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Kaplan - Pi Bond

Discussion in 'DAT Discussions' started by skyisblue, May 14, 2007.

  1. skyisblue

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    Kaplan states that: " A pi bond cannot exist independently of a sigma bond. Only after the formation of a sigma bond will the p orbitals of adjacent carbons be parallel, because without the bond the three p orbitals are orthogonal to one another."

    I don't get where there are 3 p orbitals and what does orthogonal mean?
     
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  3. Sbosu

    Sbosu Member

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    Px, Py, and Pz. Orthogonal i think basically means parallel to one another therefore they cannot overlap and form a bond
     
  4. lor

    lor

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    Based on my DAT experience:
    just know how to count pi bonds/sigma bonds for a given molecule
    tripple bond has 2 pi and one sigma
    double bond has one sigma and one pi and so on
    know that sigma bonds are stronger than pi bonds
    know that the energy goes up as the number of bonds go up, exp, you need more energy to break down a tripple bond in comparison to a double bond
    tripple bond is SP...180 degree
    double bond is SP2...120 degree
    single bond is SP3...109.5
    ===========================
    I am not a DAT guru but I'll give you as much as I know:D
     

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