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Electron Configurations & Orbital Diagrams: Fluorine, Silicon, Strontium, Protactinium, Ch, Summaries of Chemistry

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.

Typology: Summaries

2021/2022

Uploaded on 09/27/2022

wilbur
wilbur 🇺🇸

212 documents

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Download Electron Configurations & Orbital Diagrams: Fluorine, Silicon, Strontium, Protactinium, Ch and more Summaries Chemistry in PDF only on Docsity!

  • Electron configurations are written in one line
  • Arrows in orbital diagrams become exponents
  • Draw the orbital diagram for Fluorine 1s 2s 2p

1s

2

2s

2

2p

5 Orbital Diagram Electron configuration

  • Counting up all superscripts (exponents) would tell you the total amount of electrons

▪ Using this we can

determine the element

Example: Oxygen

1s

2s 2p

3s 3p 3d

4s 4p 4d 4f

5s 5p 5d 5f

6s 6p 6d 6f

7s 7p 7d 7f

• 1s

2

• 2 electrons

• 4 electrons

• Total 8 electrons

• Stop once the # e- = the

atomic number

• Last sublevel doesn’t have

to be completely filled 8 16

O

8 electrons 2s 2 2p 4

• Use your periodic

tables to find the atomic numbers and the electron configurations of the following elements:

▪ Silicon

▪ Strontium

▪ Protactinium

• Silicon

▪ 1s

2 2s 2 2p 6 3s 2 3p 2

• Strontium

▪ 1s

2 2s 2 2p 6 3s 2 3p 6 4s 2 3d 10 4p 6 5s 2

• Protactinium

▪ 1s

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

• In some cases orbitals

are more stable, if they have:

▪ Full sublevels:

s 2 , p 6 , d 10 and f 14

▪ Half-Full sublevels:

s 1 , p 3 , d 5 and f 7

• If an element is close to

ending with a full or half filled orbital it will “steal” an e

  • from the nearest “s” orbital

• Write the e

configuration for Cr

▪ Expect:

1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 3d 4

▪ Actual e- configuration:

1s 2 2s 2 2p 6 3s 2 3p 6 4s 1 3d 5

• This gives us two

half-filled orbitals…a happier Cr

  • Stealers

▪ End in d

4 or d 9

▪ Column 6 or 11 in PT

▪ Cr or Cu column

  • Will steal an e

     from 

closest “s” orbital to be more stable