7.16 Consider the isoelectronic ions F and Nat. (a) Which ion issmaller? (b) Using Equation 7.1 and assuming that core elec-trons contribute 1.00 and valence electrons contribute 0.00to the screening constant, S, calculate Zeff for the 2p electronsin both ions. (c) Repeat this calculation using Slater's rules toestimate the screening constant, S. (d) For isoelectronic ions,how are effective nuclear charge and ionic radius related?

A. Na+ is the smallest as it has lost an electron from its outermost shell thereby pulled a bit more…

Answered: 7.16 Consider the isoelectronic ions F…

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter5: Electron Configurations And The Periodic Table

Section: Chapter Questions

Problem 117QRT

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Which element would you expect to be less metallic?(a) Sb or As(b) Si or P(c) Be or Na
(ii) How would you expect the second ionization energies for Na and Mg to compare? Explain using both a qualitative and quantitative (Slater’s rules) argument. (iii) Does your answer for (ii) correspond to what you know about the common ions formed by Na and Mg? Explain.
Consider the isoelectronic ions Cl- and K+. (a) Which ionis smaller? (b) Using Equation 7.1 and assuming that coreelectrons contribute 1.00 and valence electrons contributenothing to the screening constant, S, calculate Zeff for thesetwo ions. (c) Repeat this calculation using Slater’s rules toestimate the screening constant, S. (d) For isoelectronic ions,how are effective nuclear charge and ionic radius related?
There are some exceptions to the trends of first and succes-sive ionization energies. For each of the following pairs, explainwhich ionization energy would be higher:(a) IE₁ of Ga or IE₁ of Ge(b) IE₂ of Ga or IE₂ of Ge(c) IE₃ of Ga or IE₃ of Ge(d) IE₄ of Ga or IE₄ of Ge
3. Which one of each of the following pairs has the higher electron affinity? Explain in detail for each case. (a) C or F (b) F or I (c) Te or I (d) O or S (e) S or Se
Arrange in order of increasing ionization energy. (Use the appropriate <, =, or > symbol to separate substances in the list.) (a) the Group 1A elements Na, H, and Li (b) the Period 4 elements Ga, Se, and K
Detailed calculations show that the value of Zeff for theoutermost electrons in Na and K atoms is 2.51+ and 3.49+,respectively. (a) What value do you estimate for Zeff experiencedby the outermost electron in both Na and K byassuming core electrons contribute 1.00 and valence electronscontribute 0.00 to the screening constant? (b) Whatvalues do you estimate for Zeff using Slater’s rules? (c) Whichapproach gives a more accurate estimate of Zeff? (d) Doeseither method of approximation account for the gradualincrease in Zeff that occurs upon moving down a group?(e) Predict Zeff for the outermost electrons in the Rb atombased on the calculations for Na and K.
Select the ions or atoms from the following sets that are isoelectronic with each other. (a) (b) (c) Fe²+ Cu³+ Ni2+ AP+ p.J. Na+ DRb (d) Br Cs' 82. mut Na
Predict the larger ion in each of the following pairs. Give reasons for your answers. (a) S²-, Cl- (c) Ce*, Dy³+ (b) TI*, TI³+ (d) S","
Which element would you expect to be less metallic?(a) Cs or Rn(b) Sn or Te(c) Se or Ge
Predict the larger ion in each of the following pairs. (a) K* or CI (b) Fe3+ or Fe2+ (c) N or N3- (d) I or F
Identify the true statements concerning the atoms andions of the group 6A elements. (a) The ionic radii are larger than the atomic radii becausethe ions have more electrons than their correspondingatoms.(b) Atomic radii increase going down the group because ofincreasing nuclear charge.(c) The ionic radii increase going down the group becauseof the increase in the principal quantum number ofoutermost electrons.(d) Of these ions, Se2- is the strongest base in water becauseit is largest.

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