[填空题]
Phosphorus reacts with oxygen to form two different oxides, phosphorus(III) oxide ($P_4O_6$) and phosphorus(VI) oxide ($P_4O_{10}$)
1.The oxides of phosphorus consist of cage-like molecules with the following structural formulas.
The O−P−O bond angles in the two molecules are labelled.
1.State the geometries of the bonds around each phosphorus atom in $P_4O_6$
2.State the geometries of the bonds around each phosphorus atom in $P_4O_{10}$
3.Suggest why the bond O−P−O bond angles of the two molecules are similar despite the different arrangements of bonding and non-bonding electrons around the phosphorus atoms.
4.Explain how the ability of phosphorus to form both $P_4O_6$ and $P_4O_{10}$ demonstrates that the octet rule is not always obeyed.
2.$P_4O_6$ and $P_4O_{10}$ react with an aqueous base to produce phosphite ($HPO_3^{2-}$) and phosphate ($PO_4^{3+}$) ions, respectively. The structural formulas of $HPO_3^{2-}$ and $PO_4^{3+}$ are shown.
State why resonance structures are needed to accurately represent the bonding in $HPO_3^{2-}$ and $PO_4^{3+}$.
