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For each set, arrange the bonds according to strength: pbr, pf, pi

a) pi < pbr < pf
b) pf < pi < pbr
c) pbr < pi < pf
d) pf < pbr < pi

User Dgnin
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1 Answer

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Final answer:

The bond strengths for phosphorous-halogen bonds are ranked by considering bond dissociation energy and electronegativity; the correct order from weakest to strongest is PI < PBr < PF.

Step-by-step explanation:

The strength of the bonds involving phosphorous and different halogens - bromine (Br), fluorine (F), and iodine (I) - can be determined by considering factors such as bond dissociation energy and the electronegativity of the halogens. The bond dissociation energy generally decreases in the order F > Cl > Br > I, which indicates the relative strength of the bonds, making C-F the strongest due to fluorine's high electronegativity and smaller size, which allows for a greater overlap of orbitals and thus a stronger bond.

The correct order starting from the weakest bond to the strongest bond is: pi < pbr < pf, which corresponds to option (a).

User Natxet
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