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 HNO2 (nitrous acid)?

The central nitrogen atom is bonded to two oxygen atoms, both with double bonds, and no hydrogen atom is attached.

The central nitrogen atom is bonded to two hydrogen atoms and one oxygen atom.

The central nitrogen atom is bonded to two oxygen atoms and one hydrogen atom, with one oxygen having a double bond and the other a single bond plus a hydrogen.

The central nitrogen atom is bonded to three oxygen atoms, with one oxygen also bonded to a hydrogen atom.

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Verified step by step guidance

Step 1: Identify the total number of valence electrons in HNO2. Hydrogen (H) has 1 valence electron, nitrogen (N) has 5, and oxygen (O) has 6 each. Since there are two oxygens, calculate the total as: $1 + 5 + 2 \times 6 = 18$ valence electrons.

Step 2: Determine the central atom, which is usually the least electronegative element that can form multiple bonds. Here, nitrogen (N) is the central atom bonded to two oxygen atoms.

Step 3: Connect the atoms with single bonds initially: N bonded to two O atoms, and one of the O atoms bonded to a hydrogen atom. This accounts for some of the valence electrons used in bonding.

Step 4: Distribute the remaining valence electrons to satisfy the octet rule for each atom. One oxygen will form a double bond with nitrogen to complete its octet, while the other oxygen is single bonded to nitrogen and also bonded to hydrogen, completing its octet with lone pairs.

Step 5: Confirm that the total number of electrons used in bonds and lone pairs equals the total valence electrons (18), and that the structure reflects the correct bonding: nitrogen bonded to two oxygens (one double bond, one single bond plus hydrogen).