1 / 17

Electromagnetic Radiation

Electromagnetic Radiation. Silberberg fig 7.3. Electromagnetic Radiation. Wavelength,  , lambda The distance between two adjacent identical points of the wave. Frequency,  , nu The number of wave crests passing a given point per unit time. Blackman fig 4.1. Electromagnetic Radiation.

andrew-barry
Download Presentation

Electromagnetic Radiation

An Image/Link below is provided (as is) to download presentation Download Policy: Content on the Website is provided to you AS IS for your information and personal use and may not be sold / licensed / shared on other websites without getting consent from its author. Content is provided to you AS IS for your information and personal use only. Download presentation by click this link. While downloading, if for some reason you are not able to download a presentation, the publisher may have deleted the file from their server. During download, if you can't get a presentation, the file might be deleted by the publisher.

E N D

Presentation Transcript

  1. Electromagnetic Radiation Silberberg fig 7.3

  2. Electromagnetic Radiation Wavelength, , lambda The distance between two adjacent identical points of the wave. Frequency, , nu • The number of wave crests passing a given point per unit time. Blackman fig 4.1

  3. Electromagnetic Radiation • All light waves travel at exactly the same speed (in a vacuum) – the speed of light, c, is a constant. C= 2.998  108 ms-1 • Wavelength and frequency are related to the speed of light. • c = 

  4. Electromagnetic Radiation • All radiation may have the same speed but the energy can vary. • The higher the frequency, the more rapidly the wave is oscillating and the higher the energy. • Energy = Planck’s constant  frequency • E = hh = 6.626 x 10-34Js

  5. Large wavelength Low frequency Low energy Short wavelength High frequency High energy EM Radiation - colour

  6. Atomic Spectra • When an atom is supplied with energy (eg heat, electric current) it emits electromagnetic radiation of a relatively few, fixed frequencies that are characteristic of that element – this is the atomic emission spectrum.

  7. Atomic Spectra Light emitted from a hydrogen lamp has only a few lines. • Only light of certain energies is emitted. • The pattern of lines is unique to hydrogen. • Suggests the process of emitting light from the atom is quantised (comes in discrete amounts).

  8. Atomic Spectra Our eye sees the combination of wavelengths: Pass the light through a prism to see the lines: commons.wikimedia.org/wiki/File:Flametest--Cu.swn.jpg commons.wikimedia.org/wiki/File:Flametest--Na.swn.jpg commons.wikimedia.org/wiki/File:Flametest-Co-.swn.jpg Co Cu Na Co Cu Na http://chemistry.bd.psu.edu/jircitano/periodic4.html

  9. The Bohr Model Niels Bohr • Electrons in atoms can only occupy certain energy levels (orbits). • When an electron moves from one energy level to another, energy is absorbed or emitted. • This energy corresponds to light of a specific energy/frequency. commons.wikimedia.org/wiki/File:Niels_Bohr.jpg

  10. The Bohr Model - Postulates Silberberg Fig 7.11

  11. The Bohr Model • The number of electrons that can pack into an orbit depends on the size of the orbit.

  12. Electron Structures • Neutral atoms always have the same number of electrons as the number of protons in the nucleus. Helium Z = 2 2 electrons Hydrogen Z = 1 1 electron Lithium Z = 3 3 electrons

  13. ‘Ground State’ Electron Structures 20+

  14. Electron Structures Group:no of electrons in outer shell/orbit Period: no of electron shells/orbits containing electrons

  15. Learning Outcomes: By the end of this lecture, you should: appreciate the relationship between frequency, wavelength and energy know that the speed of light (in a vacuum) is constant know that the Bohr model of an atom limits electrons to orbits of certain energies recognise the energy of light emitted from an atom represents the energy difference between two orbits know the maximum number of electrons the first, second and third shell can accommodate (2, 8, 18) recognise the connection between an atom’s electron configuration and its position in the periodic table be able to complete the worksheet (if you haven’t already done so…)

  16. Questions to complete for next lecture: • Which light: red or blue, has (a) the higher frequency, (b) the longer wavelength, (c) the faster speed and (d) the greater energy? • What is the colour of the light emitted by a ‘sodium street light’? • If the electron of a hydrogen atom moves from the first (n = 1) to the third (n = 3) orbit, will energy be absorbed or released from the surroundings? • What is the maximum number of electrons that can fit in the second (n = 2) orbit? • A vertical column in the Periodic Table is called a……….. and a horizontal row is called a…………..

  17. Questions to complete for next lecture: • How many electrons are in the outermost orbit of a ‘ground state’ magnesium atom? • What element is in Group 16 and the third period? How many electrons are in its third orbit? • Which element has two completely filled electron shells and just three electrons in the third shell? • Draw a diagram showing the electron structure of a K atom.

More Related