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

After drawing the Lewis structure of carbonyl sulfide (CSO), which of the following best describes the polarity of the molecule?

CSO is a polar molecule because it has an asymmetric distribution of electron density.

CSO is a nonpolar molecule because its molecular geometry is linear and the dipoles cancel.

CSO is a nonpolar molecule because all the atoms have similar electronegativities.

CSO is a polar molecule because it contains only nonmetals.

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Verified step by step guidance

Step 1: Draw the Lewis structure of carbonyl sulfide (CSO) by first counting the total valence electrons. Carbon (C) has 4, sulfur (S) has 6, and oxygen (O) has 6, giving a total of 16 valence electrons.

Step 2: Arrange the atoms with carbon in the center, sulfur on one side, and oxygen on the other, then distribute the electrons to satisfy the octet rule for each atom, forming double bonds as needed (typically C=O and C=S).

Step 3: Determine the molecular geometry. Since CSO is a triatomic molecule with a central atom bonded to two other atoms, the geometry is linear.

Step 4: Analyze the electronegativities of the atoms: oxygen is more electronegative than carbon, which is more electronegative than sulfur. This difference creates bond dipoles that do not cancel out due to the asymmetric distribution of electron density.

Step 5: Conclude that because the bond dipoles are unequal and the molecule is linear but asymmetric in terms of electronegativity, CSO is a polar molecule with an asymmetric distribution of electron density.