a) Define the term ionization energy.

b) What is the trend of first ionization energy across period

c) Identify two elements with larger first ionization energies than chlorine

d) Define the term 2nd ionization energy of element A using equation

e) Explain why Li, Na, and K have the highest 2nd ionization energies of the first 20 elements

f) Consider the following three ions, , and . Which ion would you expect to have the smallest radius?

g) State the electron configuration for

h) Which is larger, Zr atom or a ?

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2 Jun 2021

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Hydrogen is an unusual element because it behaves in some ways like the alkali metal elements and in other ways like nonmetals. Its properties can be explained in part by its electron configuration and by the values for its ionization energy and electron affinity. (a) Explain why the electron affinity of hydrogen is much closer to the values for the alkali elements than for the halogens. (b) Is the following statement true? “Hydrogen has the smallest bonding atomic radius of any element that forms chemical compounds.” If not, correct it. If it is, explain in terms of electron configurations. (c) Explain why the ionization energy of hydrogen is closer to the values for the halogens than for the alkali metals. (d) The hydride ion is H^–. Write out the process corresponding to the first ionization energy of the hydride ion. (e) How does the process in part (d) compare to the process for the electron affinity of a neutral hydrogen atom?