Chapter 6: Q.86E. (page 338)
Explain why Al is a member of group 13 rather than group 3?
Aluminum falls in the p block, in which elements have 3 valence electrons in the p orbital and group 13 has a single electron in a subshell.
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Based on their positions in the periodic table, rank the following atoms in order of increasing first ionization energy: F, Li, N, Rb
Which of the following atoms and ions is (are) isoelectronic with\({{\bf{S}}^{{\bf{2}} + }}:{\rm{ }}{\bf{S}}{{\bf{i}}^{4 + }}{\rm{ ,}}{\bf{C}}{{\bf{l}}^{{\bf{3}} + }},{\rm{ }}{\bf{Ar}},{\rm{ }}{\bf{A}}{{\bf{s}}^{{\bf{3}} + }},{\rm{ }}{\bf{Si}},{\rm{ }}{\bf{A}}{{\bf{l}}^{{\bf{3}} + }}\)?
Atoms of which group in the periodic table have a valence shell electron configuration of\({\bf{n}}{{\bf{s}}^{\bf{2}}}{\bf{n}}{{\bf{p}}^{\bf{3}}}\)?
Give an example of an atom whose size is smaller than fluorine.
Question:Read the labels of several commercial products and identify monatomic ions of at least six main groupelements contained in the products. Write the complete electron configurations of these cations and anions.
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