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

The Lewis electron-dot structure of H2CO has how many nonbonding electron pairs, bonding electron pairs, and what is the carbon-oxygen bond order?

2 nonbonding pairs, 4 bonding pairs, bond order of 2

0 nonbonding pairs, 6 bonding pairs, bond order of 1

3 nonbonding pairs, 3 bonding pairs, bond order of 3

1 nonbonding pair, 5 bonding pairs, bond order of 1

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Verified step by step guidance

Step 1: Identify the total number of valence electrons in H2CO. Hydrogen (H) has 1 valence electron, carbon (C) has 4, and oxygen (O) has 6. Calculate the total by adding these together: 2(1) + 4 + 6.

Step 2: Draw the skeletal structure of H2CO. Place carbon in the center, as it is the least electronegative element that can form multiple bonds. Attach the two hydrogen atoms to carbon and the oxygen atom to carbon.

Step 3: Distribute the total valence electrons around the atoms to satisfy the octet rule for carbon and oxygen, and the duet rule for hydrogen. Start by forming single bonds between C-H and C-O.

Step 4: Check if all atoms have a complete octet (or duet for hydrogen). If not, consider forming double bonds. In this case, form a double bond between carbon and oxygen to satisfy the octet rule for both atoms.

Step 5: Count the number of bonding pairs (shared electron pairs) and nonbonding pairs (lone pairs) on each atom. Determine the bond order of the carbon-oxygen bond by counting the number of bonds between them.