Ch.6 - Electronic Structure of Atoms

Brown - Chemistry: The Central Science 15th Edition

Brown15th EditionChemistry: The Central ScienceISBN: 9780137542970Non è quello che usi tu?Cambia libro di testo

Brown 15th Edition

Ch.6 - Electronic Structure of Atoms

Problema 38a

Capitolo 6, Problema 38a

Indicate whether energy is emitted or absorbed when the following electronic transitions occur in hydrogen: a. from n = 3 to n = 6

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insert step 1> Determine the initial and final energy levels of the electron in the hydrogen atom. Here, the electron transitions from n = 3 to n = 6.

insert step 2> Recall that energy is absorbed when an electron moves to a higher energy level (higher n value) and emitted when it moves to a lower energy level (lower n value).

insert step 3> Since the electron is moving from n = 3 to n = 6, it is transitioning to a higher energy level.

insert step 4> Conclude that energy is absorbed during this transition because the electron is moving to a higher energy level.

insert step 5> Remember that the energy difference between levels can be calculated using the Rydberg formula if needed, but the key concept here is the direction of the transition.

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Energy Levels in Hydrogen

In hydrogen, electrons occupy discrete energy levels, denoted by quantum numbers (n). The energy associated with each level increases with n, meaning that higher levels (larger n) have more energy. When an electron transitions between these levels, the difference in energy determines whether energy is absorbed or emitted.

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Hydrogenation Reactions

Absorption and Emission of Energy

When an electron moves from a lower energy level to a higher one (e.g., n = 3 to n = 6), it must absorb energy, typically in the form of a photon. Conversely, when an electron falls from a higher energy level to a lower one, energy is emitted. This principle is fundamental in understanding atomic spectra and the behavior of electrons in atoms.

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Emission Spectra

Quantum Mechanics and Photons

Quantum mechanics describes the behavior of particles at atomic and subatomic levels. Photons are the quanta of light and carry energy proportional to their frequency. The energy of a photon can be calculated using the equation E = hf, where h is Planck's constant and f is the frequency. This relationship is crucial for understanding how energy is exchanged during electronic transitions.

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Introduction to Quantum Mechanics

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