Table of contents

1. Intro to General Chemistry3h 48m
2. Atoms & Elements4h 16m
3. Chemical Reactions4h 10m
4. BONUS: Lab Techniques and Procedures1h 36m
5. BONUS: Mathematical Operations and Functions48m
6. Chemical Quantities & Aqueous Reactions3h 53m
7. Gases3h 49m
8. Thermochemistry2h 37m
9. Quantum Mechanics2h 58m
10. Periodic Properties of the Elements3h 9m
11. Bonding & Molecular Structure3h 29m
12. Molecular Shapes & Valence Bond Theory1h 57m
13. Liquids, Solids & Intermolecular Forces2h 23m
14. Solutions3h 1m
15. Chemical Kinetics2h 53m
16. Chemical Equilibrium2h 29m
17. Acid and Base Equilibrium5h 1m
18. Aqueous Equilibrium4h 47m
19. Chemical Thermodynamics1h 50m
20. Electrochemistry2h 42m
21. Nuclear Chemistry2h 36m
22. Organic Chemistry5h 7m
23. Chemistry of the Nonmetals2h 39m
24. Transition Metals and Coordination Compounds3h 16m

11. Bonding & Molecular Structure

Lewis Dot Structures: Ions

General Chemistry

11. Bonding & Molecular Structure

Lewis Dot Structures: Ions

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Multiple Choice

Which of the following is the correct Lewis dot structure for the phosphate ion (PO₄³⁻) with formal charges?

A central phosphorus atom single-bonded to four oxygen atoms, with one oxygen atom carrying a -1 formal charge.

A central phosphorus atom single-bonded to four oxygen atoms, with no formal charges on any atoms.

A central phosphorus atom double-bonded to two oxygen atoms and single-bonded to two oxygen atoms, with no formal charges on any atoms.

A central phosphorus atom double-bonded to one oxygen atom and single-bonded to three oxygen atoms, with each single-bonded oxygen carrying a -1 formal charge.

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Verified step by step guidance

Identify the total number of valence electrons available for the phosphate ion (PO₄³⁻). Phosphorus (P) has 5 valence electrons, each oxygen (O) has 6 valence electrons, and the ion has an additional 3 electrons due to the -3 charge.

Calculate the total number of valence electrons: 5 (from P) + 4 * 6 (from O) + 3 (extra electrons) = 32 valence electrons.

Draw the skeletal structure with phosphorus (P) as the central atom and single bonds to each of the four oxygen atoms. Distribute the remaining electrons to satisfy the octet rule for each oxygen atom.

Adjust the structure to minimize formal charges: Convert one of the P-O single bonds to a double bond, which will help reduce the formal charge on phosphorus and one of the oxygen atoms.

Assign formal charges: Calculate the formal charge for each atom using the formula: Formal Charge = (Valence electrons) - (Non-bonding electrons) - 0.5*(Bonding electrons). Ensure that the structure with the least formal charges is chosen, where the central phosphorus atom is double-bonded to one oxygen and single-bonded to three oxygens, with each single-bonded oxygen carrying a -1 formal charge.