How the effective nuclear charge (Zeff) experienced by a valence electron in tin (Sn) compare to the Zeff experienced by a valence electron in tellurium (Te)? Why is this true? Relative Zeff Explanation of Difference A) Tin has larger Zeff Tin is farther to the left on the periodic table, which is the physical reason that it has a larger Zeff. B) Tin has larger Zeff Tin has the same number of core electrons as polonium but fewer valence electrons, so there is less repulsion in the valence shell. C) Tin has smaller Zeff Tin is farther to the left on the periodic table, which is the physical reason that it has a smaller Zeff. D) Tin has smaller Zeff Tin has the same number of core electrons as polonium but fewer protons, so the “net” positive charge attracting valence electrons is smaller. E) Zeff(Sn) = Zeff(Te) Tin and tellurium are in the same row of the periodic table, so they have the same effective nuclear charge.
How the effective nuclear charge (Zeff) experienced by a valence electron in tin (Sn) compare to the Zeff experienced by a valence electron in tellurium (Te)? Why is this true?
Relative Zeff Explanation of Difference
A) Tin has larger Zeff
Tin is farther to the left on the periodic table, which is the physical reason that it has a larger Zeff.
B) Tin has larger Zeff
Tin has the same number of core electrons as polonium but fewer valence electrons, so there is less repulsion in the valence shell.
C) Tin has smaller Zeff
Tin is farther to the left on the periodic table, which is the physical reason that it has a smaller Zeff.
D) Tin has smaller Zeff
Tin has the same number of core electrons as polonium but fewer protons, so the “net” positive charge attracting valence electrons is smaller.
E) Zeff(Sn) = Zeff(Te)
Tin and tellurium are in the same row of the periodic table, so they have the same effective nuclear charge.
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