rank the following atoms in order of effective nuclear charge, from lowest to highest: na, cl, si, al, s. do…

Explanation:

Step1: Recall the formula for effective nuclear charge

The effective nuclear charge (Z_{eff}=Z - S), where (Z) is the atomic number and (S) is the number of shielding electrons. For elements in the same period, the number of shielding electrons (S) is approximately the same (equal to the number of inner - shell electrons). As (Z) (atomic number) increases across a period from left to right, (Z_{eff}) increases.

Step2: Determine the atomic numbers

The atomic numbers are: (Z_{Na}=11), (Z_{Al} = 13), (Z_{Si}=14), (Z_{S}=16), (Z_{Cl}=17).

Step3: Rank based on atomic number (since (S) is similar for same - period elements)

Since (Z_{Na}<Z_{Al}<Z_{Si}<Z_{S}<Z_{Cl}), and (Z_{eff}\propto Z) (for same - period elements with similar (S)), the order of effective nuclear charge is (Na<Al<Si<S<Cl).

Answer:

(Na<Al<Si<S<Cl)