Quantum+Numbers

A quantum is the smallest increment of radiant energy that can be absorbed or emitted. The magnitude of radiant energy is represented as hv, where h equals Planck's constant, 6.63 x 10^-34 J/s and v equals frequency.


 * Principal Quantum Number(n):** The principle quantum number can be positive numbers up to infinity (1,2,3,4,5, etc) The larger the number the farther away the electron is away from the nucleus. Electrons with a larger n value have more energy and is not as close to the nucleus of the atom.

__l=0 - S Orbital "Spheres"__ concise.britannica.com __l=1 - P Orbital "Peanuts"__ chimge.unil.ch __l=2 - D Orbital "Dutterflies"__ www.geo.arizona.edu __l=3 - F Orbital "Freaks"__ www.bytocom.com (This is only one of the many f orbitals.)
 * Azimuthal Quantum Number(l):** The azimuthal quantum number is can have a value of 0 to n-1. This number determines the shape of the orbital. Each value represents a certain type of orbital, the orbital shapes and l designation are listed below.
 * Magnetic Quantum Number(ml):** The magnetic quantum number can have a whole number value between l and -l, including 0. This number represents the orientation of the orbital in space.


 * Spin Magnetic Quantum Number(ms):** This number represents the spin of the electrons. The only values that it can be are +1/2 and -1/2. Electrons in the same orbital can not have the same spin, they must have opposite spins. Otto Stern and Walter Gerlach were able to determine in 1921 that there are only 2 ways that electrons can spin. They sent a beam of neutral atoms through a inhomogeneuos magnetic field. The magnetic field altered the course of the atoms by acting on the electrons' spin. The beam was split in 2 showing that there are only 2 spin orientations.


 * Pauli Exclusion Principle:** This principle states that no 2 electrons can have the same set of 4 quantum numbers. It was this principle that led to the discovery of the spin magnetic number.

Edited by Rob and the big hand. Source: Chemistry The Central Science Ninth Edition. By Brown LeMay and Bursten.