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Chapter 8: Problem 20

Specify in what group of the periodic table each of these elements is found: (a) [Ne]3s", (b) \([\mathrm{Ne}] 3 s^{2} 3 p^{3}\) (c) \([\mathrm{Ne}] 3 s^{2} 3 p^{6}\) (d) \([\mathrm{Ar}] 4 s^{2} 3 d^{8}\)

Short Answer

Expert verified
The elements specified in cases (a), (b), (c) and (d) belong to Group 1, Group 16, Group 18 and Group 10 of the periodic table, respectively.

Step by step solution

01

Identifying Group - Case (a)

The electron configuration provided is [Ne]3s. This indicates that the electron being referred to is in the third energy level (period) and is filling the 's' orbital. Since it only states '3s' with no superscript, we'd assume it's '3s^1'. This is the first electron in the 3s orbital section. Hence, this element belongs to Group 1 in the periodic table.
02

Identifying Group - Case (b)

The electron configuration provided is \([\mathrm{Ne}] 3 s^{2} 3 p^{3}\). This indicates that the outermost electrons are in 'p' orbitals with 3 of them (3p^3) in the third energy level. Since the 'p' block groups start from 13 extending to 18, we add the number of p electrons to the starting number 13. So, 13 + 3 equals 16. Thus, this element belongs to Group 16 in the periodic table.
03

Identifying Group - Case (c)

The electron configuration provided is \([\mathrm{Ne}] 3 s^{2} 3 p^{6}\). The element has a complete 'p' orbital in the third energy level. Hence, it is located in group 18, the noble gases.
04

Identifying Group - Case (d)

The electron configuration provided is \([\mathrm{Ar}] 4 s^{2} 3 d^{8}\). It indicates that these are transition metals with 2 electrons in the 4s subshell, and 8 electrons in the 3d subshell. This is somewhat a special case. In transition metals we have to take count of both 's' and 'd' electrons. So, it is 2 + 8 equals 10. The count of 10 implicates that the element is in Group 10 of the periodic table.

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