Firstly, I would like to know whether the followingdefinitions are correct, (i)
ID: 691587 • Letter: F
Question
Firstly, I would like to know whether the followingdefinitions are correct, (i) electron shell: collection of orbitals with the sameprincipal quantum number (n) (ii) outermost shell (of an atom in its ground state): theshell with the largest principal quantum number. Now take Argon for example, to my understanding, the outermostshell of Argon will include the 3s, 3p, and 3d orbitals. Is thiscorrect?? If not, please explain why 3d orbitals are not part ofthe outermost shell. If I were correct, that is, the outermost shell of Argonincludes 3s, 3p, and 3d orbitals, then WHY DO WE OFTEN SEE PEOPLESAYING THAT ARGON HAS A FULL OUTER SHELL??? Because it is obvious to me that the 3d orbitals aren'tfilled. I hope I have put out the question clearly......I would bevery grateful if anyone could offer me some guidance....pleaselet me know if you need further clarification to theproblem. THANKS Firstly, I would like to know whether the followingdefinitions are correct, (i) electron shell: collection of orbitals with the sameprincipal quantum number (n) (ii) outermost shell (of an atom in its ground state): theshell with the largest principal quantum number. Now take Argon for example, to my understanding, the outermostshell of Argon will include the 3s, 3p, and 3d orbitals. Is thiscorrect?? If not, please explain why 3d orbitals are not part ofthe outermost shell. If I were correct, that is, the outermost shell of Argonincludes 3s, 3p, and 3d orbitals, then WHY DO WE OFTEN SEE PEOPLESAYING THAT ARGON HAS A FULL OUTER SHELL??? Because it is obvious to me that the 3d orbitals aren'tfilled. I hope I have put out the question clearly......I would bevery grateful if anyone could offer me some guidance....pleaselet me know if you need further clarification to theproblem. THANKSExplanation / Answer
We generally know that inert gas elements are moststable because they have completely filled electrons intheir orbitals In the example of Ar which has theelectronic configuration as 1s2 2s22p6 3s2 3p6 it hascompletely filled 3p orbital as comparing to the energy the energy of 4s orbital has lower energy than 3d orbital so the concept of thefillingthe electrons in 3d orbital is not thecase for the main group elements. In thecase of transition element like Zn which has the electronconfiguration as 1s2 2s2 2p6 3s23p6 4s2 3d10 4p as in the case of Zinc their is a vacant4p orbitals available for Zn so in order to attain the stable electronic configuration Zn tends to lose thevalence two electrons present in the 4s shell being lostthat electrons it attains the stability so Zn is reactive than Arwhich has completely filled electrons in the shells. Hope this explanation helps still if you have any doubt let me knowso that i can help you.Related Questions
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