Question

All the elements beyond uranium, the trans uranium elements, have been prepared by bombardment and are not naturally occurring elements. The first trans uranium element neptunium, $\mathrm{Np}$, was prepared by bombarding $U-238$with neutrons to form a neptunium atom and a beta particle. Complete the following equation: $(5.2)$

data-custom-editor="chemistry" ${}_0{}^1\mathrm{n}+{}_{92}{}^{238}\mathrm{U}\to ?+?$

Short answer

As a result, the following is a full nuclear reaction:

${}_0{}^1\mathrm{n}+{}_{92}{}^{239}\mathrm{U}\to {}_{91}{}^{239}\mathrm{Np}+{}_{-1}{}^0\mathrm{e}$

Step-by-step solution

    Given Information 

The elements above uranium are synthetic elements that do not occur naturally.

The following procedure is used to make Neptunium $\left(\mathrm{Np}\right)$:

When neutrons attack $uranium-238$, a neptunium atom and a beta particle form.

The following is an incomplete nuclear equation:

${}_0{}^1\mathrm{n}+{}_{92}{}^{238}\mathrm{U}\to ?+?$

    Given Explanation 

The sum of the left side elements' mass numbers is $239$, which is identical to the sum of the right side elements' mass numbers.

Because the mass number of a beta particle is zero, neptunium has a mass number of $239$.

The neptunium atom and a beta particle are created during neutron bombardment. The atomic number of neptunium is $93$, and the atomic number of the beta particle is $1$with one negative charge.

    Conclusion 

The sum of the atomic numbers of the elements on the left side is $92$, which is identical to the sum of the atomic numbers of the elements on the right side, which is $92$.

As a result, the following is a full nuclear reaction:

${}_0{}^{1}n+{}_{92}{}^{239}U\to {}_{91}{}^{239}Np+{}_{-1}{}^{0}e$