An isotope is a variant of an element that differs in the number of neutrons in the atomic nucleus. Isotopes of an element have the same number of protons (which defines the element) but different numbers of neutrons. As a result, isotopes have different atomic masses.
The number of protons in an atom determines its atomic number and identifies the element. For example, hydrogen has 1 proton, carbon has 6 protons, and oxygen has 8 protons.
Regarding the question about the number of types of protons for each element, it's important to clarify that protons themselves are not differentiated into types within the context of an element. Protons are all identical and carry the same charge.
On the other hand, the question about neutrons is relevant. For a given element, there can be different isotopes with varying numbers of neutrons. These isotopes have the same number of protons but different numbers of neutrons. For example, carbon has isotopes such as carbon-12 (6 protons, 6 neutrons), carbon-13 (6 protons, 7 neutrons), and carbon-14 (6 protons, 8 neutrons).
In summary, the number of protons in an atom determines the element, and all protons within an element are the same. The number of neutrons can vary between isotopes of the same element, resulting in different atomic masses.