"A chemical bond is a lasting attraction between atoms or ions that enables the formation of molecules, crystals, and other structures."
The study of how atoms combine to form molecules through the sharing of electrons or the transfer of electrons between atoms.
Electronegativity: A measure of an atom's ability to attract electrons in a chemical bond.
Ionic bonding: The transfer of one or more electrons from a metal to a non-metal, resulting in the formation of ions.
Covalent bonding: A type of bonding where atoms share electrons in order to complete their valence electron shells.
Lewis structures: Diagrams that show the arrangement of atoms and electrons in a molecule.
Resonance: The delocalization of electrons in a molecule or ion, resulting in multiple viable structures.
Hybridization: The mixing of atomic orbitals to form hybrid orbitals that can be used to explain molecular shape and bonding.
Bond energies: The amount of energy required to break a chemical bond.
Molecular orbital theory: A theory that describes the behavior of electrons in molecules using mathematical functions.
Valence bond theory: A theory that describes chemical bonding as the overlapping of atomic orbitals.
Intermolecular forces: Forces that exist between molecules, including Van der Waals forces, dipole-dipole forces, and hydrogen bonding.
Molecular polarity: The uneven distribution of charge within a molecule, which can affect its physical and chemical properties.
Chemical reactions: The process by which atoms or molecules interact to form new substances.
Metallic bonding: The bonding between metal atoms, characterized by a sharing of electrons in a giant, delocalized network.
Quantum mechanics: The branch of theoretical chemistry that describes the behavior of atoms and molecules using mathematical models.
Chemical kinetics: The study of the rates at which chemical reactions occur and the factors that influence them.
Ionic Bonding: This type of bonding occurs between metals and non-metals. The transfer of valence electrons from metal atoms to non-metal atoms creates a lattice structure with opposite charges attracting each other, forming an ionic compound.
Covalent Bonding: This type of chemical bonding is a result of sharing electrons to form a molecule. Covalent bonds are strong and are formed between non-metal atoms.
Metallic Bonding: It is a type of bonding that exists between metallic atoms. Here, free electrons that are spread throughout the metal conduct electricity, and each metal atom is bonded to several adjacent metal atoms.
Hydrogen Bonding: Hydrogen bonding occurs when hydrogen is bonded to a highly electronegative atom such as oxygen, nitrogen, or fluorine. These bonds are weaker than covalent bonds, but play a pivotal role in the properties of molecular compounds.
Van der Waals Forces: These are intermolecular forces that occur between non-polar molecules, unlike ionic compounds or polar covalent compounds. This force is the result of temporary fluctuations in electron cloud distribution and creates dipole-dipole interactions, London dispersion forces, and hydrogen bonding.
Dipole-Dipole Bonding: Dipole-dipole bonding is a type of bonding that occurs between polar molecules. The positive and negative ends of the molecules attract each other, which strengthens this type of bond.
London Dispersion Forces: London dispersion forces occur between all molecules regardless of their polarity. A temporary dipole in one molecule can induce a corresponding dipole in a nearby molecule, resulting in attractive forces between them.
Coordinate Covalent Bonding: Coordinate covalent bonding occurs when one atom donates a pair of electrons to another atom, which requires a lone pair of electrons. This process creates a shared valence electron pair and a new molecule or compound.
Pi Bonding: Pi bonding occurs between atoms where one or more electrons in each of the orbitals in the pi bond overlap to form a single bond. These electrons are located in parallel or slightly overlapping p-orbitals. It is a weaker bond than sigma bonding.
Sigma Bonding: Sigma bonding is formed when two atomic orbitals containing a single electron with equal and opposite spin, converge together in the interatomic space between two nuclei, to form a covalent bond. It is stronger than pi bonding.
"The bond may result from the electrostatic force between oppositely charged ions as in ionic bonds, or through the sharing of electrons as in covalent bonds."
"There are 'strong bonds' or 'primary bonds' such as covalent, ionic and metallic bonds."
"There are 'weak bonds' or 'secondary bonds' such as dipole–dipole interactions, the London dispersion force, and hydrogen bonding."
"Since opposite electric charges attract, the negatively charged electrons surrounding the nucleus and the positively charged protons within a nucleus attract each other."
"Electrons shared between two nuclei will be attracted to both of them."
"Constructive quantum mechanical wavefunction interference stabilizes the paired nuclei."
"Bonded nuclei maintain an optimal distance (the bond distance) balancing attractive and repulsive effects explained quantitatively by quantum theory."
"The atoms in molecules, crystals, metals, and other forms of matter are held together by chemical bonds, which determine the structure and properties of matter."
"The octet rule and VSEPR theory are examples. More sophisticated theories are valence bond theory, which includes orbital hybridization and resonance, and molecular orbital theory which includes the linear combination of atomic orbitals and ligand field theory."
"Electrostatics are used to describe bond polarities and the effects they have on chemical substances."
"The atoms in molecules, crystals, metals, and other forms of matter are held together by chemical bonds..."
"The negatively charged electrons surrounding the nucleus and the positively charged protons within a nucleus attract each other."
"Bonded nuclei maintain an optimal distance (the bond distance) balancing attractive and repulsive effects explained quantitatively by quantum theory."
"...such as dipole–dipole interactions, the London dispersion force, and hydrogen bonding."
"The bond may result from...the sharing of electrons as in covalent bonds."
"The octet rule and VSEPR theory are examples..."
"Valence bond theory, which includes orbital hybridization and resonance, and molecular orbital theory which includes the linear combination of atomic orbitals and ligand field theory."
"Electrons shared between two nuclei will be attracted to both of them."
"The bond may result from the electrostatic force between oppositely charged ions as in ionic bonds, or through the sharing of electrons as in covalent bonds."