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Chapter 9: Problem 42

For the following groups of elements, select the one that has the property noted: (a) the largest atom: \(\mathrm{Mg}, \mathrm{Mn}, \mathrm{Mo}, \mathrm{Ba}, \mathrm{Bi}, \mathrm{Br}.\) (b) the lowest first ionization energy: \(\mathrm{B}, \mathrm{Sr}, \mathrm{Al}, \mathrm{Br}\) \(\mathrm{Mg}_{\ell} \mathrm{Pb}.\) (c) the most negative electron affinity: \(\mathrm{As}, \mathrm{B}, \mathrm{Cl}\) \(\mathrm{K}, \mathrm{Mg}, \mathrm{S}.\) (d) the largest number of unpaired electrons: \(\mathrm{F}, \mathrm{N}, \mathrm{S}^{2-}, \mathrm{Mg}^{2+}, \mathrm{Sc}^{3+}, \mathrm{Ti}^{3+}.\)

Short Answer

Expert verified
The largest atom is Ba. The element with the lowest first ionization energy is Sr. The element with the most negative electron affinity is Cl. The element with the largest number of unpaired electrons is Ti3+.

Step by step solution

01

Identifying the Largest Atom

Larger atoms are located towards the bottom of the periodic table. Out of the options Mg, Mn, Mo, Ba, Bi, and Br, Ba (Barium) is the furthest down the periodic table, making it the largest atom.
02

Finding the Element with the Lowest First Ionization Energy

The first ionization energy increases across a period and up a group in the periodic table. Thus, the element with the lowest first ionization energy is typically found towards the bottom left of the periodic table. Out of the options B, Sr, Al, Br, Mg, and Pb, Sr (Strontium) is furthest to the left and down, indicating it has the lowest first ionization energy.
03

Determining the Element with the Most Negative Electron Affinity

Electron affinity becomes more negative (indicating a stronger attraction for an added electron) as you move from left to right across a period. Thus, out of options As, B, Cl, K, Mg, and S, Cl (Chlorine) will have the most negative electron affinity.
04

Recognizing the Element with the Largest Number of Unpaired Electrons

The number of unpaired electrons typically corresponds to an element's group number in the periodic table. However, some ions also need to be considered here. For F, N, S, Mg, Sc, and Ti, it's best to refer to the electron configuration. The Ti3+ ion (Titanium) will have an electron configuration of [Ar] 3d1, thus having the largest number of unpaired electrons.

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Most popular questions from this chapter

Mendeleev's periodic table did not preclude the possibility of a new group of elements that would fit within the existing table, as was the case with the noble gases. Moseley's work did preclude this possibility. Explain this difference.

Explain why the several periods in the periodic table do not all have the same number of members.

In your own words, define the following terms: (a) isoelectronic; (b) valence- shell electrons; (c) metal; (d) nonmetal; (e) metalloid.

Consider a nitrogen atom in the ground state and comment on whether the following statements are true or false. (a) \(\mathrm{Z}_{\text {eff }}\) for an electron in a 2 s orbital is greater than that for the 1 s orbital. (b) The \(Z_{\text {eff for the } 2 p \text { and } 2 s \text { orbitals is the same. }}\) (c) More energy is required to remove an electron from a 2 s orbital than from the \(2 p\) orbital. (d) The 2 s electron is less shielded than the \(2 p\) electron.

Concerning the incomplete seventh period of the periodic table, what should be the atomic number of the element (a) for which the filling of the \(6 d\) subshell is completed; (b) that should most closely resemble bismuth; (c) that should be a noble gas?
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