Chapter 07 Notes

Chapter 07 Notes - Chapter 7 Quantum Theory and the...

Info iconThis preview shows pages 1–3. Sign up to view the full content.

View Full Document Right Arrow Icon
Chapter 7 Quantum Theory and the Electronic Structure of Atoms I. From Classical Physics to Quantum Theory A. Properties of waves 1. Wave- vibrating disturbance which energy is transmitted 2. Wavelength- distance between identical points on successive wavelengths 3. Frequency- number of waves that pass through a particular point in one second 4. Amplitude- vertical distance from the midline of the wave to peak/trough 5. μ =  v λ a. = w λ avelength = meters b. v = frequency = Hz (1 Hz = 1 cycle/s) c. μ = speed B. Electromagnetic Radiation 1. An electromagnetic wave has an electrical field component and a magnetic field  component a. Same wavelength and frequency b. Travel in perpendicular planes 2. Travel 3 x 10 8  meters/second a. This is called the speed of light (c) 3. Visible Light a. Violet =  shortest wavelength b. Infared = longest wavelength C. Planck’s Quantum Theory 1. Atoms and molecules can emit/absorb energy I n discrete amounts 2. Quantum- smallest unit of energy that can be emitted/absorbed in the form of  electromagnetic radiation 3. E = hv or E = hc/  λ a. E = energy b. h = Planck’s constant = 6.63 x 10 -34  Js c. v = frequency II. Photoelectric Effect (Einstein) A. Says that electrons are ejected from the surface of certain metals exposed to light of at  least a minimum frequency (threshold frequency) 1. Number of electrons ejected is proportional to intensity or brightness of the light B. Photon- particle of light C. So electrons are bound to metals until a certain frequency is reached (binding energy).  Any more energy after that is kinetic energy. 1. The higher the frequency, the higher the energy
Background image of page 1

Info iconThis preview has intentionally blurred sections. Sign up to view the full version.

View Full DocumentRight Arrow Icon
III. Bohr’s theory of the hydrogen atom A. Emission Spectra 1. Continuous/line spectra of radiation emitted by substances 2. If you want to see it you need to energize a sample of material either with thermal  energy or some other form of energy 3. Every element has a unique emission spectrum a. The lines in the emission spectrum may be used to identify unknown atoms B. Emission Spectra of Hydrogen Atom 1. Bohr’s model of the atom included the idea of electrons moving in circular orbits.  But 
Background image of page 2
Image of page 3
This is the end of the preview. Sign up to access the rest of the document.

This note was uploaded on 04/07/2008 for the course CHEM 184 taught by Professor Hierl during the Fall '07 term at Kansas.

Page1 / 5

Chapter 07 Notes - Chapter 7 Quantum Theory and the...

This preview shows document pages 1 - 3. Sign up to view the full document.

View Full Document Right Arrow Icon
Ask a homework question - tutors are online