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

10. Periodic Properties of the Elements

Valence Electrons of Elements

General Chemistry

10. Periodic Properties of the Elements

Valence Electrons of Elements

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Multiple Choice

Which of the following correctly states the number of valence electrons in H2S and provides the correct Lewis structure for the molecule?

H2S has 4 valence electrons; the Lewis structure shows sulfur in the center with two single bonds to hydrogen and no lone pairs on sulfur.

H2S has 8 valence electrons; the Lewis structure shows sulfur in the center with two single bonds to hydrogen and two lone pairs on sulfur.

H2S has 10 valence electrons; the Lewis structure shows sulfur in the center with two double bonds to hydrogen and two lone pairs on sulfur.

H2S has 6 valence electrons; the Lewis structure shows sulfur in the center with two single bonds to hydrogen and one lone pair on sulfur.

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Verified step by step guidance

Determine the total number of valence electrons in H2S by adding the valence electrons of each atom: hydrogen has 1 valence electron each, and sulfur has 6 valence electrons. Use the formula: $\text{Total valence electrons} = 2 \times 1 + 6$.

Draw the skeletal structure of H2S with sulfur as the central atom bonded to two hydrogen atoms using single bonds. Each single bond represents 2 electrons.

Subtract the electrons used in bonding from the total valence electrons to find the number of remaining electrons to be placed as lone pairs on sulfur.

Place the remaining electrons as lone pairs on the sulfur atom to complete its octet, ensuring sulfur has 8 electrons around it (including bonding and lone pairs).

Verify that all atoms have a complete valence shell: hydrogen atoms should have 2 electrons each (duet rule), and sulfur should have 8 electrons (octet rule). Confirm that the Lewis structure matches these criteria.