Linked Questions

4
votes
2answers
18k views

Ground state electron configuration of chromium [duplicate]

What is the ground state electron configuration of chromium? Is it $\ce{[Ar]}4s^23d^4$ or Is it $\ce{[Ar]}4s^13d^5$
2
votes
2answers
12k views

Electron orbital diagram of vanadium [duplicate]

I am learning about electron configurations and I came across the "exceptions" of $\ce{Cr}$ and $\ce{Cu}$ where electrons actually half fill the $\mathrm d$ orbitals instead of the expected $\mathrm s$...
0
votes
1answer
2k views

Why 4s lose electron to 3d? [duplicate]

In chromium and copper, the are the configuration fill up like $$\mathrm{3d^5 4s^1}$$ but not $\mathrm{4s}$ first as it has lower energy level. and why only these 2 elements.
0
votes
1answer
2k views

Why do tungsten and chromium have different electronic configurations? [duplicate]

Why is the outer structure of tungsten $\mathrm{5d^46s^2}$ instead of $\mathrm{5d^56s^1}$? I try to explain this in comparison with outer structure of chromium $\mathrm{4d^55s^1}$ taking into ...
3
votes
0answers
1k views

Electron configuration from vanadium to chromium? [duplicate]

The electron configurations for vanadium is: $\ce{1s^2 2s^2 2p^2 3s^2 3p^6 3d^3 4s^2}$, and the electron configuration for chromium is: $\ce{1s^2 2s^2 2p^6 3s^2 3p^6 3d^5 4s^1}$. In looking at the ...
-1
votes
1answer
1k views

Half-Filled Shells and Stability explanation [duplicate]

I am reading a book about Advanced Chemistry, and it is discussing the subject of half-filled orbitals. The book notes that Chromium has an electron structure of $1s^2 2s^2 2p^63s^23p^63d^54s^1$ ...
0
votes
1answer
527 views

Why does electron configuration in the periodic table is different when you follow the aufbau principle? [duplicate]

. In periodic table for example Ag has an electron configuration of [Kr] 4d10,5s1 but when you do it yourself using Aufbau principle it should be [Kr] 5s2 4d9. Why is that? When ask for Ag + valence ...
1
vote
0answers
73 views

Why tungsten does not have stable configuration? [duplicate]

Whenever there are 4 unpaired electrons in d-orbital, elements try to attain stable electronic configuration. For example copper. Electronic configuration of copper should be [Ar]3d4 4s2, but it ...
2
votes
0answers
60 views

Stability of half and fully filled orbitals [duplicate]

1) My textbook tells me that chromium's electronic configuration is $\ce{[Ar]}\space 3d^5 4s^1$ instead of $\ce{[Ar]} \space 3d^4 4s^2$, as fully filled and half filled orbitals have more stability. ...
1
vote
0answers
55 views

Why do Group 10 transition metals (and Cu) lose an S electron to fill the D shell? [duplicate]

I don't understand why it varies between Group 10 metals (as with Palladium, Platinum and Darmstadtium) and Copper (Group 11). If each of Palladium, Platinum and Darmstadtium entirely filled the 3d/4d/...
2
votes
0answers
49 views

Why electron configuration of tungsten doesn't obey the full & half full (stability) rule? [duplicate]

So I was reviewing chemistry lesson and I am curious when I saw the electron configuration in the VIB group: For $\ce{_24Cr}$ we write the electron configuration $\ce{_18[Ar] 4s^1 5d^5}$ instead of $\...
23
votes
2answers
29k views

Why does the 3rd electron shell start filling up with scandium?

The electron configuration of calcium is 2, 8, 8, 2, where up to that point each shell, asides from the first shell counts up to 8 - why then does scandium have an electron configuration of 2, 8, 9, 2?...
12
votes
2answers
23k views

Anomalous electronic configurations

Cu has an anomalous electron configuration. $\ce{Cu ~=~ 1s^2~2s^2~2p^6~3s^2~3p^6~4s^1~3d^{10}}$, it does not follow the usual pattern. In this case, the 3d subshell is filled before the 4s, which ...
3
votes
4answers
25k views

Why are there 14 electrons in the third shell of iron atom?

The third shell must contain at least 18 electrons. But in iron there are 14 electrons in third and 2 electrons in 4th. Why are there 14 electrons in the third shell of iron atom?
3
votes
2answers
15k views

Why do transition metals tend to form positive ions instead of negative ions?

I have learnt that elements on the left-hand side of the periodic table such as sodium and magnesium prefer to lose electrons to form a cation because this requires less energy to obtain a stable ...

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