Ch.7 - Quantum MechanicsSee all chapters

Sections | |||
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Wavelength and Frequency | 18 mins | 0 completed | Learn |

Diffraction vs Refraction | 5 mins | 0 completed | Learn |

The Particle Nature of Light | 10 mins | 0 completed | Learn |

Photoelectric Effect | 4 mins | 0 completed | Learn Summary |

De Broglie Wavelength | 8 mins | 0 completed | Learn |

Heisenberg Uncertainty Principle | 10 mins | 0 completed | Learn |

Bohr Model | 23 mins | 0 completed | Learn |

Introduction to Quantum Mechanics | 28 mins | 0 completed | Learn Summary |

End of Chapter 7 Problems | 49 mins | 0 completed | Learn |

Additional Practice |
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Electromagnetic Spectrum |

Bohr and Balmer Equations |

Wave Function |

Dimensional Boxes |

Solution: It is possible to determine the ionization energy for hydrogen using the Bohr equation. Calculate the ionization energy (in kJ) for a mole of hydrogen atoms, making the assumption that ionization is the transition from n = 1 to n = ∞.
A. 7.62 x 103 kJ
B. 2.76 x 103 kJ
C. 1.31 x 103 kJ
D. 3.62 x 103 kJ
E. 5.33 x 103 kJ

It is possible to determine the ionization energy for hydrogen using the Bohr equation. Calculate the ionization energy (in kJ) for a mole of hydrogen atoms, making the assumption that ionization is the transition from n = 1 to n = ∞.

A. 7.62 x 10^{3} kJ

B. 2.76 x 10^{3} kJ

C. 1.31 x 10^{3} kJ

D. 3.62 x 10^{3} kJ

E. 5.33 x 10^{3} kJ

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A ground-state H atom absorbs a photon of waveleng...

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Calculate the wavelength of light emitted when the...

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