Introduction:
A coordinate covalent bond, also known as a dative covalent bond or a coordinate bond, is a type of covalent bond in which one atom provides both of the shared electrons. This type of bonding is also known as “semi-polar covalent bonding.” The atom that donates the electrons is known as a Lewis base and the atom that accepts the electrons is known as a Lewis acid.
Definition:
A coordinate covalent bond, also known as a dative covalent bond or a coordinate bond, is a type of covalent bond in which one atom donates a pair of electrons to another atom, forming a covalent bond. The atom that donates the electrons is known as a Lewis base and the atom that accepts the electrons is known as a Lewis acid.
Formation:
Coordinate covalent bonds are formed when one atom has a spare pair of electrons and another atom has a vacant orbital. The spare pair of electrons from the first atom forms a bond with the vacant orbital of the second atom, resulting in a covalent bond. This process is known as ligand coordination.
Examples:
Examples of coordinate covalent bonds can be found in various compounds such as ethylenediamine (NH2CH2CH2NH2) and amino acids. In these compounds, the nitrogen atoms form coordinate covalent bonds with the carbon atoms. Coordinate covalent bonds are also found in complex ions such as [Fe(CN)6]4-, where the carbon and nitrogen atoms act as ligands and coordinate to the iron ion.
Properties:
A coordinate covalent bond is weaker than a regular covalent bond. It is also directional, meaning that it forms between a specific pair of atoms. The strength of the bond depends on the nature of the atoms involved and the number of electrons donated.
Chemical Reactions:
A chemical reaction involving a coordinate covalent bond typically involves the formation or breaking of the bond.
Formation of Coordinate Covalent Bond:
A common way for the formation of coordinate covalent bond is through the process of ligand substitution. In this process, a ligand (a molecule or ion that binds to a central atom) binds to a central atom, which has a vacant orbital, through a coordinate covalent bond.
For example, in the reaction between Fe(II) and ethylenediamine (NH2CH2CH2NH2) to form Fe(NH2CH2CH2NH2)2, the nitrogen atoms of ethylenediamine bind to the iron atom through coordinate covalent bonds.
Fe(II) + NH2CH2CH2NH2 → Fe(NH2CH2CH2NH2)2
Breaking of Coordinate Covalent Bond:
A coordinate covalent bond can be broken by a process called ligand dissociation. In this process, a ligand is removed from a central atom, breaking the coordinate covalent bond.
For example, in the reaction between Fe(NH2CH2CH2NH2)2 and water to form Fe(II) and NH2CH2CH2NH2, the water molecule acts as a ligand dissociating agent and removes one of the ethylenediamine molecules from the iron atom, breaking the coordinate covalent bond.
Fe(NH2CH2CH2NH2)2 + H2O → Fe(II) + NH2CH2CH2NH2
In summary, a chemical reaction involving a coordinate covalent bond typically involves the formation or breaking of the bond through ligand substitution or dissociation.
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| Coordinate Covalent Bond |
Importance:
Coordinate covalent bonds play an important role in biochemistry. For example, many enzymes use coordinate covalent bonds to bind to specific substrates. Coordinate covalent bonds are also important in the formation of coordination compounds, which are widely used in various fields including medicine, agriculture, and industry. Coordination compounds are also used as catalysts and pigments.
Conclusion:
In summary, a coordinate covalent bond is a type of covalent bond in which one atom provides both of the shared electrons. It forms when one atom has a spare pair of electrons and another atom has a vacant orbital. Coordinate covalent bonds are important in many areas such as biochemistry, chemistry, and industry. They are found in various compounds and complex ions, and play a key role in the formation of coordination compounds.
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