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 Lewis electron-dot diagram best represents the bonding in neutral potassium iodide (KI)?

K oxed{8} ext{ I} oxed{8}

K^{+} oxed{} ext{ I}^{-} oxed{8}

K^{+} oxed{8} ext{ I}^{-} oxed{1}

K oxed{1} ext{ I} oxed{7}

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Verified step by step guidance

Step 1: Understand the nature of bonding in potassium iodide (KI). KI is an ionic compound formed between potassium (K), a metal, and iodine (I), a nonmetal. Potassium tends to lose one electron to achieve a stable electron configuration, while iodine tends to gain one electron to complete its octet.

Step 2: Represent the electron transfer. Potassium (K) loses one electron to become a potassium ion (K^{+}), and iodine (I) gains one electron to become an iodide ion (I^{-}). This electron transfer results in the formation of ions with full octets.

Step 3: Draw the Lewis electron-dot diagram for K^{+}. Since potassium loses its one valence electron, it will have no dots around it, and it carries a positive charge. The symbol is written as $K^{+}$ with no dots.

Step 4: Draw the Lewis electron-dot diagram for I^{-}. Iodine gains one electron, so it will have eight dots around it representing a full octet, and it carries a negative charge. The symbol is written as $I^{-}$ with eight dots around it.

Step 5: Combine the two ions to represent the ionic bond in KI. The correct Lewis structure shows $K^{+}$ without dots and $I^{-}$ with eight dots, indicating the transfer of one electron from potassium to iodine and the resulting ionic bond.