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anonymous

  • one year ago

Which of the following compounds is saturated? A. C6H10 B. C7H14 C. C9H20 D. C9H14 Help! I am not sure how to do this problem...a step by step explanation would be wonderful. :)

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  1. anonymous
    • one year ago
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    @dan815

  2. Photon336
    • one year ago
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    Saturated compound contains a double bond if this is the first time you're doing this you may want to draw out the compound first

  3. Photon336
    • one year ago
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    let's start with C6H10 Step #1 draw out the carbon backbone |dw:1441062004377:dw| Step #2 put in all the hydrogens and count them. Remember every carbon must have four bonds to it, ALWAYS.

  4. Photon336
    • one year ago
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    |dw:1441062178715:dw| NEXT we, put in all our hydrogens, we have used 10 hydrogens. BUT what do we need to finish this figure off?

  5. Photon336
    • one year ago
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    because the carbons are in a RING structure, each carbon is bonded to a carbon on the left and to the right so, it has 2 bonds already. you just need to put in the hydrogens 2 for each carbon in the ring.

  6. anonymous
    • one year ago
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    But the two on the left have only one hydrogen attached?

  7. Photon336
    • one year ago
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    @RobinJane Yes so we must put in a double bond, so that each carbon has four bonds so it would be like this. |dw:1441062556185:dw| So now you know what saturated is right vs un saturated? a compound must not contain any double bonds for it to be saturated. |dw:1441062449685:dw| any compound that has a double bond in it is unsaturated . |dw:1441062624115:dw|

  8. Photon336
    • one year ago
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    So to figure out this problem, you do the following; 1. on a piece of paper you count out the number of carbons in the formula. 2. then you place hydrogens on each carbon to make sure that the carbons have 4 bonds. 3. if you run out of hydrogens, then you would have to put in a double bond. 4. CARBON always Makes 4 bonds.

  9. Photon336
    • one year ago
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    One last thing saturated compounds will have the formula CnH2n+2 if I remember correctly. So you can see if a formula is unsaturated/vs saturated whether it will have a double bond. so for C7H14 You can test this out first; like you can put in 7 and see how many hydrogens that your compound must have to be saturated. if it has less than this you know it's unsaturated. so for C7H14; you know that n =7 right? well plug it into this formula C7 2(7) + 2 = 16 C7H16 but we have C7H14 ; SO This must be unsaturated

  10. anonymous
    • one year ago
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    SO it is not saturated?

  11. Photon336
    • one year ago
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    nope; but why?

  12. anonymous
    • one year ago
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    That makes sense... Aren't there two formulas?

  13. anonymous
    • one year ago
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    Is it better to plug into the formula, or to draw it?

  14. anonymous
    • one year ago
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    I mean, which method is better and more accurate?

  15. Photon336
    • one year ago
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    well I suggest drawing it out, because that way you get to see for yourself why it's saturated/vs un saturated. also if you take organic chem you may not be given a molecular formula like C7H2N etc... and they won't show you how it's drawn you'll have to draw it out yourself.

  16. Photon336
    • one year ago
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    like C9H20 can you draw that out for me?

  17. anonymous
    • one year ago
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    I am trying...just a moment...

  18. anonymous
    • one year ago
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    |dw:1441063493585:dw|

  19. anonymous
    • one year ago
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    Is this right?

  20. anonymous
    • one year ago
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    @Photon336

  21. Photon336
    • one year ago
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    You're almost there, so yeah you counted the carbons, put in the hydrogens, there's just one thing it's not a ring but it's straight chained.

  22. anonymous
    • one year ago
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    Oh!

  23. anonymous
    • one year ago
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    But the idea is similar, correct?

  24. Photon336
    • one year ago
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    yep. so make sure you count out all the hydrogens

  25. anonymous
    • one year ago
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    So that one is unsaturated?

  26. anonymous
    • one year ago
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    Let me try again...

  27. Photon336
    • one year ago
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    another question i have for you was does each carbon have 4 bonds?

  28. Photon336
    • one year ago
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    like whether it's a ringed structure vs straight chain that takes practice, wish I had a way to explain it but you will have to just keep seeing them

  29. anonymous
    • one year ago
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    |dw:1441064007882:dw|

  30. anonymous
    • one year ago
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    In this one, it is saturated!

  31. anonymous
    • one year ago
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    How do you do double bonds without adding more to carbon?

  32. Photon336
    • one year ago
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    excellent

  33. anonymous
    • one year ago
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    Is the top drawing correct?

  34. Photon336
    • one year ago
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    yes that's perfect, what did you mean about the double bonds?

  35. anonymous
    • one year ago
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    When it is unsaturated.

  36. anonymous
    • one year ago
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    Or do you just use the drawing to establish unsaturated vs saturated?

  37. Photon336
    • one year ago
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    Well in the figure you drew, that's unsaturated because there are no double bonds if it were saturated then you would have a double bond

  38. Photon336
    • one year ago
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    Hope this helps

  39. anonymous
    • one year ago
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    How do you draw it?

  40. anonymous
    • one year ago
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    Double bonds, that is?

  41. Photon336
    • one year ago
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    Just when you draw the bond between the carbon place another line on top of it should look like = an equal sign. Just remember that each of your carbons has four bonds. If your carbons have four bonds each of them then you can't have a double bond there b/c then those carbons will have 5 bonds no good

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