"A chemical bond is a lasting attraction between atoms or ions that enables the formation of molecules, crystals, and other structures."
Understanding the behavior of atoms and how they form bonds with each other.
Atomic Structure: The study of the internal structure of atoms, its composition, and its properties.
Electromagnetic Spectrum: It is a range of frequencies of radiation that is separated by their wavelength and frequency.
Orbital Concepts: The study of orbitals that are used to describe the electrons’ position and movement within an atom.
Quantum Numbers: A set of four numbers that describe the state of an electron in an atomic orbital.
Electron Configuration: The arrangement of electrons within an atom.
Periodic Table: A table that organizes all the known elements based on their electronic structure.
Chemical Bonds: An attraction between atoms that allows the formation of chemical compounds.
Ionic Bonds: A type of chemical bond that is formed when one atom loses an electron to another atom.
Covalent Bonds: A type of chemical bond that is formed when atoms share their electrons.
Hybridization: The mixing of atomic orbitals to form new hybrid orbitals.
Molecular Orbital Theory: The study of the formation and properties of molecular orbitals.
Lewis Structures: The structures that represent the distribution of electrons in a molecule.
VSEPR Theory: A theory used to predict the shape of a molecule based on the arrangement of the electron pairs around the central atom.
Intermolecular Forces: Forces that exist between molecules.
Hydrogen Bonding: A type of intermolecular force that is responsible for the structure of water and other molecules.
Van der Waals Forces: Weak forces between neutral atoms or molecules.
Dipole-Dipole Forces: Attractive forces that arise between polar molecules.
London Dispersion Forces: Weak forces between nonpolar molecules.
Organic Chemistry: The study of the structure, properties, composition, reactions, and synthesis of carbon-containing compounds.
Functional Groups: A specific arrangement of atoms or bonds within a molecule that is responsible for its characteristic chemical reactions.
Covalent bonding: Shared electrons between atoms; types include single, double, and triple bonds.
Ionic bonding: Transfer of electrons from one atom to another resulting in ions being attracted to each other.
Metallic bonding: Shared mobile electrons between metal atoms resulting in a sea of electrons.
Hydrogen bonding: Strong attraction between a hydrogen atom and another highly electronegative atom such as nitrogen, oxygen, or fluorine.
Van der Waals forces: Weak attraction between non-polar molecules due to temporary dipoles.
Polar covalent bonding: Electrons are shared unevenly between atoms, resulting in a partial positive and partial negative end.
Coordinate covalent bonding: Both shared electrons come from one atom to form the bond.
pi bonding: Overlapping of unhybridized p-orbitals resulting in a double bond in molecules like ethene and benzene.
Resonance structure: When the position of double bonds can shift within a molecule resulting in multiple possible structures that contribute to the molecule's stability.
"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."