Mrs. M. Hutchins                                 A”                                                   Honors Chemistry                    

Chemical Bonding Hot List  A               Chapter 8                                              March 2006





View the sites below and answer the questions that follow

A.  Chemical Bonding

  1. Read Introduction. What did Lewis observe about atoms and what did he suggest?
  2. Read Ionic Bonding. Explain in your own words the nature of an ionic bond.
  3. Click on the Simulation of the reaction of NaCl. There are three pages. Click on the prompt at the bottom right to go to page 2 and 3.

Explain what you see.

  1. Continue reading about ionic bonding. Explain why there is no such thing as a single ionic molecule.
  2. Read Covalent Bonding.  Click on the covalent bonding simulation and explain what you see.
  3. Continue reading Covalent Bonding. Explain why ionic “molecules” do not exist but covalent molecules do.
  4. Read Multiple Bonds And Lewis Dot Structures. From your notes or text what other type of multiple covalent bond exists? Draw the Lewis dot structure of three  molecular compounds- One with single bond(s), One with double bond(s) and one with triple bond(s). Make statements about bond length and bond strength related to the number of bonds between atoms.
  5. Read Polar and Nonpolar Covalent Bonding. Click on the simulation of the water molecule. Explain what you see.

9.   From your notes explain electronegativity of atoms and how polar covalent bonds are formed.  Draw and example of a molecule with nonpolar covalent bond(s) and one with polar covalent bond(s) indicating electronegativities of each atom, differences in electronegativities and partial charges if present.

10. Read Dipole. Explain the nature of a dipole. Go back to the previous simulation and explain why water is a dipole.




.                 Chemical Bonding: polar covalence

This site has some interesting information to stretch your mind about bonding. You can go there if you dare.