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Electron Dot Structures

Electron Dot Structures. Lewis Structures. - Diagrams that show the bonding between atoms of a molecule, and the lone pairs of electrons that may exist in the molecule. - Introduced by Gilbert Lewis in 1916. Drawing Lewis Structures for Covalent Compounds. Let’s try SiH 4 (silane).

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Electron Dot Structures

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  1. Electron Dot Structures

  2. Lewis Structures - Diagrams that show the bonding between atoms of a molecule, and the lone pairs of electrons that may exist in the molecule. - Introduced by Gilbert Lewis in 1916.

  3. Drawing Lewis Structures for Covalent Compounds Let’s try SiH4 (silane) 1) First count all the valence electrons 2) Decide which atom will be your central atom -Carbon is always in the center -Hydrogen is never in the center -If no carbon, least electronegative element is placed in center 3) Decide which atom will be your central atom and then connect the atoms by electron-pair bonds 4) Make sure all H’s have two electrons and all other nonmetals satisfy the “Octet Rule” 5) Make sure your final structure has same number of electrons as you had in step 1

  4. Electron-dot formula for Methane (CH4) H H C H H Here is a Carbon atom (4 val e-’s) and four Hydrogen atoms (1 val e- each)

  5. Electron-dot formula for Methane (CH4) H Now they have formed a stable molecule. Each C atom “feels” like it has a stable octet. H C H Each H atom “feels” like a stable “He” atom with 2e-s H

  6. Electron-dot formula for Ammonia (NH3) H N H Here is a Nitrogen atom (5 val e-’s) and three Hydrogen atoms (1 val e- each) H

  7. Electron-dot formula for Ammonia (NH3) “N” now feels like it has a stable octet Each “H” feels like it has 2 e- like Helium. N H H H

  8. F F C F F Write the electron-dot formula for CF4 Because “F” is a halogen, it has 7 valence e-s, so you must show all 7 red dots around each “F” atom!

  9. Se F F Write the Electron-Dot Formula for SeF2 Because “F” is in Group 17, they have 7 valence e-s, so they must have 7 red dots around them.

  10. Formaldehyde CH2O Some elements, especially C, N, and O can share more than one pair of electrons!! Two pairs of electrons shared = double bond Three pairs of electrons shared = triple bond

  11. Resonance StructuresOzone, O3 Resonance - Bonding in molecules cannot be correctly represented by a single Lewis structure Actual structure of ozone is an average of these two structures

  12. Benzene: Classic Case of Resonance kekule's dream

  13. Yes, we can see molecules!

  14. Bond Energy vs Bond Length

  15. Bond Energy vs Bond Length

  16. Bond Energy vs Bond Length

  17. Ionic Structure Calcium Sulfide

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