orbital hybridization: The concept of mixing atomic orbitals to form new hybrid orbitals suitable for the qualitative description of atomic bonding properties and geometries.

bond length: The distance between the nuclei of two bonded atoms.

The more energy required, the stronger the bond is said to be.

bond strength: Directly related to the amount of energy required to break the bond between two atoms.

Bond lengths between atoms with multiple bonds are shorter than in those with single bonds.

Double and triple bonds offer added stability to compounds, and restrict any rotation around the bond axis.

Double and triple bonds are comprised of sigma bonds between hybridized orbitals, and pi bonds between unhybridized p orbitals.

Double and triple covalent bonds are stronger than single covalent bonds and they are characterized by the sharing of four or six electrons between atoms, respectively.

Double and Triple Covalent Bondsĭouble and triple bonds, comprised of sigma and pi bonds, increase the stability and restrict the geometry of a compound. Sigma bond in the hydrogen molecule: Higher intensity of the red color indicates a greater probability of the bonding electrons being localized between the nuclei. These bonds mostly occur between nonmetals or between two of the same (or similar) elements.Two atoms with similar electronegativity will not exchange an electron from their outermost shell the atoms instead share electrons so that their valence electron shell is filled.Įxamples of compounds that contain only covalent bonds are methane ( ext to indicate the single covalent bond between the two hydrogen atoms. Covalent CompoundsĬovalent bonds are characterized by the sharing of electrons between two or more atoms. Here, we discuss two classes of compounds based on the bond type that holds the atoms together: ionic and covalent. They have distinct chemical structures characterized by a fixed ratio of atoms held together by chemical bonds.

electronegativity: The tendency of an atom or molecule to attract electrons and form bonds.Ĭompounds are defined as substances containing two or more different chemical elements.Hydrogen and helium are exceptions because they can hold a maximum of two valence electrons. octet rule: Atoms lose, gain, or share electrons in order to have a full valence level of eight electrons.valence electrons: Electrons in the outermost principal energy (valence) level of an atom that can participate in the formation of chemical bonds with other atoms.Due to the sharing of electrons, they exhibit characteristic physical properties that include lower melting points and electrical conductivity compared to ionic compounds. Covalent compounds have bonds where electrons are shared between atoms.

Ionic compounds are formed from strong electrostatic interactions between ions, which result in higher melting points and electrical conductivity compared to covalent compounds.

Strongest sigma bond