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

13. Liquids, Solids & Intermolecular Forces

Molecular Polarity

General Chemistry

13. Liquids, Solids & Intermolecular Forces

Molecular Polarity

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Multiple Choice

Which of the following best describes the polarity of carbon tetrachloride (CCl4)?

CCl4 is polar because it has an uneven distribution of charge due to lone pairs on the central carbon atom.

CCl4 is a nonpolar molecule because its tetrahedral geometry causes the bond dipoles to cancel out.

CCl4 is a polar molecule because the C–Cl bonds are polar and the molecule contains chlorine atoms.

CCl4 is nonpolar because chlorine is less electronegative than carbon.

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Verified step by step guidance

Step 1: Identify the molecular geometry of carbon tetrachloride (CCl4). Carbon is the central atom bonded to four chlorine atoms, and there are no lone pairs on the carbon atom. This arrangement leads to a tetrahedral geometry.

Step 2: Understand the concept of bond polarity. Each C–Cl bond is polar because chlorine is more electronegative than carbon, creating a dipole moment pointing from carbon to chlorine.

Step 3: Analyze the symmetry of the molecule. In a tetrahedral geometry, the four polar C–Cl bonds are symmetrically arranged around the central carbon atom.

Step 4: Determine the net dipole moment. Because of the symmetrical tetrahedral shape, the individual bond dipoles cancel each other out, resulting in no overall dipole moment for the molecule.

Step 5: Conclude the polarity of CCl4. Despite having polar bonds, the molecule is nonpolar overall due to the symmetrical arrangement causing the bond dipoles to cancel.