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 is the best Lewis structure for the neutral compound CoCl_2?

Co atom in the center with two single bonds to Cl atoms, two lone pairs on Co, each Cl atom has three lone pairs.

Co atom in the center with two single bonds to Cl atoms, no lone pairs on Co, each Cl atom has three lone pairs.

Co atom in the center with one single bond and one triple bond to Cl atoms, no lone pairs on Co, each Cl atom has one lone pair.

Co atom in the center with two double bonds to Cl atoms, no lone pairs on Co, each Cl atom has two lone pairs.

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Verified step by step guidance

Step 1: Identify the total number of valence electrons available for bonding. Cobalt (Co) is a transition metal with variable valence electrons, but for CoCl_2, consider Co typically contributes 9 valence electrons (from its 3d and 4s orbitals), and each chlorine (Cl) atom contributes 7 valence electrons. Calculate the total valence electrons as: $9 + 2 \times 7 = 23$ electrons.

Step 2: Determine the bonding framework. Since CoCl_2 is a neutral compound, place the Co atom in the center bonded to two Cl atoms. Each bond (single, double, or triple) consists of 2 electrons. Start by assigning single bonds between Co and each Cl atom, using 4 electrons total.

Step 3: Distribute the remaining electrons to satisfy the octet rule for the Cl atoms first. Each Cl atom needs 8 electrons around it (including bonding electrons). Since each Cl is bonded by a single bond (2 electrons), assign 6 more electrons (3 lone pairs) to each Cl atom.

Step 4: Assign any leftover electrons to the central Co atom. After bonding and filling Cl atoms' octets, check if Co has any lone pairs or if it has an incomplete octet. Transition metals often have incomplete octets and can have fewer than 8 electrons around them without violating stability rules.

Step 5: Evaluate alternative bonding scenarios (double or triple bonds) and check if they satisfy the total valence electrons and the octet rule for all atoms. For CoCl_2, the best Lewis structure is the one with two single bonds, no lone pairs on Co, and three lone pairs on each Cl, as this arrangement satisfies electron counts and typical bonding patterns.