Trabajos

Organic Chemistry 6th Edition
Paula Yurkanis Bruice

Chapter 1
Electronic Structure and Bonding Acids and Bases
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Organic Chemistry
•  Carbon-containing compounds were once considered
“organ compounds” available only from living organisms. •  The synthesis of the simple organic compound urea in 1828 showed that organic compounds can be prepared in thelaboratory from non-living material. •  Today, organic natural products are routinely synthesized in the laboratory.

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Why Carbon?
•  Carbon neither gives up nor accepts electrons because it is in the center of the second periodic row. •  Consequently, carbon forms bonds with other carbons and other atoms by sharing electrons. •  The capacity of carbon toform bonds in this fashion makes it the building block of all living organisms.

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Why Study Organic Chemistry?
•  Since carbon is the building block of all living
organisms, a knowledge of Organic Chemistry is a prerequisite to understanding Biochemistry, Medicinal Chemistry, and Pharmacology.

•  Indeed, Organic Chemistry is a required course for studyingPharmacy, Medicine, and Dentistry.

•  Admission into these professional programs is highly dependent on your performance in Organic Chemistry.

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Examples of Organic Compounds Used as Drugs

Methotrexate, Anticancer Drug

5-Fluorouracil, Colon Cancer Drug

AZT, HIV Drug
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Tamiflu, Influenza Drug
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Examples ofOrganic Compounds Used as Drugs

Haldol, Antipsychotic Elavil, Antidepressant

Prozac, Antidepressant

Viagra, Treats Erectile Dysfunction
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The Structure of an Atom
•  An atom consists of electrons, positively charged protons, and neutral neutrons. •  Electrons form chemical bonds. •  Atomic number: numbers of protons in its nucleus •  Mass number: thesum of the protons and neutrons of an atom •  Isotopes have the same atomic number but different mass numbers. •  The atomic weight: the average weighted mass of its atoms •  Molecular weight: the sum of the atomic weights of all the atoms in the molecule
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The Distribution of Electrons in an Atom
•  Quantum mechanics uses the mathematical equation of wavemotions to characterize the motion of an electron around a nucleus. •  Wave functions or orbitals tell us the energy of the electron and the volume of space around the nucleus where an electron is most likely to be found. •  The atomic orbital closer to the nucleus has the lowest energy. •  Degenerate orbitals have the same energy.
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The ground-state electronic configuration describes the orbitals occupied by the atom’s electrons with the lowest energy

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The following principles determine which orbitals electrons occupy:
•  The Aufbau principle: an electron always goes to the available orbital with the lowest energy •  The Pauli exclusion principle: only two electrons canoccupy one atomic orbital and the two electrons have opposite spin •  Hund’s rule: electrons will occupy empty degenerated orbitals before pairing up in the same orbital
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Lewis’s theory: an atom will give up, accept, or share electrons in order to achieve a filled outer shell or an outer shell that contains eight electrons

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12Ionic Bonds Are Formed by the Transfer of Electrons

Attractive forces between opposite charges are called electrostatic attractions
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Covalent Bonds Are Formed by Sharing Electrons

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•  Equal sharing of electrons: nonpolar covalent bond (e.g., H2) •  Sharing of electrons...