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 best describes the Lewis dot structure for the neutral compound CF_4?

Carbon is at the center with four single bonds to four fluorine atoms; each fluorine has three lone pairs.

Carbon is at the center with one double bond and three single bonds to fluorine atoms; each fluorine has three lone pairs.

Carbon is at the center with four single bonds to four fluorine atoms; each fluorine has two lone pairs.

Carbon is at the center with two double bonds to two fluorine atoms; each fluorine has two lone pairs.

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Verified step by step guidance

Step 1: Determine the total number of valence electrons available for the molecule CF_4. Carbon has 4 valence electrons, and each fluorine atom has 7 valence electrons. Since there are 4 fluorine atoms, calculate the total valence electrons as $4 + 4 \times 7$.

Step 2: Identify the central atom, which is usually the least electronegative element. In CF_4, carbon is less electronegative than fluorine, so place carbon at the center and arrange the four fluorine atoms around it.

Step 3: Form single bonds between the central carbon atom and each fluorine atom. Each single bond consists of 2 electrons, so subtract these bonding electrons from the total valence electrons calculated in Step 1.

Step 4: Distribute the remaining valence electrons as lone pairs on the fluorine atoms to complete their octets. Remember that each fluorine atom needs 8 electrons total (including bonding electrons) to satisfy the octet rule.

Step 5: Verify that the carbon atom also has a complete octet by counting the electrons around it (from the four single bonds). Confirm that the structure has no formal charges and that all atoms satisfy the octet rule.