Consider an atom of ⁶³Cu. (c) What is the symbol for the isotope of ⁶³Cu that possesses 36 neutrons?

Key Concepts

Isotopes

Isotopes are variants of a particular chemical element that have the same number of protons but different numbers of neutrons. This difference in neutron count results in varying atomic masses. For example, copper (Cu) has several isotopes, including 63Cu, which has 29 protons and 34 neutrons. Understanding isotopes is crucial for identifying specific forms of elements based on their neutron count.

Atomic Number and Mass Number

The atomic number of an element is the number of protons in its nucleus, which defines the element itself. The mass number is the total number of protons and neutrons in the nucleus. For 63Cu, the atomic number is 29 (indicating 29 protons), and the mass number is 63 (29 protons + 34 neutrons). This relationship is essential for determining the identity and properties of isotopes.

Neutron Count Calculation

To find the neutron count of an isotope, subtract the atomic number from the mass number. In the case of 63Cu, the mass number is 63 and the atomic number is 29, resulting in 34 neutrons. If an isotope has 36 neutrons, its mass number would be 29 (protons) + 36 (neutrons) = 65. This calculation is vital for identifying the correct isotope based on neutron count.