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Lecture Organic chemistry: Chapter 1 - L. G. Wade, Jr.

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Chapter 1 introduction and review the organic chemistry. The goal is for you to learn: Review concepts from general chemistry that are essen-tial for success in organic chemistry, such as the electronic structure of the atom, Lewis structures and the octet rule, types of bonding, electronegativity, and formal charges; predict patterns of covalent and ionic bonding involving C, H, O, N, and the halogens. Identify resonancestabilized structures and compare the relative importance of their resonance forms. | Chapter 1 Chapter 1 © 2010, Prentice Hall Organic Chemistry, 7th Edition L. G. Wade, Jr. Introduction and Review Chapter 1 Organic Chemistry Organic chemistry is the chemistry of carbon compounds. Chapter 1 Electronic Structure of the Atom An atom has a dense, positively charged nucleus surrounded by a cloud of electrons. The electron density is highest at the nucleus and drops off exponentially with increasing distance from the nucleus in any direction. Chapter 1 The 2p Orbitals There are three 2p orbitals, oriented at right angles to each other. Each p orbital consists of two lobes. Each is labeled according to its orientation along the x, y, or z axis. Chapter 1 Isotopes Isotopes are atoms with the same number of protons but different number of neutrons. Mass number is the sum of the protons and neutrons in an atom. Chapter 1 Electronic Configurations of Atoms Valence electrons are electrons on the outermost shell of the atom. Chapter | Chapter 1 Chapter 1 © 2010, Prentice Hall Organic Chemistry, 7th Edition L. G. Wade, Jr. Introduction and Review Chapter 1 Organic Chemistry Organic chemistry is the chemistry of carbon compounds. Chapter 1 Electronic Structure of the Atom An atom has a dense, positively charged nucleus surrounded by a cloud of electrons. The electron density is highest at the nucleus and drops off exponentially with increasing distance from the nucleus in any direction. Chapter 1 The 2p Orbitals There are three 2p orbitals, oriented at right angles to each other. Each p orbital consists of two lobes. Each is labeled according to its orientation along the x, y, or z axis. Chapter 1 Isotopes Isotopes are atoms with the same number of protons but different number of neutrons. Mass number is the sum of the protons and neutrons in an atom. Chapter 1 Electronic Configurations of Atoms Valence electrons are electrons on the outermost shell of the atom. Chapter 1 Electronic Configurations The aufbau principle states to fill the lowest energy orbitals first. Hund’s rule states that when there are two or more orbitals of the same energy (degenerate), electrons will go into different orbitals rather than pairing up in the same orbital. Electronic configuration of carbon Chapter 1 Ionic Bonding To obtain a noble gas configuration (a full valence shell), atoms may transfer electrons from one atom to another. The atoms, now bearing opposite charges, stay together by electrostatic attraction. Chapter 1 Covalent Bonding Electrons are shared between the atoms to complete the octet. When the electrons are shared evenly the bond is said to be nonpolar or pure covalent. When electrons are not shared evenly between the atoms, the resulting bond will be polar. Chapter 1 CH4 NH3 H2O Cl2 Lewis Structures Carbon: 4 e 4 H@1 e ea: 4 e 8 e Nitrogen: 5 e 3 H@1 e ea: 3 e 8 e Oxygen: 6 e 2 H@1 e ea: 2 e 8 e 2 Cl @7 e ea: 14 e .