Question

What is the oxidation number of chlorine in Al(ClO4)3?

I don't understand this question, can someone help? Thank you!

Answers

Samba
All compounds are zero.
Al is in group III (or 13 depending onh the system used) so the oxidation state is 3.
You have 12 O at -2 each for -24. That leaves -24+3 = -21. So 3 Cl atoms must be +21 to balance the -21 there which makes +21/3 or +7 for each Cl.
Olereb48
Given
O3Cl- Al - ClO3
l
ClO3

Formal Charge = [Valence - (Bonded Electrons/2) - Non-bonded electrons]

FC(Al) = 3 - (6/2) - 0 = 3 - 3 = 0
FC(O) = 6 - (2/2) - 6 = -1
FC(Cl) = 7 - (8/2) - 0 = +3

Net Charge = 1Al + 3Cl = 9O
= 1(0) + 3(+3) + 9(-1)
= 0 + 9 - 9 = 0
Conforms to conservation of matter and of charge.
Ian
O is always a -2 oxidation state, unless it is in a peroxide, so -2*4*3 is -24, Al is +3 because an ion's oxidation state is its charge, which leaves the overall charge right now at -21, so to make the overall charge 0, 3 times the Oxidation state of Cl must equal positive 21, so the oxidation state of Cl is 7
OS71
I don't get this one
1. Combining solutions of silver nitrate and sodium chloride
produces a silver chloride precipitate:
AgNO3(aq) 1 NaCl(aq) → AgCl(s) 1 NaNO3(aq)
A researcher discovered that 32.0 mL of 0.100 mol/L silver
nitrate is required to precipitate all the chloride ions in 25 mL
of a solution of sodium chloride.
(a) What is the amount concentration of sodium ions in the
initial sodium chloride solution?
(b) What is the concentration, in g/L, of sodium chloride in
the initial sodium chloride solution?

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