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Chapter 7: Problem 25

Using only the periodic table, arrange each set of atoms in order from largest to smallest: (a) \(\mathrm{K}, \mathrm{Li}, \mathrm{Cs} ;\) (b) \(\mathrm{Pb}, \mathrm{Sn}, \mathrm{Si} ;\) (c) \(\mathrm{F}, \mathrm{O}, \mathrm{N}\)

Short Answer

Expert verified
Using the periodic table and considering the atomic size trends, we can arrange the given sets of atoms in order from largest to smallest as follows: (a) Cs > K > Li; (b) Pb > Sn > Si; (c) N > O > F.

Step by step solution

01

(a) Arrange K, Li, Cs in Order of Size

All three elements, K (Potassium), Li (Lithium), and Cs (Cesium), belong to Group 1 (alkali metals) in the periodic table. As we move down the group, the atomic size increases. So, the order of these elements, from largest to smallest, is Cs > K > Li.
02

(b) Arrange Pb, Sn, Si in Order of Size

Pb (Lead), Sn (Tin), and Si (Silicon) belong to Group 14 in the periodic table. As we move down the group, the atomic size increases. Therefore, the order of these elements, from largest to smallest, is Pb > Sn > Si.
03

(c) Arrange F, O, N in Order of Size

F (Fluorine), O (Oxygen), and N (Nitrogen) are all elements in the same period, Period 2. As you move from left to right across a period, the atomic size decreases. Thus, the order of these elements, from largest to smallest, is N > O > F.

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Most popular questions from this chapter

Potassium superoxide, \(\mathrm{KO}_{2}\), is often used in oxygen masks (such as those used by firefighters) because \(\mathrm{KO}_{2}\) reacts with \(\mathrm{CO}_{2}\) to release molecular oxygen. Experiments indicate that \(2 \mathrm{~mol}\) of \(\mathrm{KO}_{2}(s)\) react with each mole of \(\mathrm{CO}_{2}(g) .\) (a) The products of the reaction are \(\mathrm{K}_{2} \mathrm{CO}_{3}(s)\) and \(\mathrm{O}_{2}(g) .\) Write a balanced equation for the reaction between \(\mathrm{KO}_{2}(s)\) and \(\mathrm{CO}_{2}(g) .\) (b) Indicate the oxidation number for each atom involved in the reaction in part (a). What elements are being oxidized and reduced? (c) What mass of \(\mathrm{KO}_{2}(s)\) is needed to consume \(18.0 \mathrm{~g} \mathrm{CO}_{2}(g) ?\) What mass of \(\mathrm{O}_{2}(g)\) is produced during this reaction?

Consider the first ionization energy of neon and the electron affinity of fluorine. (a) Write equations, including electron configurations, for each process. (b) These two quantities will have opposite signs. Which will be positive, and which will be negative? (c) Would you expect the magnitudes of these two quantities to be equal? If not, which one would you expect to be larger? Explain your answer.

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

If the electron affinity for an element is a negative number, does it mean that the anion of the element is more stable than the neutral atom? Explain.

Some ions do not have a corresponding neutral atom that has the same electron configuration. For each of the following ions, identify the neutral atom that has the same number of electrons and determine if this atom has the same electron configuration. If such an atom does not exist, explain why. (b) \(\mathrm{Sc}^{3+}\) (d) \(\mathrm{Zn}^{2+},(\mathrm{e}) \mathrm{Sn}^{4+}\) (a) \(\mathrm{Cl}\) (c) \(\mathrm{Fe}^{2+}\)
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