(a) What trends, if any, exist for Z(eff )across a period and downa group? (b) How does Z(eff) influence atomic size, IE₁, and EN across a period?
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(a) What trends, if any, exist for Z(eff )across a period and downa group? (b) How does Z(eff) influence atomic size, IE₁, and EN across a period?
Z(eff) is the net attractive force exerted by the nucleus on the valence electrons.
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- Describe and account for the variation of first ionizationenergies along Period 2 of the periodic table . Would you expect the same variation in Period 3?The electron affinities, in kJ>mol, for the group 1B and group2B metals are as follows: (a) Why are the electron affinities of the group 2B elementsgreater than zero? (b) Why do the electron affinities of thegroup 1B elements become more negative as we move downthe group? [Hint: Examine the trends in the electron affinitiesof other groups as we proceed down the periodic table.]A ground-state atom of iron has _____ unpaired electron and is _________a. 0, diamagneticb. 6, diamagneticc. 3, paramagneticd. 4, paramagnetice. 5, paramagnetic
- Describe and account for the variation of fi rstionization energies along Period 2 of the periodic table. Would you expect the same variation in Period 3?it 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?Why is the electronic configuration of the yttrium atom [Kr]4d15s2 and that of the silver atom [Kr]4d105s 1?
- Using 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?Describe the variation of first ionisation energy moving across Period 3, from left to rightwhat are likely possibilies for X if Xn + Cl -> XCl2 can you help explain how to solve this? Would it be any element in the 2nd s2 row (Be, Mg, Ca, Sr, Ba, Ra)?
- Would you expect a tin atom to be paramagnetic or diamagnetic? Explain briefly.Silver and rubidium both form +1 ions, but silver is far lessreactive. Suggest an explanation, taking into account theground-state electron configurations of these elements andtheir atomic radii.Using Slater's Rules, calculate Zeff for the outermost s electron of vanadium, V(0)