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 molecular polarity of the chlorate ion, ClO_3^-?

ClO_3^- is polar because it has no lone pairs on the central atom.

ClO_3^- is nonpolar because it contains only nonpolar covalent bonds.

ClO_3^- is a polar molecule due to its asymmetric shape and uneven charge distribution.

ClO_3^- is a nonpolar molecule because all the Cl–O bonds are identical and the molecule is symmetrical.

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Verified step by step guidance

Step 1: Determine the Lewis structure of the chlorate ion (ClO_3^-). Count the total valence electrons from chlorine, oxygen atoms, and the extra electron due to the negative charge.

Step 2: Draw the skeletal structure with chlorine as the central atom bonded to three oxygen atoms. Distribute the remaining electrons to satisfy the octet rule, considering resonance structures and formal charges.

Step 3: Identify the molecular geometry around the central chlorine atom using VSEPR theory. Consider the number of bonding pairs and lone pairs on chlorine to predict the shape.

Step 4: Analyze the symmetry of the molecule based on its geometry. Determine if the shape is symmetrical or asymmetrical, which affects the overall polarity.

Step 5: Evaluate the bond dipoles of the Cl–O bonds and their vector sum. If the dipoles do not cancel out due to asymmetry, the molecule is polar; if they cancel, it is nonpolar.