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Understanding the Octet Rule and Molecular Polarity

This guide covers the Octet Rule, explaining the fulfillment of electron configurations in different elements, including exceptions such as hydrogen and helium. It details the dot diagrams for common molecules like CH4, O2, and NH3, focusing on the arrangement of atoms and their bonding properties. The distinction between polar and nonpolar molecules is explored, including interactions such as dipole-dipole forces, hydrogen bonding, and Van der Waals forces. The text aims to clarify molecular shapes and the factors influencing molecular polarity.

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Understanding the Octet Rule and Molecular Polarity

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Presentation Transcript

  1. Warm Up:

  2. Octet Rule • a filled layer contains 8 electrons • Exceptions (After bonding…) • H and He will have 2 • Beryllium will have 4 • Boron will have 6 • Some transition metals can have more than 8

  3. Dot Diagrams for Molecules • Atom with most unshared electrons goes in middle *capable of forming most bonds* • Count to make sure you have the right number of electrons • Each atom wants to have a full valence • Try these… • CH4 O2 CO2 • NH3 N2 H2O

  4. Domains

  5. Write the shapes of each of the dot diagrams you made before

  6. Warm Up: Label the following bonds as polar and nonpolar. • Br2 • HCl • H2 • CH4 • NH3

  7. Molecular Polarity

  8. Dipole • Molecule with an overall unequal distribution of electrons

  9. Two atom molecules • If the bond is non-polar, so is the molecule • If the bond is polar, the molecule has a dipole and is polar

  10. Do these molecules have dipoles? • N2 • O2 • CO • HF

  11. Three atom molecules • If the 2 polar effects are equal and oppositely directed, the molecule is nonpolar • Otherwise, the molecule is polar water Carbon dioxide

  12. Four atom molecules • It is possible that the 3 polar effects may cancel and produce a nonpolar molecule • It is also possible that they don’t cancel and produce a polar molecule NH3 (ammonia) Exception to octet rule

  13. Five atom molecules • It is possible that the 4 polar effects may cancel and produce a nonpolar molecule • It is also possible that they don’t cancel and produce a polar molecule CH4 CH3Cl

  14. Intermolecular Forces • Between molecules • Dipole-dipole • Hydrogen bonding • Van der Waals

  15. Dipole-Dipole • Like electrical charges and magnets, dipoles can attract one another • Stronger attractions with stronger dipoles • Stronger attractions when molecules are closer together with lower temperature and higher pressure

  16. Hydrogen Bonding • Occurs when Hydrogen and Fluorine, Oxygen, or Nitrogen are present • FON • Ammonia, hydroflouric acid, water • Higher boiling points with hydrogen bonding

  17. Van der waals • Recall that electrons have a little bit of freedom to move around their electron clouds • VDW are produced by momentary uneven electron distributions • Extremely weak • Responsible for bonding of nonpolar molecules, liquefaction of inert gases, 3 phases of halogens at STP • Stronger for molecules with more electrons • Gets stronger as molecules get closer

  18. bromine

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