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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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Question:Use an orbital diagram to describe the electron configuration of the valence shell of each of the following
atoms:
(a) N
(b) Si
(c) Fe
(d) Te
(e) Mo
Describe the properties of an electron associated with each of the following four quantum numbers:n,l,ml, andms.
Which ion with a +2 charge has the electron configuration\({\bf{1}}{{\bf{s}}^{\bf{2}}}{\bf{2}}{{\bf{s}}^{\bf{2}}}{\bf{2}}{{\bf{p}}^{\bf{6}}}{\bf{3}}{{\bf{s}}^{\bf{2}}}{\bf{3}}{{\bf{p}}^{\bf{6}}}{\bf{3}}{{\bf{d}}^{{\bf{10}}}}{\bf{4}}{{\bf{s}}^{\bf{2}}}{\bf{4}}{{\bf{p}}^{\bf{6}}}{\bf{4}}{{\bf{d}}^{\bf{5}}}\)? Which ion with a +3 charge has this configuration?
Question:What additional information do we need to answer the question “Which ion has the electron configuration1s22s22p63s23p6”?
Identify the atoms from the electron configurations given:
(a)\(\left( {{\bf{Ar}}} \right){\bf{4}}{{\bf{s}}^{\bf{2}}}{\bf{3}}{{\bf{d}}^{\bf{5}}}\)
(b)\(\left( {{\bf{Kr}}} \right){\bf{5}}{{\bf{s}}^{\bf{2}}}{\bf{4}}{{\bf{d}}^{{\bf{10}}}}{\bf{5}}{{\bf{p}}^{\bf{6}}}\)
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