Chemistry 20 Chapter 1 Review
Name:
1. Explain how a property of the noble gases leads to the octet rule.
2. When hydrogen is involved in a bond, why does it not conform to the octet rule?
3. Use electron dot diagrams to predict the formulas of the following compounds:
a. Potassium bromide
b. calcium fluoride
4. When you examine the electron dot diagram of a non-metal, such as nitrogen or sulfur, how can
you predict the number of electrons that will most likely be involved in bonding? How can you
predict the number of electrons that will not be involved in a bond?
5. Draw Lewis structures of each of the following compounds:
a)
CS2(s)
b)
Br20(g)
c)
ClF(g)
d)
NF3(g)
6. Use electron dot diagrams to illustrate, in detail, the formation of ionic bonds between calcium
atoms and chlorine atoms.
7. Use the charge of the ions to determine the formula for strontium oxide and for magnesium
nitride.
8. Explain the meaning of "lone pair" and "bonding pair" as they relate to covalently bonded atoms.
9. Because every oxygen atom needs two additional electrons to form a stable octet, how can two
oxygen atoms bond together to make an oxygen molecule in which both oxygen atoms have an
octet of electrons in their outer energy levels?
10. Explain the relationship between a structural formula and a Lewis structure for the same molecule.
11. Describe the current model for metallic bonding.
12. Write the formula for each of the following compounds:
a. tin(II) fluoride
b) cesium bromide
c) lead (IV) phosphate
Pb3(PO4)4(s)
13. Name the following compounds:
a. K2Cr207(s)
b. Al2(S04)3(s)
c) N2Cl2(g)
14. The concept of electronegativity applies to an affinity (attraction) for which electrons in an atom?
15. Summarize the trends in electronegativity within a period and within a group on the periodic table.
16. How does the sharing of bonding electrons differ between a non-polar covalent bond and a polar
covalent bond?
17. State whether a bond that would form between the following pairs of atoms would be ionic or
polar covalent:
a. zinc and oxygen
b. magnesium and iodine
∆EN = 1.7 = ionic
∆EN = 1.4 = polar covalent
18. Arrange the following sets of bonds from most polar to least polar:
a. Mn and 0, Mn and N, Mn and F
b) Be and F, Be and Cl, Be and Br
19. Given the following information, identify element X.
a. XF4, where X is in Period 2
b. CaX, where X is in Periond 2
c. XH2O, where X is in Period 2, and the molecule contains two single bonds and one double
bond.
d. XH3, where X is in Period 2 and the molecule contains only single bonds.