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Chemistry Notes

Chemistry Notes. Covalent Bonding Diagrams. An Addendum to Lewis Structures. Carbon and silicon are exceptions to the pattern of how to place electrons in a Lewis Dot Structure. An Addendum to Lewis Structures.

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Chemistry Notes

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  1. Chemistry Notes Covalent Bonding Diagrams

  2. An Addendum to Lewis Structures • Carbon and silicon are exceptions to the pattern of how to place electrons in a Lewis Dot Structure.

  3. An Addendum to Lewis Structures • This is because they have hybrid orbitals (where the s and p sublevels blend together and have four equal energy orbitals.)

  4. Covalent Bonding • A covalent bond occurs between two non-metals • Electrostatic bonding does not occur—in other words, there is no “give and take” of electrons

  5. It ends up being a “tug of war” of electrons Where the electrons end up somewhere in the middle.

  6. Single Bonds • A single bond occurs when one pair of electrons is shared by two atoms. • This pair of bonded electrons is called a shared pair.

  7. Double and Triple Bonds • Double bonds occur when two atoms have two shared pair of electrons • Triple bonds occur when two atoms share three pair of electrons

  8. Covalent Bonding Diagrams • Like the ionic bonding diagrams, first draw the dot diagram for each element • Now, however, the electrons are not being given away or taken, but shared; so signify a pair being shared by circling both electrons.

  9. Covalent Bonding Diagrams • Every element should have eight electrons (count each shared pair as two). • If there is more than one of each element in the compound, you have to have a central atom.

  10. Covalent Bonding Diagrams • The center atom will be the one with the most spots to bond to.

  11. Hydrogen • Since hydrogen is in the first energy level, it will not need 8 valence electrons to be stable—it will only need 2.

  12. H2

  13. H2O

  14. Cl2

  15. O2

  16. N2

  17. CCl4

  18. CO2

  19. HCN

  20. PCl3

  21. H2O2

  22. C2H4

  23. CSF2

  24. CO

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