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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.

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Zeff is a good nuclear charge and is calculated by the formula:

Zeff = Z - S

Z refers to the quantity of protons and S is that the Slater constant.

Further Explanation

Cations have 11 protons, the quantity of core electrons in sodium-ion is 2.

If the core electron accounts for 1.00 and also the negatron accounts for 0.00 then S = 2 for both ions.

Therefore, for Na⁺, Zeff = 11 - 2 = 9

The F⁻ ion has 9 protons, the quantity of core electrons within the F⁻ ion is 2. Therefore, for F⁻: Zeff = 9 - 2 = 7

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

On the premise of Slater's rule, for s and p orbitals, electrons within the same shell contribute 0.35 and electrons within the n-1 shell contribute 0.85.

S = (0.85 × 2) + (0.35 × 7)

= 4.15

Therefore, per Slater's rules,

For Na⁺, Zeff = 11 - 4.15 = 6.85

For F⁻, Zeff = 9 - 4.15 = 4.85

Thus, Zeff for Na⁺ and F⁻ calculated per Slater's rules is 6.85 and 4.85, respectively.

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Zeff  https://brainly.com/question/11629172#

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Details

Grade: College

Subject: Chemistry

Keyword: Zeff, cations, core

pstnonsonjoku

Na^+ is smaller than F^- ion.

The electron configuration of Na^+ is; 1s2 2s2 2p6

The electron configuration of F^- is; 1s2 2s2 2p6

We know from Slater's rule that; Zeff = Z - S

To calculate the screening (S);

The electrons in the same ns np shell contribute 0.35

The electrons in the next (n - 1) shell contribute 0.85

The electrons in the lower (n - 2) shells contribute 1.00

For an outermost electron in Na^+;

S = 7(0.35) + 2(0.85)

S = 2.45 + 1.7

S = 4.15

For an outermost electron in F^-

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

S = 2.45 + 1.7

S = 4.15

We know that;

Z = 11 for Na^+

Z = 9 for F^-

Hence

Zeff for Na^+ = 11 - 4.15 = 6.85

Zeff for F^- = 9 - 4.15 = 4.85

Note that the smaller the value of Zeff the larger the ion hence the F^- is larger than Na^+ ion. So Na^+ is smaller than  F^-.

Learn more: https://brainly.com/question/6505878

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