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 ion ICl_4^-?

ICl_4^- is polar due to its lone pair.

ICl_4^- is a nonpolar molecule.

ICl_4^- is a polar molecule.

ICl_4^- is nonpolar because it has no lone pairs.

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Verified step by step guidance

Step 1: Determine the Lewis structure of the ion ICl_4^-. Iodine (I) is the central atom bonded to four chlorine (Cl) atoms, and the ion carries a negative charge, indicating extra electrons to consider.

Step 2: Count the total valence electrons. Iodine has 7 valence electrons, each chlorine has 7, and there is 1 extra electron due to the negative charge. Calculate total electrons: 7 (I) + 4 × 7 (Cl) + 1 (charge) = 36 electrons.

Step 3: Arrange the electrons to satisfy the octet rule for each atom. Place bonding pairs between iodine and each chlorine, then distribute remaining electrons as lone pairs, especially on iodine.

Step 4: Determine the molecular geometry using VSEPR theory. With four bonding pairs and two lone pairs on iodine, the electron geometry is octahedral, but the molecular shape is square planar due to the lone pairs being opposite each other.

Step 5: Analyze the polarity. In a square planar shape, the dipole moments of the I–Cl bonds cancel out due to symmetry, and the lone pairs are arranged symmetrically, making the overall molecule nonpolar.