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

Calculate the wavelength of the light emitted when an electron in a hydrogen atom makes the transition from n=4 to n=2 using the Bohr equation.

656 nm

486 nm

486.1 nm

410 nm

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Verified step by step guidance

Start by understanding the Bohr model, which describes the electron transitions in a hydrogen atom. The energy difference between two levels can be calculated using the formula:

E = R (\frac{1}{n^{2}} - \frac{1}{m^{2}})

, where

R

is the Rydberg constant,

n

and

m

are the principal quantum numbers of the initial and final states.

Identify the initial and final energy levels for the transition. In this problem, the electron transitions from

n = 4

n = 2

Calculate the energy difference using the Bohr equation:

E = R (\frac{1}{2^{2}} - \frac{1}{4^{2}})

. Substitute the values for

R

and the quantum numbers.

Convert the energy difference to wavelength using the equation:

E = \frac{hc}{λ}

, where

h

is Planck's constant,

c

is the speed of light, and

λ

is the wavelength. Rearrange to solve for

λ

λ = \frac{hc}{E}

Substitute the calculated energy difference and constants into the wavelength equation to find the wavelength of the emitted light. This will give you the wavelength in nanometers, which corresponds to one of the given options.