Enter an Atomic Number (Z), Mass Number (A), or any known values like Number of Protons, Neutrons, or Ion Charge to calculate the complete atomic structure of any element — including its Protons (p⁺), Neutrons (n⁰), Electrons (e⁻), and full Element Information.
Element Information
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Protons (p⁺)
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Neutrons (n⁰)
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Electrons (e⁻)
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Atomic Number (Z)
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Mass Number (A)
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Net Charge
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An atom is the smallest unit of matter that retains the properties of an element. It consists of a nucleus containing protons and neutrons, surrounded by electrons in orbital shells. Protons have positive charge, electrons have negative charge, and neutrons are neutral.
The atomic number (Z) equals the number of protons in the nucleus and defines the element. The mass number (A) is the sum of protons and neutrons. For example, carbon-12 has atomic number 6 and mass number 12.
In a neutral atom, the number of protons equals the number of electrons. The number of neutrons equals the mass number minus the atomic number (n = A - Z). Ions have unequal protons and electrons, creating a net charge.
To find neutrons, subtract the atomic number from the mass number: Neutrons = Mass Number - Atomic Number. For example, carbon-14 has 14 - 6 = 8 neutrons.
The number of protons (atomic number) determines an element's identity. All atoms with 6 protons are carbon, regardless of the number of neutrons or electrons. Changing the number of neutrons creates isotopes, while changing electrons creates ions.
Ions are atoms that have gained or lost electrons, resulting in a net electric charge. Cations (positive ions) have fewer electrons than protons, while anions (negative ions) have more electrons than protons.
The mass number would be 4 (2 protons + 2 neutrons). This describes helium-4, the most common isotope of helium with atomic number 2.
Yes, atoms of the same element can have different numbers of neutrons, creating isotopes. For example, carbon-12 has 6 neutrons while carbon-14 has 8 neutrons, but both have 6 protons and are carbon.