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Questions and Answers
What does the variable 'n' represent in the equation $E_n = -2.18 \times 10^{-18} J (\frac{1}{n^2})$?
What does the variable 'n' represent in the equation $E_n = -2.18 \times 10^{-18} J (\frac{1}{n^2})$?
- The energy of the electron
- The number of electrons
- The ionization energy
- The principal quantum number (correct)
How does the energy of an electron change as 'n' increases in the Bohr model?
How does the energy of an electron change as 'n' increases in the Bohr model?
- The energy increases
- The energy becomes more positive (correct)
- The energy remains constant
- The energy decreases
What is true about the wavelength of light emitted during an electronic transition in a one-electron atom?
What is true about the wavelength of light emitted during an electronic transition in a one-electron atom?
- It remains constant regardless of the transition
- It is inversely proportional to the energy change (correct)
- It is irrelevant in electronic transitions
- It is directly proportional to the energy change
If an electron transitions from n=3 to n=2, what happens to its energy?
If an electron transitions from n=3 to n=2, what happens to its energy?
In the equation $E_n = -2.18 \times 10^{-18} J (\frac{1}{n^2})$, what does the negative sign signify?
In the equation $E_n = -2.18 \times 10^{-18} J (\frac{1}{n^2})$, what does the negative sign signify?
Flashcards
Bohr Model
Bohr Model
A planetary model of the atom showing electron orbits.
Energy Equation
Energy Equation
Formula for electron energy: E_n = -2.18 × 10^-18 J (1/n^2).
Electron Energy Calculation
Electron Energy Calculation
Determine electron energy using the Bohr model's equation.
Energy Change
Energy Change
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Wavelength of Light
Wavelength of Light
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Study Notes
Bohr Model
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The Bohr model describes the electron's orbit around the nucleus of an atom.
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Electrons orbit the nucleus in specific, stable energy levels (quantized).
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Energy levels are indexed by the principal quantum number, n (n=1, 2, 3...).
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As n increases, the electron's energy and distance from the nucleus increase.
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The electron's energy is quantized and calculated using the equation:
𝐸n=−2.18×10−18J(1𝑛2) where n is the principal quantum number.
Electron Energy Calculation
- Electron energy depends directly on the principal quantum number (n).
- As n increases, the electron energy becomes less negative, and moves away from the nucleus (higher energy state).
- When n=1, the electron is in its lowest energy state (ground state).
- The ground state energy of the atom is a negative value.
Electronic Transitions
- Electrons can jump between energy levels by absorbing or emitting photons (light) of specific energy.
- The energy difference between energy levels corresponds to the energy of the absorbed or emitted photon.
- The Δ𝐸 represents the energy change during the transition: Δ𝐸 = 𝐸final - 𝐸initial
Energy Change Calculation
- The energy change during a transition between two energy levels (ninitial and nfinal) is calculated using: Δ𝐸 = 𝐸nfinal - 𝐸ninitial = −2.18×10−18 J [(1/nfinal2) − (1/ninitial2)]
Wavelength Calculation
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If the energy change (Δ𝐸) of a transition is known, the wavelength of the emitted or absorbed photon can be calculated using the equation:
Δ𝐸 = h𝑐/𝜆
where:
- Δ𝐸 is the energy change
- h is Planck's constant (6.626 x 10-34 J•s)
- 𝑐 is the speed of light (3.00 x 108 m/s)
- 𝜆 is the wavelength.
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