Question

Write the balanced nuclear equation for the following. (Use the lowest possible coefficients. Omit states-of-matter in your answer.)
(a) electron capture by neptunium-232

Answer 1

Answer:

$_{93}^{232}\text{Np} + _{-1}^{0}\text{e} \longrightarrow _{92}^{232}\text{U}$

Explanation:

The unbalanced nuclear equation is

$_{93}^{232}\text{Np} + _{1}^{0}\text{e} \longrightarrow ?$

It is convenient to replace the question by an atomic symbol, $_{x}^{y}\text{Z}$, where x = the atomic number, y = the mass number, and Z = the symbol of the element.

$_{93}^{232}\text{Np} + _{1}^{0}\text{e} \longrightarrow _{x}^{y}\text{Z}$

Then your equation becomes

$_{93}^{232}\text{Np} + _{1}^{0}\text{e} \longrightarrow _{x}^{y}\text{Z}$

The main point to remember in balancing nuclear equations is that the sums of the superscripts and of the subscripts must be the same on each side of the equation.  

Then

93 – 1 = x, so x = 92

232 + 0 = y, so y = 232

Element 92 is uranium, so the nuclear equation becomes

$_{93}^{232}\text{Np} + _{-1}^{0}\text{e} \longrightarrow _{92}^{232}\text{U}$