Chapter8

Chapter8 - Chapter 8: Electron Congurations and the...

Info iconThis preview shows pages 1–16. Sign up to view the full content.

View Full Document Right Arrow Icon
Chem 6A Michael J. Sailor, UC San Diego Chapter 8: Electron Confgurations and the Periodic Table 1
Background image of page 1

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

View Full DocumentRight Arrow Icon
Chem 6A Michael J. Sailor, UC San Diego Fri, Oct 29 2
Background image of page 2
Chem 6A Michael J. Sailor, UC San Diego The Periodic Table of the Elements 3
Background image of page 3

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

View Full DocumentRight Arrow Icon
Chem 6A Michael J. Sailor, UC San Diego Electron Confgurations AuFbau ="Building up" As each proton is added to the nucleus, you add an electron to the hydrogen-like orbitals. Add to s, then d, then p orbitals oF the same principle quantum number 4
Background image of page 4
Chem 6A Michael J. Sailor, UC San Diego 5 Quantum numbers Quantum Number Called Describes n Principle quantum number SIZE and ENERGY l Angular momentum (Azimuthal) quantum number SHAPE m l Magnetic quantum number ORIENTATION m s Electron spin quantum number INTRINSIC ANGULAR MOMENTUM OF THE ELECTRON
Background image of page 5

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

View Full DocumentRight Arrow Icon
Chem 6A Michael J. Sailor, UC San Diego The Periodic Table of the Elements 6
Background image of page 6
Chem 6A Michael J. Sailor, UC San Diego The Periodic Table of the Elements 7 1s 2s 2p 3s 3p 4s 3d 4p 5s 4d 5p 6s 5d 6p 7s
Background image of page 7

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

View Full DocumentRight Arrow Icon
Chem 6A Michael J. Sailor, UC San Diego Electron Confgurations How to fll up orbitals with electrons? • Electrons go in lowest energy orbital frst, they spread over all the empty orbitals with the same spin, then they pair up. Pauli Exclusion Principle: No more than 2 electrons per orbital, must be oF opposite spin. Hund's rule: When there is more than one orbital with the same energy, fll up empty orbitals frst, keeping the spins the same. 8
Background image of page 8
Chem 6A Michael J. Sailor, UC San Diego 9 from T. Moeller “Inorganic Chemistry” Wiley 1952 Similar figure in your textbook The Building-up Principle (aufbau) Pauli exclusion principle: no more than 2 electrons in each orbital. Pairs of electrons in the same orbital must have opposite spins. Hund’s rule: When there is more than one orbital with the same energy (degenerate), Fll up empty orbitals with one electron before pairing the electrons, keep the spins the same.
Background image of page 9

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

View Full DocumentRight Arrow Icon
Chem 6A Michael J. Sailor, UC San Diego 10 Stern-Gerlach Experiment: This experiment tells us that each individual electron has a magnetic moment; there must be a 4th quantum number: Electron spin, or m s
Background image of page 10
Chem 6A Michael J. Sailor, UC San Diego Mon, Nov 1 11
Background image of page 11

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

View Full DocumentRight Arrow Icon
Chem 6A Michael J. Sailor, UC San Diego 0 10 20 30 40 50 60 70 80 F D C- C C+ B- B B+ A- A A+ Grade Projection Quizzes 1-6 Number of students
Background image of page 12
Chem 6A Michael J. Sailor, UC San Diego Electron Confgurations Example Electron confgurations: Potassium 1s 2 2s 2 2p 6 3s 2 3p 6 4s 1 shorthand: [Ar]4s 1 Vanadium [Ar]4s 2 3d 3 Selenium [Ar]4s 2 3d 10 4p 4 Note: (n+1)s orbitals always fll up beFore nd. 4F and 5d orbitals have similar energies, Lanthanides fll up 4F and 5d orbitals in somewhat random order. Don’t worry about lanthanides For now. 13
Background image of page 13

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

View Full DocumentRight Arrow Icon
Chem 6A Michael J. Sailor, UC San Diego Electron Confgurations 14
Background image of page 14
Chem 6A Michael J. Sailor, UC San Diego Electron Confgurations-Exceptions Exceptions: everything flls up normally, with a Few exceptions: Cr: [Ar]4s 1 3d 5 Why? halF-flled shells are unusually stable.
Background image of page 15

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

View Full DocumentRight Arrow Icon
Image of page 16
This is the end of the preview. Sign up to access the rest of the document.

This note was uploaded on 08/31/2011 for the course CHEM 6A taught by Professor Pomeroy during the Winter '08 term at UCSD.

Page1 / 56

Chapter8 - Chapter 8: Electron Congurations and the...

This preview shows document pages 1 - 16. Sign up to view the full document.

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