Do all transition metals have the n2 and (n-1)d orbitals?

In summary, there is no clear consensus on whether all transition metals have their n2 and (n-1)d orbitals as valence electrons. Some sources suggest that this is the case, while others claim that only certain transition metals follow this pattern. The formal oxidation number may be used as an indication of the number of valence electrons, but this can vary depending on the specific element. Ultimately, there is no definitive answer and more research is needed to fully understand the valence electrons of transition metals.
  • #1
Silhorn
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Does all transition metals have their n2 and ( n-1)d orbitals as valence electrons?
I have been scouring the internet to the answer of this question but have mixed results.
Iron has an electron configuration of: 1s2,2s2,2p6,3s2,3p6,4s2,3d6
Aparantly it has 8 valence electrons because 4s2 + 3d6 = 8 electrons.
Nickel has an electron configuration of: 1s2,2s2,2p6,3s2,3p6,4s2,3d8
Some people say it has 10 valence electrons because 4s2 + 3d8 = 10 electrons.
And some other people say it is wrong, it only has 2 valence electrons because the d orbital is in the 3rd energy level.

And then I come across another thing saying only certain transition metals you count the electrons in the n2 and ( n-1)d orbitals and the rest is just count the electrons in the outside shell as normal. This seems to be the solution but am I right and which ones?

Could someone clear this up for me?
 
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  • #2
There is no clear-cut difference between valence and non-valence electrons. With d-group elements, you may consider the formal oxidation number as an indication of the number of valence electrons. As d-electrons become more tightly bound to the nucleus the farther right you move in the period and the farther up you move in the column, in the first period, the maximal oxidation number is reached with + VII with manganum which hence uses all its 4s and 3d electrons. Its right neighbour, iron, has a maximal oxidation number of +VI, and not VIII so that it can't use all its 4s and 3d electrons. On the other hand, in the 3rd long period, the maximal oxidation number is reached with Iridium with +IX while its right neighbour, Platin, only reaches +VI.
 
  • #3
Ok, I understand.
Thanks for the help.
 

1. What are transition metals?

Transition metals are a group of elements located in the middle of the periodic table, between the highly reactive alkali metals and the relatively unreactive noble gases. They are characterized by their ability to form multiple oxidation states and their partially filled d orbitals.

2. What is the significance of the n2 and (n-1)d orbitals in transition metals?

The n2 and (n-1)d orbitals refer to the outermost electron shell and the second-to-outermost electron shell, respectively. In transition metals, these orbitals are only partially filled, giving these elements unique properties such as high melting and boiling points, the ability to form complex compounds, and catalytic activity.

3. Do all transition metals have the n2 and (n-1)d orbitals?

Yes, all transition metals have the n2 and (n-1)d orbitals. This is because these elements have atomic numbers greater than 20, meaning their electron configurations include electrons in the n=2 and n=3 energy levels.

4. Are there any exceptions to the presence of n2 and (n-1)d orbitals in transition metals?

No, there are no exceptions to the presence of n2 and (n-1)d orbitals in transition metals. These orbitals are a defining characteristic of this group of elements and are present in all of them.

5. How do the n2 and (n-1)d orbitals contribute to the properties of transition metals?

The partially filled n2 and (n-1)d orbitals in transition metals allow for the formation of strong metallic bonds, which contribute to their high melting and boiling points. These orbitals also allow for the formation of complex compounds, which gives transition metals their characteristic bright colors and catalytic activity.

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