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Chemical Bonding
Term | Definition |
---|---|
ionic bond | the electrostatic attraction that binds oppositely charged ions together |
bent molecular shape | molecule with 2 bonding electron pairs and 2 non-bonding electron pairs on the central atom; bond angle of 104.5° |
ionic compound | a compound composed of positive and negative ions |
bond angle | angle between bonds in a molecule |
intermolecular forces | attractive forces that exist between molecules |
pyramidal molecular shape | molecule with 3 bonding pairs and 1 non-bonding electron pairs on the central atom; bond angle of 107° |
bonding electron pairs | electrons that are shared between atoms within a molecule |
chemical bond | attraction that holds atoms together with a compound |
linear molecular shape | molecular shape with a bond and of 180°. |
conductivity | ability of a substance to conduct heat/electricity |
lone electron pair | non-bonding electron pair on an atom |
covalent bond | a bond formed by the sharing of electrons between atoms |
metallic bond | the force of attraction between free-floating sea of electrons and positively charged metal ions |
tetrahedral molecular shape | molecule with 4 bonding pairs and 0 non-bonding electron pairs on the central atom; bond angle of 109.5° |
nonbonding electron pair | electron pair not involved in a chemical bond |
trigonal planar molecular shape | molecule with 3 bonding pairs and 0 non-bonding pairs on the central atom; bond angle of 120° |
electronegativity | the ability of an atom to attract bonding electrons when the atom is in a compound |
nonpolar covalent bond | a covalent bond in which the electrons are shared equally by the two atoms |
valence electrons | an electron in the highest occupied energy level of an atom |
van der Waals forces | the weakest intermolecular attractions—dispersion interactions |
sigma bond (σ bond) | The strongest type of covalent bond formed from the head-on overlap of orbitals. |
pi bond (π bond) | Weaker than a 𝜎 bond formed from the sideways overlap of p orbitals. |
Hybridization | It is the mixing of the atomic orbitals in an atom to produce a set of hybrid orbitals. |
Dative (Coordinate) Covalent bond | A covalent bond where both electrons in the shared pair are donated by one of the bonding atoms only |
Permanent Dipoles | A permanent dipole is a permanent difference in the partial charges of covalently bonded atoms. |