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Summary Descriptive Inorganic Chemistry 9-Hybrid Orbitals, Shapes of Molecules, Texas A&MU 2019
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Lewis Structures Hybrid Orbitals Shapes of Molecules (Common Stereochemistries in Main Group Compounds)
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Lecture 9 February 4, 2019Lewis Structures
Hybrid Orbitals
Shapes of Molecules (Common
Stereochemistries in Main Group
Compounds)
,Two Electrons Shared between Two Atoms
Make a Bond! G.N. Lewis
(G. = Gilbert
N. = Newton
Lewis as in Lewis Structures!)
Lewis Structures and VSEPR:
Workshop Study
Simple Review videos
https://www.youtube.com/watch?v=1ZlnzyHahvo
https://www.youtube.com/watch?v=xNYiB_2u8J4
, Rules for Oxidation State Assignment
Rule 1: The oxidation number of an element in its free (uncombined) state is zero —
for example, Al(s) or Zn(s). This is also true for elements found in nature as diatomic (two‐atom) elem
and for sulfur, found as:
Rule 2: The oxidation number of a monatomic (one‐atom) ion is the same as the charge on the ion
Rule 3: The sum of all oxidation numbers in a neutral compound is zero. The sum of all oxidation
numbers in a polyatomic (many‐atom) ion is equal to the charge on the ion
that may have multiple oxidation states, if the other atoms in the ion have known oxidation numbers.
Rule 4: The oxidation number of an alkali metal (IA family) in a compound is +1;
the oxidation number of an alkaline earth metal (IIA family) in a compound is +2.
Rule 5: The oxidation number of oxygen in a compound is usually –2. If, however, the oxygen
is in a class of compounds called peroxides (for example, hydrogen peroxide),
then the oxygen has an oxidation number of –1.
Rule 6: The oxidation state of hydrogen in a compound is usually +1.
If the hydrogen is part of a binary metal hydride (compound of hydrogen and some metal),
then the oxidation state of hydrogen is –1.
Rule 7: The oxidation number of fluorine is always –1.
Chlorine, bromine, and iodine usually have an oxidation number of –1,
unless they’re in combination with an oxygen or fluorine.
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