We usually denote oxidation states as -3, -2 or -1....
Then why is it denoted as +5 and so..
2006-09-15 17:07:18 · 7 answers · asked by Anonymous in Science & Mathematics ➔ Chemistry
but then are these oxdn states same as -3, -2 or -1....
In our text, it has been given that the flourine family has an oxdn state of +7, oxygen - +6 and so on......
So...is that possible
2006-09-15 17:54:55 · update #1
Thank you very much for the response...
yeah..its true that i m totally confused, but still....in our text, it has been given in a box under the topic - oxdn states....so thats perfectly clear...no doubts there.....
2006-09-17 02:25:32 · update #2
Apparently you are a bit confused.
+7 and -1 are not the same:
In terms of oxidation number +x means that the atom of the element has "lost" x electrons (either literally lost them in an ionic bond, or it participates in covalent bonds with more electronegative elements)
-x is the opposite that is the atom has "gained" x electrons (either literally gained them in an ionic bond, or it participates in covalent bonds with less electronegative elements)
There are elements that can have oxidation number +5, +6,+7 like in the examples mentioned in the other answers (e.g. N has +5 in HNO3, Cr has +6 in K2Cr2O7, Mn has +7 in KMnO4 etc)
The sentence you are mentioning "In our text, it has been given that the flourine family has an oxdn state of +7, oxygen - +6 and so on" sounds completely wrong; I am sure you didn't understand what was written in your textbook, so I can't really say more than the following. The elements in the same group with fluorine (halogens) have 7 e in their outer shell so their most common oxidation number is -1 (gaining 1 e to have a complete octet in the outer shell). However there are exceptions, e.g. chlorine has oxidation number +7 in KClO4 and +5 in KClO3
You might have confused the number of e in the outer shell with the oxidation state
2006-09-16 10:30:34 · answer #1 · answered by bellerophon 6 · 0⤊ 0⤋
Sure ! Look at phosphorus pentoxide, P2O5 (phosphorus +5), sulphur trioxide, SO3 (sulphur +6) and potassium permanganate, KMnO4 (manganese +7).
The normal oxidation states of highly electronegative elements like oxygen and chlorine are negative. In compounds of these with less electronegative ones, the latter can have oxidation states +1 to +7 ; precisely which state depends on their position in that rogues' gallery -- the periodic table.
2006-09-16 01:11:34 · answer #2 · answered by Problem Child 2 · 0⤊ 0⤋
Yes. Of course there can be higher oxidation states. It just means that more electrons are being lost. A chlorate anion has an oxidation state of +5. Chromate and permanganate anions have oxidation states of +6. A perchlorate anion has an oxidation state of +7.
2006-09-16 00:22:36 · answer #3 · answered by عبد الله (ドラゴン) 5 · 0⤊ 0⤋
Oxidation state is defined as the no. of electrons that are transferred(gained or lossed) in a reaction. If electrons then + ve oxidation state is obtained, it electrons are gained then -ve. Oxidation state of Mn in KMnO4 is +7.So no more confusion in future
2006-09-18 14:22:29 · answer #4 · answered by vsgr06 2 · 0⤊ 0⤋
oxidation states of +5,+6,+7 are all possible.also highest oxidation number of +8 is shown by osmium
2006-09-16 12:36:11 · answer #5 · answered by Anonymous · 0⤊ 0⤋
Yes. Examples: +5, HNO3; +6, H2SO4; +7, KCrO4.
2006-09-16 00:24:26 · answer #6 · answered by Anonymous · 0⤊ 0⤋
+7 in MnO 4- +8 is also seen in ru(below fe)
2006-09-16 00:47:02 · answer #7 · answered by v2en2ka5trg 1 · 0⤊ 0⤋