|
|
|
|
|
| Author |
Message |
![[Post New]](/templates/default/images/icon_minipost_new.gif) 21 Mar 2008 13:03:11 IST
|
|
|
BaO2 is peroxide but MnO2 s dioxide-why?
|
SREE |
|
|
|
21 Mar 2008 13:05:37 IST
|
|
|
dude in BaO2 the oxidation state of O is -1 and in MnO2 it is -2.
|
PROGRESS ISN'T MADE BY EARLY RISERS OR HARD WORKERS, BUT BY LAZY PEOPLE TRYING TO FIND EASIER WAY TO DO THE SAME.....SO BE LAZZZZYY!!!! |
this reply: 0 points
(with 0 
in 0 votes ) [?]
|
|
You have to be logged on to rate
|
|
|
21 Mar 2008 13:41:29 IST
|
|
|
stability of peroxides and superoxides increases with increase in atomic somic. Ba2+ is much larger in size than Mn2+ and hence it readily forms peoxide.
|
Guide to latex:
http://www.goiit.com/posts/list/community-shelf-a-guide-to-latex-48056.htm
|
this reply: 0 points
(with 0
in 0 votes ) [?]
|
|
You have to be logged on to rate
|
|
|
31 Mar 2008 00:42:13 IST
|
|
|
How can you compare BaO2 with MnO2. BaO2 belongs to second group and has an oxidation state of +2. So oxygen has oxidation state of -1 and hence BaO2 is peroxide.
Mn is a trasition metal and in MnO2 its oxidation state is +4 and that of Oxygen is -2 So its a normal oxide
|
Krishna Gopal Singh
B.Tech Chemical Engg
IIT Delhi 2002
Currently doing PhD from IIT Delhi |
this reply: 0 points
(with 0
in 0 votes ) [?]
|
|
You have to be logged on to rate
|
|
|
|
|
|
|
|
|
|
Moderation Team
![[Up]](/templates/default/images/icon_up.gif "[Up]"){kind=icon}
2
