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Covalent Compounds: Lewis Dot Structures

Learn about covalent compounds, writing Lewis dot structures, and how atoms aim to achieve the octet rule. Understand single, double, and triple bonds through examples like Carbon Tetrachloride and Ethylene Acetylene.

raphael-bernard
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Covalent Compounds: Lewis Dot Structures

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  1. Warm Up • Name the following compound • Cl02 • Give the following formula 2. Disilicon Hexafluoride 3. Carbon tetrachloride

  2. Covalent Compounds:Writing Lewis Dot Structures

  3. What are the atoms trying to achieve?Octet rule = atoms want 8 electrons in their valence shell Exception #1: Hydrogen and Helium only want 2

  4. . . H H : H H Covalent Bonding in H2 Two hydrogen atoms, each with 1 electron, can share those electrons in a covalent bond. • Sharing the electron pair gives each hydrogen an electron configuration analogous to helium.

  5. .. .. . . : : F F .. .. .. .. : : : F F .. .. Covalent Bonding in F2 Two fluorine atoms, each with 7 valence electrons, can share those electrons in a covalent bond. • Sharing the electron pair gives each fluorine an electron configuration analogous to neon.

  6. . .. . . . : C F .. . .. : : F .. .. .. : : : F C : F .. .. .. : : F .. Example Combine carbon (4 valence electrons) andfour fluorines (7 valence electrons each) to write a Lewis structure for CF4. The octet rule is satisfied for carbon and each fluorine.

  7. .. : : F .. .. .. : : : F C : F .. .. .. : : F .. : : F .. .. : : C F F .. .. : : F .. Example It is common practice to represent a covalentbond by a line. We can rewrite .. as

  8. So… 2 shared electrons can be rewritten as a single line. The line is called a ‘single bond’. • TRY IT!! • Draw the lewis dot structure for Phosphorus Triiodide • Draw it again, this time replacing pairs of shared electrons with a single line.

  9. Phosphorus Triiodide : I : : . : : : : : . : : I I P . . : : : : I : _ _ : : : I I . . P _ : :

  10. .. .. : : : : : : C O O Double bonds • Some atoms share more than 2 pairs of electrons between them. • You still replace each pair of shared electrons with a line but if two lines are present between 2 atoms, it is called a DOUBLE BOND. Try drawing the double bonds for carbon dioxide Carbon dioxide

  11. .. .. .. .. : : : : : : : : C C O O O O becomes

  12. : : : : : : H H C N C N Triple Bonds Hydrogen cyanide

  13. REMEMBER… • The atoms want to have 8 valence electrons! • Shared electron pairs can be represented by a line, which shows that the atoms are bonded.

  14. H H .. .. : : : : H H C C : : : : : H H C C Let’s practice! Replace the electron pairs by drawing in the bonds Ethylene Acetylene

  15. H H H H .. .. : : : : H H C C C C H H : : : : : H H H H C C C C Ethylene Acetylene

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