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

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Multiple Choice

Which of the following best represents the Lewis dot structure for neutral H3PO4 (phosphoric acid)?

A central P atom bonded to four H atoms and one O atom, with all atoms having complete octets.

A central P atom bonded to two O atoms (one double-bonded), and three H atoms directly bonded to P.

A central P atom bonded to three O atoms, each O atom bonded to an H atom, and one lone pair on P.

A central P atom bonded to four O atoms, one of which is double-bonded; three O atoms each bonded to an H atom, with all atoms having complete octets.

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Verified step by step guidance

Identify the central atom in H3PO4, which is phosphorus (P), because it is less electronegative than oxygen and hydrogen and can form multiple bonds.

Determine the total number of valence electrons: phosphorus has 5, each oxygen has 6, and each hydrogen has 1. Calculate the sum for all atoms in H3PO4.

Arrange the atoms with phosphorus in the center, bonded to four oxygen atoms. Three of these oxygen atoms will be bonded to hydrogen atoms (forming OH groups), and one oxygen will be double-bonded to phosphorus.

Distribute the remaining valence electrons to satisfy the octet rule for oxygen and phosphorus atoms, remembering that phosphorus can have an expanded octet (more than 8 electrons).

Verify that all hydrogen atoms have one bond (duet rule), all oxygen atoms have complete octets, and phosphorus has a stable structure with one double bond to oxygen and three single bonds to oxygen atoms that are each bonded to hydrogen.