An element \({ }_{88}^{226} X\) undergoes radioactive decay by emitting two alpha particles and a beta radiation. Which of the following nuclei correctly describe the product formed by the reaction?
A. \({ }_{89}^{22}\) T B. \({ }_{84}^{218} S\) C. \({ }_{85}^{218} R\) D. \({ }_{87}^{222} Q\)
Correct Answer: C
Explanation
The equation of the reaction is represented by \({ }_{88}^{226} X \rightarrow{ }_{y}^{x} Y +2_{2}^{4} H +{ }_{-1}^{0} e\)y balancing the equation: $$ \begin{aligned} &226=x+2(4)+0 \\ &226=x+8 \\ &x=226-8=218 \end{aligned} $$lso, $$ \begin{aligned} &88=y+2(2)+(-1) \\ &y=88-3 \\ &y=85 \end{aligned} $$ \(\therefore\) The product is \({ }_{85}^{218} Y \equiv{ }_{85}^{218} R\)
