Help:( I'm not so much interested in the answer to this as how to do it. I'm not sure how you figure out what the most stable ion would be for aluminum.
2006-09-06 08:45:46 · 5 answers · asked by Kiko 3 in Science & Mathematics ➔ Chemistry
I don't think I will ever understand why people answer a question they don't know the answer to.... oh wait, points!
2006-09-06 08:48:19 · update #1
Oh wow, and now it wants to know how many oxygen atoms there are in one formula unit aluminum nitrate. Why is there oxygen in it!?
2006-09-06 09:24:27 · update #2
Okay, here's the scoop:
Aluminum is in group IIIA on the periodic table of the elements. That means it has three valence electrons. If you do the orbital shell filling method, it would be written as 1s2, 2s2, 1p6, 3s2, 2p1.
All atoms are attempting, in some manner, to reach an optimally stable electron configuration -- one that resembles one of the noble gases. That means that they'd need to either gain electrons or lose electrons to empty or fill shells to match a noble gas. In the case of Aluminum, the atom can either gain five electrons (which would give it an ionic charge of -5) to resemble Argon, or it can lose three electrons (giving it a charge of +3) to resemble Neon. Which do you think would be easier?
Right, it will **lose** 3 electrons, so the Aluminum ion is Al+3.
The nitrate ion, (NO3)-, has an ionic charge of negative one. If you do the Lewis dot structure of nitrate ion, you can see that it would need one more electron to form filled outer shells, and this is how it acheives the negative charge. Those electrons, in the case of the compound you are examining, would HAVE to come from the Aluminum. Aluminum gives up three that go, one apiece, to the nitrate!
Therefore, the salt Aluminum nitrate has the chemical formula
Al(NO3)3.
The previous poster mentioned the hydrated form of the compound, aluminum nitrate nonahydrate. Sounds a bit to me like a red herring -- don't worry about the hydrated form unless the prof/teacher specifically asks for it.
Hope this helps.
2006-09-06 10:15:45 · answer #1 · answered by Dave_Stark 7 · 1⤊ 1⤋
ok, So aluminium varieties 3+ ions and oxygen varieties 2- ions, and standard a compound ought to have a independent can charge: a) (3+)x2 = +6. (-2)x3 = -6 standard +6+(-6) = 0 this is the only compound of the three to have a independent can charge, so is the only compound that would variety. wish that helps
2016-12-18 05:58:59 · answer #2 · answered by Anonymous · 0⤊ 0⤋
I got this off the website below...hope it helps.
The nonahydrate aluminum nitrate, Al(NO3)3·9H2O (CAS No. 7784-27-2), is the stable form of this compound.
2006-09-06 08:54:03 · answer #3 · answered by CC 2 · 0⤊ 1⤋
whoa....I will have to wait for my husband to come home to answer that one....watch for him...railroaddave!!!!
2006-09-06 08:48:14 · answer #4 · answered by vampire angel 3 · 1⤊ 3⤋
Not sure.
2006-09-06 08:47:17 · answer #5 · answered by rab 4 · 0⤊ 3⤋