Transisiton metal electronic structure question.

In summary, the conversation discusses the electronic structure of transition metals, specifically the idea that Chromium and Copper donate one of their electrons from the 4s sub-shell to the 3d sub-shell. The question is whether this is true for all transition metals. It is noted that there are exceptions among heavier elements and additional resources are recommended for further reading on the topic of electron configurations.
  • #1
MattA147
14
0
Transisiton metal electronic structure question. :)

Hey guys, basically I know that Chromium and Copper "donate" one of their electrons from the 4s sub-shell to the 3d sub-shell. Is this true for ALL transition metals?

Any help would be greatly appreciated. :)
 
Chemistry news on Phys.org
  • #2


There are a number of heavier elements that are exceptions. You can find further reading on this topic "en.wikipedia.org/wiki/Electron_configuration" and "chemwiki.ucdavis.edu/Inorganic_Chemistry/Electronic_Configurations" . While the explanation of filled and half-filled shells being favorable applies for copper and chromium in a fairly transparent manner, it becomes a far more complicated matter for other elements.
 
Last edited by a moderator:

1. What is the electronic structure of transition metals?

The electronic structure of transition metals is characterized by the presence of partially filled d orbitals. This allows for the formation of multiple oxidation states and the ability to form complex compounds.

2. How do transition metals differ from other elements in terms of electronic structure?

Transition metals have an incomplete d subshell, which gives them unique properties such as high melting and boiling points, variable oxidation states, and the ability to form colorful compounds.

3. Why are transition metals good catalysts?

Transition metals have the ability to easily donate and accept electrons due to their partially filled d orbitals. This allows them to participate in a variety of chemical reactions, making them effective catalysts.

4. How does the electronic structure of transition metals affect their physical properties?

The presence of partially filled d orbitals in transition metals results in strong metallic bonding, leading to high melting and boiling points. The ability to form multiple oxidation states also contributes to their diverse range of physical properties.

5. How does the electronic structure of transition metals impact their chemical reactivity?

The electronic structure of transition metals allows them to easily donate and accept electrons, making them highly reactive. This reactivity is further enhanced by their ability to form multiple oxidation states and complex compounds.

Similar threads

Selection rules in electron transitions
    • Chemistry
Replies
2
Views
1K
Reactivity Series: How to Understand Metal Reactions
    • Chemistry
Replies
1
Views
1K
Why do transition metal ions lose s electrons first?
    • Chemistry
Replies
2
Views
30K
Chemistry How do we know ##BF_3## has Lewis structure but ##Al_2S_3## does not?
    • Biology and Chemistry Homework Help
Replies
1
Views
627
I Questions about my Understanding of Thermodynamics and Statistical Mechanics
    • Thermodynamics
Replies
2
Views
480
B Conductors in the triboelectric series
    • Electromagnetism
Replies
2
Views
797
Calculating Collision Frequency of Electrons in Copper Cube
    • Introductory Physics Homework Help
Replies
2
Views
984
Electron shell, Oxidation number
    • Chemistry
Replies
1
Views
1K
Work function of electrons in a metal
    • Introductory Physics Homework Help
Replies
3
Views
908
A Yes, there is a typo. The correct electronic configuration for Yb+ is 4f146s.
    • Atomic and Condensed Matter
Replies
1
Views
1K

Hot Threads

Recent Insights

Back
Top