Question: Why do the successive ionization energies of an atom always
Why 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 silicon as you removed all the electrons, one by one, beyond those shown in the table?
Answer to relevant QuestionsThe radius trend and the ionization energy trend are exact opposites. Does this make sense? Define electron affinity. Electron affinity values are both exothermic (negative) and endothermic (positive). However, ionization ...The first ionization energies of As and Se are 0.947 MJ/ mol and 0.941 MJ/mol, respectively. Rationalize these values in terms of electron configurations. The electron affinities of the elements from aluminum to chlorine are 244 kJ/ mol, 2120 kJ/ mol, 274 kJ/ mol, 2200.4 kJ/ mol, and 2348.7 kJ/ mol, respectively. Rationalize the trend in these values. Elements with very large ionization energies also tend to have highly exothermic electron affinities. Explain. Which group of elements would you expect to be an exception to this statement? Using data from this chapter, calculate the change in energy expected for each of the following processes. a. Na(g) + Cl(g) → Na+(g) + Cl-(g) b. Mg(g) + F(g) → Mg+(g) + F-(g) c. Mg+(g) + F(g) → Mg2+(g) + F-(g) d. Mg(g) ...
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