Electronegativity

Use a periodic table with [|electronegativities]

 * 1) ==Which element has the highest electronegativity?==
 * 2) ==Subtract the electronegativity of oxygen from that of fluorine. What is the difference?==
 * 3) ==Do the same for O – N==
 * 4) ==N - C==
 * 5) ==C – B==
 * 6) ==B – Be==
 * 7) ==Be – Li==
 * 8) ==What is the pattern?==


 * 1) ==What other patterns can you find?==


 * 1) ==Find the difference in negativity for the following bonds:==
 * 2) ==H-F==
 * 3) ==H-Cl==
 * 4) ==C-H==
 * 5) ==C-Cl==
 * 6) ==C-S==
 * 7) ==Na-Cl==
 * 8) ==S-O==
 * 9) ==K-Br==
 * 10) ==Mg-Br==
 * 11) ==Si-O==
 * 12) ==Use the difference in electronegativity (ΔEN) to predict bond type as follows: ΔEN < 0.5 non-polar covalent; ΔEN 0.5 to 1.6 polar covalent; ΔEN >2.0 ionic. For 1.6-2.0 the rule is if a metal is involved, the bond is ionic, if no metal is involved the bond is polar covalent.==

Go back to a-h in #4 and characterize each bond as non-polar covalent, polar covalent, or ionic

 * 1) ==_==
 * 2) ==_==
 * 3) ==_==
 * 4) ==_==
 * 5) ==_==
 * 6) ==_==
 * 7) ==_==
 * 8) ==_==
 * 9) ==_==
 * 10) ==_==