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 a neutral molecule of I2?

Two iodine atoms connected by a single bond, each with three lone pairs.

Two iodine atoms connected by a triple bond, each with one lone pair.

Two iodine atoms connected by a double bond, each with two lone pairs.

Two iodine atoms connected by a single bond, each with two lone pairs.

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Verified step by step guidance

Step 1: Determine the total number of valence electrons for the I2 molecule. Each iodine atom is in group 17, so it has 7 valence electrons. For two iodine atoms, total valence electrons = 7 + 7 = 14.

Step 2: Connect the two iodine atoms with a single bond. A single bond consists of 2 electrons shared between the atoms, so subtract 2 electrons from the total valence electrons to account for the bonding pair.

Step 3: Distribute the remaining electrons as lone pairs around each iodine atom to satisfy the octet rule. Each iodine atom should have 8 electrons around it (including bonding electrons).

Step 4: Calculate the number of lone pairs on each iodine atom. Since each iodine shares 2 electrons in the bond, the remaining electrons around each iodine are lone pairs. Divide the leftover electrons equally between the two atoms.

Step 5: Confirm that each iodine atom has a complete octet (8 electrons total) and that the molecule is neutral with no formal charges. This will verify the correct Lewis structure.