Yes. Isotopes have the same atomic number because all of their atoms have the same number of protons. They have different mass numbers because their atoms have different numbers of neutrons, and mass number is the sum of the numbers of protons and neutrons.
If two atoms are isotopes, it means they have the same number of protons but different numbers of neutrons. Thus, they have the same atomic numbers, but different atomic masses.
If they have the same atomic number but different mass, then they have a different number of neutrons, and they are called ISOTOPES.
Yes; isotopes of the same element have the same atomic number but differ in their atomic masses.
No. Isotopes have the same atomic number, protons and electrons. They have different neutrons.
The atomic number of the isotopes of an element is identical; the mass number is different.
The different mass numbers are due to different numbers of neutrons.
Isotopes of an element have nuclei with the same number of protons (the same atomic number) but different numbers of neutrons Neutrons (:
Not a question of why. It just is, isotopes have the same atomic number, (which means that they are all the same element) with different neutron numbers.
No. By definition isotopes of an element have the same number of protons (that is what makes them uranium, for example) but different numbers of neutrons (neutral particules in the nucleus which provide mass).
Isotopes have different numbers of electrons, but not different atomic numbers (numbers of protons) or they'd be different elements.
The different isotopes have different atomic mass numbers, because the isotope has different numbers of neutrons. The protons and electrons are the same, so the change in mass number is the same as the change in the number of neutrons.
The isotopes of an element must have a different amount of neutrons. I'm pretty sure you know what these are, but just in case: A neutron is a sub-atomic part of an atom, together with protons and electrons.