Question

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Which is the electron configuration for bromine?
1s²2s22p63s23p4s23d104p5
1s22s²2p3s23p64s23d104p
1s 2s22p63s23p'4s23d104p5
O1s22s22p3s23p64s23dº4p5

Answer 1

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`s^(2)`2
`s^(2)`2
`p^(6)`3
`s^(2)`3
`p^(6)`3
`d^(10)`4
`s^(2)`4
`p^(6)` (alternatively 1s2 2s2 2p6 3s2 3p6 3d10 4s2 4p6)

Step-by-step explanation:

The correct configuration for bromide (
`Br^(-)`) is:

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`s^(2)`2
`s^(2)`2
`p^(6)`3
`s^(2)`3
`p^(6)`3
`d^(10)`4
`s^(2)`4
`p^(6)` (it has one more electron in 4p orbital than bromine)

You can also write it as [Ar]
`4s^(2)`
`3d^(10)`
`4p^(6)`, since noble gases are very stable

First can't be correct because there is nothing in 3p orbital and 4p has only 5 electrons here

1s² 2s2 2p6 3s2 3p 4s2 3d10 4p5

Second can't be correct because there is nothing in 2p and 4p orbitales 1s2 2s² 2p 3s2 3p6 4s2 3d10 4p

Third can't be correct because there is nothing in 3p orbital and 4p has only 5 electrons here

1s 2s2 2p6 3s2 3p' 4s2 3d10 4p5

Fourth can't be correct because there is nothing in 2p and 3d orbitales, and 4p has only 5 electrons here

1s2 2s2 2p 3s2 3p6 4s2 3dº 4p5