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

Previous problemNext problem

Struggling with General Chemistry?

Join thousands of students who trust us to help them ace their exams!Watch the first video

Multiple Choice

Which of the following statements correctly describes how to draw a Lewis structure for a neutral compound?

Count the total number of valence electrons for all atoms in the compound.

Assign all electrons to the most electronegative atom first.

Place all lone pairs on hydrogen atoms.

Ignore the octet rule for second-period elements.

Previous problemNext problem

Verified step by step guidance

Step 1: Understand that drawing a Lewis structure begins with determining the total number of valence electrons available in the molecule. This is done by summing the valence electrons of all atoms present in the compound, considering their group number in the periodic table.

Step 2: Recognize that after counting valence electrons, the next step is to arrange the atoms, usually placing the least electronegative atom in the center (except hydrogen, which is always terminal).

Step 3: Connect the atoms with single bonds initially, each bond representing two electrons, and then distribute the remaining electrons as lone pairs to satisfy the octet rule (or duet rule for hydrogen) for each atom.

Step 4: Assign lone pairs starting with the more electronegative atoms to complete their octets, rather than assigning all electrons first to the most electronegative atom or placing lone pairs on hydrogen, which can only have two electrons.

Step 5: Remember that the octet rule generally applies to second-period elements (like C, N, O, F), so it should not be ignored; exceptions exist but are rare and must be justified.