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 neutral CoCl2?

Cobalt is surrounded by two chlorine atoms, each forming a single bond, and cobalt has two lone pairs.

Cobalt forms double bonds with each chlorine atom, and each chlorine has two lone pairs.

Cobalt is surrounded by two chlorine atoms, each forming a single bond, and cobalt has no lone pairs.

Cobalt forms a triple bond with one chlorine and a single bond with the other chlorine.

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Verified step by step guidance

Step 1: Identify the valence electrons for each atom involved. Cobalt (Co) is a transition metal with valence electrons primarily in the 3d and 4s orbitals, while chlorine (Cl) has 7 valence electrons in the 3s and 3p orbitals.

Step 2: Determine the bonding pattern based on typical coordination and bonding behavior. Transition metals like cobalt often form coordinate covalent bonds with halogens, usually single bonds, and do not commonly form multiple bonds (double or triple) with chlorine.

Step 3: Draw the Lewis structure by placing cobalt in the center and connecting it to two chlorine atoms with single bonds. Each chlorine atom will have three lone pairs to complete its octet.

Step 4: Assess the presence of lone pairs on cobalt. In many coordination compounds, cobalt uses its valence electrons to bond with ligands and typically does not retain lone pairs in the Lewis structure representation.

Step 5: Confirm that the overall structure is neutral by ensuring the total number of electrons around cobalt and chlorine atoms matches their valence requirements, with cobalt bonded to two chlorines via single bonds and no lone pairs on cobalt.