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 the product formed when sodium reacts with chlorine to form a neutral compound?

Na and Cl each with one dot between them, sharing a pair of electrons

Na with one dot and Cl with seven dots, not interacting

Na surrounded by eight dots and Cl with seven dots

Na with no dots and Cl surrounded by eight dots, with Na and Cl adjacent

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Verified step by step guidance

Identify the nature of the elements involved: Sodium (Na) is a metal and chlorine (Cl) is a nonmetal. Sodium tends to lose one electron to achieve a stable electron configuration, while chlorine tends to gain one electron to complete its octet.

Recall that in ionic bonding, electrons are transferred rather than shared. Sodium will lose its one valence electron, becoming a Na⁺ ion with no dots (no valence electrons), and chlorine will gain that electron, becoming a Cl⁻ ion with eight valence electrons (represented as eight dots around Cl).

Draw the Lewis dot structure for the product by showing Na with no dots (indicating it has lost its valence electron) and Cl with eight dots around it (indicating a full octet), placing Na and Cl adjacent to each other to represent the ionic bond formed by electrostatic attraction.

Understand that the other options involving shared dots or incomplete octets do not represent the ionic nature of the compound formed between sodium and chlorine.

Conclude that the correct Lewis structure for the neutral compound formed (NaCl) is Na with no dots and Cl surrounded by eight dots, placed next to each other to indicate the ionic bond.