The elemental ion in question has 34 protons, which means it is an ion of selenium (Se), as the atomic number of selenium is 34. The number of neutrons is given as 44.
To identify the isotope, we need to calculate the mass number, which is the sum of the protons and neutrons. In this case, the mass number is:
- Mass number = Protons + Neutrons = 34 + 44 = 78
Thus, the isotope is represented as selenium-78 (Se-78). The additional information about having 36 electrons indicates that this selenium ion has a -2 charge, as it has 2 more electrons than protons.
In summary, the isotope of this elemental ion is selenium-78, written as Se-78, with a net charge of -2 due to the excess electrons.