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 51m
7. Gases3h 49m
8. Thermochemistry2h 35m
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 34m
22. Organic Chemistry5h 7m
23. Chemistry of the Nonmetals2h 39m
24. Transition Metals and Coordination Compounds3h 16m

9. Quantum Mechanics

Electromagnetic Spectrum

General Chemistry

9. Quantum Mechanics

Electromagnetic Spectrum

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Multiple Choice

Which of the following sources of electromagnetic radiation will have the highest frequency?

Visible Light (λ = 595 nm)

Visible Light (ΔE = 4.39 x 10^-19 J)

Visible Light (λ = 690 nm)

Visible Light (ν = 4.11 x 10¹⁵ s^-1)

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Verified step by step guidance

Understand that frequency (ν) and wavelength (λ) are related by the equation: c = λν, where c is the speed of light (approximately 3.00 x 10^8 m/s).

Convert the given wavelengths from nanometers to meters by using the conversion factor: 1 nm = 1 x 10^-9 m.

For the first option (λ = 595 nm), convert the wavelength to meters and use the equation c = λν to solve for frequency (ν).

For the second option (ΔE = 4.39 x 10^-19 J), use the equation ΔE = hν, where h is Planck's constant (6.626 x 10^-34 J·s), to solve for frequency (ν).

For the third option (λ = 690 nm), convert the wavelength to meters and use the equation c = λν to solve for frequency (ν). Compare the calculated frequencies to determine which source has the highest frequency.