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

Previous problemNext problem

Struggling with General Chemistry?

Join thousands of students who trust us to help them ace their exams!Watch the first video

Multiple Choice

After drawing the Lewis structure of BH3, which of the following best describes the polarity of the BH3 molecule?

BH3 is a nonpolar molecule because it has a tetrahedral geometry.

BH3 is a polar molecule because it contains a lone pair on boron.

BH3 is a nonpolar molecule because its shape is trigonal planar and the dipoles cancel.

BH3 is a polar molecule because boron is less electronegative than hydrogen.

Previous problemNext problem

Verified step by step guidance

Step 1: Draw the Lewis structure of BH3 by placing boron (B) in the center and three hydrogen (H) atoms around it, forming three single bonds. Note that boron has only six valence electrons in this structure, so it does not have a complete octet and no lone pairs.

Step 2: Determine the molecular geometry of BH3 using the VSEPR theory. Since there are three bonding pairs and no lone pairs on the central boron atom, the shape is trigonal planar.

Step 3: Analyze the polarity of each B-H bond by considering the electronegativity difference between boron and hydrogen. Although boron is slightly less electronegative than hydrogen, the difference is small, and each bond has a small dipole moment.

Step 4: Consider the overall molecular polarity by looking at the symmetry of the molecule. In a trigonal planar shape, the three B-H bond dipoles are arranged 120° apart and symmetrically cancel each other out.

Step 5: Conclude that because the dipole moments cancel due to the trigonal planar geometry and the absence of lone pairs, BH3 is a nonpolar molecule.