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Chapter 7: Problem 26

Using only the periodic table, arrange each set of atoms in (b) \(\mathrm{Sn}, \mathrm{Sb}, \mathrm{As} ;(\mathbf{c}) \mathrm{Al},\) order of increasing radius: (a) \(\mathrm{Ba}, \mathrm{Ca}, \mathrm{Na} ;\) Be, Si.

Short Answer

Expert verified
The order of increasing atomic radius for each set is: (a) Na < Ca < Ba; (b) As < Sb < Sn; (c) Be < Si < Al.

Step by step solution

01

Set (a): Arrange Ba, Ca, Na

To arrange Ba, Ca, and Na in order of increasing atomic radius, we look at their positions on the periodic table. Ba(Barium) is in Group 2 and Period 6, Ca(Calcium) is in Group 2 and Period 4, and Na(Sodium) is in Group 1 and Period 3. Since atomic radius increases down a group and decreases across a period, the order of increasing atomic radius will be: Na < Ca < Ba.
02

Set (b): Arrange Sn, Sb, As

To arrange Sn, Sb, and As in order of increasing atomic radius, we look at their positions on the periodic table. Sn(Tin) is in Group 14 and Period 5, Sb(Antimony) is in Group 15 and Period 5, and As(Arsenic) is in Group 15 and Period 4. Since atomic radius increases down a group and decreases across a period, the order of increasing atomic radius will be: As < Sb < Sn.
03

Set (c): Arrange Al, Be, Si

To arrange Al, Be, and Si in order of increasing atomic radius, we look at their positions on the periodic table. Al(Aluminium) is in Group 13 and Period 3, Be(Beryllium) is in Group 2 and Period 2, and Si(Silicon) is in Group 14 and Period 3. Since atomic radius increases down a group and decreases across a period, the order of increasing atomic radius will be: Be < Si < Al.

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Most popular questions from this chapter

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.

The first ionization energy and electron affinity of Ar are both positive values. (a) What is the significance of the positive value in each case? (b) What are the units of electron affinity?

Make a simple sketch of the shape of the main part of the periodic table, as shown. (a) Ignoring \(\mathrm{H}\) and He, write a single straight arrow from the element with the smallest bonding atomic radius to the element with the largest. Ignoring \(\mathrm{H}\) and He, write a single straight arrow from the element with the smallest first ionization energy to the element with the largest. (c) What significant observation can you make from the arrows you drew in parts (a) and (b)? [Sections 7.3 and 7.4]

One way to measure ionization energies is ultraviolet photoelectron spectroscopy (UPS, or just PES), a technique based on the photoelectric effect. coo (Section 6.2 ) In PES, monochromatic light is directed onto a sample, causing electrons to be emitted. The kinetic energy of the emitted electrons is measured. The difference between the energy of the photons and the kinetic energy of the electrons corresponds to the energy needed to remove the electrons (that is, the ionization energy). Suppose that a PES experiment is performed in which mercury vapor is irradiated with ultraviolet light of wavelength \(58.4 \mathrm{nm}\). (a) What is the energy of a photon of this light in eV? (b) Write an equation that shows the process corresponding to the first ionization energy of \(\mathrm{Hg}\). (c) The kinetic energy of the emitted electrons is measured to be \(10.75 \mathrm{eV}\). What is the first ionization energy of Hg in kJ/mol? (d) Using Figure 7.9 , determine which of the halogen elements has a first ionization energy closest to that of mercury.

(a) Why does the quantum mechanical description of manyelectron atoms make it difficult to define a precise atomic radius? (b) When nonbonded atoms come up against one another, what determines how closely the nuclear centers can approach?
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