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Name:
1. Describe the difference between a shared pair and an unshared pair of electrons/
2. Describe a molecular dipole.
3. Why is the electronegativity of an element important in determining polarity?
4. How does a covalent bond differ from an ionic bond?
5. Predict whether the bonds between the following pairs of elements are ionic, polar covalent or nonpolar covalent: a. Na - F
b. H - I
c. N - O
d. Al - O
e. S - O
f. H - H
g. Cl - Br
h. Sr - O
6. Explain why the melting points of covalent compounds tend to be much lower than those ionic compounds.
7. On a separate piece of paper, draw the Lewis dot diagram for the elements boron, nitrogen, and phosphorus.
8. What do the dots in a Lewis Dot Diagram represent?
9. Name the following covalent compounds: a. SF4
b. XeF4
c. PBr5
d. N2O5
e. Si3N4
f. PBr3
g. Np3O8
10. Why do electron pairs around a central atom stay as far away as possible?
11. Name the following three molecular shapes:
12. On a separate piece of paper, draw the Lewis dot diagram for the following molecules: a. NF3 b. CH3OH c. ClF d. CCl2F2 e. HOCl
13. On a separate piece of paper, draw the Lewis structures for the following polyatomic ions and determine the molecular shapes a. OH- b. O22- c. NO-2 d. NO+2 e. AsO4-3
14. On a separate piece of paper, draw the Lewis structures for the following compounds and determine their mo0lecular shapes: a. O2 b. CS2 c. N2O
15. On a separate piece of paper, draw the Lewis Dot diagrams and determine the shapes for the following compounds: a. CF4 b. Cl2O
16. According to VSEPR, what molecular shapes are associated with the following types of molecules? a. AB
b. AB2
c. AB3
d. AB4
17. What type of atoms tend to form the following bonds? a. ionic
b. covalent
c. metallic
