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Ch.7 - Periodic Properties of the Elements
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All textbooksBrown 14th EditionCh.7 - Periodic Properties of the ElementsProblem 21b

Chapter 7, Problem 21b

Tungsten has the highest melting point of any metal in the periodic table: 3422 °C. The distance between W atoms in tungsten metal is 274 pm. (b) If you put tungsten metal under high pressure, predict what would happen to the distance between W atoms.

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All right. Hi, everyone. So this question says that chromium has a very high melting point of 1907 °C. The difference between or excuse me, the distance between chromium atoms in chromium metal is 252 PICO meter. If you put chromium metal under high pressure, predict what would happen to the distance between chromium atoms. Option A says the distance between chromium atoms is expected to increase. Option B says the distance is expected to decrease and option C says the distance is expected to remain the same. Now for a question like this, right? It's worth mentioning that the question describes placing chromium metal under very high pressure. In other words, we're going to compress our sample of chromium metal now because we're compressing the sample and we're subjecting it to such high pressure. Then what that means is that the chromium atoms are going to be pushed closer together, right? That pressure surrounding chromium is going to push chromium atoms even closer together still now because chromium metal is a solid, there's already such little space between them, but the added pressure is going to force the chromium atoms even closer together still. So really the distance between them is expected to decrease as a result of this compression. Now, it's worth mentioning also that because chromium metal is a solid, right, the effects of this compression may not necessarily be visible to the naked eye. And this is because a solid already has its atoms or particles in general, incredibly close together to maintain its solid shape. Now, this is in comparison to subjecting either a gas or a liquid to the same high pressure when compressing either a gas or a liquid. By that point, you're more likely to see some sort of visible change, for example, a phase change. But nonetheless, in the case of a solid, the distance between chromium atoms is expected to decrease, even still, you just might not be able to see a difference. So that means our answer is going to be option B in the multiple choice and there you have it. So with that being said, thank you so very much for watching and I hope you found this hopeful.
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Textbook Question

With the exception of helium, the noble gases condense to form solids when they are cooled sufficiently. At temperatures below 83 K, argon forms a close-packed solid whose structure is shown below. (b) Is this value larger or smaller than the bonding atomic radius estimated for argon in Figure 7.7?

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Textbook Question

With the exception of helium, the noble gases condense to form solids when they are cooled sufficiently. At temperatures below 83 K, argon forms a close-packed solid whose structure is shown below. (c) Based on this comparison would you say that the atoms are held together by chemical bonds in solid argon?

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Textbook Question

Tungsten has the highest melting point of any metal in the periodic table: 3422 °C. The distance between W atoms in tungsten metal is 274 pm. (a) What is the atomic radius of a tungsten atom in this environment? (This radius is called the metallic radius.)

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Textbook Question

Which of the following statements about the bonding atomic radii in Figure 7.7 is incorrect? (i) For a given period, the radii of the representative elements generally decrease from left to right across a period. (ii) The radii of the representative elements for the n = 3 period are all larger than those of the corresponding elements in the n = 2 period. (iii) For most of the representative elements, the change in radius from the n = 2 to the n = 3 period is greater than the change in radius from n = 3 to n = 4. (iv) The radii of the transition elements generally increase moving from left to right within a period. (v) The large radii of the Group 1 elements are due to their relatively small effective nuclear charges.

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Estimate the As¬I bond length from the data in Figure 7.7 and compare your value to the experimental As ¬I bond length in arsenic triiodide, AsI3, 2.55 Å.

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The experimental Pb¬Cl bond length in lead(II)chloride, PbCl2, is 244 pm. Based on this value and data in Figure 7.7, predict the atomic radius of Pb.

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