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Chapter 9

Chapter 9. Intermediate Type of Bonding. 9.1 Incomplete Electron Transfer in Ionic Compounds 9.2 Electronegativity of Elements 9.3 Polarity of Covalent Bonds. 9.1 Incomplete Electron Transfer in Ionic Compounds (SB p.234). Expt al value of H lattice .

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Chapter 9

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  1. Chapter 9 Intermediate Type of Bonding 9.1 Incomplete Electron Transfer in Ionic Compounds 9.2 Electronegativity of Elements 9.3 Polarity of Covalent Bonds

  2. 9.1 Incomplete Electron Transfer in Ionic Compounds (SB p.234) Exptal value of Hlattice Theoretical Values of Lattice Enthalpy Born-Haber Cycle for the formation of sodium chloride Hlatticecan be found from the Born-Haber Cycle

  3. 9.1 Incomplete Electron Transfer in Ionic Compounds (SB p.234) Another way of getting the value of Hlattice Assuming perfect ionic model 1. Ions are perfect spheres with uniform charge distribution. 2. The cations and anions are in contact with each other and with electrostatic interactions in between.

  4. 9.1 Incomplete Electron Transfer in Ionic Compounds (SB p.234) _ R + q1 q2 Theoretical value of Hlattice Another way of getting the value of Hlattice The force(F) between two point charges q1 and q2 separated by a distance R is given by: Hlattice = work done when the ions are allowed to be brought from infinite separation to the internuclear distance in the ionic lattice where r is the normal internuclear distance

  5. 9.1 Incomplete Electron Transfer in Ionic Compounds (SB p.236) Polarizing power of cation polarizability of anion Increasing polarization of a negative ion by a positive ion Polarization / Distortion of electron cloud = Covalent character in ionic bond

  6. 9.1 Incomplete Electron Transfer in Ionic Compounds (SB p.236) Polarizing power of cation Increasing polarization of a negative ion by a positive ion Polarizing power of a cationincreases as its charge density(charge/volume ratio) increases. polarizing power:Al3+ > Mg2+ > Na+ andLi+ > Na+ > K+

  7. 9.1 Incomplete Electron Transfer in Ionic Compounds (SB p.236) polarizability of anion Increasing polarization of a negative ion by a positive ion Polarizability of a anionincreases as its size increases. polarizability:I- > Br- > Cl- andS2- > O2-

  8. 9.2 Electronegativity of Elements (SB p.238) Electronegativity values of some representative elements XY X: Y Electronegativity is defined as the relative tendency of an atom to attract a bonding pair of electrons towards itself.

  9. 9.3 Polarity of Covalent Bonds (SB p.239) a pure covalent bond a polar covalent bond Bond Polarization

  10. 9.3 Polarity of Covalent Bonds (SB p.239) Relationship between the type of bond and difference in electronegativity between two bonded atoms

  11. 9.3 Polarity of Covalent Bonds (SB p.240) Relationship between bond nature and difference in electronegativity between bonded atoms.

  12. 9.3 Polarity of Covalent Bonds (SB p.240) represented by dipole moment () Polarity of Molecules How polar is the molecule?  (Debye, D) = q x d

  13. 9.3 Polarity of Covalent Bonds (SB p.241) The effect of an electric field on polar molecules

  14. 9.3 Polarity of Covalent Bonds (SB p.241) The effect of an electric field on non-polar molecules

  15. 9.3 Polarity of Covalent Bonds (SB p.242) Non-polar Molecules

  16. 9.3 Polarity of Covalent Bonds (SB p.242) Non-polar Molecules (Cont’d)

  17. 9.3 Polarity of Covalent Bonds (SB p.243) Polar Molecules

  18. 9.3 Polarity of Covalent Bonds (SB p.243) Use of Dipole Moments

  19. 9.3 Polarity of Covalent Bonds (SB p.244) Effect of a Non-uniform Electric Field on polar and Non-polar Liquid

  20. The END

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