Write a Lewis structure for each of the following polyatomic...

Write a Lewis structure for each of the following polyatomic ions. Show all bonding valence electron pairs as lines and all nonbonding valence electron pairs as dots. For those ions that exhibit resonance, draw the various possible resonance forms. a. hydrogen phosphate ion, $\mathrm{HPO}_{4}^{2-}$ b. dihydrogen phosphate ion, $\mathrm{H}_{2} \mathrm{PO}_{4}^{-}$ c. phosphate ion, $\mathrm{PO}_{4}^{3-}$

Write a Lewis structure for each of the following polyatomic ions. Show all bonding valence electron pairs as lines and all nonbonding valence electron pairs as dots. For those ions that exhibit resonance, draw the various possible resonance forms.
a. hydrogen phosphate ion, $\mathrm{HPO}_{4}^{2-}$
b. dihydrogen phosphate ion, $\mathrm{H}_{2} \mathrm{PO}_{4}^{-}$
c. phosphate ion, $\mathrm{PO}_{4}^{3-}$

Key Concepts

Octet Rule

The octet rule is a guideline stating that atoms tend to form bonds to complete an eight-electron configuration in their valence shell, similar to the electron configuration of noble gases. This principle is fundamental when constructing stable Lewis structures for molecules and ions.

Formal Charge Calculation

Formal charge calculation is a method used to estimate the charge distribution within a molecule by comparing the number of valence electrons in an isolated atom to the number of electrons assigned to it in a Lewis structure. This calculation helps identify the most stable Lewis structure by minimizing charges and ensuring that negative formal charges reside on more electronegative atoms.

Resonance Structures

Resonance structures are alternative Lewis structures for a single molecule or ion that depict different possible arrangements of electrons, particularly in cases where electrons are delocalized across two or more atoms. These forms, when considered together, provide a more complete picture of the true electron distribution.

Polyatomic Ions

Polyatomic ions are charged species composed of two or more atoms covalently bonded together, with an overall positive or negative charge. Understanding their structure requires accounting for both the bonding interactions and the additional electrons or electron deficiencies that contribute to the net charge.

Lewis Structures

Lewis structures are schematic representations that show how atoms in a molecule or ion are bonded and how valence electrons are distributed among them. They use lines to indicate bonding electron pairs and dots for nonbonding (lone) electron pairs, aiding in visualizing the overall electron arrangement.

Valence Electrons

Valence electrons are the electrons located in the outermost energy level of an atom. They are critical for chemical bonding because they participate in the formation of bonds between atoms. In drawing Lewis structures, the total number of valence electrons determines how atoms in a molecule or polyatomic ion connect and share electrons.

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