Table of contents

1. Intro to General Chemistry3h 48m
2. Atoms & Elements4h 16m
3. Chemical Reactions4h 10m
4. BONUS: Lab Techniques and Procedures1h 38m
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: Neutral Compounds

General Chemistry

11. Bonding & Molecular Structure

Lewis Dot Structures: Neutral Compounds

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 statements correctly describes the Lewis dot structure of the neutral compound P2O?

The two phosphorus atoms are connected by a triple bond, and the oxygen atom is bonded to one phosphorus atom with a single bond.

The oxygen atom forms a double bond with each phosphorus atom, resulting in a linear structure.

Each phosphorus atom forms a double bond with the oxygen atom, and the phosphorus atoms are connected by a single bond.

Each phosphorus atom forms a single bond with the oxygen atom, and the phosphorus atoms are not bonded to each other.

Previous problemNext problem

Verified step by step guidance

Step 1: Determine the total number of valence electrons available for bonding in the molecule P2O. Phosphorus (P) has 5 valence electrons, and oxygen (O) has 6 valence electrons. Since the molecule is neutral, sum these electrons accordingly: $2 \times 5 + 6$.

Step 2: Consider the possible bonding arrangements between the atoms. Since there are two phosphorus atoms and one oxygen atom, think about how these atoms can connect to satisfy the octet rule (or expanded octet for phosphorus) and minimize formal charges.

Step 3: Draw possible Lewis structures by connecting the atoms with single, double, or triple bonds. For each structure, distribute the remaining electrons as lone pairs to complete the octets of oxygen and phosphorus atoms.

Step 4: Calculate the formal charges for each atom in the different Lewis structures to identify the most stable arrangement. The best Lewis structure usually has formal charges closest to zero and places negative charges on the more electronegative atoms.

Step 5: Analyze the given options in light of your Lewis structures and formal charge calculations. The correct structure will be the one where the phosphorus atoms are connected by a triple bond, and the oxygen atom is bonded to one phosphorus atom with a single bond, as this arrangement best satisfies the octet rule and formal charge criteria.