Textbook Question
Which combinations of n and l represent real orbitals, and which do not exist? a. 1s b. 2p c. 4s d. 2d
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Ch.7 - Quantum-Mechanical Model of the Atom
Chapter 7, Problem 65
An electron in a hydrogen atom is excited with electrical energy to an excited state with n = 2. The atom then emits a photon. What is the value of n for the electron after the emission?
Verified step by step guidance1
Identify the initial excited state of the electron, which is given as n = 2.
Understand that when an electron emits a photon, it transitions to a lower energy level.
Recall that the lowest energy level for a hydrogen atom is n = 1, which is the ground state.
Since the electron is initially at n = 2 and emits a photon, it will transition to the next lower energy level.
Conclude that the value of n for the electron after the emission is n = 1.
Related Practice
Textbook Question
Sketch the 1s and 2p orbitals. How do the 2s and 3p orbitals differ from the 1s and 2p orbitals?
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Textbook Question
Sketch the 3d orbitals. How do the 4d orbitals differ from the 3d orbitals?
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Textbook Question
Determine whether each transition in the hydrogen atom corresponds to absorption or emission of energy. a. n = 3 → n = 1 b. n = 2 → n = 4 c. n = 4 → n = 3
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Open Question
According to the quantum-mechanical model for the hydrogen atom, which electron transition produces light with the longer wavelength: 2p to 1s or 3p to 1s?
Textbook Question
According to the quantum-mechanical model for the hydrogen atom, which electron transition produces light with the longer wavelength: 3p → 2s or 4p → 3p?
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