explain why transition elements have similar properties in terms of electronic structure
Answers
Explanation:
The reason that that elements in the same 'group' have similar chemical properties is because they have the same number of valence electrons. ... Iron when reacting in chemical reactions loses electrons from its 4s orbital instead of its d orbital.
Concept: Transition metals are described as elements with partially full d orbitals (or that quickly produce them). Transition elements are the d-block elements in groups 3–11. Because the d orbital is partially occupied before the f orbitals, the f-block elements, also known as inner transition metals (lanthanides and actinides), also meet this condition. The copper family (group 11) fills the d orbitals, hence the next family (group 12) is technically not a transition element. Group 12 elements, on the other hand, share many of the same chemical properties as transition metals and are frequently mentioned in transition metal talks. Some scientists consider the elements of Group 12 to be transition metals.
Explanation: The atoms of the first row transition elements have essentially the same electrical configuration. Starting with scandium, the 3d orbitals gradually fill as the sequence progresses. This filling is irregular, because the population of 3d orbitals increases when an electron from the 4s shell is acquired in chromium and copper. This demonstrates an essential generalisation regarding the first row transition series' orbital energies. Both the 3d and 4s orbitals are occupied in chromium, but neither is totally filled in favour of the other. This indicates that the energies of the 3d and 4s orbitals for atoms in this row are relatively similar.
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