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

9. Quantum Mechanics

Bohr Equation

General Chemistry

9. Quantum Mechanics

Bohr Equation

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Multiple Choice

Using the Bohr equation, calculate the wavelength (in nm) for the electron transition from n=4 to n=1 in the Lyman series.

410 nm

121 nm

97 nm

656 nm

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Verified step by step guidance

Understand the Bohr model: The Bohr model describes the electron transitions between energy levels in an atom. The energy difference between these levels can be used to calculate the wavelength of the emitted photon.

Identify the formula: The energy difference for an electron transition in the Bohr model is given by the formula:

- \frac{R_{H} (n^{2})}{n^{2}}

, where

R_{H}

is the Rydberg constant (approximately 2.18 x 10^-18 J), and

n

is the principal quantum number.

Calculate the energy difference: Use the formula to calculate the energy difference between the initial and final states (n=4 and n=1). The energy difference is given by:

- R_{H} (\frac{1}{n^{2}} - \frac{1}{n^{2}})

, where

n

is the initial and final quantum numbers.

Convert energy to wavelength: Use the equation

E = \frac{hc}{λ}

to convert the energy difference to wavelength, where

h

is Planck's constant (6.626 x 10^-34 J·s) and

c

is the speed of light (3.00 x 10^8 m/s). Rearrange the formula to solve for wavelength:

λ = \frac{hc}{E}

Convert the wavelength to nanometers: Since the problem asks for the wavelength in nanometers, convert the result from meters to nanometers by multiplying by 10^9 (1 m = 10^9 nm).