Home›Calculators›Chemistry›Atom Calculator

Atom Calculator

Chemistry

Calculate the number of protons, neutrons, electrons, and mass number for any element and isotope. Includes ion configuration and nuclear composition.

1118
12
0

Protons

6
Neutrons
6
Electrons
6
Mass Number
12
Atom / Ion Type
Neutral C atom

This calculator computes your Protons, Neutrons, Electrons, Mass Number, Atom / Ion Type from the values you enter.

Inputs
Atomic Number (Z)Mass Number (A)Ion Charge
Outputs
ProtonsNeutronsElectronsMass NumberAtom / Ion Type

What is a Atom?

The Atom Calculator computes the number of protons, neutrons, and electrons for any atom or ion given its atomic number (Z), mass number (A), and ion charge. Enter these three values to get the complete nuclear and electronic composition.

Protons = Z (always equal to the atomic number — this defines the element). Neutrons = A − Z (mass number minus atomic number). Electrons = Z − charge (for a neutral atom, charge = 0, so electrons = protons; for Na⁺ with charge +1, electrons = 11 − 1 = 10). The calculator also identifies the atom or ion type — neutral atom, cation (positive), or anion (negative).

This is the starting point for understanding atomic structure in NCERT Class 9 (Structure of the Atom), Class 11 (Atomic Structure chapter), and all JEE/NEET atomic structure problems. The Atomic Mass Calculator provides the standard atomic mass (in g/mol) for each element. The Electron Configuration Calculator shows how the electrons are distributed across subshells.

How to use this Atom calculator

  1. Enter Atomic Number Z — look up on the periodic table (H=1, C=6, Na=11, Cl=17, Fe=26).
  2. Enter Mass Number A — the isotope's mass (must be ≥ Z). If not specified, use the most abundant isotope's A from the Atomic Mass Calculator.
  3. Enter Ion Charge — 0 for neutral atom, +1 for singly charged cation (e.g. Na⁺), −1 for anion (Cl⁻), +2 for doubly charged (Mg²⁺), etc.
  4. Read Protons (= Z), Neutrons (= A − Z), Electrons (= Z − charge).
  5. Use the Atom/Ion Type description to confirm the species — e.g., "Na⁺ cation (lost 1 electron)".

Formula & Methodology

Subatomic particle formulas:

Protons   = Z           (atomic number — defines the element) Neutrons  = A − Z       (mass number minus atomic number) Electrons = Z − charge  (charge=0 neutral, charge>0 cation, charge<0 anion) Mass Number = A = Z + N

Worked example — Fe³⁺ ion (¹⁶Fe, the most common iron isotope ⁵⁶Fe):

Z = 26 (iron), A = 56, charge = +3.

Protons   = 26 Neutrons  = 56 − 26 = 30 Electrons = 26 − 3  = 23 Ion type  = Fe³⁺ cation (lost 3 electrons)

Fe³⁺ with 23 electrons has the configuration [Ar] 3d⁵ — a half-filled d-subshell, which is particularly stable. Fe³⁺ (ferric iron) is the form found in rust (Fe₂O₃), haematite (iron ore mined in Odisha and Chhattisgarh), and many industrial catalysts. SAIL's blast furnaces in Bhilai process millions of tonnes of Fe₂O₃ annually, reducing Fe³⁺ to Fe⁰ (metallic iron) using coke (carbon) as the reducing agent.

Frequently Asked Questions

An atom is the smallest unit of matter that retains the chemical properties of an element. It consists of three types of subatomic particles: protons (positive charge, mass ≈ 1 u, in the nucleus), neutrons (neutral, mass ≈ 1 u, in the nucleus), and electrons (negative charge, mass ≈ 0.00055 u, in shells around the nucleus). The number of protons (atomic number Z) defines which element the atom is. The number of neutrons determines which isotope of that element. The number of electrons determines whether the atom is neutral or an ion.
Atomic number (Z) = number of protons in the nucleus — uniquely identifies the element (Z=6 is always carbon, regardless of isotope or ion state). Mass number (A) = number of protons + number of neutrons — determines which isotope. Neutron number (N) = A − Z — number of neutrons. For carbon-12: Z=6, A=12, N=6. For carbon-13: Z=6, A=13, N=7. For carbon-14 (radioactive): Z=6, A=14, N=8. All three are the same element (carbon) because Z is unchanged.
An ion is an atom (or molecule) that has gained or lost one or more electrons, giving it a net electric charge. Cation (positive ion): an atom that lost electrons → fewer electrons than protons. Anion (negative ion): an atom that gained electrons → more electrons than protons. For any ion: electrons = Z − charge. For Na⁺ (Z=11, charge=+1): electrons = 11 − 1 = 10. For Cl⁻ (Z=17, charge=−1): electrons = 17 − (−1) = 18. Both Na⁺ and Cl⁻ have 10 and 18 electrons respectively — the same as Ne and Ar, making them isoelectronic with noble gases.
Enter Atomic Number Z (1–118), Mass Number A (must be ≥ Z), and Ion Charge (0 for neutral, +1 for cation, −1 for anion, etc.). The calculator returns protons = Z, neutrons = A − Z, electrons = Z − charge, mass number, and the atom/ion type description. Default: ¹²C (Z=6, A=12, charge=0) — carbon-12, neutral atom, 6 protons, 6 neutrons, 6 electrons.
Isotopes are atoms of the same element (same Z, same proton count) with different mass numbers (different neutron counts). ¹²C: 6 protons, 6 neutrons. ¹³C: 6 protons, 7 neutrons. ¹⁴C: 6 protons, 8 neutrons. All are carbon isotopes. ²³⁵U: 92 protons, 143 neutrons. ²³⁸U: 92 protons, 146 neutrons. Both are uranium isotopes. The [Average Atomic Mass Calculator](/average-atomic-mass-calculator/) computes the weighted average mass over all isotopes based on natural abundance.
The maximum electrons in shell n = 2n². Shell 1 (K): max 2 electrons. Shell 2 (L): max 8. Shell 3 (M): max 18. Shell 4 (N): max 32. However, the outermost shell (valence shell) holds a maximum of 8 electrons in main-group elements (octet rule). The [Electron Configuration Calculator](/electron-configuration-calculator/) gives the detailed subshell distribution (1s², 2s², 2p⁶, etc.) for any element. The Atom Calculator gives the total count; the Electron Configuration Calculator gives the arrangement.
Light elements tend to have equal or nearly equal proton and neutron counts in their most stable isotope: ¹H (1p, 0n), ⁴He (2p, 2n), ¹²C (6p, 6n), ¹⁴N (7p, 7n), ¹⁶O (8p, 8n), ²⁴Mg (12p, 12n), ⁴⁰Ca (20p, 20n). As Z increases, the neutron/proton ratio increases above 1 to provide additional nuclear binding force — ²⁰⁸Pb has 82 protons and 126 neutrons (ratio ≈ 1.54). Elements beyond Z=83 (bismuth) have no stable isotopes.
Na⁺ (Z=11, A=23, charge=+1): 11 protons, 12 neutrons, 10 electrons. Mg²⁺ (Z=12, A=24, charge=+2): 12 protons, 12 neutrons, 10 electrons. Al³⁺ (Z=13, A=27, charge=+3): 13 protons, 14 neutrons, 10 electrons. Cl⁻ (Z=17, A=35, charge=−1): 17 protons, 18 neutrons, 18 electrons. Ca²⁺ (Z=20, A=40, charge=+2): 20 protons, 20 neutrons, 18 electrons. O²⁻ (Z=8, A=16, charge=−2): 8 protons, 8 neutrons, 10 electrons. Na⁺, Mg²⁺, Al³⁺, and O²⁻ are all isoelectronic — they all have 10 electrons like neon.
Proton mass: m_p = 1.00728 u = 1.67262 × 10⁻²⁷ kg. Neutron mass: m_n = 1.00866 u = 1.67493 × 10⁻²⁷ kg (slightly heavier than proton). Electron mass: m_e = 0.000549 u = 9.10938 × 10⁻³¹ kg (about 1836 times lighter than a proton). The electron mass is negligible for atomic mass calculations — the total atomic mass ≈ number of protons × 1.00728 + number of neutrons × 1.00866, minus the nuclear binding energy (mass defect). The mass defect is what holds the nucleus together.
Atomic number Z is the fundamental organising principle of the periodic table — it increases by 1 with each element and uniquely identifies each element. Mendeleev's original table ordered by atomic mass; Moseley (1913) showed atomic number (number of protons) is the more fundamental quantity. The periodic table period (row) indicates the highest principal quantum number of the valence electrons. The group (column) indicates the number of valence electrons. The [Effective Nuclear Charge Calculator](/effective-nuclear-charge-calculator/) shows how Z affects the attraction electrons feel as inner-shell shielding increases down a group.