exp 2 questions
robert zellmer
zellmer.1 at osu.edu
Wed Jan 24 16:29:10 EST 2018
I've received a some questions about exp 2 report.
3) Discussion Section:
It's quite possible most of you didn't get the correct formula
following the
correct procedure. Multiplying by a factor to get whole number
subscripts
might not give you a reasonable formula (within 0.1 of a whole
number).
For instance it's unlikely to have something like Pb_12 O_21 for
an empirical
formula for an ionic compound. Generally speaking, the most positive
charges (oxidation numbers) wouldn't exceed +8 and the most negative
wouldn't exceed -3. So what should you do?
You should discuss whether your formula is reasonable. How do you
know?
I've discussed what the normal charges for representative metals
are based on
what group they're in. Group 3A (13) metals are usually +3 (Al is
always +3)
but can be +1. Group 5A would be +5 or +3. I discussed lead, Pb,
in lecture
and stated it is +2 or +4. If you don't see the pattern, the
charges for the
representative metals in groups 3A-6A equals the group # or (group
# - 2).
Based on this you should be able to predict the normal charges for
Sn. That will
allow you to predict the most likely compounds for Sn and O. Then
look at your
original ratio before you multiplied by the factor you used to get
the whole number
ratio. Address why you might not have obtained the correct ratio?
To give an example, iron can form a +2 and +3 ion. This would
give FeO and
Fe2O3. The Fe2O3 will result as the iron is oxidized over time
and converts from
Fe to Fe^2+ (it's usually oxidation state in solution, at least
initially) and then to
Fe^3+. This is particularly true when there's a greater amount of
oxygen available
to react with the iron.
If you've already turned in the report you can "fix" things if you
like and turn it in
again. The TA will grade the most recent submission.
Dr. Zellmer
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