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 best describes the Lewis dot structure of the neutral compound C2H2 (ethyne)?

The two carbon atoms are connected by a single bond, and each carbon has three hydrogen atoms attached.

The two carbon atoms are connected by a triple bond, and both hydrogens are attached to the same carbon atom.

Each carbon atom is connected by a triple bond, and each carbon has one hydrogen atom attached.

Each carbon atom is connected by a double bond, and each carbon has two hydrogen atoms attached.

Previous problemNext problem

Verified step by step guidance

Step 1: Determine the total number of valence electrons available for bonding in C2H2. Carbon has 4 valence electrons and hydrogen has 1 valence electron. Since there are 2 carbons and 2 hydrogens, calculate the total valence electrons as: $2 \times 4 + 2 \times 1$.

Step 2: Recognize that the molecule is neutral, so the total number of valence electrons calculated will be used to form bonds and satisfy the octet rule for carbon atoms and the duet rule for hydrogen atoms.

Step 3: Consider the bonding possibilities between the two carbon atoms. Carbon atoms can form single, double, or triple bonds. The structure must allow each carbon to have a full octet and each hydrogen to have 2 electrons (a duet).

Step 4: Evaluate the options given: a single bond between carbons with three hydrogens on each carbon would exceed the number of hydrogens in the formula; a triple bond between carbons with both hydrogens on the same carbon would not satisfy the molecular formula C2H2; a double bond with two hydrogens on each carbon would also exceed the number of hydrogens.

Step 5: Conclude that the correct Lewis structure has a triple bond between the two carbon atoms, with each carbon atom bonded to one hydrogen atom, satisfying both the octet rule for carbon and the duet rule for hydrogen, and matching the molecular formula C2H2.