Chemical Bonding PDF

01 EP 02 =CVE + no. of MV...

01 EP 02 =CVE + no. of MV 03 VALENCE BOND THEORY 05 BOND ORDER VSEPR 2 HYBRIDISATION C - C = 1 bond 2 - 1 - Diamagnetic MV Remaining Monoatomic C = C = 1 + 1π Total 3 - 0.5 - Paramagnetic 2,0- Linear - 180o surrounding 2- sp - Linear C - = C = 1 + 2π no.of 4 - 0 - Diamagnetic 3,0- Trigonal planar - 120 o BP LP atoms e- 5 - 0.5 - Paramagnetic 3- sp2 - Trigonal planar MOLECULAR ORBITAL THEORY 6 - 1 - Diamagnetic 2,1- Bent shape 7- 0.5- Paramagnetic EP =CVE + 0 4- sp 3 - Tetrahedral Up to N2 the energy order is, 8 - 0 - Diamagnetic 4,0- Tetrahedral - 109o28| 2 5- sp3d - Trigonal pyramidal 9 - 0.5 - Paramagnetic 3,1- Pyramidal - 107o DV Remaining Diatomic 1s< *1s< 2s< *2s O2 WALLAH 3 2.5 2 B.L-O2>O2 >O2 + 2+ 1) Max B.A-1800[sp] 1) Polar molecule, = 0 Resonance Changes B.O. 1) B.L with Size of atom BOND 1) Hybridisation DIPOLE Irregular geometry. 1) Benzene BOND 2) Hybridisation BOND MOMENT a) Different bonds RESONANCE ANGLE sp > sp2 > sp3 HI > HBr > HCl > HF ENERGY sp> sp2 >sp3 ( ) b) Lone pairs 3 NO2+ > NO2 > NO2- LENGTH 2) B.E. B.O. (No. of Bonds) c) Different surrounding atoms = 2 = 1.5 sp sp 2 2) B.L decreases with eg: SF4, CH3Cl 3) if LP B.A N2> O2 >F2 2) Non polar molecule, =0 CH4 > NH3 > H2O [sp3] multiplicity B.L.: C2H6 > C6H6 > C2H4 > C2H2 3) B.E. E.N. difference Regular geometry 0 LP 1 LP 2 LP C-C>C=C>C=C a) Same bonds B.O.: 1 1.5 2 3 HF> HCl > HBr > HI b) Zero lone pairs 4) If electronegativity of 2) O3 3 C.A B.A 4) Halogens (B.E.) c) Same surrounding atoms = 2 = 1.5 NH3 > PH3 > AsH 3 > SbH3 eg: CH4, CO2 Cl2> Br2 > F2 > I2 CH3OH > CH3Cl > H2O> NH3> NF3> BF3 B.L.: H2O2 > O3 > O2 5) If electronegativity oF S.A B.A X X X =0 NI 3> NBr3 > NCl 3> NF3 X > B.O.: 1 1.5 2 O > O X O X Q9 The correct order of increasing Q8 The correct order of bond angle is: Q5 Which of the following molecules has the maximum bond enthalpy? Q6 Which of the following will have maximum dipole moment? Q7 The correct order in which the O-O bond length 1) H2O > NH3 > CH4 > CO2 bond length of C-H,C-O,C-C & C=C is: 1) C-C < C=C < C-O < C-H 1) N2 2) CO decreases in the following is 2) H2O < NH3 < CO2 > CH4 2) C-O < C-H < C-C < C=C 1) NF3 2) NH3 1) O3 > H2O2 > O2 2) O2 > O3 > H2O2 3) H2O < NH3 > CO2 > CH4 3) C-H < C-O < C-C < C=C 3) F2 4) HF 3) CH4 4) PCl3 3) O2 > H2O2 > O3 4) H2O2 > O3 > O2 4) CO2 > CH4 > NH3 > H2O 4) C-H < C=C < C-O < C-C Fajan‛s Rule - Indicates Covalent character in an ionic bond. Hydrogen bond- Formation of bond between hydrogen & most electronegetive elements like F,O,N 1) Size of the cation- Smaller the cation higher is the polarisation, so covalent character increases Intramolecular - H – Bonding occur within one single molecule. LiCl > NaCl > KCl > RbCl > CsCl 2) Size of anion- As the size of anion increases, polarisation increases, covalent character increases Intermolecular - H Bonding between two different molecules of same or different compounds. AgF < AgCl < AgBr < AgI Intramolecular H bonding increases the boiling point. eg: Intermolecular H bond in p-nitrophenol 3) Charge on the cation- As the charge increases, Covalent character also increases increases the boiling point. HF(HB) > HI > HBr > HCl. H2O(4HB) > H2Te > H2Se > H2S LiCl < BeCl2 < BCl3 < CCl4