Asked by annie
Why is;
a) antimony pentafluroide
Sb(-3) + F5(-1) --> SbF4 ?
b) aluminium bromide hexahydrate
Al(-1) + Br(-1) --> AlBr3 . 6H2O ?
The charges don't add up for (b), is there something to do with the "ide"? I don't get it.
And for (a) how did "pentafluoride" end up to be "F4"? --- shouldn't the answer be Sb(F5)3?
a) antimony pentafluroide
Sb(-3) + F5(-1) --> SbF4 ?
b) aluminium bromide hexahydrate
Al(-1) + Br(-1) --> AlBr3 . 6H2O ?
The charges don't add up for (b), is there something to do with the "ide"? I don't get it.
And for (a) how did "pentafluoride" end up to be "F4"? --- shouldn't the answer be Sb(F5)3?
Answers
Answered by
bobpursley
Antimony has an electronic structure of
# Ground state electron configuration: [Kr].4d10.5s2.5p3
Which means its valences can be +5, or +3. I don't know of a fluoride SbF4, and suspect one does not exist.
Aluminum has a common valence of +3. Take a look at its electronic structure.
# Ground state electron configuration: [Kr].4d10.5s2.5p3
Which means its valences can be +5, or +3. I don't know of a fluoride SbF4, and suspect one does not exist.
Aluminum has a common valence of +3. Take a look at its electronic structure.
There are no AI answers yet. The ability to request AI answers is coming soon!
Submit Your Answer
We prioritize human answers over AI answers.
If you are human, and you can answer this question, please submit your answer.