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 CCl4, determine whether the molecule is polar or nonpolar.

CCl4 is ionic.

CCl4 is a polar molecule.

CCl4 has both polar and nonpolar bonds.

CCl4 is a nonpolar molecule.

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Verified step by step guidance

Step 1: Draw the Lewis structure of CCl\_4 by placing the carbon atom in the center and surrounding it with four chlorine atoms, each connected by a single bond. Carbon has 4 valence electrons, and each chlorine has 7 valence electrons, so the structure satisfies the octet rule for all atoms.

Step 2: Identify the type of bonds between carbon and chlorine. Since chlorine is more electronegative than carbon, each C–Cl bond is polar, with a dipole moment pointing from carbon to chlorine.

Step 3: Analyze the molecular geometry of CCl\_4. The molecule has a tetrahedral shape because there are four bonding pairs and no lone pairs on the central carbon atom, leading to bond angles of approximately 109.5°.

Step 4: Determine the overall polarity by considering the symmetry of the molecule. In a tetrahedral geometry with four identical polar bonds symmetrically arranged, the individual bond dipoles cancel each other out.

Step 5: Conclude that despite having polar bonds, the symmetrical arrangement causes the dipoles to cancel, making CCl\_4 a nonpolar molecule overall.