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Consider the isoelectronic ions F- and Na +. (a) Which ion
Chapter , Problem 7.31(choose chapter or problem)
Consider the isoelectronic ions F- and Na +. (a) Which ion is smaller? (b) Using Equation 7.1 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. (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 F- and Na +. (a) Which ion is smaller? (b) Using Equation 7.1 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. (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:- +Consider the isoelectronic ions F and Na . (a) Which ion is smaller (b) Using Equation 7.1 and assuming that core electrons contribute 1.00 and valence electrons contribute 0.00 to the screening constant, S , calculate Z feffthe 2p electrons in both ions. (c) Repeat this calculation using Slater's rules to estimate the screening constant, S. (d) For isoelectronic ions, how are effective nuclear charge and ionic radius related Step-by-step solution Step 1 of 4 (a) - +The F and Na ions are isoelectronic. Both of them have a total of 10 electrons. For isoelectronic ions, the ion with greater atomic number has smaller size. The effective + -nuclear charge is more in Na ion than F Therefore, sodium ion Na is smaller than fluoride ion F . -