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Table 2.1

Table 2.1. Lewis structures of some common molecules. H. H. N. H. N. N. S. O. O. O. O. O. O. H. N. H. P. O. O. O. 3. -. O. Cl. O. O. O. P. O. -. O. 2-. O. O. O. O. O. S. O. O. coordinate covalent. 2. -. Molecule. Lewis structures*. H 2. C. O.

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Table 2.1

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  1. Table 2.1 Lewis structures of some common molecules H H N H N N S O O O O O O H N H P O O O 3 - O Cl O O O P O - O 2- O O O O O S O O coordinate covalent 2 - Molecule Lewis structures* H2 C O N2,CO O3, SO2,NO2- NH3, SO32- PO43-, SO42-, ClO4-

  2. Formal Charge (F.C.)

  3. What is the oxidation number of (a) nitrogen in the azide ion, and (b) manganese in the permanganate ion, (a) 3 x O.N(N) = -1. O.N.(N) = Oxidation number of an element (b) O.N.(Mn) + 4 x O.N.(O) = -1 O.N.(Mn) = -1-4x(-2) = +7.

  4. In fact these are called the the resonance structures of the carbonate oxyanion. Resonance

  5. Resonance

  6. Resonance has two man effects: The BF3 molecule, for instance, is a resonance structures 1. Resonance averages the bond characteristics over 2. Resonance reduces the energy of the molecule any single contributing structure.

  7. Write resonance structures for the NO2F molecule and identify the dominant structures.

  8. Write resonance structures for the ion. :

  9. Hypervalent compounds. : SF6, PCl5,

  10. Stoichiometry of covalent molecules In this way the stoichiometry of covalent molecules is determined by the number of valence electrons available for sharing and forming two electron pairs. Dative covalent bond.

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