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Chapter 22: Problem 20

Which isotope of hydrogen is radioactive? Write the nuclear equation for the radioactive decay of this isotope.

Short Answer

Expert verified
The radioactive isotope of hydrogen is tritium (\(^3_1\)H). Its radioactive decay occurs through beta decay, and the nuclear equation for this process is \[^3_1 H \rightarrow ^3_2 He + ^0_{-1} e\]. In this equation, tritium decays into a helium-3 nucleus (\(^3_2\)He) and a beta particle (an electron: \(^0_{-1} e\)).

Step by step solution

01

Identifying Hydrogen Isotopes

Hydrogen has three known isotopes: protium (\(^1_1\)H), deuterium (\(^2_1\)H), and tritium (\(^3_1\)H). Protium is the most common isotope and has one proton and no neutrons. Deuterium has one proton and one neutron. Tritium has one proton and two neutrons.
02

Determining the Radioactive Hydrogen Isotope

Among the three hydrogen isotopes, tritium (\(^3_1\)H) is radioactive. Tritium undergoes radioactive decay by emitting a beta particle.
03

Writing the Nuclear Equation for Radioactive Decay of Tritium

Now, we need to write the nuclear equation for the radioactive decay of tritium. A beta decay occurs when a neutron in an unstable nucleus turns into a proton and emits an electron, called a beta particle. The atomic number (Z) of the resulting element increases by 1, while the mass number (A) remains the same. The nuclear equation for the beta decay of tritium can be represented as: \[^3_1 H \rightarrow ^3_2 He + ^0_{-1} e\] Here, tritium decays into a helium-3 nucleus (\(^3_2\)He) and a beta particle (an electron: \(^0_{-1} e\)).

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Most popular questions from this chapter

Complete and balance the following equations: (a) \(\mathrm{Mg}_{3} \mathrm{~N}_{2}(\mathrm{~s})+\mathrm{H}_{2} \mathrm{O}(l) \longrightarrow\) (b) \(\mathrm{NO}(g)+\mathrm{O}_{2}(g) \longrightarrow\) (c) \(\mathrm{N}_{2} \mathrm{O}_{5}(g)+\mathrm{H}_{2} \mathrm{O}(l) \longrightarrow\) (d) \(\mathrm{NH}_{3}(a q)+\mathrm{H}^{+}(a q) \longrightarrow\) (e) \(\mathrm{N}_{2} \mathrm{H}_{4}(l)+\mathrm{O}_{2}(g) \longrightarrow\)

Complete and balance the following equations: (a) \(\mathrm{NaOCH}_{3}(\mathrm{~s})+\mathrm{H}_{2} \mathrm{O}(l) \longrightarrow\) (b) \(\mathrm{CuO}(\mathrm{s})+\mathrm{HNO}_{3}(a q) \longrightarrow\) (c) \(\mathrm{WO}_{3}(\mathrm{~s})+\mathrm{H}_{2}(g) \stackrel{\Delta}{\longrightarrow}\) (d) \(\mathrm{NH}_{2} \mathrm{OH}(l)+\mathrm{O}_{2}(g) \longrightarrow\) (e) \(\mathrm{Al}_{4} \mathrm{C}_{3}(\mathrm{~s})+\mathrm{H}_{2} \mathrm{O}(l) \longrightarrow\)

Write a balanced net ionic equation for each of the following reactions: (a) Dilute nitric acid reacts with zinc metal with formation of nitrous oxide. (b) Concentrated nitric acid reacts with sulfur with formation of nitrogen dioxide. (c) Concentrated nitric acid oxidizes sulfur dioxide with formation of nitric oxide. (d) Hydrazine is burned in excess fluorine gas, forming \(\mathrm{NF}_{3}\). (e) \(\mathrm{Hy}\) drazine reduces \(\mathrm{CrO}_{4}{ }^{2-}\) to \(\mathrm{Cr}(\mathrm{OH})_{4}^{-}\) in base (hydrazine is oxidized to \(\mathrm{N}_{2}\) ).

Explain the following observations: (a) for a given oxidation state, the acid strength of the oxyacid in aqueous solution decreases in the order chlorine \(>\) bromine \(>\) iodine. (b) Hydrofluoric acid cannot be stored in glass bottles. (c) Hi cannot be prepared by treating NaI with sulfuric acid. (d) The interhalogen \(\mathrm{ICl}_{3}\) is known, but \(\mathrm{BrCl}_{3}\) is not.

(a) List three industrial uses of \(\mathrm{O}_{2} .\) (b) List two industrial uses of \(\mathrm{O}_{3}\)
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