Detailed calculations show that the value of Zeff for the outermost electrons in Na and K atoms is 2.51 + and 3.49 +, respectively. (a) What value do you estimate for Zeff experienced by the outermost electron in both Na and K by assuming core electrons contribute 1.00 and valence electrons contribute 0.00 to the screening constant? (b) What values do you estimate for Zeff using Slater's rules? (c) Which approach gives a more accurate estimate of Zeff? (d) Does either method of approximation account for the gradual increase in Ziff that occurs upon moving down a group? (e) Predict Zeff for the outermost electrons in the Rb atom based on the calculations for Na and K.
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Student Solutions Manual To Black Exercises For Chemistry: The Central Science
- 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?arrow_forwardUsing Slater’s rule, determine Z* for a.) a 2p electrons in O2-, F- , Na+ and Mg2+. Is the calculated value of Z* consistent with the relative sizes of these atoms? b.) a 4f electrons in Ce, Pr and Nd. There is a decrease in size, commonly known as the Lanthanide contraction, with increasing atomic number in lanthanides. Are your values of Z* consistent with this trend?arrow_forwardit is clear that the first ionization energy of He is very large. Would you expect the first ionization energy of H– (hydride ion) to be larger, smaller, or about the same as the first ionization energy of He, and why?arrow_forward
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- Chemistry: The Molecular ScienceChemistryISBN:9781285199047Author:John W. Moore, Conrad L. StanitskiPublisher:Cengage Learning