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Mass number (A) is the total number of protons and neutrons in an atomic nucleus. It is approximately equal to the atomic mass of the atom in atomic mass units. Learn how mass number changes in radioactive decay and how it differs from atomic weight and isotopic mass.
Atomic number is the number of protons in the atomic nucleus of an element. It can be used to identify and order elements in the periodic table, and it is related to the charge, mass and spectral properties of atoms.
Potassium is a silvery white metal and an alkali metal with symbol K and atomic number 19. It reacts vigorously with water and oxygen, and is essential for plants and animals. Learn about its discovery, isotopes, applications and more.
A table or chart of nuclides is a graph of isotopes of the elements, based on their numbers of neutrons and protons. Isodiaphers are nuclides with the same difference between their numbers of neutrons and protons (N − Z), and they follow diagonal lines at right angles to the isobar lines.
Neutron number is the number of neutrons in a nuclide. Learn about its properties, relation to atomic number and mass number, and examples of stable and unstable nuclides with different neutron numbers.
An atom is the smallest particle of an element that has the same chemical properties as the element. It consists of a nucleus of protons and neutrons, surrounded by electrons. Learn about the history of atomic theory, the structure and properties of atoms, and how they form compounds.
Learn about the periodic table of the chemical elements, an ordered arrangement of the elements by atomic number and properties. Explore the history of the table, from Mendeleev's predictions to the discovery of new elements and blocks.
This web page shows the number and stability of isotopes for each element in the periodic table. A stable atom that has a large nucleus most likely contains more neutrons than protons, as the ratio of neutrons to protons affects the stability of the nucleus.