Coordinate Ionic Bond
Ionic bonds are chemical bonds that occur between an atom with a positive charge (cation) and an atom with a negative charge (anion). In an ionic bond, the cation and anion are held together by electrostatic forces of attraction. These forces are so strong that breaking the bond requires a significant amount of energy.
A coordinate ionic bond is a type of ionic bond where the bonding electron pair is shared between the two atoms. This is in contrast to a regular ionic bond, where the electron is given and accepted by the two atoms.
In a coordinate ionic bond, one atom donates a lone pair of electrons to another atom. This creates a covalent bond between the two atoms. The atom donating the lone pair of electrons becomes positively charged, while the atom receiving the lone pair of electrons becomes negatively charged. This results in the formation of an ionic bond between the two atoms.
Coordinate ionic bonds are commonly found in compounds containing metal ions and ligands. The metal ion donates a pair of electrons to the ligand, which forms a coordinate covalent bond.
Examples of Coordinate Ionic Bonds
An example of a coordinate ionic bond can be seen in the formation of the ammonia complex ion. In this reaction, ammonia (NH3) acts as a ligand and donates a pair of electrons to a metal ion, such as copper (Cu2+). This creates a coordinate covalent bond between the ammonia and copper ion, resulting in the formation of the ammonia complex ion or [Cu(NH3)4]2+.
Another example of a coordinate ionic bond occurs in the formation of the hexaaquacobalt(II) ion. Water molecules (H2O) act as ligands and donate their lone pairs of electrons to the cobalt (II) ion (Co2+), creating a coordinate covalent bond. The resulting compound is [Co(H2O)6]2+.
Comparison with Regular Ionic Bond
Regular ionic bonds occur when one atom donates an electron to another atom. The donating atom becomes positively charged, while the accepting atom becomes negatively charged. In a coordinate ionic bond, one atom donates a lone pair of electrons to another atom. This creates a covalent bond, which results in the formation of an ionic bond between the two atoms.
The main difference between the two is in the way the bond is formed. In a regular ionic bond, the atom donates an electron, while in a coordinate ionic bond, the atom donates a pair of electrons. The resulting bond strength is also different, with coordinate covalent bonds being generally stronger than regular ionic bonds.
FAQs
Q: What is the difference between a coordinate covalent bond and a covalent bond?
A: In a covalent bond, two atoms share a pair of electrons. In a coordinate covalent bond, one atom donates a lone pair of electrons to the other atom, creating a covalent bond.
Q: What is a ligand?
A: A ligand is an ion or molecule that donates a pair of electrons to a metal ion, creating a coordinate covalent bond.
Q: What is a metal ion?
A: A metal ion is an ion that has lost or gained electrons, resulting in a positively charged or negatively charged ion.
Q: Why are coordinate covalent bonds stronger than regular ionic bonds?
A: Coordinate covalent bonds are stronger than regular ionic bonds because they are formed by the sharing of two electrons, rather than the donation of one electron. This results in a stronger bond between the two atoms.
Q: What are some examples of compounds that contain coordinate covalent bonds?
A: Compounds that contain coordinate covalent bonds include metal complexes, such as the [Cu(NH3)4]2+ ion, and coordination compounds, such as [Co(H2O)6]2+.