procedure: for part 1, write the lewis dot (or electron dot) structure for each atom, followed by the ions that each element would form, the compound that would be formed from the combination of the two elements and finally the lewis dot structure for the compound.
for part 2, show the lewis dot structure for each molecules, its axe designation and finally its electron pair/ geometric shape geometries. also indicate any partial charges that may exist on that molecule.
part 1: ions and ionic bonding
lewis dot for atoms ions formed formula for compound lewis dot for compound
li f
k o
na n
mg cl
ca s
al br
mg p
part 2: lewis structures and geometry for molecules
lewis structure/ axe / electron pair geo./geometric shape
ch4
h2o
h3o+
hcl
nh3
h2co
cl2o
bro3-
so4 ^-2
co2
hcn
co
ccl4
c2h6
co3 ^-2
no2 ^-
so2
c2h4
c2h2
n2h4
cf3cl
clo3 ^-
ch3oh
cf4
question #1 :
which of the molecules in this exercise have polar bonds, but the molecule itself is non-polar? what makes that molecule(s) non-polar?
**you should find nine (9) structures! . remember that a difference of electronegativities greater than 0.1 determines a polar covalent bond, but a symmetrical structure will cancel bond polarity and be a non-polar molecule.**