Short Answer

Atoms are made up of three main subatomic particles: electrons, protons, and neutrons. Each particle has a specific charge and mass. Protons are positively charged, electrons are negatively charged, and neutrons have no charge.

In terms of mass, protons and neutrons are nearly equal and much heavier than electrons. Understanding the charges and masses of these particles helps explain atomic structure, chemical behavior, and the stability of atoms.

Detailed Explanation :

Subatomic Particles: Charges and Masses

An atom consists of a nucleus and electrons surrounding it. The nucleus contains protons and neutrons, while electrons move in orbitals around it. The three subatomic particles have distinct properties:

Electron (e⁻)

Charge: Negative, –1 elementary charge (–1.602 × 10⁻¹⁹ C)
Mass: Very small, approximately 9.109 × 10⁻³¹ kg (about 1/1836 of a proton)
Location: Outside the nucleus in orbitals
Role: Electrons determine chemical properties, bonding, and reactivity of atoms. Their negative charge balances the positive charge of protons, making the atom electrically neutral.

Proton (p⁺)

Charge: Positive, +1 elementary charge (+1.602 × 10⁻¹⁹ C)
Mass: About 1.673 × 10⁻²⁷ kg (roughly 1836 times heavier than an electron)
Location: Inside the nucleus
Role: Protons determine the atomic number of an element and its identity. The positive charge helps attract electrons and holds the nucleus together with neutrons.

Neutron (n⁰)

Charge: Neutral (0)
Mass: About 1.675 × 10⁻²⁷ kg (slightly more than a proton)
Location: Inside the nucleus
Role: Neutrons provide mass to the atom and stabilize the nucleus by reducing repulsion between positively charged protons.

Comparison of Masses and Charges

Particle	Charge	Mass (kg)	Relative Mass
Electron	–1	9.109 × 10⁻³¹	1
Proton	+1	1.673 × 10⁻²⁷	1836
Neutron	0	1.675 × 10⁻²⁷	1839

Electrons have negligible mass compared to protons and neutrons.
Protons and neutrons contribute almost all the mass of an atom.

Importance in Atomic Structure

Electrical Neutrality: Atoms have equal numbers of protons and electrons, balancing charges.
Atomic Mass: The sum of protons and neutrons determines the atomic mass of the element.
Chemical Behavior: Electrons determine how an atom reacts chemically, while protons and neutrons maintain stability.
Isotopes: Atoms of the same element with different numbers of neutrons have different masses but similar chemical properties.

Historical Context

Electron: Discovered by J.J. Thomson in 1897 using cathode ray experiments.
Proton: Identified by Ernest Rutherford in 1917 through nuclear experiments.
Neutron: Discovered by James Chadwick in 1932, explaining the missing mass in nuclei.

Summary of Roles

Electrons: Chemical reactions, bonding, electrical behavior.
Protons: Define element identity, positive charge in nucleus.
Neutrons: Nuclear stability, contribute to mass.

Visual Representation

Nucleus: Contains protons (p⁺) and neutrons (n⁰), dense and massive.
Electron Cloud: Electrons (e⁻) occupy orbitals around the nucleus.

This distribution explains atomic stability, charge neutrality, and mass distribution in atoms.

Conclusion

Subatomic particles—electrons, protons, and neutrons—have distinct charges and masses that define atomic structure. Electrons are negatively charged and light, protons are positively charged and heavy, and neutrons are neutral with similar mass to protons. Understanding these properties is fundamental for explaining chemical behavior, atomic mass, isotopes, and nuclear stability, forming the foundation of modern chemistry.