University:
Eastern Kentucky University
Course:
CHE 361 | Organic Chemistry I
Academic year:

2020
Views:

359

Pages:

1
Author:

emplanasf3fe

Organic Chemistry 3: Bondin Atomic Orbitals & Quantum Numbers Hybridization Quantum Numbers: Describe the size, shape, orientation, and number of atomic orbitals in an element sp3: 25% s character and 75% p character Tetrahedral geometry with 109.5° bond angles Quantum Number sp2: 33% s character and 67% p character Trigonal planar geometry with 120° bond angles Name What it Labels n Principal e- energy level or shell number l Azimuthal 3D shape of orbital ml Magnetic Orbital sub-type ms Spin Electron spin Possible Values Notes 1, 2, 3, … Except for d-orbitals, the shell # matches the row of the periodic table 0, 1, 2, …, n-1 0 = s orbital 1 = p orbital 2 = d orbital 3 = f orbital 4 = g orbital Integers –l ® +l " " + #$, − # Maximum e- in terms of n = 2n2 Maximum e- in subshell = 4l + 2 Molecular Orbitals Bonding Orbitals: Created by head-to-head or tail-to-tail overlap of atomic orbitals of the same sign. ¯energy "stable Antibonding Orbitals: Created by head-to-head or tail-to-tail overlap of atomic orbitals of opposite signs. "energy ¯stable Single Bonds: 1 s bond, contains 2 electrons Double Bonds: 1 s + 1 p Pi bonds are created by sharing of electrons between two unhybridized p-orbitals that align side-by-side Triple Bonds: 1 s + 2 p Multiple bonds are less flexible than single bonds because rotation is not permitted in the presence of a p bond. Multiple bonds are shorter and stronger than single bonds, although individual p are weaker than s bonds sp: 50% s character and 50% p character Linear geometry with 180° bond angles Resonance: Describes the delocalization of electrons in molecules that have conjugated bonds Conjugation: Occurs when single and multiple bonds alternate, creating a system of unhybridized p orbitals down the backbone of the molecule through which p electrons can delocalize