Download presentation

Presentation is loading. Please wait.

Published byWendy Knight Modified over 2 years ago

1
People, Experiments, Conclusions

2
Democritus – Ancient Greeks (5th century B.C.) believed in a small, indivisible particle – “atomos” Dalton – Modern theory (1803)– indivisible atom J.J. Thomson – Plum Pudding model (1897); Used Cathode Ray tube to experiment; Atoms have identical, removable (- ) charged particles. http://highered.mcgraw- hill.com/olcweb/cgi/pluginpop.cgi?it=swf::100%25::100%25 ::/sites/dl/free/0072512644/117354/01_Cathode_Ray_Tube.s wf::Cathode%20Ray%20Tube

3
Millikan (1909) – Oil Drop experiment to determine the charge on electron and mass of electron. Ernest Rutherford (1911) – Gold Foil Experiment – Discovered nucleus as dense (+) charged center. http://micro.magnet.fsu.edu/electromag/java/rutherford/ Niels Bohr (1913) – Electrons in orbit around the nucleus – based on work with Hydrogen. http://www.dlt.ncssm.edu/tiger/Flash/phase/ElectronOrbits. html

4
Erwin Schrodinger (1926) – Quantum theory – treats electrons as waves. Quantized energy levels. No exact “path” for electrons – just a probability of location for the electrons in an area. Electron Cloud – picture of probability Surface of cloud gives approximate shape and 90% chance of e - location (Fig 13.2 in text)

5
Quantum “numbers” - describe electrons Principal Quantum Numbers: n = 1, 2, 3, 4, 5 n = principal energy level Angular momentum Quantum Number In “English” – sublevel within each energy level. Each sublevel has a different shape. Current sublevels: s, p, d, f orbitals no g orbitals no g orbitals with g orbitals with g

6
Magnetic Quantum Number Deals with distribution inside the sublevel. Orientation along the axes. Spin Quantum Number - +1/2 or -1/2

7
Electron distribution Max # of e- in any given energy level is = 2n 2. (n=energy level) Level1234567 Max e-2818 Sublevels sss Availablepp d

8
Orbitals – areas within the sublevel where electrons can “hang out” Each orbital can hold 2 electrons Sublevel# of orbitals# e- s1 2 p3 6 d5 10 f7 14

9
Electron Configurations Sample: N = Say: one “s” two, two “s” two, two “p” three

10
More Examples - C – F – Li – Mg P

Similar presentations

OK

Brief History of Atomic Theory. 1 st atomic models In 400 BC, the model looked like a solid indivisible ball In 400 BC, the model looked like a solid.

Brief History of Atomic Theory. 1 st atomic models In 400 BC, the model looked like a solid indivisible ball In 400 BC, the model looked like a solid.

© 2017 SlidePlayer.com Inc.

All rights reserved.

Ads by Google

Microsoft office ppt online maker Ppt on power sharing in democracy who has the power Ppt on marketing management free download Ppt on world food day Ppt on resistance temperature detector manufacturers Ppt on old movies vs new movies Ppt on active magnetic bearing Ppt on causes of road accidents Ppt on conservation of plants and animals download Ppt on product specification document