The species having bond order different from that in $CO$ is
- ${NO}^-$
- ${NO}^+$
- ${CN}^-$
- $N_2$
The Correct Option is A
Approach Solution - 1
Approach Solution -2
Bond order is defined as the number of covalent bonds that are present between a pair of atoms. The stability of the molecule is determined by the bond order. The formula to find the bond order is given by:
Bond order= ½ (Nb-Na)
Where Na is the electrons in the antibonding orbitals
Nb is the electrons in the bonding orbitals.
Bond order can be both positive and negative that will determine the stability of the molecule. If the electrons in the bonding orbitals are greater than the electrons present in the antibonding orbitals (Nb>Na), the bond order will be positive. The Molecule formed will be stable.
On the other hand if the electrons in the bonding orbitals is less than the electrons present in the antibonding orbitals (Nb<Na), the bond order will be negative. The Molecule formed will be unstable.
In the question, the bond order of CO is 3. CO has 14 electrons.
There are 10 electrons in the bonding orbitals and 4 electrons in the antibonding orbitals.
B.O = ½ (Nb-Na)
= ½ (10-4) = 3
The other given compound that is N₂, NO⁺ and CN⁻ are isoelectronic with CO. Isoelectronics are the molecules that have the same number of electrons. As all these compounds are isoelectronic they have the same bond order that is 3.
On the other hand, NO⁻, have 16 electrons and have the bond order of 2.
Top Questions on Bond Parameters
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D. The magnitude of H bonding depends on the physical state of the compound.
E. H-bonding has powerful effect on the structure and properties of compounds.
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Concepts Used:
Bond Parameters
Covalent bonds can be characterized on the basis of several bond parameters such as bond length, bond angle, bond order, and bond energy (also known as bond enthalpy). These bond parameters offer insight into the stability of a chemical compound and the strength of the chemical bonds holding its atoms together.
Bond parameters
- Bond length: it is an equilibrium distance between the centres of the nuclei of the two bonded atoms. It is expressed in terms of A.
- Bond Angle: It is characterized as the point between the orbitals consisting of holding electron sets around the focal iota in an atom/complex particle. Bond points are communicated in degrees which are tentatively controlled by spectroscopic strategies.
- Bond Enthalpy: the measure of energy needed to break one mole of obligations of a specific sort between two molecules in a vaporous state. The unit of bond enthalpy is kJ mol–1. The more the bond enthalpy, the more grounded the bond is.
For example, The H—H bond enthalpy in hydrogen is 435.8 kJ mol-1. \
- Bond Order: According to Lewis, Bond Order is given by the number of connections between the two atoms in a particle.
Bond order of H2 (H —H) =1
Bond order of 02 (O = O) =2
Bond order of N2 (N = N) =3
- Resonance Structures: It is observed that there are many molecules whose behaviour cannot be explained by a single Lewis structure.
Read More: Chemical Bonding and Molecular Structure