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 best describes the Lewis dot structure for the neutral compound SeO_2?

The selenium atom is bonded to two oxygen atoms with single bonds, and each oxygen has three lone pairs.

The selenium atom is bonded to two oxygen atoms with double bonds, and each oxygen has two lone pairs.

The selenium atom is bonded to one oxygen atom with a double bond and to the other with a single bond; the single-bonded oxygen has three lone pairs.

The selenium atom is bonded to two oxygen atoms with triple bonds, and each oxygen has one lone pair.

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Verified step by step guidance

Step 1: Determine the total number of valence electrons available for the SeO_2 molecule. Selenium (Se) is in group 16 and has 6 valence electrons, and each oxygen (O) atom also has 6 valence electrons. So, total valence electrons = 6 (Se) + 2 × 6 (O) = 18 electrons.

Step 2: Draw a skeletal structure with selenium as the central atom bonded to two oxygen atoms. Connect Se to each O with single bonds initially, using 2 electrons per bond, which accounts for 4 electrons.

Step 3: Distribute the remaining electrons to satisfy the octet rule for the oxygen atoms first by adding lone pairs. Each oxygen needs 8 electrons total (including bonding electrons). After placing lone pairs, check if the octet rule is satisfied for oxygen and selenium.

Step 4: If selenium does not have a complete octet, consider forming double bonds by converting lone pairs on oxygen into bonding pairs between Se and O. This will reduce lone pairs on oxygen and increase bonding electrons, helping selenium reach an octet.

Step 5: Confirm the final Lewis structure by counting all electrons to ensure the total matches the valence electrons calculated in Step 1, and verify that all atoms have complete octets (or expanded octet if applicable). The most stable structure will have selenium bonded to two oxygens with double bonds, and each oxygen having two lone pairs.