Bonding Types – ionic and covalentCovalent Bonding – equal/unequal sharing Bonding Model – Lewis Structures (withformal ch...
How compounds are held together:    covalent vs ionic bonding
Electronegativity:measure of attraction for electrons in a bond
EN and Bond Polarity Scale           Very slightly polar                 No sharing           (called nonpolar)           ...
Electronegativity Trends
Bond vs Molecular Polarity
Lewis Structures: model to describe  bonding in covalent molecules- Valence electrons represented by dots- Bonding pair re...
Formal Charge: way of keeping track* of   where charge is within a molecule Electrons that contribute to atom’s charge: 1....
Resonance (when 1 Lewis structure    doesn’t tell the story well)
Resonance “rules of thumb”• Must be valid Lewis structure• Move electrons, not nuclei• Number of unpaired electrons (if an...
Comparing Resonance Structures• As many octets as possible• As many bonds as possible• Any negative charges on electronega...
Common Bonding Patterns
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Ch1 a

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Ch1 a

  1. 1. Bonding Types – ionic and covalentCovalent Bonding – equal/unequal sharing Bonding Model – Lewis Structures (withformal charge and resonance structures)
  2. 2. How compounds are held together: covalent vs ionic bonding
  3. 3. Electronegativity:measure of attraction for electrons in a bond
  4. 4. EN and Bond Polarity Scale Very slightly polar No sharing (called nonpolar) (Ionic bond)Nonpolar Polar 0 0.4 1.9 Electronegativity Difference
  5. 5. Electronegativity Trends
  6. 6. Bond vs Molecular Polarity
  7. 7. Lewis Structures: model to describe bonding in covalent molecules- Valence electrons represented by dots- Bonding pair represented by line- Valence e- so 2 for H and 8 for 2nd row elements
  8. 8. Formal Charge: way of keeping track* of where charge is within a molecule Electrons that contribute to atom’s charge: 1. All of unshared electrons 2. Half of shared electronsFC = group number – nonbonding e- – ½ shared e-
  9. 9. Resonance (when 1 Lewis structure doesn’t tell the story well)
  10. 10. Resonance “rules of thumb”• Must be valid Lewis structure• Move electrons, not nuclei• Number of unpaired electrons (if any) remain the same• Major contributor has lowest energy (see other rules)• Resonance – most important when charge is delocalized
  11. 11. Comparing Resonance Structures• As many octets as possible• As many bonds as possible• Any negative charges on electronegative atoms• As little charge separation as possible
  12. 12. Common Bonding Patterns
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