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Understanding Lewis Dot Formulas: Valence Electrons, Rules, and Ion Formation

Explore how Lewis dot structures work, representing valence electrons and following specific rules for creating ions. Learn the dot order, guess elements, and understand the octet rule.

austin-wilson
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Understanding Lewis Dot Formulas: Valence Electrons, Rules, and Ion Formation

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  1. ELECTRON DOT FORMULAS—HOW DO THEY WORK? (also known as Lewis dot structures)

  2. THE “DOT” • 1) Represents an electron • 2) Specifically valence electrons (electrons in the outermost shell)

  3. #1. Cs C I

  4. #2. S Ca B Guess: #3 Sr Cl Xe

  5. Guess: #4. O Ba N Guess: #5 Kr Mg P

  6. What are the rules? • 1) Number of dots = last digit of group # • 2) Order of dots: • 3) Why this order?  first 2 are “s” electrons; next 6 are “p” electrons: 2 1 X 3 8 6 5 7 4

  7. Guess: #6. F Al Si Guess: #7 Ar Be Na

  8. - 2- - OK, so you think you have it?Try these: Guess#8 Cl- Br- S2- Cl Br S

  9. 2- 3- Just one more: Guess #9 O2- N3- Si4+ 4+ O N Si

  10. What are the rules for ions? • 1) Add or subtract the appropriate number of electrons • 2) Place brackets around the Lewis dot structure • 3) Write ion’s charge to the upper right hand corner

  11. Octet Rule • Notice there’s a trend for forming ions • The octet rule states that atoms will form ions by gaining or losing electrons so they will have a “full” valence shell of 8 (an “octet” of) electrons just like a noble gas • Exception: The duet rule is for hydrogen and helium—they obtain a full shell of 2 (a duet of) electrons

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