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 is the correct Lewis structure for OSF4, where sulfur (S) is the central atom and all atoms have a formal charge of zero?

S is bonded to one oxygen (O) atom with a single bond and four fluorine (F) atoms with single bonds, with one lone pair on the sulfur.

S is bonded to one oxygen (O) atom with a double bond and four fluorine (F) atoms with single bonds, with two lone pairs on the oxygen.

S is bonded to one oxygen (O) atom with a double bond and four fluorine (F) atoms with single bonds, with one lone pair on the sulfur.

S is bonded to one oxygen (O) atom with a single bond and four fluorine (F) atoms with double bonds, with no lone pairs on the oxygen.

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Verified step by step guidance

Identify the central atom in the molecule. In OSF4, sulfur (S) is the central atom.

Determine the total number of valence electrons available. Oxygen (O) has 6 valence electrons, sulfur (S) has 6 valence electrons, and each fluorine (F) has 7 valence electrons. Calculate the total: 6 (O) + 6 (S) + 4 * 7 (F) = 40 valence electrons.

Arrange the atoms around the central sulfur atom. Connect sulfur to oxygen with a double bond and to each fluorine with a single bond. This uses 2 electrons for the S=O bond and 8 electrons for the S-F bonds (2 electrons per bond).

Distribute the remaining electrons to satisfy the octet rule. Place two lone pairs on the oxygen atom to complete its octet, using 4 electrons. Place one lone pair on the sulfur atom, using 2 electrons.

Verify the formal charges. Calculate the formal charge for each atom using the formula: Formal Charge = Valence Electrons - (Non-bonding Electrons + 1/2 Bonding Electrons). Ensure all atoms have a formal charge of zero.