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Consider the isoelectronic ions Cl - and K+. (a) Which ion
Chapter , Problem 7.32(choose chapter or problem)
Consider the isoelectronic ions Cl - and K+. (a) Which ion is smaller? (b) Using Equation 7.1 and assuming that core electrons contribute 1.00 and valence electrons contribute nothing to the screening constant, S, calculate Zeff for these two ions. (c) Repeat this calculation using Slaters rules to estimate the screening constant, S. (d) For isoelectronic ions, how are effective nuclear charge and ionic radius related?
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QUESTION:
Consider the isoelectronic ions Cl - and K+. (a) Which ion is smaller? (b) Using Equation 7.1 and assuming that core electrons contribute 1.00 and valence electrons contribute nothing to the screening constant, S, calculate Zeff for these two ions. (c) Repeat this calculation using Slaters rules to estimate the screening constant, S. (d) For isoelectronic ions, how are effective nuclear charge and ionic radius related?
ANSWER:Problem 7.32Consider the isoelectronic ions Cl and K . (a) Which ion is smaller (b) Using Equation 7.1 andassuming that core electrons contribute 1.00 and valence electrons contribute nothing to thescreening constant, S, calculate Z efffor these two ions. (c) Repeat this calculation using Slater'srules to estimate the screening constant, S. (d) For isoelectronic ions, how are effective nuclearcharge and ionic radius related Step-by-step solution Step 1 of 4 ^ + - +(a) The K ion is smaller than Cl . The effective nuclear charge is more on K ion by the nucleus.So attraction of the nucleus on the valency electron is more so distance between themdecreases. So K is smaller. But in the case of Cl ion an extra electron is added to the valencyshell. So repulsions expand the electron cloud with an increase in the size.