1. 1)Since CO2 is a nonpolar molecule its Lewis dot structure differs from CH4. It has lone pairs which is important to show.

    2. For counting the number of electrons you are correct if you counted a total of 18 electrons. Six electrons from each oxygen and four electron from the carbon mounting a totally of 18 electrons.

    3. After forming the first two bonds, extra double bonds are required to satisfy the octet rules for oxygen and carbon.

    4. Distribute lone pairs around oxygen to complete the structure

    5. 2) Since NH3 is a polar molecule do not forget to add the two electrons to satisfy the nitrogen’s octet.

    6. Connect each hydrogen utilizing a pair of electrons, so three hydrogen will use up 6 electrons from the total of 8. Just 2 extra for the lone pairs mentioned above.

    7. No double bond is required due to nitrogen’s satisfied octet rule.
    8. 3) Be careful in this problem due to the fact that it has two central atoms, two carbons connected to each other by two electrons forming one bond.

    9. Connect the hydrogen to respective carbons trying to satisfy the carbon’s octet. Use 2 electrons per bond made.

    10. Remember to keep count of electron’s used up to prevent mistakes

    11. Distribute remaining electrons, in this case none.


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