene nucleus e.g.
Cl
Chloro benzene
2. Aralkyl halides
In this type of compounds halogen is linked to the carbon atom of the side chain.
CH2Cl
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1 - Chloro - 1 - phenyl methane
åå 516 åå
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11. ALCOHOL, ETHER & PHENOLIntroduction:Hydroxy Compounds(Alcohols)
Hydroxy compound can be classified into following three categories
H H
Monohydric H OH Contain only one-OH groupC C
H H
H H
Dihydric HO OH Contain two-OH groupC C
H H
H H H
Polyhydric H H Contain three and more than three hydroxyl group.C C C
OH OH OH
Monohydric alcohols are of three types.
Monohydric Alcohols
Primary or 10 Secondaryor 20
Tertiary or 30 Alcohol
R CH 2OHOH OH
R C R R C R
H R
Illustration 1:
Classify the following into primary, secondary and tertiary alcohols:
CH3 OH HO
(A)
OH
(B) H
3C
(C)
Solution:
(A) Tertiary
(B) Secondary
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(C) Tertiary
åå 578 åå
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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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Solution: (i) CH CH CHO
(ii) OHC − CH2 − CH2 − CH2 − CHO
åå 682 åå
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Sura’s NEET CHEMISTRY
SUBJECTIVE
Section A
Board Type Questions
Prob 1. Write chemical reactions to effect the following transformation.
(a) Butan-1-ol to butanoic acid
(b) Benzyl alcohol to phenylacetic acid
(c) Bromobenzene to benzoic acid
(d) p-methylacetophenone to benzene-1, 4-dicarboxylic acid
Sol. (a)CH3 − CH2 − CH2 − CH2
Aq. KMnO 4 Dil. H2SO4
− OH → CH3 CH2CH2 COOK →CH3CH2 CH2COOHButan-1-ol Pot. Butanoate Butanoic acid
(b) PBr3 KCN Hydrolysis C H CH COOHC H CH OH →C H CH Br → C H CH CN →
6 5 2 or HBr 6 52 6 5 2 H /H2 O 6 52
Benzyl alcohol Benzyl bromide Phenylacetic acid
(c)Mg Dry ice
H O
H COOH3C H Br → C H MgBr → C H COOMgBr →C
6 5 dry ether 6 5 6 5 6 5
Bromo benzene Phenyl mag. bromide Benzoic acid
i.e. CO2 (s)
(d)
H C COCH
3
KMnO4 /KOH,
COOK
Dil. H2 SO4
COOH3 → KOOC → HOOC
P-methylacetophenone Dipotassium benzene-1, 4- Benzene-1, 4-dicarboxylic acid
dicarboxylate
Prob 2. Arrange the following compounds in order of increasing acid strength.
CH3CH2CH(Br)COOH, CH3CH(Br)CH2COOH, (CH3)2CHCO2H, CH3CH2CH2COOH
Sol. We know that +I effect decreases while –I effect increases the acid strength of carboxylic acids. Since +I
effect of isopropyl group is more than that of propyl group. Therefore, (CH3)2CHCOOH is weaker acid than
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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.
åå 775 åå
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Sura’s NEET CHEMISTRY
CH3 H3C COOH
COOH COOHH3C COOH < H3C < <
H3C
Br Br
Prob 3. Arrange the following compounds in increasing order of their boiling points:
acetic acid, methyl formate, acetamide, propan-1-ol
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
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Prob 6: Arrange the following compounds in order of increasing acid strength:
åå 776 åå
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Sura’s NEET CHEMISTRY
L&+ &+ &+%U&22+ &+ &+%U&+ &22+ &+&+&2 + &+ &+ &+ &22+
(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:
4 − methoxybenzoic acid benzoic acid 4 − nitrobenzoic acid
3,4 − dinitrobenzoic acid
Prob 7: Why does benzoic acid not undergo Friedel-Crafts reaction?
Sol: Due to deactivation of the benzene ring by electrons withdrawing effect of the COOH group.
Prob 8: Identify (A) and (B) in the following sequence of reactions.
CH3COOH excess distil
(i)CH ≡ CH → A → B CH CHO
HgSO4 3
(ii) AIPO4 CH3COOHCH COOH →A →B
3 1075K
CH3COOH excess OOCCH distil CH CO
2 O CH CHOCH ≡ CH → CH − CH →
Sol: (i)Acetylene HgSO4 3 3 2 3 3
Ethylidene diacetate Acetic anhydride Acetaldehyde
AIPO4 , 1075K CH3COOH
2O(ii) CH COOH → CH C O → CH CO
3 −H2 O 2 3
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KetoneAcetic acid Acetic anhydride
åå 777 åå
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Sura’s NEET CHEMISTRYProb 9: Complete the following:
(a) H5C6 OH
PCl5 →heat
O
(b) H3C OK
H2 O →Electrolysis
O
Sol: (a) COOH COCl
PCl5 → HCl POCl3
(b) electrolysis −
K
CH3 COOK H2 O → CH3COOAt anode:
2CH3 COO− →
CH3
2CO 2 2e−
CH3
At cathode:
2e− 2H O → 2OH− H2 2
Prob 10: Arrange the following in decreasing order of the boiling points: CH3CH2CH2CH2OH, CH3CH2OCH2CH3.
CH3CH2CH2COOH.
Sol: CH3CH2CH2COOH > CH3CH2CH2CH2OH > CH3CH2OCH2CH3
Hint: Due to hydrogen bond
1. Among the carboxylic acids:
O OHO
O O O
H and
CH3 OH OH
(a) (b) (c)
the, one or more than one undergoing decarboxylation readily is (are)
(A) Only a (B) Both a and b
(C) a, b and d
Ans.C
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OBJECTIVE NO2
COOH
(d)
åå 778 åå
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Sura’s NEET CHEMISTRY2. In the following reaction,
γ − hydroxy carboxylic acid i) DIBALH →+
A isii) H
(A) γ − lactone (B) Lactide
(C) a hemiacetal (D) α, β- unsaturated acid
Ans. C
3. Which of the following can form an anhydride on heating?
OO
(A) H (B)HO O
OHHO
O OO
O(C) (D)
HOHO OH
OH
Ans. D
4.
Oi) ND3 ,
→Product is
ii) KOH, Br2 , H2O
OH
NH2 ND2
(A) (B)
O NH2 O ND2
(C) (D)
Ans. D
5. Acetamide is treated separately with the following reagents. Which one of these would give methylamine?
(A) PCl5 (B) Sodalime (C) NaOH + Br2 (D) None of these
Ans. C
6.
O||
→Pr oductPh − C − OH CH N2 2
(A) PhCOOCH2N2 (B) PhCOOCH3
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(C) PhCH3 (D) none of these
Ans. B
åå 779 åå
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A O
C O
7. H C H CB
O H D O(C O) bond lengths designated by A, B, C, D are in order
(A) A = C < B = D (B) A < B < C = D
(C) A < C = D < B (D) all are equal
Ans. B
NH / KBrO HNO8. A (monobasic acid) →3 B →C →2 (H3C)3C OH
or
(H3C)3C Bror
H3CC
CH3
CH2
A is
(A) CH3 3 C − COOH(B)
CH3
H3C CH CH2 COOH
(C) H3C CH2 CH2 COOH (D) CH3
H3C C CH COOH
CH3
Ans. A
O O
9. on saponification forms
O O
(A) H O (B) 2CH3OH, 2HCOOHOH
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OH
H O
(C) HO O (D)OH
O
OH
H OHOH OH C
HO O
Ans. C
åå 780 åå
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10.
(A)
(C)
Ans. B
O
C NH2 →P4O10 A
O
C CH3
O
C
MeMgBr i Ca OH2B → C → ii I2 , H3 O
H3 O
(B)
COOH
(D)
MCQ
1. Which of the following are nucleophiles?
(A) Water (B) Ammonia
(C) triphenylsulphate (D) Iodides
Ans. A,B,C,D
2. Which of the following arrangements show a correct order of nuclophilicity?
(A) I− Br − Cl − F− (B) RS− RO−
(C) R3 N : R3P : (D) RO− RS−
Ans. A,B
3. Which of the following reactions can be used for the preparation of alkyl halides?
anhyd.ZnCl2 (B) CH CH OH HCl →(A) CH CH OH HCl →
3 2 3 2
(C) CH3 3 COH HCl →anhyd.ZnCl2
(D) CH3 2 CHOH HCl →Ans.A,C,D
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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
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(C) H3CHC CH3(D) CH3
H3COH C OH
CH3
Ans.A,B,C
ASSIGNMENT
SUBJECTIVE
1. Describe the following:
(a) Saponification (b) Decarboxylation
2. How is acetic acid prepared from?
(i) Acetylene (ii) Ethyl alcohol
3. How is Grignard reagent employed to prepare a carboxylic acid?
4. Explain the following about acetic acid:
(i) Its boiling point is higher than that of n – propanol.
(ii) It is weaker acid than formic acid.
(iii) It is stronger acid than phenol.
5. Acid anhydrides have higher boiling points than the corresponding carboxylic acids.
6. Give IUAPC name for each of the following compounds.
(a) H3CHC CHCOOH (b)COOH
(c) CHCOOH (d) Cl2CHCOOH
CH3
(e) O
HOC(CH2)3COOH
7. HOCH2CH2CH2CH2COOH can be prepared from HOCH2CH2CH2CH2Br in two ways. One is through Grignard
synthesis and the other through nitrile synthesis. Which method would you prefer?
8. Why the bond length of C = O in carboxylic acids is bit longer than in aldehydes?
9. Acetic acid can be halogenated in presence of phosphorus and chlorine but formic acid cannot be haloge-
nated in the same way.
10. During the preparation of esters from a carboxylic acid and an alcohol in the presence of an acid catalyst, the
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water or the ester should be removed as fast as it is formed. Explain.
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