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 statements correctly describes the Lewis dot structure of the neutral compound TeF_2?

Te is the central atom with two double bonds to F atoms and no lone pairs on Te.

Te is the central atom with two single bonds to F atoms and two lone pairs on Te.

Te is the central atom with two single bonds to F atoms and one lone pair on Te.

Te is the central atom with three single bonds to F atoms and one lone pair on Te.

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Verified step by step guidance

Step 1: Determine the total number of valence electrons available for the molecule TeF_2. Tellurium (Te) is in group 16, so it has 6 valence electrons, and each fluorine (F) atom has 7 valence electrons. Since there are two fluorine atoms, total valence electrons = 6 (Te) + 2 × 7 (F) = 20 electrons.

Step 2: Identify the central atom, which is usually the least electronegative element. Here, Te is less electronegative than F, so Te is the central atom.

Step 3: Connect the central atom to each fluorine atom with single bonds. Each single bond consists of 2 electrons, so 2 bonds use 4 electrons, leaving 16 electrons to be distributed as lone pairs.

Step 4: Distribute the remaining electrons to satisfy the octet rule for the fluorine atoms first. Each fluorine needs 6 more electrons (3 lone pairs) to complete its octet, so 2 fluorines require 12 electrons. Subtracting these 12 electrons from the remaining 16 leaves 4 electrons to be placed as lone pairs on Te.

Step 5: Assign the remaining 4 electrons as two lone pairs on the central Te atom. This arrangement satisfies the octet rule for all atoms and matches the description: Te with two single bonds to F atoms and two lone pairs on Te.