Coordinate bond

A coordinate bond is a sort of covalent binding that is unique. It’s a type of alternative covalent bond where the electron pair is shared by only one atom. In other words, the shared pair’s electrons are both from the same atom. Dative bonds or dipolar bonds are other names for coordinate bonds. Because it is a special type of covalent connection, a coordinate bond is also known as a Coordinate Covalent bond.

Other names of coordinate bond

The coordinate bond is also called as

•  Dative bond
•  Dipolar bond
•  Coordinate covalent bond

Properties of coordinate bond:

• They have a low boiling point

Boiling point: The temperature at which liquid converts into vapours.

• They have a low melting point

Melting point: The temperature at which solids melts into liquid form

• • No electrostatic forces of attraction: Because the shared pair of electrons is in between two atoms, there are no electrostatic forces of attraction.

• Do not conduct electricity

Electricity is not conducted either in liquid or dissolved state

•  They are less soluble in water

Characteristics of coordinate bond

• The donor in coordinate bonding is the atom that shares a pair of electrons with the other atom.
• The acceptor, also known as the receptor, is the atom that accepts the electron pair that the donor shares in order to achieve stability.
• The coordinate bond is shown as a short line segment with an arrow pointing to the acceptor, showing the direction of electron pair sharing. “→” is the symbol used.
• The donor and acceptor achieve stability by sharing and receiving the electron pair.
• The Lewis theory of chemical bonding is analogous to coordinate bonding.

Formation coordinate bond:

A coordinate covalent bond is a type of covalent bond in which only one of the linked atoms contributes to the shared pair of electrons. An arrow mark (“→”) pointing towards the acceptor atom represents this link. The atom that donates an electron pair for sharing is known as a donor, while the atom that accepts the electron pair is known as an acceptor.

Example of formation of coordinate bond

For example, consider the formation of the ammonium ion (NH4+): The union of the NH3 molecule with the H+ ion produces the ammonium ion. The core ‘N’ atom in the NH3 molecule possesses one lone pair of electrons, while the H+ ion has an empty orbital. As a result, the N- atom of the NH3 molecule gives its lone pair to the vacant orbital of the H+ ion, producing a covalent connection.

Examples of coordinate covalent bond

1. Formation of Ammonium ion

The nitrogen atom in ammonia gives its electron pair to the free orbital of the H+ ion, forming a co-ordinate bond.

2. Formation Of Ammonia Boron Trifluoride

  The nitrogen atom in ammonia donates one pair of electrons to the empty orbital of the boron atom in boron trifluoride, making nitrogen the donor and boron the acceptor.

Coordinate covalent bond:

• A coordinate covalent bond is a type of covalent bond, where all the electrons are shared by only one atom.
• Coordinate bonds are also as strong as covalent bonds.
• When two nonmetal atoms share a pair of electrons, covalent bonds are produced.

             LEWIS BASE:

A lewis base can be defined as the special substance that donates atoms or lone pairs of electrons.

               LEWIS ACID:

A Lewis acid can be defined as a special chemical that accepts the atoms or lone pair of electrons. This can also be called an acceptor.

• In acidic solutions, hydrogen ions (H3O+) are generated when water molecules make coordinate covalent connections with hydrogen atom ions (H+).
• Up to six water molecules can establish coordinating covalent connections with many metal ions.
• When triatomic beryllium chloride (BeCl2) molecules establish coordinate covalent connections with one another, they can form lengthy polymers. This can also be called a donator.
• Mostly the coordinate covalent bond occurs when we have a lone pair of electrons.

Example of coordinate covalent bond:

The best example for a coordinate covalent bond can be seen in carbon monoxide(CO), which is one of the gases released when we burn fossil fuels.

The number of electrons in carbon is 6, But the number of electrons in oxygen is 8. Therefore, Oxygen follows the octet rule.

Octet rule: Octet rule can be defined as elements should have 8 electrons in their valence shell just like oxygen,

Both carbon and oxygen share each of their electrons and form a double bond between them, Which is not stable because carbon does not obtain the octet rule and the structure is not correct. In order to obtain stability, Oxygen has to  share the lone pair of electrons in order to form a triple bond, Which makes stronger 

In the above equation, both carbon and oxygen have formed a triple bond. This is because oxygen donated a lone pair of electrons to carbon so as to form a triple bond. Here, Oxygen is the donor and carbon is the acceptor. This is the example of the coordinate covalent bond as the contribution of a lone pair of electrons is done.

Conclusion:

A coordinate bond is simply a type of covalent bond. But the only difference is, In a covalent bond, sharing is done by both elements. But in a coordinate bond, only lone pairs of electrons are shared by a single element. The coordinate bond is also stronger just like the covalent bond.