Complete this radioactive-decay formula: $^{212}_{83}Bi$ → ? + $^4_2He$ 1. None of these 2. $^{216}_{81}Tl$ 3. $^{208}_{81}Tl$ 4. $^{208}_{81}Hg$ 5. $^{216}_{85}At$ 6. $^{216}_{85}Po$ 7. $^{208}_{85}At$
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Step 1: The atomic number of the unknown element is 83 - 2 = 81. Show more…
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Which element in the following series will be present in the greatest amount after one year? $$\begin{aligned} &_{83}^{214} \mathrm{Bi} \stackrel{\alpha}{\rightarrow}^{210} \mathrm{r} 1 \stackrel{\beta}{\rightarrow}_{82}^{210} \mathrm{Pb} \stackrel{\beta}{\rightarrow}^{210} \mathrm{s}_{3} \mathrm{Bi} \rightarrow\\ &t_{1 / 2}=20 \min 1.3 \min 20 \mathrm{yr} \quad 5 \mathrm{d} \end{aligned}$$
An atom undergoes radioactive decay according to this equation: 209/83 Bi -> ___ + 4/2 He What is the identity of the resulting atom?
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$\mathrm{Bi}^{214}$ decays to $A$ by $\alpha$ -emission; $A$ then decays to $B$ by beta emission, which decays to $C$ by 83 another beta emission. Element $C$ decays to $D$ by still another beta emission, and $D$ decays by t-emission to a stable isotope $E$. What is an element $E$ ? (a) $_{81} \mathrm{Tl}^{207}$ (b) ${ }_{80} \mathrm{Hg}^{206}$ (c) ${ }_{79} \mathrm{Au}^{206}$ (d) ${ }_{82} \mathrm{~Pb}^{206}$
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