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A step-by-step guide on how to draw orbital diagrams and determine electron configurations for various elements, including Fluorine, Silicon, Strontium, Protactinium, Chromium, and Copper. Learn about the significance of full and half-filled sublevels and how certain elements 'steal' electrons from neighboring 's' orbitals to achieve stability.
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2
2
5 Orbital Diagram Electron configuration
determine the element
2
atomic number
to be completely filled 8 16
8 electrons 2s 2 2p 4
tables to find the atomic numbers and the electron configurations of the following elements:
2 2s 2 2p 6 3s 2 3p 2
2 2s 2 2p 6 3s 2 3p 6 4s 2 3d 10 4p 6 5s 2
2 2s 2 2p 6 3s 2 3p 6 4s 2 3d 10 4p 6 5s 2 4d 10 5p 6 6s 2 4f 14 5d 10 6p 6 7s 2 5f 3
are more stable, if they have:
s 2 , p 6 , d 10 and f 14
s 1 , p 3 , d 5 and f 7
ending with a full or half filled orbital it will “steal” an e
configuration for Cr
1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 3d 4
1s 2 2s 2 2p 6 3s 2 3p 6 4s 1 3d 5
half-filled orbitals…a happier Cr
4 or d 9
from
closest “s” orbital to be more stable