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    Use the Lewis structure for to show the structures of the elements

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    5. Use the Lewis structure form to show the structures of the element F2 and N2 and the compounds NaCl, NH3 and H2O. Write out the molecules with stick formulae.

    6. Use Lewis structures for the elements and so suggest a structure for the compound CCl2F2 called Freon-12.

    7. Suggest why sodium exists as Na+ and not Na2+ in its compounds.

    8. In water molecules the O atom attracts the electrons in the H-O bonds more strongly than the H atom does. What effect will this have on the position of the electron pair in each of the H-O bonds? Then explain how this accounts for water being a liquid at normal temperatures, rather than a gas (as for such a small molecule).

    9. a molecule of glucose has the structure. Try to explain why this compound is so soluble in water.

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    To create Lewis structures you need to look up on the Periodic Table how many valence (outer) electrons a compound has. In the case of F, it has seven outer electrons. Therefore, you place 7 electron dots around each F, and put them in pairs as much as you can. In so doing, you will see that each F has a single unpaired electron leftover. Therefore, to combine the two F atoms, you create a single covalent bond, each F atom sharing one atom in the bond, thereby giving each F atom eight electrons now. (Check out the attached graphic which illustrates all the Lewis and stick formulas.)

    You do the same thing for NH3 as well, where N has five electrons, made up of one pair and three singles. Why do we put the five electrons around N like that? Each of the N singles can pair up with the single electron on each H to form three covalent bonds. Therefore, N ends up with 8 electrons, and of course, H with only two (which is all it needs).

    Oxygen has 6 electrons in its outer shell---two pairs and two lone pairs. Each lone pair shares with the single electron in hydrogen to form two covalent bonds. As a result, ...

    Solution Summary

    822 words answer 4 questions on Lewis structures.