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 correct Lewis dot structure for the neutral compound S2O?

The two sulfur atoms are bonded to each other with a double bond (S=S), and one sulfur is bonded to the oxygen atom with a double bond (S=O), with all atoms having complete octets.

The two sulfur atoms are bonded to each other with a single bond (S–S), and each sulfur is bonded to the oxygen atom with a single bond (S–O), with all atoms having complete octets.

Both sulfur atoms are bonded to the oxygen atom, with one S=O double bond and one S–O single bond, and each atom has a complete octet.

The oxygen atom is bonded to both sulfur atoms with single bonds (O–S–S), and all atoms have complete octets.

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Verified step by step guidance

Step 1: Determine the total number of valence electrons available for the molecule S2O. Sulfur (S) has 6 valence electrons, and oxygen (O) also has 6 valence electrons. Since there are two sulfur atoms and one oxygen atom, calculate the total as: $2 \times 6 + 6 = 18$ valence electrons.

Step 2: Consider possible bonding arrangements between the atoms. Since the molecule is S2O, the sulfur atoms can bond to each other and to the oxygen atom. Explore structures where sulfur atoms are bonded together and to oxygen, keeping in mind the octet rule (each atom tends to have 8 electrons around it).

Step 3: Draw Lewis structures for each proposed bonding pattern, distributing the 18 valence electrons as bonding pairs (shared electrons) and lone pairs (non-bonding electrons) to satisfy the octet rule for each atom. Remember that double bonds count as two pairs of shared electrons.

Step 4: Evaluate each Lewis structure for formal charges on each atom to identify the most stable structure. The best Lewis structure usually has formal charges closest to zero and places negative charges on the more electronegative atoms (oxygen in this case).

Step 5: Identify the structure where the two sulfur atoms are connected by a double bond (S=S), and one sulfur is double bonded to the oxygen atom (S=O), with all atoms having complete octets and minimal formal charges. This structure best satisfies the octet rule and formal charge considerations.