Atomic structure

Atoms: The building blocks of matter consist of atoms. These are composed of protons, neutrons, and electrons, and they determine the properties of matter.

Elemental composition of atoms: Each atom is unique and is characterized by its number of protons, which determines its elemental identity.

Valence electrons: An atom's outermost electrons that participate in chemical bonding are known as valence electrons.

Chemical bonds: A chemical bond is the force that holds atoms together in chemical compounds. These may be covalent, ionic, or metallic.

Lewis dot structures: A simple way to depict the valence electrons of an atom or molecule is using Lewis dot structures.

Electronegativity: Electronegativity is a measure of an atom's ability to attract electrons when involved in a chemical bond.

Ions: Atoms or molecules that have gained or lost electrons, resulting in a net charge, are called ions.

Electron configuration: The distribution of electrons in an atom or ion's various energy levels is referred to as its electron configuration.

Hybridization: The process that occurs when orbitals of similar energies mix to form hybrid orbitals.

Molecular geometry: The three-dimensional arrangement of atoms in a molecule is referred to as its molecular geometry.

Orbital hybridisation: Mixing of atomic orbitals forming hybrid orbitals and provide bonding.

Bond polarity: A term to describe the degree of inequality in electron sharing between two atoms in a covalent bond.

Molecular Orbital Theory: A theory that describes the electronic structure of molecules using a combination of atomic orbitals to form molecular orbitals.

VSEPR theory: The Valence Shell Electron Pair Repulsion theory helps us predict the shapes of molecules based on the repulsion between electrons.

Intramolecular Bonding: Bonding within a single molecule, which is responsible for its stability and properties.

Ionic Bonding: This type of bonding involves the transfer of electrons between two atoms. One atom loses electrons and becomes positively charged, and the other atom gains electrons and becomes negatively charged. These oppositely charged ions attract one another and form an ionic bond.

Covalent Bonding: This type of bonding involves the sharing of electrons between two atoms. The electrons are shared between the atoms in such a way as to create a stable molecule.

Metallic Bonding: This type of bonding involves the sharing of electrons between all the atoms in a metal. The electrons move freely through the metal and create a "sea" of electrons that hold the metal together.

Hydrogen Bonding: This is an electrostatic attraction between a hydrogen atom in a polar covalent bond and an electronegative atom, such as oxygen or nitrogen, in another molecule. This attraction occurs because the hydrogen has a partial positive charge and the other atom has a partial negative charge.

Van der Waals Bonding: This type of bonding is a weak intermolecular force that occurs between non-polar molecules. The attraction is caused by temporary fluctuations in electron density around the atoms in the molecule.

Dipole-Dipole Bonding: This type of bonding occurs when two polar molecules interact with one another. The positive end of one molecule is attracted to the negative end of the other molecule.

Coordinate Covalent Bond: This type of bonding occurs when both electrons in a covalent bond are contributed by one of the atoms. The atom that contributes both electrons is called the donor, and the atom that accepts the electrons is called the acceptor.

Pi Bonding: This type of bonding occurs when two atoms share electrons in a region of high electron density above and below the plane of the bonding atoms. This occurs in double and triple covalent bonds.

Sigma Bonding: This type of bonding occurs when two atoms share electrons in a region along an imaginary axis between the two atoms. This occurs in single covalent bonds.