Name______Date______Period______

  1. How are ionic bonds and covalent bonds different?
  1. How does a polar bond differ from a nonpolar bond?
  1. How do electronegativity values help us determine the type of bond created?

  1. For each of the following molecules, determine if it isnonpolar covalent, polar covalent, or ionic.

Bond characteristic based on difference in electronegativity(see chart above)

3.3 1.70.3 0.0

Name______Date______Period______

Molecule / Electronegativity Values / Difference in Electronegativity / Bond Type
H – Cl / H:
Cl:
H - I / H:
I:
Cl - Cl / Cl:
Cl:
C – O / C:
O:
Ca – O / Ca:
O:
H2O / H:
O:
Al – Fe / Al:
Fe:
  1. Does electronegativity increase or decrease when you go across a period on the periodic table? Does it increase or decrease when you move down a group on the periodic table?
  1. For each of the following sets of elements, identify the element expected to be most electronegative (EN) and which is expected to be least electronegative (EN).
  1. K, Sc, Camost EN= ______least EN=______
  1. Br, F, Atmost EN= ______least EN=______
  1. C, O, Nmost EN= ______least EN=______
  1. Label the partial charges of each element in the bond with (δ- or δ+)or the arrow (+)

a)H—Brb) Li—Cl c) O—N d) F—F

  1. For each of the following pairs of bonds, circle the bond that is more polar.

a)H—P, H—C b) O—F, O—I c) N—O, S—Od) N—H, Si—H

  1. What does it mean to say a bond is polar? What does it mean to say a bond is a nonpolar?

10) For Water (H2O).

1) Draw a Lewis dot structure

2) Draw the arrows over each bond to show the partial charges of each bond.

3) Name the shape that is formed

4) State if it is a polar or nonpolar MOLECULE: (can you cut it in half and have one positive side & one negative)