Hybrid Theory Worksheet

 

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  1. Consider CH4

      2.  

    1. What orbitals are available for bonding for each atom involved in the molecule?

      2.  

    2. Based on this would you expect all the C-H bonds in methane (CH4) to be identical?

      3.  

    3. What have experiments shown?

      4.  

    4. What does this indicate?

     

     

  2. This means that when an atom patricpiates in a bond, _____________
    __________________________________________________________.

    3.  

     

  3. How does the energy of the hybrids compare to the atomic orbitals?

    4.  

     

  4. The number of hybrid orbitals formed is equal to  _________________.

    5.  

     

  5. What should you do first, when trying to determine the type of hybrid orbitals needed? 

      6.  

    1. Why?

      2.  

    2. How many areas of electron density do the following account for?

        3.  

      1. Lone Pairs

        2.  

      2. Single bond

        3.  

      3. Double Bond

        4.  

      4. Triple Bond

     

     

  6. Fill In the Following


    7.  

     

  7. Draw the following

      8.  

    1. CH4

      2.  

    2. CH2O

     

     

  8. What are sigma and pi bonds?

    9.  

     

  9. What are each type of bond composed of?

    10.  

     

  10. Predict the shape, hybridization of central atom and polarity for the following

      11.  

    1. OF2

      2.  

    2. TeF4

      3.  

    3. BF3

     

     

  11. Label the hybridization of C, O, and N in the following molecules.  Also count total number of sigma bonds and total number of pi bonds.
                         

    12.  

     

  12. Are all the atoms in the same plane?

      13.  

    1. C2H2

      2.  

    2. CH2CCH2                   

     

     

  13. How can CO32- help us understand the short falls of LE model?

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