MSE Midterm 1 Set 3: Bonding

bonding energy

The energy required to separate two atoms that are chemically bonded to each other. It may be expressed on a per-atom basis or per mole of atoms.

primary bonds

Interatomic bonds that are relatively strong and for which bonding energies are relatively large. Primary bonding types are ionic, covalent, and metallic.

ionic bond

A coulombic interatomic bond that exists between two adjacent and oppositely charged ions.

Metal and Non-Metal

coulombic force

A force between charged particles such as ions; the force is attractive when the particles are of opposite charge.

covalent bond

A primary interatomic bond that is formed by the sharing of electrons between neighboring atoms.

metallic bond

A primary interatomic bond involving the nondirectional sharing of nonlocalized valence electrons ("sea of electrons") that are mutually shared by all the atoms in the metallic solid.

secondary bonds

Interatomic and intermolecular bonds that are relatively weak and for which bonding energies are relatively small. Normally, atomic or molecular dipoles are involved. Examples of secondary bonding types are van der Waals forces and hydrogen bonding.

van der Waals bond

A secondary interatomic bond between adjacent molecular dipoles that may be permanent or induced.

dipole (electric)

A pair of equal and opposite electrical charges separated by a small distance.

hydrogen bond

Bonds between molecules with electronegativity difference due to hydrogen being bonded to either a O, N, or F

polar molecule

A molecule in which there exists a permanent electric dipole moment by virtue of the asymmetrical distribution of positively and negatively charged regions.