Protons are located in the nucleus and carry a positive charge, which distinguishes them from electrons and neutrons. The positron is the antimatter counterpart of the electron.

Electrons have a negative charge and are located outside the nucleus in the electron cloud. Protons are positively charged and neutrons have no charge.

Neutrons are neutral particles found in the nucleus, carrying no electrical charge. Electrons and protons have negative and positive charges respectively, and an ion is a charged atom.

The nucleus is the central part of the atom and contains protons and neutrons, which account for most of the atom's mass. Electron clouds and orbitals refer to regions where electrons are likely to be found.

The atomic number is defined by the number of protons in an atom, which distinguishes one element from another. Although atomic mass also involves neutrons, the atomic number is solely determined by protons.

Isotopes of an element all have the same number of protons, which defines the element's identity, even though the number of neutrons may vary. This difference in neutrons leads to variations in atomic mass.

Atomic mass is roughly the sum of protons and neutrons since electrons have a negligible mass relative to them. This approximation is sufficient for most high school level calculations.

Electron configuration details how electrons are arranged in the available orbitals around the nucleus. It is essential for understanding chemical reactions and bonding.

The s-orbital is spherical in shape, which means it has the same shape in all directions. Other orbitals such as p, d, and f have more complex geometries.

A p-subshell consists of three orbitals, each of which can hold 2 electrons, giving a total capacity of 6 electrons. This is a key concept in understanding electron configurations.

The Bohr model describes electrons as moving in fixed orbits or energy levels around the nucleus. This was an early model that helped explain atomic emission spectra.

The principal quantum number 'n' specifies the main energy level of an electron in an atom. It is fundamental to determining the electron's overall energy and distance from the nucleus.

The electron cloud model describes electrons as being found in areas of probability, rather than in fixed orbits. This model better represents the behavior of electrons in atoms.

In a neutral atom, the number of electrons equals the number of protons, balancing the positive and negative charges. This balance is essential for the atom to remain electrically neutral.

The Bohr model was the first to introduce the concept of electrons in fixed orbits around the nucleus. This model provided a stepping stone toward our modern understanding of atomic structure.

A d-subshell contains 5 orbitals, each capable of holding 2 electrons. This gives the d-subshell a total capacity of 10 electrons.

The Aufbau principle states that electrons occupy the lowest energy orbitals available before moving to higher energy levels. This concept is fundamental to constructing accurate electron configurations.

The superscript in an electron configuration denotes how many electrons are present in a specific subshell or orbital. It is a critical notation for understanding the distribution of electrons in an atom.

An f-subshell consists of 7 orbitals, each capable of holding 2 electrons, resulting in a maximum of 14 electrons. This capacity is an important factor in the properties of f-block elements.

Electron spin is one of the four quantum numbers and distinguishes electrons from one another. The Pauli Exclusion Principle relies on differing spins to ensure that no two electrons in the same orbital share all identical quantum numbers.