Determine the number of protons and the number of neutrons in each isotope. a. ⁴⁰₁₉K b. ²²⁶₈₈Ra c. ⁹⁹₄₃Tc d. ³³₁₅P

Isotopes are variants of a particular chemical element that have the same number of protons but different numbers of neutrons. This means they share the same atomic number but have different mass numbers. For example, potassium-40 (40 19K) has 19 protons and 21 neutrons, while potassium-39 would have 19 protons and 20 neutrons.

The atomic number of an element, represented by the lower number in isotope notation, indicates the number of protons in the nucleus. The mass number, shown as the upper number, is the total count of protons and neutrons. For instance, in 40 19K, the atomic number is 19 (protons), and the mass number is 40, leading to the calculation of neutrons as 40 - 19 = 21.

The nuclear composition of an atom refers to the arrangement and quantity of protons and neutrons within its nucleus. Understanding this composition is essential for identifying isotopes and their properties. For example, knowing that 226 88Ra has 88 protons allows us to determine it has 138 neutrons (226 - 88 = 138), which is crucial for understanding its stability and behavior in nuclear reactions.