Types of Chemical Bonds

Study Notes

Covalent Bond: formed when two or more atoms share one or more pairs of electrons to form a molecule
Ionic Bond: formed when one or more electrons are transferred from one atom to another, resulting in the formation of ions with opposite charges
Hydrogen Bond: a weak bond between a hydrogen atom bonded to a highly electronegative atom (F, O, N) and another electronegative atom
Polar Covalent Bond: a covalent bond between two atoms with different electronegativities, resulting in a partial positive and partial negative charge

Valence Shell Electron Pair Repulsion (VSEPR) Theory: predicts the shape of molecules based on the arrangement of electron pairs around the central atom
Molecular Orbital (MO) Theory: describes the distribution of electrons in molecules in terms of molecular orbitals

Bond Length: the distance between the nuclei of two bonded atoms
Bond Strength: the energy required to break a bond
Bond Angle: the angle between two bonds formed by a central atom
Bond Polarity: the distribution of electrons in a bond, resulting in a partial positive and partial negative charge

Electronegativity: the ability of an atom to attract electrons in a covalent bond
Polarity: the distribution of electrons in a molecule, resulting in a partial positive and partial negative charge
Hybridization: the mixing of atomic orbitals to form hybrid orbitals, which are used to describe bonding in molecules

Covalent bonds form when atoms share one or more pairs of electrons to create a molecule.
Ionic bonds occur when one or more electrons are transferred, resulting in ions with opposite charges.
Hydrogen bonds are weak bonds between a hydrogen atom bonded to a highly electronegative atom (F, O, N) and another electronegative atom.
Polar covalent bonds occur between atoms with different electronegativities, resulting in partial positive and partial negative charges.

VSEPR Theory predicts molecular shapes based on electron pair arrangements around the central atom.
MO Theory describes electron distribution in molecules using molecular orbitals.

Bond length is the distance between the nuclei of two bonded atoms.
Bond strength is the energy required to break a bond.
Bond angle is the angle between two bonds formed by a central atom.
Bond polarity results in partial positive and partial negative charges due to electron distribution.

Electronegativity is an atom's ability to attract electrons in a covalent bond.
Polarity results from electron distribution in a molecule, creating partial positive and partial negative charges.
Hybridization involves mixing atomic orbitals to form hybrid orbitals, describing bonding in molecules.