Lecture_2 - Lecture 2 Chapter 1: Structure and...

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Unformatted text preview: Lecture 2 Chapter 1: Structure and Bonding Reac7ons of Organic Compounds bonds break bonds form bonds result from sharing electrons How easy a bond breaks and how easy it forms depends on what electrons are shared, which depends on the atoms to which they belong. We need to look at the structure of an atom: what electrons it has and where they are located. The Structure of an Atom protons are posi+vely charged neutrons have no charge electrons are nega+vely charged atomic number = # of protons atomic number of carbon = 6 neutral carbon has 6 protons and 6 electrons The Distribu7on of Electrons in an Atom   The first shell is closest to the nucleus.   The closer the atomic orbital is to the nucleus, the lower its energy.   Within a shell, s < p AuBau, Hund, Pauli  Which one is the Pauli Exclusion Principle? A. Electrons are filled in degenerate orbitals singly before being paired up B. No more than two electrons can occupy an atomic orbital C. An electron goes into an orbital with the lowest energy first Electrosta7c Map Poten7als Formal Charge PROBLEM 13 Give each atom the appropriate formal charge: Representa7on of Structure  Drawing Lewis Dot Structures: 1.  2.  3.  4.  Determine # Valence E ­ for each atom Arrange atoms rela+ve to each other Fill electrons on outer atoms to maximum H has 1 bond, if no octet on others form double bond 5.  Assign formal charges, draw resonance Lewis Structures  SO3 ...
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