Can someone explain to me why the electronic configuration of Pt is [Xe]4f145d96s1 instead of [Xe]6s24f145d10?

Question

the right one [Xe] 4f14 5d9 6s1
my Q: why not [Xe] 4f14 5d8 6s2? or [Xe] 4f14 5d10?

Answer 1

There are a couple things you need to remember:

1) When you right the shorthand electron configuration the look at the Atomic Number (Z) of the noble gas you're using and subtract it from Atomic number of the element you're using.

For Example:Pt has an Atomic Number=78
Xe has an Atomic Number= 54

That leaves 24 electrons remaining to account for so automatically you should see that [Xe]6s(2)4f(14)4d(10) is incorrect because 2+14+10=26

--This is a good way to check yourself in equations such as these.

The primary reason is because of Aufbau Principle: electrons enter the orbital at the lowest energy first.

Here is a list of how they would enter and I hope this helps to explain it better:

1s
2s 2p
3s 3p 3d
4s 4p 4d 4f
5s 5p 5d 5f 5g
6s 6p 6d 6f 6g
7s 7p 7d 7f 7g

Therefore a 4f orbital has to enter before (5d) and (6s) respectively

Answer 2

Electron Configuration For Pt

Answer 3

Pt Electron Configuration

Answer 4

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RE:
Can someone explain to me why the electronic configuration of Pt is [Xe]4f145d96s1 instead of [Xe]6s24f145d10?

Answer 5

I believe the 6s subshell is less energetic than the 5d subshell. Check back and see where the 6s subshell is cleared to fill inner subshells. That group of compounds starts with the 6s subshell filling up first.

Answer 6

bsta it's like that... tungsten is a transition metal so...