Consider the isoelectronic ions f - and na+. part a which ion is smaller? f - na + submitmy answersgive up correct part b using the equation zeff=z-s and assuming that core electrons contribute 1.00 and valence electrons contribute 0.00 to the screening constant, s, calculate zeff for the 2p electrons in both ions. express your answers as integers. enter your answers numerically separated by a comma. zeff f-, zeff na + = 7,9 e - submitmy answersgive up correct part c repeat this calculation using slater's rules to estimate the screening constant, s. express your answers using two decimal places. enter your answers numerically separated by a comma.

Zeff is the effective nuclear charge and is calculated by the formula:

Zeff = Z - S

Z refers to the number of protons and S is the Slater's constant.

Na⁺ cation has 11 protons, the number of core electron in sodium ion are 2.

If the core electrons donates 1.00 and the valence electrons donate 0.00 then S = 2 for both the ions.

Hence, for Na⁺, Zeff = 11 - 2 = 9

F⁻ ion has 9 protons, the number of core electrons in F⁻ ion are 2. Hence, for F⁻ : Zeff = 9 - 2 = 7

Therefore, Zeff for Na⁺ and F⁻ are 9 and 7 respectively.

On the basis of Slater's rules, for s and p orbitals, the electrons in the similar shell donates 0.35 and the electrons in the n - 1 shell donates 0.85.

S = (0.85 * 2) + (0.35 * 7)

= 4.15

Hence, according to Slater's rule,

For Na⁺, Zeff = 11 - 4.15 = 6.85

For F⁻, Zeff = 9 - 4.15 = 4.85

Thus, Zeff for Na⁺ and F⁻ calculated on the basis of Slater's rules are 6.85 and 4.85 respectively.