Quantum Mechanics 2

Formula of Energy of a Photon

E photon=hc/lamda

Ψ or Psi

Energy state of an atom

Forms of Waves

Gamma Rays > X-Rays > Ultra-Violet > Visible > Infrared >Microwaves > Radio/TV waves / (Listed Shortest to Longes and strongest to weakest) The longer the wave the lower the frequency

Energy Level Trend/Increase

Increase from s ->f

Ground State

Lowest energy level

ml

Magnetic Quantum Number Values: [-l...0...l] Each value describes an allowed orientation of an orbital

How man electrons are allowed per level, n?

Max electrons per level = 2xn^2

Louis de Broglie

Proposed dual wave/particle nature for the electrons in Bohr's stationary states. lamda = h/mv (m is mass and v is velocity) or P = h/lamda. The wave description of the electron was quantized in that the wavelength must fit in the circumference of the Bohr radius.

Schroedinger

Used the work of Bohr and de Broglie to propose that the electron was represented as a wave that filled three dimensional space. The result was "Wave Mechanics," which proposed that electrons were distributed around the nucleus in probability regions called orbitals. To locate an electron four quantum numbers are needed.

Orbital

a three dimensional region of space where the probability of finding an electron is 90%. It is not possible to locate the exact position of an electron.

Mechanical Wave

a vibrating disturbance in a medium by which energy is transferred

Electromagnetic Wave

a wave that does not need a medium to transfer energy

Node

each place where the wave intersects the level where the wave is neutral

Amplitude

the distance between neutral level and the crest

Aufbau Principle

the ground state electron configurations for many electron atoms can be approximated by using the excited states of hydrogen. For all electrons with more than one electron, the presence of electron-electron interactions changes the energy of the hydrogenic orbitals. They are no longer degenerate.

Crest

the highest peak of a wave

Trough

the lowest peak of a wave

Wave

the transmition of energy from one place to another without transmitting matter

Pauli Exclusion Principle

"No two electrons in the same atom can have the same four quantum numbers."

Hund's Rule

"the most stable arrangement of electrons in a subshell is the one with the greatest number of parallel spins."

Formula for # of Photons

#Photons = E burst/E photon

Frequency

(V or nu or f) the number of waves per unit of time

Wavelength

(lambda) the length of a wave measured crest to crest of trough to trough

Max Planck

1900 / introduces the idea of quantization of energy to solve problems with Blackbody radiation, but had not experimental verification (Fudge Factor). The father of modern Quantum Mechanics, who proposed that the classical physical laws did not apply on an atomic level. 1 <Energy is directly proportional to Frequency> 2 <Energy is quantized and not continuously absorbed or emitted>

Albert Einstein

1905 / uses Planck's idea to explain the photoelectric effect with scientific data. When he graphed data on the photoelectric effect it resulted in the appearance of "Planck's constant," proving light is quantized. Einstein also discovered concluded from the data that Plank's assumptions were correct.

Neils Bohr

1913 / developed the first quantized model of the atom that can be used to explain the hydrogen atom electron model. The model, however, still used the planetary system.

Formula for Momentum of Photon

P = h/lamda or lamda = h/mv

Heisenberg

Pioneered "Matrix Mechanics", an approach to determining the location of an electron. Said one could not determine the exact speed and location of an electron simultaneusly

ms

Spin Quantum Number Values: +1/2, -1/2 Describes the magnetic spin energy of an electron

l

The Angular Momentum Quantum Number Values: [0...(n-1)] Practical Max = 3 Describes the shape of an Orbital

n

The Principle Quantum Number Values: [1,2,3,...,7] Represents energy level / In the H atom the energy is only dependent on n - Describes Sublevel