Respuesta :
Answer:
The correct option is: Carbonate ion < Carbon dioxide < Carbon monoxide
Explanation:
Bond energy is defined as the average energy needed to break a chemical covalent bond and signifies the strength of chemical covalent bond.
The bond strength of a covalent bond depends upon the bond length and the bond order.
Carbon monoxide molecule (CO) has two covalent bond and one dative bond. Bond order 2.6
Carbon dioxide (CO₂) has two carbon-oxygen (C-O) double bonds of equal length. Bond order 2.0
Carbonate ion (CO₃²⁻) has three C-O partial double bonds. Bond order 1.5
Also, the bond length is inversely proportional to the bond order and bond strength.
Therefore, order of C-O bond length: Carbon monoxide<Carbon dioxide<Carbonate ion
Order of C-O bond order: Carbonate ion<Carbon dioxide<Carbon monoxide
Order of C-O bond strength or energy: Carbonate ion<Carbon dioxide<Carbon monoxide
Answer:
The carbonate ion will have minimum bond strength, while carbon monoxide will have maximum bond strength.
Explanation:
Bond order can be defined as the half the number of electrons in the bonding orbital minus antibonding orbital. It can also be defined as the energy required to break a bond.
Bond length has an inverse relation with the bond order.
Bond order of Carbon monoxide is 2.6.
Bond order of Carbon dioxide is 2.0.
Bond order of Carbonate ion is 1.5.
The correct order for the increasing bond order or bond strength will be:
Carbonate [tex]>[/tex] carbon dioxide [tex]>[/tex] carbon monoxide.
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