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 ClF_5?

Chlorine is surrounded by five single bonds to fluorine atoms and no lone pairs.

Chlorine is surrounded by four single bonds to fluorine atoms and two lone pairs.

Chlorine is surrounded by six single bonds to fluorine atoms and no lone pairs.

Chlorine is surrounded by five single bonds to fluorine atoms and one lone pair.

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Verified step by step guidance

Step 1: Determine the total number of valence electrons in ClF_5. Chlorine (Cl) has 7 valence electrons, and each fluorine (F) atom has 7 valence electrons. Since there are 5 fluorine atoms, calculate the total as: $7 + 5 \times 7$.

Step 2: Draw a skeletal structure with chlorine as the central atom bonded to five fluorine atoms using single bonds. Each single bond represents 2 electrons shared between atoms.

Step 3: Subtract the electrons used in the bonds from the total valence electrons to find the remaining electrons that will be placed as lone pairs.

Step 4: Distribute the remaining electrons as lone pairs to complete the octets of the fluorine atoms first, since fluorine is highly electronegative and typically completes its octet with lone pairs.

Step 5: Place any leftover electrons on the central chlorine atom as lone pairs. Since chlorine can expand its octet, it can accommodate more than 8 electrons, so check if chlorine has one lone pair after bonding with five fluorines.