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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?
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?
- Blue (correct)
- Orange
- Red
- Green (correct)
- Indigo (correct)
- Yellow
- Violet (correct)
Classify these electron transitions by whether they result in the absorption or emission of light:
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)?
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?
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?
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?
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?
What is the energy of an electron in a hydrogen atom in the ground state?
What is the energy of an electron in a hydrogen atom in the ground state?
What is the energy of the electron in the n=3 level of an excited-state hydrogen atom?
What is the energy of the electron in the n=3 level of an excited-state hydrogen atom?
What information is needed to determine the energy of an electron in a many-electron atom? (Select all that apply)
What information is needed to determine the energy of an electron in a many-electron atom? (Select all that apply)
What information is most important in determining the size of an orbital?
What information is most important in determining the size of an orbital?
What information is needed to determine the orientation of an orbital?
What information is needed to determine the orientation of an orbital?
What information is needed to determine the general shape of an orbital?
What information is needed to determine the general shape of an orbital?
What quantum numbers specify these subshells?
What quantum numbers specify these subshells?
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.
