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

Which of the following correctly represents the Lewis dot structure for the neutral compound CHF?

C is the central atom with single bonds to H and F; C has no lone pairs, F has three lone pairs, H has none.

C is the central atom with single bonds to H and F; C has two lone pairs, F has three lone pairs, H has none.

C is the central atom with single bonds to H and F; C has one lone pair, F has two lone pairs, H has one lone pair.

C is the central atom with double bonds to H and F; C has one lone pair, F has two lone pairs, H has none.

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Verified step by step guidance

Step 1: Determine the total number of valence electrons for the molecule CHF. Carbon (C) has 4 valence electrons, hydrogen (H) has 1, and fluorine (F) has 7. Add these together to find the total valence electrons available for bonding and lone pairs.

Step 2: Identify the central atom. Carbon is less electronegative than fluorine and hydrogen, so it will be the central atom. Arrange the atoms with carbon in the center, and hydrogen and fluorine bonded to it.

Step 3: Draw single bonds between the central carbon atom and each of the other atoms (H and F). Each single bond represents 2 electrons shared between atoms.

Step 4: Distribute the remaining valence electrons as lone pairs to satisfy the octet rule for each atom where applicable. Hydrogen only needs 2 electrons (a duet), carbon aims for 8 electrons, and fluorine also aims for 8 electrons. Remember that carbon typically does not have lone pairs in simple molecules like CHF.

Step 5: Verify the Lewis structure by checking that the total number of electrons used (bonding and lone pairs) equals the total valence electrons calculated in Step 1, and that each atom satisfies its electron requirements (octet or duet).