To identify the isotope, we first need to determine the atomic number and the mass number of the element.
The atomic number is defined by the number of protons in the nucleus of the atom. In this case, the element has 22 protons, which corresponds to titanium (Ti) on the periodic table. Therefore, the atomic number of this element is 22.
Next, we calculate the mass number by adding the number of protons and neutrons together. Here, the element has 22 protons and 26 neutrons:
Mass Number = Protons + Neutrons = 22 + 26 = 48
This means that the isotope of titanium in question is titanium-48, commonly written as Ti-48. The number indicates the total number of protons and neutrons in the nucleus of the atom.
Additionally, since the element has 20 electrons, it has a charge. Normally, a neutral titanium atom would have 22 electrons (equal to the number of protons). However, since there are only 20 electrons, this indicates that the ion has a +2 charge (it has lost two electrons).
In summary, the isotope of the elemental ion with 22 protons, 20 electrons, and 26 neutrons is Titanium-48 (Ti-48), and it is a positively charged ion with a charge of +2.