1. Use Lewis Lewis electron dot structures to show the formation of ionic compounds of MgO, MgCl2, LiCl, AlF3
2. ” formation of covalent compounds of Cl2, H2S, NH3, NH4Cl, H20
3. Write the molecular formula for:
a. Barium Sulfide
b. Sodium Oxide
c. Calcium Bromide
d. Aluminum Oxide
e. Potassium Iodide
f. Sodium Sulfate
g. Calcium Hydroxide
h. Aluminum Nitrate
4. Given the follwing molecular formulas write the empirical formula:
1. C4H8
2. C6H14
3. C8H14
4. C6H1206
5. C6H5(OH)3
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For all the ionic compounds, just move the “extra” electrons from the metal to the nonmetal. When I say extra, I mean the electrons beyond what the metal needs to have the same electron configuration as the previous noble gas.
For MgO, for example, you move 2 electrons from Mg to O, giving O the same electron configuration as Ne, and Mg the same electron configuration as Ne as well.
The molecular forumulae are:
BaS
Na2O
CaBr2
KI
Al2O3
Na2S
Ca(OH)2
Al(NO3)3
These formulae can be derived by the same procedure as above, but you need to stop when you get to the noble gas configuration, which is why it’s not 1:1.
Empirical formulae are obtained by simply dividing the subscripts by the common factor.
For example:
C4H8 -> CH2