We’re being asked to **calculate the effective nuclear charge (Z _{eff})** of the

Recall that the ** effective nuclear charge** is the force exerted by the nucleus onto an electron and is given by:

$\overline{){{\mathbf{Z}}}_{{\mathbf{eff}}}{\mathbf{}}{\mathbf{=}}{\mathbf{}}{\mathbf{Z}}{\mathbf{}}{\mathbf{-}}{\mathbf{S}}}$

where **Z** = nuclear charge or atomic number and **S** = shielding constant.

For this problem, we need to do the following steps:

*Step 1:* Determine the atomic number.

*Step 2:* Determine the electron configuration and group them by n-values.

*Step 3:* Calculate for the shielding constant using Slater's Rules.

*Step 4:* Calculate for Z_{eff}.

What is the effective nuclear charge (Z_{eff}) felt by a valence electron in a Cl atom?

A) 5

B) 6

C) 7

D) 8

E) 9

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