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Ch.7 - Periodic Properties of the Elements

Chapter 7, Problem 23

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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Hello everyone today. We have the following problem. The experimental arsenic bromine bromine bond length and arsenic try bromide is 233 p. M. Or PICO meters. Estimate the arsenic bromine bond length based on the image below it compared to the experimental arsenic bromine bond length. So this problem is super simple. The first thing you wanna do is you want to find the individual bond lengths and add them up. So for arsenic here we have 120 PICO meters. And for browning we have 114 m. So you're going to take arsenic, we're going to add it to the bombing, Which will be equal to 120 PK m Plus 114 km to give us 234 m. We can therefore conclude that it is slightly and very slightly longer than the experimental value. And with that we have our answer. I hope this helped. And until next time.
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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

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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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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