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A chemical element is an identity shared by all chemical atoms whose atomic nuclei contain the same number of protons. That number is its atomic number, $Z$: six means carbon, eleven means sodium. The identity survives differences in neutron count, which distinguish isotopes, and differences in Electron count, which distinguish neutral chemical atoms from ions. See the IUPAC Gold Book, chemical element.

The same name can also denote a pure chemical substance containing only that chemical element. These two uses answer different questions. Molecular oxygen, ${\mathrm{O}}_2$, is a chemical substance made entirely of oxygen; water, ${\mathrm{H}}_2\mathrm{O}$, is a chemical compound containing both hydrogen and oxygen. A water molecule contains three chemical atoms but only two chemical elements. Joining chemical atoms through chemical bonds changes their arrangement without changing their atomic numbers.

This distinction makes stoichiometry possible: ordinary chemical reactions rearrange chemical atoms, so one can count each chemical element before and after a transformation. Changing the proton count instead changes the chemical element and requires a nuclear reaction. The periodic table organizes these identities into a useful map, while atomic number bookkeeping keeps identity, isotope, and electric charge separate.

A nuclear reaction transforms one or more atomic nuclei through interactions with particles or other nuclei. Total energy, momentum, electric charge and nucleon number constrain ordinary low-energy reaction bookkeeping. Nuclear fusion, alpha capture, neutron capture and photodisintegration are important examples in stellar nucleosynthesis. Weak processes can also change the proton-to-neutron ratio.

Nucleosynthesis is the production of atomic nuclei through nuclear reactions. It includes Big Bang nucleosynthesis, stellar nucleosynthesis and production in explosive or compact-remnant environments. Making nuclei and delivering them to the interstellar medium are separate steps in chemical enrichment.