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 CHF, determine whether the molecule is polar or nonpolar.

Polar

Nonpolar

Cannot be determined

Ionic

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Verified step by step guidance

Step 1: Draw the Lewis structure of CHF by first counting the total valence electrons. Carbon (C) has 4 valence electrons, hydrogen (H) has 1, and fluorine (F) has 7, giving a total of 12 valence electrons.

Step 2: Arrange the atoms with carbon as the central atom, since it is less electronegative than fluorine. Connect carbon to hydrogen and fluorine with single bonds, using 2 electrons per bond.

Step 3: Complete the octet for fluorine by adding the remaining electrons as lone pairs around it. Carbon will have 8 electrons around it (including bonding pairs), and hydrogen will have 2 electrons (bonding pair).

Step 4: Determine the molecular geometry around the central carbon atom. Since carbon is bonded to two atoms and has no lone pairs, the shape is linear.

Step 5: Assess the polarity by considering the difference in electronegativity between carbon, hydrogen, and fluorine. Fluorine is highly electronegative, creating a dipole moment. Because the molecule is linear but the atoms bonded are different, the dipoles do not cancel, making CHF a polar molecule.