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 ICl_5?

The central iodine atom is surrounded by five chlorine atoms and one lone pair.

The central iodine atom is surrounded by six chlorine atoms and no lone pairs.

The central iodine atom is surrounded by four chlorine atoms and two lone pairs.

The central iodine atom is surrounded by five chlorine atoms and no lone pairs.

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Verified step by step guidance

Identify the central atom in the compound ICl_5. Since iodine (I) is less electronegative than chlorine (Cl), iodine will be the central atom.

Determine the total number of valence electrons available. Iodine has 7 valence electrons, and each chlorine atom has 7 valence electrons. For ICl_5, total valence electrons = 7 (I) + 5 × 7 (Cl) = 7 + 35 = 42 electrons.

Draw single bonds between the central iodine atom and each of the five chlorine atoms. Each bond uses 2 electrons, so 5 bonds use 10 electrons.

Subtract the bonding electrons from the total valence electrons to find the remaining electrons: 42 - 10 = 32 electrons. These remaining electrons are placed as lone pairs to satisfy the octet rule for the chlorine atoms first, then any leftover electrons are placed on the iodine atom.

Since iodine is in period 5, it can have an expanded octet. After placing lone pairs on the chlorines, the leftover electrons will form one lone pair on iodine, resulting in iodine being surrounded by five chlorine atoms and one lone pair.