Atomic Weight: Atomic weight, also known as relative atomic mass, is the average mass of an element's atoms, taking into account the abundance of different isotopes. Isotopes are atoms of the same element that have different numbers of neutrons in their nuclei, resulting in variations in their atomic masses. Atomic weight is expressed in atomic mass units (u) and is typically listed below the element's symbol on the periodic table. It represents the weighted average of the masses of all naturally occurring isotopes of an element.
Atomic Mass: Atomic mass refers to the mass of a single atom of an element. It is also expressed in atomic mass units (u) and is typically very close to the atomic weight of the element. However, since atomic mass considers a single atom, it may not account for the slight variations in isotopic abundances found in nature.
Atomic Number: Atomic number represents the number of protons in an atom's nucleus and determines the element's identity. It is a fundamental property of an element and is used to organize elements in the periodic table. Atomic number is represented by the whole number above an element's symbol in the periodic table.
All three of these properties are included in the periodic table. The periodic table provides a structured arrangement of elements based on their atomic number, with elements organized into periods (rows) and groups (columns). The atomic number, symbol, and atomic weight are typically listed for each element in the periodic table, providing key information about an element's identity and atomic properties.