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

Previous problemNext problem

Struggling with General Chemistry?

Join thousands of students who trust us to help them ace their exams!Watch the first video

Multiple Choice

Which of the following is the correct Lewis structure for OSF4, ensuring that the formal charges of all atoms are zero?

S is the central atom with one double bond to O and four single bonds to F, with lone pairs on O and S.

S is the central atom with one single bond to O and four single bonds to F, with lone pairs on O and S.

S is the central atom with one single bond to O and four single bonds to F, with lone pairs only on O.

S is the central atom with one double bond to O and four double bonds to F, with lone pairs on O and S.

Previous problemNext problem

Verified step by step guidance

Identify the central atom in the molecule OSF4. Typically, the least electronegative atom is chosen as the central atom, which in this case is sulfur (S).

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

Arrange the atoms with sulfur in the center, bonded to oxygen and four fluorine atoms. Initially, connect each atom with a single bond, which uses up 10 electrons (5 bonds x 2 electrons per bond).

Distribute the remaining electrons to satisfy the octet rule, starting with the outer atoms (fluorine and oxygen). Each fluorine needs 6 more electrons to complete its octet, using up 24 electrons (4 F x 6 electrons). Oxygen will need 4 more electrons to complete its octet, using up the remaining 6 electrons.

Check the formal charges to ensure they are zero. Adjust the bonds if necessary. For sulfur to have a formal charge of zero, it should have a double bond with oxygen, as sulfur can expand its octet. This configuration will ensure all atoms have a formal charge of zero.