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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

Write equations that show the processes that describe the first, second, and third ionization energies of a boron atom.

When magnesium metal is burned in air (Figure 3.5), two products are produced. One is magnesium oxide, \(\mathrm{MgO}\). The other is the product of the reaction of \(\mathrm{Mg}\) with molecular nitrogen, magnesium nitride. When water is added to magnesium nitride, it reacts to form magnesium oxide and ammonia gas. (a) Based on the charge of the nitride ion (Table 2.5), predict the formula of magnesium nitride. (b) Write a balanced equation for the reaction of magnesium nitride with water. What is the driving force for this reaction? (c) In an experiment a piece of magnesium ribbon is burned in air in a crucible. The mass of the mixture of \(\mathrm{MgO}\) and magnesium nitride after burning is \(0.470 \mathrm{~g}\). Water is added to the crucible, further reaction occurs, and the crucible is heated to dryness until the final product is \(0.486 \mathrm{~g}\) of \(\mathrm{MgO}\). What was the mass percentage of magnesium nitride in the mixture obtained after the initial burning? (d) Magnesium nitride can also be formed by reaction of the metal with ammonia at high temperature. Write a balanced equation for this reaction. If a \(6.3-\mathrm{g} \mathrm{Mg}\) ribbon reacts with \(2.57 \mathrm{~g} \mathrm{NH}_{3}(\mathrm{~g})\) and the reaction goes to \(\mathrm{com}\) pletion, which component is the limiting reactant? What mass of \(\mathrm{H}_{2}(\mathrm{~g})\) is formed in the reaction? (e) The standard enthalpy of formation of solid magnesium nitride is \(-461.08 \mathrm{~kJ} / \mathrm{mol}\). Calculate the standard enthalpy change for the reaction between magnesium metal and ammonia gas.

(a) Which will have the lower energy, a 4 s or a \(4 p\) electron in an As atom? (b) How can we use the concept of effective nuclear charge to explain your answer to part (a)?

Identify the element whose ions have the following electron configurations: (a) a \(2+\) ion with \([\operatorname{Ar}] 3 d^{9}\), (b) a \(1+\) ion with \([\mathrm{Xe}] 4 f^{14} 5 d^{10} 6 \mathrm{~s}^{2}\). How many unpaired electrons does each ion contain?

Consider the gas-phase transfer of an electron from a sodium atom to a chlorine atom: $$ \mathrm{Na}(\mathrm{g})+\mathrm{Cl}(\mathrm{g}) \longrightarrow \mathrm{Na}^{+}(\mathrm{g})+\mathrm{Cl}^{-}(g) $$ (a) Write this reaction as the sum of two reactions, one that relates to an ionization energy and one that relates to an electron affinity. (b) Use the result from part (a), data in this chapter, and Hess's law to calculate the enthalpy of the above reaction. Is the reaction exothermic or endothermic? (c) The reaction between sodium metal and chlorine gas is highly exothermic and produces \(\mathrm{NaCl}(\mathrm{s})\), whose structure was discussed in Section 2.7. Comment on this observation relative to the calculated enthalpy for the aforementioned gas-phase reaction.
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