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 N2O?

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

The two nitrogen atoms are bonded to each other with a triple bond, and oxygen is attached with a single bond.

All three atoms are connected in a straight line with only single bonds.

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

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Verified step by step guidance

Step 1: Identify the total number of valence electrons available for 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 skeletal structure of the molecule. For N2O, the atoms are typically arranged linearly as N–N–O or N–O–N. The problem suggests considering nitrogen as the central atom, so arrange the atoms as N (central) bonded to N and O.

Step 3: Distribute electrons to form bonds between atoms. Start by placing single bonds between the central nitrogen and the other nitrogen and oxygen atoms. Each single bond accounts for 2 electrons.

Step 4: Complete the octets of the outer atoms (the terminal nitrogen and oxygen) by adding lone pairs, then adjust bonding (single, double, or triple bonds) to satisfy the octet rule for all atoms and to use all 16 valence electrons.

Step 5: Verify the formal charges on each atom to ensure the most stable Lewis structure. The correct Lewis structure will have the central nitrogen atom double bonded to one nitrogen and single bonded to oxygen, with formal charges minimized and the octet rule satisfied.