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Chapter 9: Problem 61

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?

Short Answer

Expert verified
(a) B is the metal. (b) A has a greater ionization energy. (c) A has a larger atomic radius. (d) B has a greater electron affinity.

Step by step solution

01

Identify the element is a metal

The rule is that any atom with an unfilled electron shell is considered a metal. Element A has an electron configuration: [Kr] 4 s^2. Element B has an electron configuration: [Ar] 3d^10 4s^2 4p^5. B ended at 4p^5, it has an unfilled shell, so, B is a metal.
02

Determine which element has a greater ionization energy

Ionization energy is the energy required to remove an electron from a neutral atom in its gaseous phase. Elements with a greater atomic number and a full outer shell will have a higher ionization energy since they are more stable in nature. Here, A has a full outer shell, so A has a greater ionization energy.
03

Determine the element with a larger atomic radius

Atomic radius decreases across a period on the periodic table and increases down a group. This is because when you move down the groups, there are more electron shells. Here, A with configuration [Kr] 4 s^2 is presumed to have a larger atomic radius compared to B since it likely belongs to a lower period.
04

Establish the element with a greater electron affinity

Electron affinity is the amount of energy released when electrons are added to a neutral atom to form a negative ion. Elements that do not have a full outer shell tend to have a higher electron affinity since they can experience stability once there are enough electrons to fill their outer shell. In this case, B with an unfilled shell (having its electron configuration end in 4p^5) would have a higher electron affinity as it is closer to filling its outer shell than A.

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Most popular questions from this chapter

The \(\mathrm{Na}^{+}\) ion and the Ne atom are isoelectronic. The ease of loss of an electron by a gaseous Ne atom, \(I_{1}\) has a value of \(2081 \mathrm{kJ} / \mathrm{mol} .\) The ease of loss of an electron from a gaseous \(\mathrm{Na}^{+}\) ion, \(I_{2}\), has a value of \(4562 \mathrm{kJ} / \mathrm{mol} .\) Why are these values not the same?

Compare the elements \(\mathrm{Al}, \mathrm{Si}, \mathrm{S},\) and \(\mathrm{Cl}.\) (a) Place the elements in order of increasing ionization energy. (b) Place the elements in order of increasing electron affinity.

The masses of individual atoms can be determined with great precision, yet there is considerable uncertainty about the exact size of an atom. Explain why this is the case.

Write electron configurations consistent with the following data on numbers of unpaired electrons: \(\mathrm{Ni}^{2+}, 2 ; \mathrm{Cu}^{2+}, 1 ; \mathrm{Cr}^{3+}, 3.\)

Explain why the radii of atoms do not simply increase uniformly with increasing atomic number.
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