Answer: Two electron configurations of elements that would have similar chemical properties are (2) and (4).
Explanation:
(1) [tex]1s^22s^22p^4[/tex]
(2) [tex]1s^22s^22p^5[/tex]
(3) [tex][Ar]4s^23d^5[/tex]
(4) [tex][Ar]4s^23d^{10}^4p^5[/tex]
Valence electrons : These are the electrons present in last principal quantum number of an atom of the element.
Two electron configurations represent elements that would have similar chemical properties are (2) and (4). This is because number of valence electrons present in both of them are same that is seven valence electrons . Also valence electrons of both the elements are present in p-orbital which means that they both belongs to same group in a periodic table. The members of same group in a periodic table have similar chemical properties.
Electronic configuration of a chemical element is the distribution of electrons of an atom in it's atomic orbit.
Names of elements with the electronic configuration above:
Electronic configuration which have thesame chemical properties above are:
2. Flourine - 1s² 2s² 2p5 and
Flourine - 1s² 2s² 2p5 and4. Bromine - {Ar} 4s² 3d10 4p5
Because elements in thesame group have thesame number of valence electrons. In this case, the number of valence electrons is 7.
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