Ch.6 - Electronic Structure of Atoms

Brown - Chemistry: The Central Science 15th Edition

Brown15th EditionChemistry: The Central ScienceISBN: 9780137542970당신이 사용하는 게 아니라요?교과서 변경

Brown 15th Edition

Ch.6 - Electronic Structure of Atoms

문제 40b2

6장, 문제 40b2

Consider a transition of the electron in the hydrogen atom from n = 4 to n = 9. b. Will the light be absorbed or emitted?

검증된 단계별 안내

insert step 1> Determine the initial and final energy levels of the electron transition. Here, the electron is transitioning from n = 4 (initial) to n = 9 (final).

insert step 2> Understand that when an electron moves to a higher energy level (from a lower n to a higher n), it absorbs energy. Conversely, when it moves to a lower energy level, it emits energy.

insert step 3> Since the electron is moving from n = 4 to n = 9, it is transitioning to a higher energy level.

insert step 4> Conclude that the electron must absorb energy to make this transition.

insert step 5> Therefore, light will be absorbed during this transition.

비슷한 문제에 대한 검증된 영상 답변:

이 영상 해법은 위 문제에 도움이 된다고 튜터들이 추천한 것입니다.

영상 길이:

주요 개념

질문에 올바르게 답하기 위해 반드시 이해해야 하는 핵심 개념들은 다음과 같습니다.

Energy Levels in Atoms

In an atom, electrons occupy specific energy levels, denoted by quantum numbers (n). The energy associated with these levels increases with n, meaning that higher levels (like n=9) have more energy than lower levels (like n=4). When an electron transitions between these levels, it either absorbs or emits energy in the form of light.

Photon Absorption and Emission

When an electron moves from a lower energy level to a higher one, it absorbs a photon, which provides the necessary energy for the transition. Conversely, when an electron falls from a higher energy level to a lower one, it emits a photon. The direction of energy transfer determines whether light is absorbed or emitted during the transition.

Wavelength and Energy Relationship

The energy of a photon is inversely related to its wavelength, described by the equation E = hc/λ, where E is energy, h is Planck's constant, c is the speed of light, and λ is the wavelength. A transition from a lower to a higher energy level (n=4 to n=9) indicates that energy is absorbed, resulting in a photon with a specific wavelength corresponding to that energy difference.

관련 실천

교과서 질문

The Lyman series of emission lines of the hydrogen atom are those for which nf = 1. (a) Determine the region of the electromagnetic spectrum in which the lines of the Lyman series are observed.

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교과서 질문

The visible emission lines observed by Balmer all involved nf = 2. (b) Calculate the wavelengths of the first three lines in the Balmer series—those for which ni = 3, 4, and 5—and identify these lines in the emission spectrum shown in Figure 6.11.

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교과서 질문

Is energy emitted or absorbed when the following electronic transitions occur in hydrogen? b. from an orbit of radius 2.12 Å to one of radius 8.46 Å

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교과서 질문

The visible emission lines observed by Balmer all involved nf = 2. (a) Which of the following is the best explanation of why the lines with nf = 3 are not observed in the visible portion of the spectrum: (i) Transitions to nf = 3 are not allowed to happen, (ii) transitions to nf = 3 emit photons in the infrared portion of the spectrum, (iii) transitions to nf = 3 emit photons in the ultraviolet portion of the spectrum, or (iv) transitions to nf = 3 emit photons that are at exactly the same wavelengths as those to nf = 2.

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교과서 질문

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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교과서 질문

a. Using Equation 6.5, calculate the energy of an electron in the hydrogen atom when n = 2 and when n = 6. Calculate the wavelength of the radiation released when an electron moves from n = 6 to n = 2.

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