Electron vs. Proton — What's the Difference?

Electrons carry a negative charge.

Significantly greater than that of electrons.

Found in the orbits around an atom's nucleus.

Resides within the nucleus of an atom.

Extremely small compared to protons.

Number remains constant in chemical reactions.

Essential for chemical bonding and reactions.

Protons carry a positive charge.

Loss or gain leads to ionization.

Defines the chemical element.

The electron is a subatomic particle, symbol e− or β−, whose electric charge is negative one elementary charge. Electrons belong to the first generation of the lepton particle family, and are generally thought to be elementary particles because they have no known components or substructure.

A proton is a subatomic particle, symbol p or p+, with a positive electric charge of +1e elementary charge and a mass slightly less than that of a neutron. Protons and neutrons, each with masses of approximately one atomic mass unit, are jointly referred to as "nucleons" (particles present in atomic nuclei).

A stable elementary particle in the lepton class having a negative electric charge of 1 elementary unit (about 1.602 × 10-19 coulombs) and a mass of about 9.11 × 10-28 grams. Electrons are found in shells orbiting the nuclei of atoms and can also move freely through space as cathode rays in a cathode-ray tube or as beta particles emitted by radioactive nuclei, or flow in a current through a conducting material impelled by an electric potential difference.

The stable, positively charged nucleon, having a mass 1,836 times that of an electron and being a baryon composed of two up quarks and one down quark. The proton is a basic component of all atomic nuclei and the nucleus of the protium isotope of hydrogen.

(particle) The subatomic particle having a negative charge and orbiting the nucleus; the flow of electrons in a conductor constitutes electricity.

(particle) A positively charged subatomic particle forming part of the nucleus of an atom and determining the atomic number of an element, composed of two up quarks and a down quark.

Alloys of magnesium and other metals, like aluminum or zinc, that were manufactured by the German company Chemische Fabrik Griesheim-Elektron.

The atomic nucleus of protium hydrogen-1}}

Amber; also, the alloy of gold and silver, called electrum.

Synonym of primordium

One of the fundamental subatomic particles, having a negative charge and about one thousandth the mass of a hydrogen atom. The electron carries (or is) a natural unit of negative electricity, equal to 3.4 x 10-10 electrostatic units, and is classed by physicists as a lepton. Its mass is practically constant at the lesser speeds, but increases due to relativistic effects as the velocity approaches that of light. Electrons are all of one kind, so far as is known. Thus far, no structure has been detected within an electron, and it is probably one of the ultimate composite constituents of all matter. An atom or group of atoms from which an electron has been detached has a positive charge and is called a cation. Electrons are projected from the cathode of vacuum tubes (including television picture tubes) as cathode rays and from radioactive substances as the beta rays. Previously also referred to as corpuscle, an obsolete term. The motion of electrons through metallic conductors is observed as an electric current. A particle identical to the electron in mass and most other respects, but having a positive instead of a negative charge, is called a positron, or antielectron

A stable particle with positive charge equal to the negative charge of an electron

An elementary particle with negative charge

Electrons participate directly in chemical reactions through the formation of bonds by either sharing electrons between atoms or transferring them from one atom to another.

It becomes an ion; loss of electrons results in a positive ion (cation), while gain of electrons results in a negative ion (anion).

Yes, when this occurs, the atom is no longer neutral and is referred to as an ion.

Neutrons, located in the nucleus alongside protons, contribute to an atom's mass but not its charge. They play a critical role in the stability of the nucleus.

The number and arrangement of electrons in an element determine its chemical properties, as these affect how it interacts and bonds with other elements.

Electron orbitals define the regions around an atom's nucleus where electrons are likely to be found, influencing an atom's chemical behavior and bonding capabilities.

The balance between the number of protons (positive charge) and electrons (negative charge) determines an atom's overall charge.

Because its mass is so much smaller than that of protons or neutrons, it has minimal impact on the total mass of an atom.

In chemical reactions, no, but in nuclear reactions, such as nuclear decay or fusion, the number of protons can change, transforming one element into another.

The number of protons determines the atomic number, which defines the element and its position on the periodic table, influencing its chemical properties.

Chemical reactions involve the rearrangement of electrons between atoms; changing the number of protons would involve altering the nucleus, which requires nuclear reactions.

Ionization energy is the energy required to remove an electron from an atom or ion, reflecting the strength of an atom's hold on its electrons.

Both are fundamental subatomic particles essential to the structure and function of atoms, with opposite charges that attract each other, maintaining atomic stability.

Electrons form bonds between atoms by either sharing in covalent bonds or transferring in ionic bonds, determining the molecular structure of compounds.

In nuclear reactions, the number of protons can change, altering the element itself; electrons may be affected indirectly through changes in charge balance but are not the focus of nuclear transformations.