Explain why the first ionization energy tends to increase as one proceeds from left to right across a period. Why is the first ionization energy of aluminum lower than that of magnesium and the first ionization energy of sulfur lower than that of phosphorus?
Answer to relevant QuestionsWhy do the successive ionization energies of an atom always increase? Note the successive ionization energies for silicon given in Table. Would you expect to see any large jumps between successive ionization energies of ...In each of the following sets, which atom or ion has the smallest radius? a. H, He b. Cl, In, Se c. Element 120, element 119, element 117 d. Nb, Zn, Si e. Na-, Na, Na+ In the second row of the periodic table, Be, N, and Ne all have endothermic (unfavorable) electron affinities, whereas the other second- row elements have exothermic (favorable) electron affinities. Rationalize why Be, N, ...It takes 208.4 kJ of energy to remove 1 mole of electrons from the atoms on the surface of rubidium metal. If rubidium metal is irradiated with 254-nm light, what is the maximum kinetic energy the released electrons can ...The following graph plots the first, second, and third ionization energies for Mg, Al, and Si. Without referencing the text, which plot corresponds to which element? In one of the plots, there is a huge jump in energy ...
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