The atom is fundamentally composed of a nucleus and three key subatomic particles: protons, neutrons, and electrons. Each of these particles has distinct characteristics, particularly in terms of mass and charge. A crucial concept in understanding atomic mass is the atomic mass unit (AMU), which serves as a standard for measuring the relative mass of atoms and subatomic particles.
By definition, 1 AMU is equivalent to 1/12th the mass of a carbon atom, providing a reference point for atomic mass calculations. It's important to note that 1 AMU is also equal to 1 Dalton (DA), a term named after John Dalton, a pivotal figure in the field of chemistry. Dalton's contributions, along with those of other foundational chemists, have significantly advanced our understanding of atomic structure, subatomic particles, and radioactivity.
For practical applications, remember that 1 AMU can be converted to kilograms using the conversion factor: 1 \text{ AMU} = 1.66 \times 10^{-27} \text{ kg}. This relationship allows for seamless interconversion between AMU and kilograms, which is essential for various calculations in chemistry and physics.