CH 6 study guide by O3L09H

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									Chemistry                                                                                 NAME:
Chapter 6                                                                                 PERIOD:
Study Guide                                                                               DATE

6.1
      1) In general, what is the difference between ionic bonds, as in NaCl, and covalent bonds, as in H 2O?




      2) When two or more atomic orbitals overlap, molecular orbitals are formed. Using diagrams and your knowledge of charges
         and electrical attraction, explain this statement.




      3) Explain the relationship between potential energy and the formation of a covalent bond.




      4) Why is the hydrogen molecule, H2, more stable than the individual hydrogen atoms that bond to form it.




      5) In your own words, explain the “bond/spring” analogy for bond length between bonded atoms.
6) In table 6-1, which molecule has the highest bond energy? What does this tell us about the molecule?




7) List four examples of covalently bonded compounds.




8) Describe electronegativity. Who first assigned electronegativity values to the elements?




9) How does an element’s electronegativity relate to its position on the periodic table?




10) Compare and contrast polar and nonpolar covalent bonds.




11) What is a dipole? Give an example.
Chemistry                                                                              NAME:
Chapter 6.2                                                                            PERIOD:
Study Guide                                                                            DATE:

   12) Which electrons in an atom are involved with bonding?


   13) What was G.N. Lewis’ contribution to chemistry?



   14) What are the drawbacks of Lewis Dot structures?




   15) In a Lewis dot structure diagram, what is represented by the symbol of the element?




   16) How many electrons are required for a stable configuration? What is this configuration called?




   17) Compare and contrast paired and unshared electron pairs?




   18) List the rules for Drawing Lewis Structures with many atoms.




   19) What are the steps for drawing Lewis structures?




   20) Why would atoms require sharing more than one pair of electrons in a bond?
21) What are the steps for drawing Lewis structures with multiple bonds?




22) What is a resonance structure?




23) Why are resonance structures necessary?




24) What are the steps for drawing Lewis structures of polyatomic ions?




25) How are covalent compounds named?
Chemistry                                                                             NAME:
Chapter 6                                                                             PERIOD:
Study Guide                                                                           DATE

Section 6.3

    26) What is the valence shell electron pair repulsion (VSEPR) theory ?




    27) In general, how do electron pairs position themselves in an electron cloud?




    28) What are the four steps needed to predict molecular shapes?




    29) What is a molecular dipole?
Section 6.4
    30) In general, how does the melting point of covalent compounds compare to that of ionic compounds? Why is this so?




    31) What are intermolecular forces?




    32) What is a hydrogen bond?




    33) How does hydrogen bonding account for water’s unique properties?




    34) What is a London force?

								
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