Isotopes - Practice

Isotopes are variants of a particular chemical element that have the same number of protons but different numbers of neutrons, resulting in different mass numbers.

To find the number of neutrons, subtract the atomic number (number of protons) from the mass number (A). Neutrons = A - Z.

The atomic number is the number of protons in the nucleus of an atom, which determines the element's identity.

The mass number (A) is the total number of protons and neutrons in the nucleus of an atom.

53 neutrons (89 - 36 = 53).

Isotopes of the same element have the same atomic number and number of protons.

In a neutral atom, the number of protons equals the number of electrons.

22 protons.

The mass number indicates the total number of nucleons (protons + neutrons) in the nucleus, affecting the isotope's stability.

Isotopes differ in the number of neutrons, while ions differ in the number of electrons, resulting in a charge.