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

How many electrons (including both lone pairs and bonding pairs) are shown in the correct Lewis dot structure of the neutral compound HClO?

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Verified step by step guidance

Step 1: Determine the total number of valence electrons for the neutral compound HClO by adding the valence electrons of each atom. Hydrogen (H) has 1 valence electron, chlorine (Cl) has 7 valence electrons, and oxygen (O) has 6 valence electrons. So, total valence electrons = 1 + 7 + 6.

Step 2: Draw the skeletal structure of HClO, typically with chlorine as the central atom bonded to hydrogen and oxygen. Connect the atoms with single bonds initially. Each single bond represents 2 shared electrons.

Step 3: Distribute the remaining valence electrons as lone pairs around the atoms to satisfy the octet rule (or duet for hydrogen). Remember that hydrogen only needs 2 electrons, while oxygen and chlorine generally need 8 electrons each.

Step 4: Count all the electrons shown in the Lewis structure, including both bonding pairs (shared electrons in bonds) and lone pairs (non-bonding electrons) on all atoms.

Step 5: Verify that the total number of electrons counted matches the total valence electrons calculated in Step 1, ensuring the Lewis structure is correct and complete.