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

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Multiple Choice

After drawing the Lewis structure of BeH2, determine whether the molecule is polar or nonpolar.

BeH2 has polar bonds and is therefore polar.

BeH2 is a polar molecule.

BeH2 is a nonpolar molecule.

BeH2 is ionic and does not have polarity.

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Verified step by step guidance

Step 1: Draw the Lewis structure of BeH\_2. Beryllium (Be) is the central atom with two hydrogen (H) atoms bonded to it. Be has 2 valence electrons, and each H has 1 valence electron, so the total valence electrons are 4.

Step 2: Arrange the atoms so that Be is in the center with two single bonds to the two H atoms. This satisfies the octet rule for hydrogen (which only needs 2 electrons) but Be will have only 4 electrons around it, which is common for Be compounds.

Step 3: Determine the molecular geometry using VSEPR theory. With two bonding pairs and no lone pairs on Be, the molecule adopts a linear shape with a bond angle of 180°.

Step 4: Consider the polarity of the Be-H bonds. Although Be-H bonds are polar due to the difference in electronegativity, the linear geometry causes the bond dipoles to cancel each other out because they are equal in magnitude and opposite in direction.

Step 5: Conclude that because the bond dipoles cancel, the overall molecule has no net dipole moment, making BeH\_2 a nonpolar molecule despite having polar bonds.