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 statements correctly describes the Lewis dot structure of the neutral compound SCl_4?

Sulfur is the central atom, surrounded by two single bonds and two double bonds to chlorine atoms.

Sulfur is the central atom, surrounded by four double bonds to chlorine atoms and no lone pairs.

Sulfur is the central atom, surrounded by four single bonds to chlorine atoms and one lone pair.

Sulfur is the central atom, surrounded by four single bonds to chlorine atoms and no lone pairs.

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Verified step by step guidance

Step 1: Identify the total number of valence electrons in the molecule SCl_4. Sulfur (S) is in group 16 and has 6 valence electrons, and each chlorine (Cl) atom is in group 17 with 7 valence electrons. Multiply the number of chlorine atoms by 7 and add sulfur's 6 electrons to get the total.

Step 2: Determine the central atom. Sulfur is less electronegative than chlorine, so sulfur will be the central atom with four chlorine atoms bonded to it.

Step 3: Draw single bonds between sulfur and each chlorine atom. Each single bond represents 2 electrons shared between atoms. Subtract these bonding electrons from the total valence electrons to find the remaining electrons.

Step 4: Distribute the remaining electrons as lone pairs to satisfy the octet rule for the chlorine atoms first, since chlorine atoms typically complete their octet with three lone pairs each.

Step 5: Check the number of electrons around sulfur. Since sulfur is in period 3, it can have an expanded octet. After placing bonding pairs and lone pairs on chlorine, assign any leftover electrons as lone pairs on sulfur. This will help determine if sulfur has any lone pairs and confirm the correct Lewis structure.