electron configuration contd ms. mcgrath chemistry 11
DESCRIPTION
Pauli exclusion principle States that an orbital can be empty, have one electron, or at most have two electronsTRANSCRIPT
![Page 1: Electron Configuration contd MS. MCGRATH CHEMISTRY 11](https://reader035.vdocuments.net/reader035/viewer/2022062317/5a4d1b8c7f8b9ab0599bf29f/html5/thumbnails/1.jpg)
Electron Configurationcont’d
MS. MCGRATHCHEMISTRY 11
![Page 2: Electron Configuration contd MS. MCGRATH CHEMISTRY 11](https://reader035.vdocuments.net/reader035/viewer/2022062317/5a4d1b8c7f8b9ab0599bf29f/html5/thumbnails/2.jpg)
Aufbau principle• States that in going from a hydrogen atom to a larger atom, you add protons to the nucleus and electrons to orbitals
• You start at the orbitals having the lowest energy level and fill them, in order of increasing energy, until you run out of electrons
![Page 3: Electron Configuration contd MS. MCGRATH CHEMISTRY 11](https://reader035.vdocuments.net/reader035/viewer/2022062317/5a4d1b8c7f8b9ab0599bf29f/html5/thumbnails/3.jpg)
Pauli exclusion principle• States that an orbital can be empty, have one electron, or at most have two electrons
![Page 4: Electron Configuration contd MS. MCGRATH CHEMISTRY 11](https://reader035.vdocuments.net/reader035/viewer/2022062317/5a4d1b8c7f8b9ab0599bf29f/html5/thumbnails/4.jpg)
Hund’s rule• States that electrons in the same sublevel will not pair up (occupy the same orbital) until all the orbitals in the sublevel have been at least half filled
![Page 5: Electron Configuration contd MS. MCGRATH CHEMISTRY 11](https://reader035.vdocuments.net/reader035/viewer/2022062317/5a4d1b8c7f8b9ab0599bf29f/html5/thumbnails/5.jpg)
Electron configurations•The lanthanides are the 14 elements removed from period 6 of the periodic table• The actinides are the 14 elements removed from period 7 of the periodic table
• The above two groups do have unique electron configurations
![Page 6: Electron Configuration contd MS. MCGRATH CHEMISTRY 11](https://reader035.vdocuments.net/reader035/viewer/2022062317/5a4d1b8c7f8b9ab0599bf29f/html5/thumbnails/6.jpg)
Electronic configuration - Lanthanides
Lanthanum, atomic number 57: 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s2 4d10 5p6 6s2 5d1
or shorthand notation:[Xe]6s2 5d1
![Page 7: Electron Configuration contd MS. MCGRATH CHEMISTRY 11](https://reader035.vdocuments.net/reader035/viewer/2022062317/5a4d1b8c7f8b9ab0599bf29f/html5/thumbnails/7.jpg)
Electronic configuration - Lanthanides
Erbium, atomic number 68: 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s2 4d10 5p6 6s2 5d1 4f11
or shorthand notation:[Xe]6s2 5d1 4f11
![Page 8: Electron Configuration contd MS. MCGRATH CHEMISTRY 11](https://reader035.vdocuments.net/reader035/viewer/2022062317/5a4d1b8c7f8b9ab0599bf29f/html5/thumbnails/8.jpg)
Electronic configuration - Lanthanides
Hafium, atomic number 72: 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s2 4d10 5p6 6s2 5d1 4f14 5d1
or shorthand notation:[Xe]6s2 5d1 4f14 5d1
![Page 9: Electron Configuration contd MS. MCGRATH CHEMISTRY 11](https://reader035.vdocuments.net/reader035/viewer/2022062317/5a4d1b8c7f8b9ab0599bf29f/html5/thumbnails/9.jpg)
Electronic configuration - Lanthanides
Note: We place one electron in 5d then we fill up 4f with fourteen electrons then return to 5d and place the remaining nine electrons
![Page 10: Electron Configuration contd MS. MCGRATH CHEMISTRY 11](https://reader035.vdocuments.net/reader035/viewer/2022062317/5a4d1b8c7f8b9ab0599bf29f/html5/thumbnails/10.jpg)
Electron configuration - Actinides
Now you try: Radium, atomic number 88 Uranium, atomic number 92 Rutherfordium, atomic number 104
![Page 11: Electron Configuration contd MS. MCGRATH CHEMISTRY 11](https://reader035.vdocuments.net/reader035/viewer/2022062317/5a4d1b8c7f8b9ab0599bf29f/html5/thumbnails/11.jpg)
Electron configuration - Actinides
Radium, atomic number 88: 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s2 4d10 5p6 6s2 5d1 4f14 5d9 6p6 7s2
or shorthand notation: [Rn]7s2
![Page 12: Electron Configuration contd MS. MCGRATH CHEMISTRY 11](https://reader035.vdocuments.net/reader035/viewer/2022062317/5a4d1b8c7f8b9ab0599bf29f/html5/thumbnails/12.jpg)
Electron configuration - Actinides
Uranium, atomic number 92: 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s2 4d10 5p6 6s2 5d1 4f14 5d9 6p6 7s2 6d1 5f3
or shorthand notation: [Rn]7s2 6d1 5f3
![Page 13: Electron Configuration contd MS. MCGRATH CHEMISTRY 11](https://reader035.vdocuments.net/reader035/viewer/2022062317/5a4d1b8c7f8b9ab0599bf29f/html5/thumbnails/13.jpg)
Electron configuration - Actinides
Rutherfordium, atomic 104: 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s2 4d10 5p6 6s2 5d1 4f14 5d9 6p6 7s2 6d1 5f14 6d1
or shorthand notation: [Rn]7s2 6d1 5f14 6d1
![Page 14: Electron Configuration contd MS. MCGRATH CHEMISTRY 11](https://reader035.vdocuments.net/reader035/viewer/2022062317/5a4d1b8c7f8b9ab0599bf29f/html5/thumbnails/14.jpg)
Electron configuration - Actinides
Note: We place one electron in 6d then we fill up 5f with fourteen electrons then return to 6d and place the remaining nine electrons
![Page 15: Electron Configuration contd MS. MCGRATH CHEMISTRY 11](https://reader035.vdocuments.net/reader035/viewer/2022062317/5a4d1b8c7f8b9ab0599bf29f/html5/thumbnails/15.jpg)
Electron configuration - exceptionsChromium and Copper
See video and make notes
![Page 16: Electron Configuration contd MS. MCGRATH CHEMISTRY 11](https://reader035.vdocuments.net/reader035/viewer/2022062317/5a4d1b8c7f8b9ab0599bf29f/html5/thumbnails/16.jpg)
Electron configuration for ions Watch video and copy notes
![Page 17: Electron Configuration contd MS. MCGRATH CHEMISTRY 11](https://reader035.vdocuments.net/reader035/viewer/2022062317/5a4d1b8c7f8b9ab0599bf29f/html5/thumbnails/17.jpg)
Electron configuration for ions Practice