To solve this problem, we need to identify the type of nuclear reaction taking place. Here is a step-by-step approach:
1. Examine the given nuclear equation:
[tex]\[
{ }_8^{15} O \longrightarrow{ }_7^{15} N +{ }_{+1}^0 e
\][/tex]
2. Identify the particles involved:
- On the left side of the equation, we have an oxygen-15 nucleus ([tex]\( _8^{15}O \)[/tex]).
- On the right side of the equation, we have a nitrogen-15 nucleus ([tex]\( _7^{15}N \)[/tex]) and a positron ([tex]\( _{+1}^0 e \)[/tex]).
3. Determine the changes in atomic and mass numbers:
- The oxygen nucleus has an atomic number of 8 and a mass number of 15.
- The nitrogen nucleus has an atomic number of 7 and a mass number of 15.
- The positron has an atomic number of +1 and a mass number of 0.
4. Check the conservation of atomic and mass numbers:
- Mass number (A) on both sides: 15 (oxygen) [tex]\(\longrightarrow\)[/tex] 15 (nitrogen) + 0 (positron).
- Atomic number (Z) on both sides: 8 (oxygen) [tex]\(\longrightarrow\)[/tex] 7 (nitrogen) + 1 (positron).
Both atomic and mass numbers are conserved in this reaction.
5. Identify the type of decay:
In this reaction, a proton in the nucleus of oxygen-15 is converted into a neutron, resulting in a nitrogen-15 nucleus and the emission of a positron. This kind of nuclear transformation is characteristic of beta plus decay (also known as positron emission).
Therefore, the correct identification of the type of reaction is:
Beta plus decay
