1. Atomic Orbitals: A Quantum Mechanical Description of Electrons around the Nucleus 1-6 The electron is described by wave equations. An electron within an atom can have only certain definite energies called energy states. Moving particles such as electrons exhibit a wavelength determined by the de Broglie relation: Where h is Plank’s constant, m is the mass of the electron in kg, and v is the velocity of the electron in m/s.

2. The electron waves contain nodes, where the amplitude of the wave changes sign, and can interact with each other, producing either constructive or destructive interference:

3. Atomic orbitals have characteristic shapes. In an artists rendition of an atomic orbital, a surface is drawn which contains most of the probability of finding the electron at a given time. Nodes in the a function become points or planes of 0 probability of finding the electron. Higher energy wave functions have more nodes than do lower energy wave functions. The simplest atomic orbitals are spherical in shape and are called s orbitals. The lowest energy s orbital is the 1s orbital.

4. The next highest energy orbital is the 2s orbital. Note that it contains a spherical nodal surface. Of slightly higher energy than the 2s orbital are 3 degenerate 2p orbitals. These orbitals are shaped like a figure 8 and point along the 3 Cartesian axes.

5. 1.Lower energy orbitals are filled before those with higher energy (Aufbau Principle). 2.No orbital may be occupied by more than two electrons. (Pauli Exclusion Principle). If two electrons occupy a single orbital, they must have opposite spins. Electrons of opposite spins in the same orbital are called paired electrons. 3.Degenerate orbitals must each receive a single electron of the same spin before pairing of electrons occurs. (Hund’s rule) Following the 1s, 2s, and 2p orbitals are the 3s, 3p, 4s, 3d, etc. orbitals. Organic chemistry deals primarily with the lower s and p orbitals.

7. Molecular Orbitals: and Covalent Bonding 1-7 The bond in the hydrogen molecule is formed by the overlap of 1s atomic orbitals. Atomic orbitals on different atoms may overlap. The overlap of electron waves represented by the atomic orbitals may result in constructive (in phase) or destructive (out of phase) interference. In phase overlap between two 1s orbitals results in a new orbital having lower energy than either of the s orbitals. This new orbital concentrates the electron probability between the two nuclei. Out of phase overlap between two 1s orbitals results in a new orbital having higher energy than either of the s orbitals. This new orbital places most of the electron probability to the left and right of the two nuclei.