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 is the correct Lewis dot structure for the neutral compound HC2H (acetylene)?

H–C=C–H, with a double bond between the carbon atoms and each hydrogen atom bonded to a carbon

H–C≡C–H, with each carbon atom having a complete octet and each hydrogen atom having a single bond

H=C=C=H, with each atom connected by double bonds

H–C–C–H, with single bonds only between all atoms

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Verified step by step guidance

Step 1: Identify the total number of valence electrons in the molecule HC2H (acetylene). Hydrogen has 1 valence electron each, and carbon has 4 valence electrons each. Calculate the sum: $2 \times 1 + 2 \times 4 = 10$ valence electrons.

Step 2: Arrange the atoms with carbon atoms in the center and hydrogen atoms at the ends, since hydrogen can only form one bond. The skeletal structure is H–C–C–H.

Step 3: Connect the atoms with single bonds initially. Each single bond represents 2 electrons. Assign electrons to bonds: 3 bonds total (H–C, C–C, C–H) use 6 electrons, leaving 4 electrons to be distributed as lone pairs or additional bonds.

Step 4: To satisfy the octet rule for carbon atoms (8 electrons around each carbon), add multiple bonds between the two carbon atoms. Since each carbon is bonded to one hydrogen, the remaining electrons form a triple bond between the carbons (one sigma and two pi bonds).

Step 5: Verify that each hydrogen has 2 electrons (a single bond) and each carbon has 8 electrons (from the single bond to hydrogen and the triple bond between carbons). This confirms the correct Lewis structure is H–C≡C–H.