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FORMAL CHARGE

. . . . :. N. N. :. H. . . H. FORMAL CHARGE. Unbonded. Bonded. Number of All One half of = valence electrons unshared + all shared

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FORMAL CHARGE

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  1. .. . . . : N N : H . . H FORMAL CHARGE Unbonded Bonded Number of All One half of = valence electrons unshared + all shared in the neutral electrons electrons atom Formal Charge . NH2- . 6e- 5e- ( Formal Charge = 5 - 4 - 2 = -1 )

  2. When drawing a Lewis Diagram remember these rules. LEWIS DIAGRAMS SHOW IT ALL ! - all atomsincluding hydrogens - all bonds (lines not dots ) - all unshared pairs ( dots ) - allformal charges - all atoms with octets ( except H ) - the correct number of electrons ( count! )

  3. Rumus Kimia • Rumus empirik • Rumus Molekul • Rumus struktur • Rumus struktur lengkap • Rumus struktur panjang (expanded) • Rumus struktur termampatkan (condensed)

  4. Rumus Struktur pada senyawa siklis – sikloheksana • Expanded formula

  5. Rumus Struktur pada senyawa siklis – sikloheksana • Polygon formula(condensed formula)

  6. Rumus Struktur pada senyawa siklis – sikloheksana • Condensed formula

  7. Contoh Molekul siklis

  8. Beberapa cara penulisan struktur

  9. Molekul polar dan Nonpolar • To determine if a molecule is polar, we need to determine • if the molecule has polar bonds • the arrangement of these bonds in space • Molecular dipole moment (): the vector sum of the individual bond dipole moments in a molecule • reported in debyes (D)

  10. are due to differences in electronegativity. depend on the amount of charge and distance of separation. In debyes,  = 4.8 x (electron charge) x d(angstroms) Bond Dipole Moments

  11. Molecular Dipole Moments • Depend on bond polarity and bond angles. • Vector sum of the bond dipole moments. • Lone pairs of electrons contribute to the dipole moment.

  12. Polar and Nonpolar Molecules • these molecules have polar bonds, but each has a zero dipole moment

  13. Polar and Nonpolar Molecules • these molecules have polar bonds and are polar molecules

  14. Polar and Nonpolar Molecules • formaldehyde has polar bonds and is a polar molecule

  15. Intermolecular Forces • Strength of attractions between molecules influence m.p., b.p., and solubility; esp. for solids and liquids. • Classification depends on structure. • Dipole-dipole interactions • London dispersions • Hydrogen bonding

  16. Dipole-Dipole =>

  17. Dipole-Dipole Forces • Between polar molecules • Positive end of one molecule aligns with negative end of another molecule. • Lower energy than repulsions, so net force is attractive. • Larger dipoles cause higher boiling points and higher heats of vaporization.

  18. => London Dispersions • Between nonpolar molecules • Temporary dipole-dipole interactions • Larger atoms are more polarizable. • Branching lowers b.p. because of decreased surface contact between molecules.

  19. Dispersions =>

  20. Hydrogen Bonding • Strong dipole-dipole attraction • Organic molecule must have N-H or O-H. • The hydrogen from one molecule is strongly attracted to a lone pair of electrons on the other molecule. • O-H more polar than N-H, so stronger hydrogen bonding

  21. H Bonds

  22. Boiling Points and Intermolecular Forces

  23. ASAM DAN BASA

  24. Brønsted-Lowry Theory of Acids and Bases • Acid: Proton Donor • Base: Proton Acceptor Conjugate Acid: Base + Proton Conjugate Base: Acid - Proton

  25. Strong Acids and Bases • Strong acid - completely ionized in aqueous solution. Examples are: • HCl, HBr, HI, HNO3, HClO4, and H2SO4 • Strong base - completely ionized in aqueous solution. Examples are: • LiOH, NaOH, KOH, Ca(OH)2, and Ba(OH)2

  26. Weak Acids and Bases • Acetic acid is a weak acid • it is incompletely ionized in aqueous solution

  27. Lewis Theory of Acids and Bases • Acid: Electron-Pair Acceptor • Electrophile • Base: Electron-Pair Donor • Nucleophile

  28. Weak Acids and Bases • The equation for the ionization of a weak acid, HA, in water and the acid ionization constant, Ka, for this equilibrium are

  29. Weak Acids and Bases

  30. Acidity Constant (Ka)

  31. pKa pKa = - log Ka Strong acid = large Ka = small pKa Weak acid = small Ka = large pKa

  32. Relative Acid Strength

  33. Acid Strength • Strong Acid • Conjugate base is weak • pKa is small • Weak Acid • Conjugate base is strong • pKa is large

  34. Base Strength • Strong Base • Conjugate acid is weak • pKa is large • Weak Base • Conjugate acid is strong • pKa is small

  35. Position of equilibrium • Favors reaction of the stronger acid and stronger base to give the weaker acid and weaker base

  36. Position of equilibrium • Stronger acid and stronger base react to give weaker acid and weaker base

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