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Chapter 7: Problem 25

Using only the periodic table, arrange each set of atoms in order from largest to smallest: \((\mathbf{a}) \mathrm{Ar},\) As, \(\mathrm{Kr} ;\) (b) $\mathrm{Cd}, \mathrm{Rb}, \mathrm{Te} ;(\mathbf{c})$ \(\mathrm{C}, \mathrm{Cl}, \mathrm{Cu}\).

Short Answer

Expert verified
Using the periodic trends in atomic size, we can order the sets of atoms as follows: (a) As > Ar > Kr, (b) Rb > Cd > Te, and (c) Cu > Cl > C.

Step by step solution

01

Locate the atoms on the periodic table

Locate each atom in the periodic table by finding its symbol and identifying its position in terms of the periods (rows) and groups (columns).
02

Compare the elements within the set

Use the periodic trends in atomic size to compare the elements' sizes within each set. If they are in the same period, compare their positions from left to right. If they are in the same group, compare their positions from top to bottom. (a) Ar, As, Kr:
03

Step 3(a): Arrange the atoms from largest to smallest

Ar is in period 3, As is in period 4, and Kr is in period 4. As and Kr are in the same period, with Kr being on the right side of As, therefore As is larger than Kr. Comparing Ar and As, we find that As is below Ar (in the same group), so As is larger. Thus, the order is As > Ar > Kr. (b) Cd, Rb, Te:
04

Step 3(b): Arrange the atoms from largest to smallest

Cd is in period 5, Rb is in period 5, and Te is in period 5. All three elements are in the same period. Comparing their positions from left to right: Rb is the farthest left, followed by Cd and then Te. Hence, the order is Rb > Cd > Te. (c) C, Cl, Cu:
05

Step 3(c): Arrange the atoms from largest to smallest

C is in period 2, Cl is in period 3, and Cu is in period 4. Cl and Cu are in the same period, with Cu being on the left side of Cl, therefore Cu is larger than Cl. Comparing Cl and C, we find that Cl is below C (in the same group), so Cl is larger. Thus, the order is Cu > Cl > C.

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Most popular questions from this chapter

The following observations are made about two hypothetical elements \(\mathrm{A}\) and \(\mathrm{B}:\) The \(\mathrm{A}-\mathrm{A}\) and \(\mathrm{B}-\mathrm{B}\) bond lengths in the elemental forms of \(\mathrm{A}\) and \(\mathrm{B}\) are 236 and \(194 \mathrm{pm}\), respectively. A and \(B\) react to form the binary compound \(A B_{2}\), which has a linear structure (that is \(\left.\angle \mathrm{B}-\mathrm{A}-\mathrm{B}=180^{\circ}\right) .\) Based on these statements, predict the separation between the two B nuclei in a molecule of \(\mathrm{AB}_{2}\).

For each of the following pairs, indicate which element has the smaller first ionization energy: (a) $\mathrm{Cs}, \mathrm{Cl} ;(\mathbf{b}) \mathrm{Fe}, \mathrm{Zn} ;\( (c) \)\mathrm{I}, \mathrm{Cl} ;(\mathbf{d}) \mathrm{Se}, \mathrm{Sn}$

(a) Use orbital diagrams to illustrate what happens when an oxygen atom gains two electrons. (b) Why does \(\mathrm{O}^{3-}\) not exist?

(a) Why is calcium generally more reactive than beryllium? (b) Why is calcium generally less reactive than rubidium?

Elemental barium reacts more violently with water than does elemental calcium. Which of the following best explains this difference in reactivity? (i) Calcium has greater metallic character than does barium. (ii) The electron affinity of calcium is smaller than that of barium. (iii) The first and second ionization energies of barium are less than those of calcium. (iv) The atomic radius of barium is smaller than that of calcium. (v) The ionic radius of the barium ion is larger than that of the calcium ion.
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