How do you write a balanced nuclear equation for the positron emission of nitrogen-13?

Answer 1

If oxygen-16 was to undergo positron emission (beta plus decay), a proton in its nucleus would transform into a neutron (mediated by the weak force). The oxygen-16 would become nitrogen-16, and we'd see a positron and a neutrino appear. The equation might look like this: 816O => 716N + e+ + ve It is easy to write a balanced nuclear equation for any nuclide undergoing positron emission. Note the subscript numerals at the beginning of each element. That's the atomic number of that element. The superscript numerals are the Atomic Mass of the nuclide. When beta plus decay occurs, nuclear transformation takes place. The atomic number of the element goes down by one, and one element becomes another element. The subscripted numerals will reflect that decrease of one, and the atomic mass (the superscripted numerals) will remain the same. Note the last two factors in the equation, as they are the positron and the neutrino, respectively. That's the long and short of the beta plus decay of O-16, as asked. We'll add, however, that oxygen-16 is a stable isotope of oxygen. It does not undergo beta decay, but for the sake of argument, it did here. And with the results shown. By the way, it is oxygen-15 that is the radioactive isotope of oxygen that will undergo beta plus decay. You'll find links below for more information.

Answer 2

815O -> beta+ (T1/2 = 122.24 s) -> 715N + e+ + ve

Answer 3

Oxygen 15 decays to Nitrogen 15 by emitting a positron and a neutrino. The equation is written thus:-

15O => 15N + e+ + ve

Answer 4

12N7--> 0e+1 +12C6