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

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• 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