Question

define bond order,bond length and bond enthalpy

Answer 1

Bond Length

The bond length refers to the distance between the centers of the nuclei of two bonded atoms in an equilibrium position. 

Bond Enthalpy

The amount of energy which is needed in order to break one mole of the bond of a particular type between two atoms in a gaseous state is referred to as the Bond Enthalpies. 

Bond Order

As per the Lewis description of covalent bonds, the bond order is the number of bonds that forms in between the two atoms in a molecule. 

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Answer 2

Bond order: No. of covalent bond formed between two atoms. If 1 covalent bond is formed between two atom then its bond order=1, If 2 covalent bond is formed between two atom then its bond order=2 and so on. This is according to Valance bond theory but according to Molecular orbital theory bonds between two atoms can be fractional like .5, 1.5 2.5. Bond order is proportional to stability. That means more is the Bond order, more the bond is stable. That means, if bond order is more then it will need more energy to break that bond. That is why it is more stable. Bond length is inversely proportional to Bond Order. That means greater is the Bond Order, lesser is the bond length.

Bond Length: It is the distance between two nuclei which formed covalent bond. Bond strength is inversely proportional to Bond Length. That means Lesser is the bond length, stronger is the bond.

Bond enthalpy: Amount of energy required to break 1 mole bonds. for example to break 1 mole O-H bond it requires 463 kilojoules of energy. Hence to break 1 bond it requires 463 kJ÷ (6.02×100000000000000000000000 i.e 1 mole) energy.