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 for the neutral dinitrogen monoxide (N2O) molecule?

The central atom is nitrogen, with a triple bond to one nitrogen and a single bond to oxygen.

The molecule has a linear structure with all atoms connected by single bonds.

The central atom is oxygen, with single bonds to each nitrogen atom.

The two nitrogen atoms are bonded to each other by a single bond, and both are singly bonded to oxygen.

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Verified step by step guidance

Step 1: Identify the total number of valence electrons in the N2O molecule. Nitrogen has 5 valence electrons and oxygen has 6 valence electrons. Since there are two nitrogen atoms and one oxygen atom, calculate the total valence electrons as: $2 \times 5 + 6 = 16$ electrons.

Step 2: Determine the central atom. In N2O, nitrogen is less electronegative than oxygen, so nitrogen is typically the central atom. This means the structure will have nitrogen in the center bonded to the other nitrogen and oxygen atoms.

Step 3: Arrange the atoms linearly as N–N–O or N–O–N and try to distribute the 16 valence electrons to satisfy the octet rule for each atom. Consider multiple bonding possibilities (single, double, triple bonds) to achieve full octets.

Step 4: Evaluate bonding patterns. A common and stable Lewis structure for N2O has the central nitrogen atom forming a triple bond with one nitrogen atom and a single bond with the oxygen atom. This arrangement satisfies the octet rule and accounts for all valence electrons.

Step 5: Confirm the molecular geometry. The Lewis structure with the central nitrogen atom triple bonded to nitrogen and single bonded to oxygen results in a linear molecule, consistent with experimental observations.