Question
In $\mathrm{PO}_{4}^{3}$ the formal charge on each oxygen atom and the P-O bond order are respectively(1) $-0.75,0.5$(2) $-0.75,1.25$(3) $-0.75,1.0$$(4)-3,1.25$
Step 1
The formal charge is calculated by the formula: \[ Formal\ Charge = Valence\ Electrons - (Non-bonding\ Electrons + \frac{1}{2} Bonding\ Electrons) \] For oxygen, the number of valence electrons is 6. In $\mathrm{PO}_{4}^{3-}$, each oxygen is bonded to the Show more…
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The correct order of the O-O bond length in $\mathrm{O}_{2}, \mathrm{H}_{2} \mathrm{O}_{2}$ and $\mathrm{O}_{3}$ is (1) $\mathrm{O}_{2}>\mathrm{O}_{3}>\mathrm{II}_{2} \mathrm{O}_{2}$ (2) $\mathrm{O}_{3}>\mathrm{II}_{2} \mathrm{O}_{2}>\mathrm{O}_{2}$ (3) $\mathrm{II}_{2} \mathrm{O}_{2}>\mathrm{O}_{3}>\mathrm{O}_{2}$ (4) $\mathrm{O}_{2}>\mathrm{II}_{2} \mathrm{O}_{2}>\mathrm{O}_{3}$
The bond order of a molecule is given by (1) Half the difference between number of bonding electrons and anti-bonding electrons. (2) The difference between the number of bonding electrons and anti-bonding electrons. (3) Twice the difference between the number of bonding electrons and anti-bonding electrons. (4) The total number of bonding electrons.
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