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Chapter 7: Problem 27

(a) Why are monatomic cations smaller than their corresponding neutral atoms? (b) Why are monatomic anions larger than their corresponding neutral atoms? (c) Why does the size of ions increase as one proceeds down a column in the periodic table?

Short Answer

Expert verified
(a) Monatomic cations are smaller than their corresponding neutral atoms because the loss of valence electrons results in an increased positive charge, causing the remaining electrons to be more strongly attracted to the nucleus and the electron cloud to contract. (b) Monatomic anions are larger than their corresponding neutral atoms because the addition of valence electrons increases the shielding effect, causing the electron cloud to expand due to repulsion between electrons. (c) The size of ions increases as one proceeds down a column in the periodic table because additional electron shells are added, increasing the shielding effect and making the attractive force between the outer electrons and the nucleus weaker, resulting in a more diffuse electron cloud and larger ionic size.

Step by step solution

01

(a) Monatomic cations are smaller than their corresponding neutral atoms:

Monatomic cations are formed when a neutral atom loses one or more of its valence electrons. This loss results in an increased positive charge within the atom, causing the remaining electrons to be attracted more strongly to the nucleus. Consequently, the electron cloud surrounding the nucleus contracts and the overall size of the ion is reduced. Therefore, monatomic cations are smaller than their corresponding neutral atoms.
02

(b) Monatomic anions are larger than their corresponding neutral atoms:

Monatomic anions are formed when a neutral atom gains one or more valence electrons. This addition of electrons leads to an increased shielding effect, where the extra negative charge repels the other electrons, making them less attracted to the nucleus. As a result, the electron cloud expands and the overall size of the ion increases. Therefore, monatomic anions are larger than their corresponding neutral atoms.
03

(c) The size of ions increases as one proceeds down a column in the periodic table:

As we move down a column (or group) in the periodic table, additional electron shells are added to the atomic structure. Each new electron shell is further away from the nucleus compared to the previous one. At the same time, the shielding effect of the inner shell electrons also increases, making the attractive force between the outer electrons and the nucleus weaker. As a result, the electron cloud becomes more diffuse, and the overall ionic size increases when going down a column in the periodic table.

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Most popular questions from this chapter

Chlorine reacts with oxygen to form \(\mathrm{Cl}_{2} \mathrm{O}_{7} .\) (a) What is the name of this product (see Table 2.6)? (b) Write a balanced equation for the formation of \(\mathrm{Cl}_{2} \mathrm{O}_{7}(l)\) from the elements. (c) Under usual conditions, \(\mathrm{Cl}_{2} \mathrm{O}_{7}\) is a colorless liquid with a boiling point of \(81^{\circ} \mathrm{C}\). Is this boiling point expected or surprising? (d) Would you expect \(\mathrm{Cl}_{2} \mathrm{O}_{7}\) to be more reactive toward \(\mathrm{H}^{+}(a q)\) or \(\mathrm{OH}^{-}(a q) ?\) Explain.

(a) What is the trend in first ionization energies as one proceeds down the group 7 A elements? Explain how this trend relates to the variation in atomic radii. (b) What is the trend in first ionization energies as one moves across the fourth period from \(\mathrm{K}\) to \(\mathrm{Kr}\) ? How does this trend compare with the trend in atomic radii?

Based on their positions in the periodic table, predict which atom of the following pairs will have the larger first ionization energy: (a) \(\mathrm{Cl}\), \(\mathrm{Ar} ;\) (b) Be, \(\mathrm{Ca} ;\) (c) \(\mathrm{K}, \mathrm{Co}\); (d) S, Ge; (e) \(\mathrm{Sn}\), Te.

Detailed calculations show that the value of \(Z_{\text {eff }}\) for \(\mathrm{Na}\) and \(K\) atoms is \(2.51+\) and \(3.49+\), respectively. (a) What value do you estimate for \(Z_{\text {eff }}\) experienced by the outermost electron in both Na and \(K\) by assuming core electrons contribute \(1.00\) and valence electrons contribute \(0.00\) to the screening constant? (b) What values do you estimate for \(Z_{\text {eff }}\) using Slater's rules? (c) Which approach gives a more accurate estimate of \(Z_{\text {eff }} ?\) (d) Does either method of approximation account for the gradual increase in \(Z_{\text {eff }}\) that occurs upon moving down a group?

Consider \(\mathrm{S}, \mathrm{Cl}\), and \(\mathrm{K}\) and their most common ions. (a) List the atoms in order of increasing size (b) List the ions in order of increasing size. (c) Explain any differences in the orders of the atomic and ionic sizes.
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