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 statements correctly describes the Lewis dot structure of the Cl$_3^-$ ion?

It is made up of three chlorine atoms, each with a single bond to the others and no formal charge.

It contains three chlorine atoms connected in a linear arrangement, with one central atom bearing a negative charge and two lone pairs.

It has two chlorine atoms bonded to a central chlorine atom, with the negative charge distributed equally among all atoms.

It consists of three chlorine atoms arranged in a triangle, each sharing one electron with the others and no lone pairs.

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Verified step by step guidance

Step 1: Identify the species and its components. The Cl$_3^-$ ion consists of three chlorine atoms and an overall negative charge of -1.

Step 2: Determine the total number of valence electrons. Each chlorine atom has 7 valence electrons, so for three atoms, that's $3 \times 7 = 21$ electrons. Add 1 extra electron for the negative charge, giving a total of 22 valence electrons.

Step 3: Consider the possible bonding arrangements. Since chlorine typically forms one single bond and prefers to complete its octet with lone pairs, think about how the atoms can be connected to satisfy the octet rule and accommodate the extra electron.

Step 4: Analyze the geometry and formal charges. The most stable Lewis structure will minimize formal charges and place the negative charge on the atom best able to accommodate it (usually the central atom). The linear arrangement with a central chlorine atom bearing the negative charge and two lone pairs on it fits this description.

Step 5: Compare the given statements to the Lewis structure principles. The correct description should mention three chlorine atoms connected linearly, with the central atom carrying the negative charge and having lone pairs, consistent with the octet rule and formal charge distribution.