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

In the Lewis dot structure of the neutral compound ClO_2, how many unshared (non-bonding) electrons are present in total?

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Determine the total number of valence electrons for the ClO_2 molecule. Chlorine (Cl) has 7 valence electrons, and each oxygen (O) has 6 valence electrons. Since there are two oxygens, calculate the total as: $7 + 2 \times 6$.

Draw a skeletal structure for ClO_2, placing chlorine as the central atom bonded to the two oxygen atoms with single bonds initially.

Distribute the remaining valence electrons around the atoms to satisfy the octet rule, starting by completing the octets of the oxygen atoms with lone pairs (non-bonding electrons).

If necessary, form double bonds between chlorine and oxygen atoms to ensure that the total number of electrons matches the total valence electrons and that the octet rule is satisfied as much as possible.

Count all the lone pairs (non-bonding electrons) on all atoms in the final Lewis structure. Each lone pair consists of 2 electrons, so multiply the number of lone pairs by 2 to find the total number of unshared electrons.