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

Previous problemNext problem

Struggling with General Chemistry?

Join thousands of students who trust us to help them ace their exams!Watch the first video

Multiple Choice

Which of the following is the correct Lewis structure for the phosphate ion (PO4^3-) including formal charges?

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

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

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

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

Previous problemNext problem

Verified step by step guidance

Identify the total number of valence electrons in the phosphate ion (PO4^3-). 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: 5 + (4 * 6) + 3 = 32 valence electrons.

Determine the central atom, which is typically the least electronegative element. In this case, phosphorus (P) is the central atom.

Arrange the oxygen atoms around the phosphorus atom and distribute the electrons to form bonds. Start by forming single bonds between the phosphorus and each oxygen atom, using 8 electrons (2 electrons per bond).

Distribute the remaining electrons to satisfy the octet rule for each oxygen atom. After forming single bonds, 24 electrons remain. Distribute these electrons to the oxygen atoms, giving each oxygen atom 6 additional electrons to complete their octets.

Calculate the formal charges for each atom. The formal charge is calculated as: Formal Charge = (Valence electrons) - (Non-bonding electrons) - (Bonding electrons/2). For the structure with a double bond to one oxygen, the formal charges are: P = 0, double-bonded O = 0, and each single-bonded O = -1. Verify that the sum of formal charges equals the overall charge of the ion, which is -3.