"A chemical bond is a lasting attraction between atoms or ions that enables the formation of molecules, crystals, and other structures."
The types of chemical bonds that hold materials together, such as covalent, ionic, and metallic bonds.
Types of Chemical Bonds: It includes covalent, ionic, metallic, and hydrogen bonds. Knowing the characteristics and differences between each type of bond is essential.
Lewis Dot Structure: A method of representing the valence electrons of an atom and drawing the structures of covalent molecules.
Electronegativity: A measure of an atom's ability to attract electrons in a chemical bond.
Octet Rule: A concept stating that atoms tend to combine in a way that results in a full outer shell of eight valence electrons.
Molecular Geometry: The arrangement of atoms in a molecule and its effects on properties like polarity and reactivity.
Hybridization: A model that describes how atomic orbitals combine to form new hybrid orbitals adapted to the bonding situation in molecules.
Resonance: A phenomenon where a molecule can have multiple valid Lewis structures that differ only in the placement of electrons.
Intermolecular Forces: Attractions between molecules that affect the properties of materials like melting point, boiling point, and solubility.
Lewis Acid-Base Chemistry: A framework for understanding acid-base reactions at the molecular level.
Crystal Structure: The arrangement of atoms in a crystal lattice and its effects on the properties of solids like conductivity, refractive index, and hardness.
Ionic Bond: A chemical bond between two ions with opposite charges.
Covalent Bond: A chemical bond in which atoms share pairs of electrons.
Metallic Bond: A bond formed between metal atoms in which the outer electrons of each atom are delocalized and shared amongst all atoms in the metal.
Hydrogen Bond: A weak electrostatic attraction that occurs when a hydrogen atom covalently bound to an electronegative atom (such as nitrogen, oxygen, or fluorine) is attracted to another electronegative atom in a different molecule.
Van der Waals Forces: Weak attractions between molecules, including dipole-dipole interactions, London dispersion forces, and hydrogen bonding.
Coordinate Covalent Bond: A bond in which one atom donates a pair of electrons to another atom to form a covalent bond.
Pi Bond: A type of covalent bond formed when two atomic orbitals overlap side-by-side to create a cloud of electron density above and below the plane of the nuclei.
Sigma Bond: A type of covalent bond formed when two atomic orbitals overlap head-to-head to create a linear bond.
Polar Covalent Bond: A covalent bond in which electrons are shared unequally between atoms, resulting in a polar molecule.
Nonpolar Covalent Bond: A covalent bond in which electrons are shared equally between atoms, resulting in a nonpolar molecule.
Halogen Bond: A type of weak intermolecular interaction that occurs between a halogen atom and an electronegative element such as oxygen or nitrogen.
Ionic-Covalent Hybrid Bond: A bond that exhibits properties of both ionic and covalent bonds, often found in materials such as ceramics.
Peptide Bond: A covalent bond that links amino acids together to form proteins.
Dipole-Dipole Interaction: A type of intermolecular force that occurs between polar molecules, where the positive end of one molecule is attracted to the negative end of another molecule.
Electrostatic Bond: A bond formed between charged particles due to the attraction between oppositely charged ions.
Metal-Metal Bond: A bond formed between two metal atoms, often involving delocalized electrons.
Intermolecular Forces: Weak forces that exist between molecules, including van der Waals forces, hydrogen bonds, and dipole-dipole interactions.
Intramolecular Forces: Forces that exist within molecules, including covalent bonds, ionic bonds, and metallic bonds.
Thioester Bond: A covalent bond between a sulfur atom and a carbon atom in which the sulfur is double-bonded to an oxygen atom.
Glycosidic Bond: A covalent bond that links two monosaccharides together to form a disaccharide or polysaccharide.
Peptidyl Bond: A covalent bond that links an amino acid to another molecule, such as another amino acid or a tRNA molecule.
Ester Bond: A covalent bond between an oxygen atom and a carbon atom.
Hydrophobic Interaction: A weak interaction between nonpolar molecules due to the exclusion of water molecules.
Olefinic Bond: A covalent bond that involves a carbon-carbon double bond.
Carboxylate Bond: A covalent bond between a carboxyl group and another molecule, often found in organic acids.
Nucleoside Bond: A covalent bond that links a nucleotide to another molecule, such as another nucleotide or a ribose sugar.
Epoxy Bond: A covalent bond that involves a three-membered ring, often found in epoxides or polymers.
Peptide-Link Glycosidic Bond: A covalent bond that links two carbohydrates together to form a more complex molecule.
Ether Bond: A covalent bond between an oxygen atom and two carbon atoms, often found in organic compounds.
Amide Bond: A covalent bond between a carbonyl group and an amino group, often found in peptides and proteins.
"The bond may result from the electrostatic force between oppositely charged ions as in ionic bonds."
"The bond may result from...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."
"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."
"All bonds can be described by quantum theory, but, in practice, simplified rules and other theories allow chemists to predict the strength, directionality, and polarity of bonds."
"The octet rule and VSEPR theory are examples."
"More sophisticated theories are valence bond theory, which includes orbital hybridization and resonance."
"More sophisticated theories...include 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 strength of chemical bonds varies considerably."
"The octet rule is an example [of a theory] that allows chemists to predict the strength, directionality, and polarity of bonds."
"The VSEPR theory is an example [of a theory] that allows chemists to predict the strength, directionality, and polarity of bonds."
"Orbital hybridization is a component of valence bond theory."
"Ligand field theory is a component of molecular orbital theory."