Element W has an electron affinity of ?150 kJ/mol, and element Z has an electron affinity of ?38 kJ/mol. Do the valence electrons in element Z feel a greater effective nuclear charge than those in element W? Explain how you arrived at your answer.

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Tod ThielLv2

25 Aug 2019

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How do you calculate the ionization energy (in kJ/mol) of the He+ ion?

A H- like ion is an ion containing only one electron. The energies of the electron in a hydrogen-like ion are given by $E (n) = - (2.18 \cdot 10^{- 18} J) Z^{2} (\frac{1}{n^{2}})$

where $n$ is the principal quantum number and $Z$ is the atomic number of the element.

magentaraven208

A H^- like ion is an ion containing only one electron. The energies of the electron in a hydrogen-like ion are given by

where n is the principal quantum number and Z is the atomic number of the element. How do you calculate the ionization energy (in kJ/mol) of the He⁺ ion?

pucekoala488

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?