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Chapter 9: Problem 8

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?

Short Answer

Expert verified
The atomic number of the element where the 6d subshell is filled is 114. The element in the 8th period of group 15 that should resemble Bismuth should be 133. The noble gas in the 8th period of the periodic table should be 136.

Step by step solution

01

Identify atomic number of element where 6d subshell is completed

The first \(4 f\) electron is filled at atomic number 58, then 14 electrons in the \(4 f\) and then another 2 electrons in the \(5 d\) at atomic number 72. The \(6 p\) subshell starts after two more electrons are filled to \(5 d\) i.e. at atomic number 74. So, the \(6 d\) subshell begins at atomic number 104, after the \(5 f\) subshell is completed. As \(6 d\) takes 10 elements to fill up the d sublevel completely. Therefore, 104 + 10 = 114. Thus, atomic number of predicted element which completes \(6 d\) subshell should be 114.
02

Identify element resembling Bismuth

Bismuth is a member of group 15 and is in the 6th period of the Periodic Table. The element that most resembles Bismuth would be found two periods below; in other words, in the 8th period of the Table. The group 15 elements of the 7th period is Moscovium with atomic number 115. Thus, the group 15 elements of the 8th period should have the atomic number 115 + 18 (as there are 18 elements in a period) = 133.
03

Identify noble gas

Noble gases lie in Group 18 of the Periodic Table. The element of Group 18, in the 6th period, is Radon which has atomic number 86. The element of the same group in the 7th period should be element 86 + 32 (since there are 32 elements between the beginning of the 6th period and the beginning of the 7th period) = 118. Similarly, the element of the same group in the 8th period should be 118 + 18 = 136. This is the undiscovered noble gas of Period 8.

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Most popular questions from this chapter

Which of the following ions are likely to be found in chemical compounds: \(\mathrm{Na}^{2+}, \mathrm{Li}^{+}, \mathrm{Al}^{4+}, \mathrm{F}^{2-},\) or \(\mathrm{Te}^{2-} ?\) Explain briefly.

Which of the following ions are unlikely to be found in chemical compounds: \(\mathrm{K}^{+}, \mathrm{Ga}^{4+}, \mathrm{Fe}^{6+} \mathrm{S}^{2-}, \mathrm{Ge}^{5+},\) or \(\mathrm{Br}^{-} ?\) Explain briefly.

The fourth-period element with the largest atom is (a) \(\mathrm{K} ;\) (b) \(\mathrm{Br} ;\) (c) \(\mathrm{Pb} ;\) (d) \(\mathrm{Kr}\).

A method for estimating electron affinities is to extrapolate \(Z_{\text {eff }}\) values for atoms and ions that contain the same number of electrons as the negative ion of interest. Use the data in the table on the next page to answer the questions that follow. $$\begin{array}{lll} \hline \begin{array}{l} \text { Atom or lon: } \\ \text { I(kJmol }^{-1} \text {) } \end{array} & \begin{array}{l} \text { Atom or lon: } \\ \text { I(kJmol }^{-1} \text {) } \end{array} & \begin{array}{l} \text { Atom or lon: } \\ \text { I(kJmol }^{-1} \text {) } \end{array} \\ \hline \text { Ne: 2080 } & \text { F: 1681 } & \text { O: } 1314 \\ \text { Na }^{+}: 4565 & \text { Ne }^{+}: 3963 & \text { F }^{+}: 3375 \\ \text { Mg }^{2+} \text { : 7732 } & \text { Na }^{2+}: 6912 & \text { Ne }^{2+}: 6276 \\ \text { A1 }^{\text {3 }^{+}: 11,577} & \text { Mg }^{3+}: 10,548 & \text { Na }^{3+}: 9540 \\ \hline \end{array}$$ (a) Estimate the electron affinity of \(F\), and compare it with the experimental value. (b) Estimate the electron affinities of \(\mathrm{O}\) and \(\mathrm{N}\) (c) Examine your results in terms of penetration and screening.

Among the following ions, several pairs are isoelectronic. Identify these pairs. \(\mathrm{Fe}^{2+}, \mathrm{Sc}^{3+}, \mathrm{Ca}^{2+}, \mathrm{F}^{-}\) \(\mathrm{Co}^{2+}, \mathrm{Co}^{3+}, \mathrm{Sr}^{2+}, \mathrm{Cu}^{+}, \mathrm{Zn}^{2+}, \mathrm{Al}^{3+}.\)
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