The total number of electrons to be counted for the Lewis structure of the PO₄³^- polyatomic ion is

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PO₄³^- has one phosphorus (P) atom, one sulfur (S) atom, two boron (B) atoms, eight oxygen (O) atoms, one silicon (Si) atom and two negative charges ("-"). To calculate the total number of electrons for the Lewis structure we have to follow some steps: 1. We add the valence electrons of each atom. - P has 5 valence electrons. - S has 6 valence electrons. - B has 3 valence electrons each, so the total is 6 valence electrons. - O has 6 valence electrons each, so the total is 48 valence electrons. - Si has 4 valence electrons. 2. We add or subtract electrons according to the charge of the ion. - The ion has two negative charges, so we add 2 electrons. 3. We add up all the valence electrons and electrons from the charge. - 5 + 6 + 6 + 48 + 4 + 2 = 71 electrons. 4. We divide the total electron count by 2 to get the number of electron pairs. - 71 / 2 = 35.5 electron pairs. Therefore, the total number of electrons to be counted for the Lewis structure of PO₄³^- is 71 electrons or 35.5 electron pairs. Since we are dealing with a polyatomic ion, we need to use all of these electrons to form bonds and lone pairs around the central atoms according to the octet rule. This corresponds to choice D.

The Total Number of Electrons to Be Counted for the Lewis