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8.1 Covalent Bonds

8.1 Covalent Bonds. Molecular compounds = 2 non metals that share 1 or more pairs of electrons … group is electrically neutral. Draw the dot structure for CF 4. A dash shows a molecular bond and represents 2 electrons. How is water (H 2 O) different from sodium chloride (NaCl)?.

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8.1 Covalent Bonds

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  1. 8.1 Covalent Bonds

  2. Molecular compounds= 2 non metals that share 1 or more pairs of electrons… group is electrically neutral.

  3. Draw the dot structure for CF4

  4. A dash shows a molecular bond and represents 2 electrons

  5. How is water (H2O) different from sodium chloride (NaCl)?

  6. Review Bond Types:Copy into powerpoint notes.IONIC: Metal and Non Metal ions. Electrons jump from metal to non metal to make “magnets”.METALLIC: Metal and Metal ions. Electron sea floats between positive ions.CoVALENT: Non Metal and Non Metal atoms (Not ions). Share electrons.

  7. IONIC review: NaCl=Formula Unit=lowest ratio of ions in an ionic compound -atoms gained or lost e- to form ions that are electrostatically bonded to each other (metal)

  8. H2O =Molecular Formula= (Nonmetals) molecule atoms share electrons to form stable noble gas configurations (atoms don’t form ions but still follow the octet rule) H=2 electrons

  9. Notice the octet rule H = He 2e-O=Ne 8e-

  10. Molecular formula= shows the number and types of atoms in a molecule Discuss VESPER Theory and shapes of these molecules (electron pairs make 4 point pyramid). Discuss the Lewis Structures.

  11. How is the molecular formula different from a formula unit? Covalent Bond Ionic Bond

  12. Sharing 2 or 3 pair of electrons

  13. Sharing 2 pairs of electrons

  14. Draw the compound CO2

  15. Bond dissociation energy= amount of energy needed to break a single covalent bond

  16. The higher the BDE the stronger and more stable the bond.

  17. 7 diatomic elements found on earth H2, N2, O2, F2, Cl2, Br2, I2 Diatomic elements: 7,

  18. VSEPR = valence-shell electron-pair repulsion theory. Causes shape of molecules.repulsion between electron pairs causes molecular shapes to adjust so that the valence-electrons pairs stay as far apart as possible(SEE p242)

  19. Polar bonds : electron pair is shared unevenly. Causes the molecule to act like a magnet.(the element with higher electronegativity (p.xxx) has the electron more often and become slightly negative)

  20. Subtract the electronegativity of the two atoms to find the type of bond. (pg 248) Bond Type0-0.39 Nonpolar covalent0.4-1.0 Moderately polar1.0-1.9 Very Polar2.0 + Ionic or Metallic

  21. Hydrogen Bonds – hydrogen bonded to an atom with a high electronegativity is weakly bonded to a nearby molecules unshared electrons

  22. Bond Typep.238 table 8.3Electronegativity Difference0.0-0.39 nonpolar covalent0.4-1.9 polar covalent metal = Ionic

  23. Polar molecules – a molecule that has two poles (positive and negative, only happens with polar bonds) based on VSEPR shape

  24. Label bond type on worksheetIdentify VSEPR shapeIdentify polar molecules

  25. POLYATOMIC IONS:Sharing too many electrons… Polyatomic ions (molecules with a charge)

  26. Review

  27. Draw the compound SCl2

  28. Draw the compound SCl2

  29. Molecules:Covalent Sharing of Electrons

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