Use the periodic table to identify the element with each electron configuration.
(a) \([N e] 3 s^{2} 3 p^{5}\)
(b) \([A r] 4 s^{2} 3 d^{10} 4 p^{1}\)
(c) \([A r] 4 s^{2} 3 d^{6}\)
(d) \([K r] 5 s^{1}\)
Equation Transcription:
Text Transcription:
[Ne]3s^2 3p^5
[Ar]4s^2 3d^10 4p^1
[Ar]4s^2 3d^6
[Kr]5s^1
Solution 75P
Here, we have to identify the element with each configuration.
(a) [Ne]3s23p5
The atomic number of the element is 17
From electronic configuration, valence electron of the element = 7
Thus, it is an element of Group 17 (VIIA).
Therefore, the name of the element is Chlorine (Cl).
(b) [Ar]4s23d104p1
The atomic number of the element is 31
From electronic configuration, valence electron of the element = 3
Thus, it is an element of Group 13 (IIIA).
Therefore, the name of the element is Gallium (Ga).
(c) [Ar]4s23d6
The atomic number of the element is 26
From electronic configuration, valence electron of the element = 8
Thus, it is an element of Group 8 (8B).
Therefore, the name of the element is Iron (Fe).
(d) [Kr]5s1
The atomic number of the element is 37
From electronic configuration, valence electron of the element = 1
Thus, it is an element of Group I (IA).
Therefore, the name of the element is Rubidium (Rb).
