The correct order in which the O—O bond length increases in the following is:
H2O2<O2<O3
O3<H2O2<O2
O2<O3<H2O2
O2<H2O2<O3
The Correct Option is C
Solution and Explanation
The relationship between bond length and bond strength is inverse, while the relationship between bond strength and bond dissociation energy is direct. Since H2 O2 has a single bond, O3 has a partial double bond due to resonance, and O2 has a double bond, the right sequence is O2 O3H2 O2. O-O's bond length in O2 is 1.21A0, O3 is 1.2730A0, and H2 O2 is 1.49A0.
Therefore, the correct option is (C): O2<O3<H2O2
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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