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PROBLEM SOLVINGTECHNIQUES
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ELECTROCHEMICAL SERIES
R R R
REDUCTION POTENTIAL REDUCED RIGHT
HIGHER THE REDUCTION POTENTIAL MORE EASILY REDUCED PLACED AT RIGHT
1. Formation of electrochemical cell
2. Calculation of E0 &e.m.f cell
3. Study of displacement reaction
4. Prediction of feasibility of redox reaction
5. Protection of metal from corrosion.
6. Prediction of the product of electrolysis
PRODUCT OF ELECTROLYSIS
MOLTEN ELECTROLYTE Aq.ELECTROLYTE
OPPOSITE IONS ARE NEUTRALISEDAT OPPOSITE ELECTRODE
Inert electrode Same metal electrode
in case of (- ve ions)
Simple ion is oxidised at anode
in case of (+ ve ions)
Cathode reaction issame but None of thenegative ions areOxidised at cathodein stead of allnegative ionsElectrodes itselfoxidised
Higher reduction potential is reduced at cathode
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An aqueous solution of AgNO3 with silver electrodes.An aqueous solution of AgNO3 with platinum electrodes
HIGHER THE REDUCTION POTENTIAL MORE EASILY REDUCED PLACED AT RIGHT
AT CATHODE OUT OF Ag+ AND H+ ,Ag+ IS REDUCEDDUE TO HIGHER REDUCTION POTENTIAL
AT ANODE OUT OF OH- & NO3 –, OH- IS SIMPLE IONS SO OXIDISEDwith platinum electrodes
IF Ag ELECTRODES IS USE- CATHODE REACTION IS SAME
AT ANODE INSTEAD OF ALL –IVE IONS Ag ELECTRODE IT SELF OXIDISED
H & Cu,Ag Hg
H WITH OTHER
Prediction of feasibility of redox reaction
HIGHER THE REDUCTION POTENTIAL MORE EASILY REDUCED PLACED AT RIGHT
What would happen if Nickel spatula is usedto stir a solution of CuSO4?E0Cu2+ / Cu = 0.34 V, E0Ni 2+ / Ni = -0.25V?
. SOLUTION – CONTAINER = POSITIVE VALUE THAT CANNOT BE STORED
Cu2+ IS SOLUTION
Ni IS CONTAINER
0.34 – (-0.25) = 0.59 IS POSITIVE VALUE
CANNOT BE STORED/USED
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USES OF VANT HOFF FACTOR
DIFFERENT NO OF MOLE SAME NO OF MOLE
COLLIGATIVE PROPERTY α i α I/molar mass3% urea&3% GLUOSE
CALCULATE i
FREZING POINT ,VAPOUR PRESURE α I/ i
OTHER COLIGATIVE PROPERTIES α i
0.1 M UREA &0.1M NaCl
P BLOCK ELEMENT
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MO
If p
No
BOND ORDER
BOND ORDER OF DIATOMICLECULES / IONS BOND ORDER OF
POLATOMICMOLECULES / IONS
-electrons are up to 6
of p–electrons = BO2
If p-electrons > 6
Total no of bondB
O Total no of resonating structure
6 – more p electrons than 6 = BO2
BOND ANGLE
HYBRIDISATION IS SAMELONE PAIRS ARE DIFFERENT
HYBRIDISATIONIS SAME LONEPAIRS ARE SAME
Bond angle α 1/no of lone pairs Bond angle α electronegativity α 1/size
PH4+ & PH3
NH3 & PH3
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BOND POLARITY
DIATOMIC MOLECULE POLYATOMIC MOLECULE
HomoatomicNon polar
HeteroatomicPolar
Regular moleculeOnly bond pair Irregular molecule
Lone pair
I2 ICl Polar
Same surrounding elementNon polar
Different surrounding elementpolar NH3
BOND LENGTH
BOND LENGTHS ARE SAME BOND LENGTHS ARE DIFFERENT
DUE TO RESONANCE DUE TO ELECTRONIC REPULSION
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ACIDIC PROPERTIES
NON OXOACID OXOACID
ACIDIC NATURE α SIZE α 1/B.E ACIDIC NATURE α STABILISATION OFCONJUGATE BASE
HI > HBr > HClHClO4 > HClO3 > HClO2 > HClO
BASIC NATURE
HYDROXY BASE (-OH PRESENT ) NON HYDROXY BASE ( -OH NOT PRESENT)
OH- REMOVAL CAPACITY H+ ATTRACTION CAPACITY
BASIC NATURE α SIZE α 1/BE BASIC NATURE α ELECTRONEGATIVITY
KOH > NaOH > LiOH NH3 PH3 AsH3
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REDUCTION PROPERTIES
HYDRIDEOXOACID
REDUCTION PROPERTIES α SIZE α 1/B.E REDUCTION PROPERTIES α NO OF (E-H)SINGLE BOND
H2S < H2Te H3PO2 > H3PO3
BOILING POINT
MOLECULAR FORCE
HYDROGEN BONDING VANDERWAAL FORCE
B. P α MOLECULAR MASS α 1/ branching
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OXOACID OF PHOSPHORUS
STRUCTURE TETRAHEDRAL AT LEASTONE P=O AND ONE P-OH GROUP,
FUNCTION NUMBER OF P-OHBOND =BASICITY
NUMBER OF P-H BOND=REDUCTIONCAPACITY
TYPE OF OXOACID
ORTHO- PARENT ACIDPYRO- 2 X ORTHOACID-H2OHYPO – ORTHOACID-OMETA-ORTHO ACID-H2OPEROXOMONO-ONE-OH IS REPLACED
BY – OOHPEROXODI- FROM PYRO – O-IS
REPLACEDBY –OO-
COMPARASION OF OXIDATION STATE BOTTOM ELEMENT AND OTHER –INERT PARE EFFECT
COMPARASION OF PHYSICAL STATE OF THE SECOND PERIOD &AND THIRDPERIOD ELEMENTS---- P∏-P∏ BONDING
INCREASE OF COVALENCY –VACAND d ORBITAL
LOWEST OXIDATION STATE -OUTERMOST ELECTRONS-8, STABILITY DECREASESDOWN THE GROUP DUE TO ELECTRONEGATIVY DECREASES
HIGHEST OXIDATION STATE =OUTERMOST ELECTRONS STABILITYDECREASES DOWN THE GROUP-DUE TO INERT PAIR EFFECT
CATENATION PROPERTY α B.D.E α 1/SIZE α 1/ELECTRONIC REPLUCTION
THERMAL STABILITY α 1/SIZE
OXIDISING POWER OF OXO ACID DECREASES WITH INCREASE OF OXIDATION STATE
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Meta
IE α
llic and non metalliccharacter
1/Metallic property
IONISATIONENTHALAPY
Stability of oxidation state
METALLIC AND NONMETALLIC NATURE
BOND ENTHALPY
∆EN α 1/BONDLENGTH
BOND
ENERGY αELECTRONEG
ATIVITYDIFFRENCE
ACIDIC STRENGTH OF HYDRIDEBOND ENERGY α STABILITY
OF MOLECULE
APPLICATION OFELECTRONEGATIVITY
REACTIVITYDIFFRENCE IN
ELECTRONEGATIVITY α STABILITYα 1/REACTIVITY
NATURE OF BOND ANDPRCENTAGE OF IONIC CHARECTER
NOMENCLATURE OFINORGANIC
COMPOUNDSOF2 OXYGEN DIFLORIDE
ACIDIC NATURE OFTHE OXIDE α
ELECTRONEGATIVITY
NATURE OF HYDROXIDE
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HYBRIDISATION STATE
TOTAL σ bond pair+ lone pair=Hybridisation state
Organic chemistry
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/+I
ACID
NUCLEOPHILIC SUBSTITUTION
SN2 SN1
STERIC HINDRANCE,NATURE OF LEAVING GROUP
S T A B I L I T Y O F C A R B O C A T I O NN A T U R E O F L E A V I N G G R O U P
Stability of Carboanion
Stability of (C –) α –I
INDUCTIVEEFFECT POLAR
ITY OFORGA
NICCOMPOUND
IC STRENGTH
Acidic Strength α -I/+I
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ing St
Electron den
Stability of Carboanion
Stability α No of resonat
RESONANCEEFFECT Reactivity of
BenzeneTowards
electrophilicsubstitution
ACIDC NATURE
BASIC NATURE
Basic nature α +R, +I/-R, -I
sity increases by resonance H + attraction capacityMore basic & vice-versa
Directive nature of group attached to benzene
Ortho/para directingContain lonepair electron
Meta directingDouble bond/triple bond presentThat must attach to one moreElectnegative element
+R effect -Reffect
-OH,-OR,-NH2 -CHO,-COOH,-SO3H
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