draw the lewis structure for the polyatomic phosphite (po₃³⁻) anion. be sure to include all resonance…

Explanation:

Step1: Calculate valence - electrons

Phosphorus (P) has 5 valence electrons, oxygen (O) has 6 valence electrons. The phosphate ion has a charge of - 3. So the total number of valence electrons is (5+3\times6 + 3=26).

Step2: Determine the central atom

Phosphorus is the central atom as it is less electronegative than oxygen.

Step3: Connect atoms and distribute electrons

Connect the P atom to the three O atoms with single bonds ((P - O)). This uses 6 electrons. Then distribute the remaining (26 - 6=20) electrons as lone - pairs on the O atoms to satisfy the octet rule.

Step4: Check for resonance

To satisfy the octet rule on P and get resonance structures, we can form a double bond between P and one of the O atoms. There are 3 possible resonance structures with a double bond between P and one of the three O atoms.

Answer:

Draw three resonance structures where in each structure, the P atom is the central atom bonded to three O atoms. In one structure, there is a (P = O) double bond and two (P - O) single bonds. The other two resonance structures are obtained by moving the double - bond to the other two O atoms. Each O atom has 3 lone - pairs in the single - bonded form and 2 lone - pairs in the double - bonded form, and the P atom has an octet in all structures. The overall ion has a charge of - 3.