Questions and Answers
Which of the colors of visible light have enough energy to eject electrons from a metal with a threshold frequency of $5.45 imes 10^{14}$ Hz?
Classify these electron transitions by whether they result in the absorption or emission of light:
n=3 to n=2 = Emission n=3 to n=5 = Absorption n=1 to n=3 = Absorption n=2 to n=1 = Emission
Which transition is associated with the greatest energy change (ignoring sign)?
n=1 to n=3
When an electron in a hydrogen atom is in the n=3 state, is it on average closer to, farther from, or the same distance to the nucleus than in the ground state?
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Does it take more, less, or the same amount of energy to ionize a hydrogen atom in the n=3 state than one in the ground state?
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What is the energy of an electron in a hydrogen atom in the ground state?
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What is the energy of the electron in the n=3 level of an excited-state hydrogen atom?
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What information is needed to determine the energy of an electron in a many-electron atom? (Select all that apply)
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What information is most important in determining the size of an orbital?
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What information is needed to determine the orientation of an orbital?
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What information is needed to determine the general shape of an orbital?
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What quantum numbers specify these subshells?
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Study Notes
Threshold Frequency and Visible Light
- A metal foil has a threshold frequency of 5.45 × 10¹⁴ Hz.
- Colors of visible light that can eject electrons: green, blue, indigo, violet.
Electron Transitions in Hydrogen-like Atoms
- Transitions resulting in absorption: n=1 to n=3, n=3 to n=5.
- Transitions resulting in emission: n=3 to n=2, n=2 to n=1.
Energy Changes in Electron Transitions
- Greatest energy change occurs in the transition from n=1 to n=3.
- As energy levels increase, the energy difference between them decreases.
Electron Distance from Nucleus
- An electron in the n=3 state is farther from the nucleus compared to its ground state.
Ionization Energy of Hydrogen Atom
- It requires less energy to ionize a hydrogen atom in the n=3 state than in the ground state.
Energy of Electrons in Hydrogen Atom
- Energy of an electron in the ground state (n=1): -2.18 x 10⁻¹⁸ J.
- Energy of an electron in the excited state (n=3): -2.42 x 10⁻¹⁹ J.
Determining Energy in Many-Electron Atoms
- To determine the energy of an electron in a many-electron atom, the values of principal quantum number (n) and azimuthal quantum number (l) are necessary.
Orbital Size and Orientation
- The size of an orbital is primarily determined by the principal quantum number (n).
- The orientation of an orbital is specified by the magnetic quantum number (m sub l).
Orbital Shape Identification
- The shape of an orbital is determined by the azimuthal quantum number (l).
Quantum Numbers for Subshells
- For subshell 6s: n=6, l=0.
- For subshell 6p: n=6, l=1.
- For subshell 6d: n=6, l=2.
- Each subshell corresponds to different values of l:
- s (l=0)
- p (l=1)
- d (l=2)
- f (l=3)
- g (l=4)
- h (l=5)
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Description
This quiz contains flashcards based on Chapter 6 of the Sapling homework related to the properties of light and electron transitions in hydrogen-like atoms. Test your knowledge on threshold frequencies and the classification of electron transitions involving light absorption and emission.
