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Chapter 2: Problem 48

a. List the noble gas elements. Which of the noble gases has only radioactive isotopes? (This situation is indicated on most periodic tables by parentheses around the mass of the element. See inside front cover.) b. Which lanthanide element and which transition element have only radioactive isotopes?

Short Answer

Expert verified
The noble gas elements are Helium (He), Neon (Ne), Argon (Ar), Krypton (Kr), Xenon (Xe), and Radon (Rn). Among them, Radon (Rn) has only radioactive isotopes. The lanthanide element with only radioactive isotopes is Promethium (Pm) with atomic number 61, and the transition element with only radioactive isotopes is Technetium (Tc) with atomic number 43.

Step by step solution

01

Part a: Listing the noble gas elements

The noble gases are the elements found in Group 18 (VIII) of the periodic table. These elements include: 1. Helium (He) 2. Neon (Ne) 3. Argon (Ar) 4. Krypton (Kr) 5. Xenon (Xe) 6. Radon (Rn)
02

Identifying the noble gas with only radioactive isotopes

Among the noble gases, Radon (Rn) is the only one with radioactive isotopes. It is usually indicated on the periodic table by parentheses around its mass number.
03

Part b: Identifying the lanthanide element and the transition element with only radioactive isotopes

We will again refer to the periodic table to find the required elements. 1. The lanthanide element with only radioactive isotopes is Promethium (Pm). Its atomic number is 61. 2. The transition element with only radioactive isotopes is Technetium (Tc). Its atomic number is 43.

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Most popular questions from this chapter

You have gone back in time and are working with Dalton on a table of relative masses. Following are his data. \(0.602 \mathrm{~g}\) gas A reacts with \(0.295 \mathrm{~g}\) gas \(\mathrm{B}\) \(0.172 \mathrm{~g}\) gas \(\mathrm{B}\) reacts with \(0.401 \mathrm{~g}\) gas \(\mathrm{C}\) \(0.320 \mathrm{~g}\) gas \(\mathrm{A}\) reacts with \(0.374 \mathrm{~g}\) gas \(\mathrm{C}\) a. Assuming simplest formulas \((\mathrm{AB}, \mathrm{BC}\), and \(\mathrm{AC}\) ), construct a table of relative masses for Dalton. b. Knowing some history of chemistry, you tell Dalton that if he determines the volumes of the gases reacted at constant temperature and pressure, he need not assume simplest formulas. You collect the following data: 6 volumes gas \(A+1\) volume gas \(B \rightarrow 4\) volumes product 1 volume gas \(\mathrm{B}+4\) volumes gas \(\mathrm{C} \rightarrow 4\) volumes product 3 volumes gas \(\mathrm{A}+2\) volumes gas \(\mathrm{C} \rightarrow 6\) volumes product Write the simplest balanced equations, and find the actual relative masses of the elements. Explain your reasoning.

By analogy with phosphorus compounds, name the following: \(\mathrm{Na}_{3} \mathrm{AsO}_{4}, \mathrm{H}_{3} \mathrm{AsO}_{4}, \mathrm{Mg}_{3}\left(\mathrm{SbO}_{4}\right)_{2}\)

For lighter, stable isotopes, the ratio of the mass number to the atomic number is close to a certain value. What is the value? What happens to the value of the mass number to atomic number ratio as stable isotopes become heavier?

For each of the following atomic numbers, use the periodic table to write the formula (including the charge) for the simple ion that the element is most likely to form in ionic compounds. a. 13 c. 56 e. 87 b. 34 d. \(\underline{7}\) f. 35

Knowing the names of similar chlorine oxyanions and acids, deduce the names of the following: \(\mathrm{IO}^{-}, \mathrm{IO}_{2}^{-}, \mathrm{IO}_{3}^{-}, \mathrm{IO}_{4}^{-}, \mathrm{HIO}\) \(\mathrm{HIO}_{2}, \mathrm{HIO}_{3}, \mathrm{HIO}_{4}\)
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