Atomic Structure and Electron Configuration

The formula 2n^2 determines the maximum number of electrons that can occupy a specific energy level or shell in an atom. 'n' represents the energy level or shell number. For example, the first shell (n=1) can hold a maximum of 2 electrons (2*1^2).

The first electron shell (also known as the K-shell) can hold a maximum of 2 electrons.

The second electron shell (L-shell) can hold a maximum of 8 electrons.

The third electron shell (M-shell) can hold a maximum of 18 electrons.

The fourth electron shell (N-shell) can hold a maximum of 32 electrons. The maximum number of electrons in each shell increases as the shell distance from the nucleus increases.

Electrons are filled in energy shells in a step-wise manner, meaning that the inner shells must be completely filled before electrons can occupy higher energy shells.

The outermost shell of an atom is called the valence shell, and the electrons in this shell are called valence electrons. For instance, in sodium (Na), the outermost shell (M-shell) has 1 electron, so it has 1 valence electron.

Atoms with 8 electrons in their outermost shell are considered stable and have a low tendency to form chemical bonds. These elements are known as inert gases, like Helium (He) and Neon (Ne), which are very unreactive.

Valency is the number of electrons an atom can gain, lose, or share during the formation of a chemical bond. The valency of elements determines their bonding capacity.

Atoms of the same element with the same number of protons but different numbers of neutrons. For example, Carbon-12 and Carbon-14 are isotopes of carbon, differing in the number of neutrons.

Atoms of different elements with the same mass number (total number of protons and neutrons). For instance, Calcium-40 (20 protons + 20 neutrons) and Argon-40 (18 protons + 22 neutrons) are isobars.

The average atomic mass of an element is the weighted average of the masses of its isotopes, taking into account their relative abundances. For example, chlorine, with isotopes of mass 35 u and 37 u, has an average atomic mass of 35.5 u.

A rule that states the maximum number of electrons that can occupy a specific energy level or shell in an atom.

Electrons fill energy shells in a stepwise manner, starting from the lowest energy shell and working their way outward. The inner shells must be completely filled before the electrons can occupy higher energy shells.

The average atomic mass of an element is calculated by taking the weighted average of the masses of its isotopes, considering their relative abundances. It is, therefore, not the mass of a single atom but a representative mass of all the isotopes present.

The distribution of electrons in different shells of an atom is called the electronic configuration.

The outermost shell of an atom that contains valence electrons, which are responsible for the atom's chemical properties.

A stable configuration where an atom has a full complement of eight electrons in its valence shell.

The number of protons present in the nucleus of an atom, determining its chemical identity.

The total number of protons and neutrons in the nucleus of an atom, determining its mass.

The subatomic particles that carry a positive charge and reside in the nucleus.

The subatomic particles that carry a negative charge and orbit the nucleus in specific energy levels.

The subatomic particles that carry no charge and reside in the nucleus.

A model that describes the arrangement of electrons in energy levels or shells around the nucleus.

The tendency of an atom to either gain, lose, or share electrons to achieve a stable electronic configuration.

Atoms that have gained or lost electrons, resulting in a net positive or negative charge.

The process of an atom losing electrons, resulting in a positive charge.

The process of an atom gaining electrons, resulting in a negative charge.

A force of attraction between atoms that holds them together in molecules and compounds.

The sharing of electrons between two atoms to achieve stability.

The transfer of electrons from one atom to another, resulting in the formation of ions and ionic bonds.

A bond formed by the sharing of electrons between two atoms that have a large difference in electronegativity.

A bond formed by the sharing of electrons between two atoms that have similar electronegativity.