Atomic Mass Calculation and Isotopes Quiz

The atomic mass number of a carbon atom is calculated by adding the number of protons and neutrons, which is equal to 6 protons + 6 neutrons = $6 \times 1.672 \times 10^{-24} + 6 \times 1.674 \times 10^{-24} = 12.0939$ amu.

Elements that have no isotopes are called monotropic elements. For example, $^{15}P$ is a monotropic element.

Isotopes are nuclides of the same element that possess the same number of protons and electrons but differ in the number of neutrons. An example is carbon isotopes, such as $^{12}C$, $^{13}C$, and $^{14}C$.

<p>The relative atomic mass (Ar) of an element is the weighted average of the mass numbers of all its isotopes. An example calculation for naturally occurring chlorine is: $Ar = (75.77% \times 35.45) + (24.23% \times 36.97) = 35.45$.</p> Signup and view all the answers

<p>The unit of atomic mass number is the atomic mass unit (amu = $1.66 \times 10^{-24}$ g). It is convenient to use this unit because it allows for easy comparison of atomic masses and simplifies calculations involving atomic mass.</p> Signup and view all the answers