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Chapter 9: Problem 77

The element whose atoms have the electron configuration \([\mathrm{Kr}] 4 d^{10} 5 \mathrm{s}^{2} 5 p^{3}(\mathrm{a})\) is in group 13 of the periodic table; (b) bears a similarity to the element Bi; (c) is similar to the element \(\mathrm{Te} ;\) (d) is a transition element.

Short Answer

Expert verified
The element is Thallium (Tl). (a) It's in group 13; (b) It shares group properties with Bi as it's in the same group; (c) It has similar size and same number of energy levels as Te as they are in the same period; (d) Tl isn't a transition element as it's in the p-block.

Step by step solution

01

Identifying the Element

Using the given electron configuration \([\mathrm{Kr}] 4d^{10} 5s^{2} 5p^{3}\), let's identify the element. The electron configuration belongs to the element thallium (Tl). The outermost electron shell configuration is \(5s^{2} 5p^{3}\), which is the structure in group 13.
02

Comparison with Bi

Checking the similarity to Bi (bismuth), we can see that Bi is also in group 15 of the Periodic Table like Tl, which means they share the same group properties.
03

Comparison with Te

Te (tellurium) is in the same period (5th period) as Tl. Elements in the same period have the same number of electron shells. So, Tl and Te will have similar size and same number of energy levels.
04

Checking for Transition Element

Transition elements are found in the d-block of the periodic table. However, Tl is found in the p-block, hence, it is not a transition element.

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Most popular questions from this chapter

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.

Briefly describe each of the following ideas or phenomena: (a) the periodic law; (b) ionization energy; (c) electron affinity; (d) paramagnetism.

Is it possible for two different atoms to be isoelectronic? two different cations? two different anions? a cation and an anion? Explain.

In estimating the boiling point and melting point of bromine in Example \(9-5,\) could we have used Celsius or Fahrenheit instead of Kelvin temperature? Explain.

Two elements, \(A\) and \(B\), have the electron configurations shown. $$ \mathrm{A}=[\mathrm{Kr}] 4 s^{2} \quad \mathrm{B}=[\mathrm{Ar}] 3 d^{10} 4 s^{2} 4 p^{5} $$ (a) Which element is a metal? (b) Which element has the greater ionization energy? (c) Which element has the larger atomic radius? (d) Which element has the greater electron affinity?
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