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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 one of the following molecules is polar?

CCl4

XeF4

XeF2

BrF5

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Verified step by step guidance

Step 1: Understand that molecular polarity depends on both the polarity of individual bonds and the overall molecular geometry, which determines if bond dipoles cancel out or add up.

Step 2: Analyze the molecular geometry of each molecule using VSEPR theory: CCl4 is tetrahedral, XeF4 is square planar, XeF2 is linear, and BrF5 is square pyramidal.

Step 3: Determine the symmetry of each molecule: CCl4 and XeF4 are highly symmetrical, so their bond dipoles cancel, making them nonpolar; XeF2 is linear and symmetrical, so it is also nonpolar.

Step 4: Examine BrF5, which has a square pyramidal shape with one lone pair on the central atom, causing an asymmetrical shape and resulting in a net dipole moment, making it polar.

Step 5: Conclude that among the given molecules, BrF5 is polar due to its asymmetrical geometry and the presence of polar bonds that do not cancel out.