chapter2

1. lowry definition

1.1. Hydronium ion, the product that results when the base H₂O gains a pro- ton, is called the conjugate acid of the base Another way to predict acid-base reactivity is to remember that the prod uct conjugate acid in an acid-base reaction must be weaker and less reactive than the starting acid and that the product conjugate base must be weaker and less reactive than the starting base

2. bases

2.1. Organic bases are characterized by the presence of an atom (reddish in electro- static potential maps) with a lone pair of electrons that can bond to H+

3. lewis definition

3.1. most oxygen- and nitrogen-containing organic compounds can act as Lewis bases because they have lone pairs of electrons. A divalent oxygen compound has two lone pairs of electrons, and a trivalent nitrogen compound has one lone pair. Note in the following examples that some compounds can act as both acids and bases, just as water can

4. electronegativity

4.1. electron distribution between atoms is not symmetrical

5. dipole moments

5.1. Molecular polarity results from the vector summation of all individual bond polarities and lone-pair contributions in the molecule

6. formal charges

6.1. a typical covalent bond is formed when each atom donates one electron

7. resonance

7.1. The atoms them- selves occupy exactly the same place in both resonance forms, the connec tions between atoms are the same, and the three-dimensional shapes of the resonance forms are the same

8. rules

8.1. Rule 1 Individual resonance forms are imaginary, not real Rule 2 Resonance forms differ only in the placement of their or nonbonding elec trons Rule 3 Different resonance forms of a substance don't have to be equivalent Rule Rule 4 Resonance forms obey normal rules of valency Rule 5 The resonance hybrid is more stable than any individual resonance form