Math Problem Statement
Calculate the maximum wavelength of light capable of removing an electron for a hydrogen atom from the energy state characterized by n = 1, by n = 2.
Solution
To determine the maximum wavelength of light capable of removing an electron from a hydrogen atom from a given energy state, we need to calculate the energy required to ionize the electron from that state and then relate it to the wavelength using the relationship between energy and wavelength.
Step 1: Calculate the ionization energy for each state
The energy of an electron in a hydrogen atom at a particular energy level is given by the formula:
where:
- is the energy of the electron at level .
- is the ionization energy from the ground state (n = 1).
For :
The energy required to ionize the electron from (i.e., to remove it from the atom) is .
For :
The energy required to ionize the electron from is .
Step 2: Convert the energy to wavelength
The energy of a photon is related to its wavelength by the equation:
where:
- is the energy of the photon (in joules),
- is Planck's constant (),
- is the speed of light in a vacuum (),
- is the wavelength of the photon (in meters).
We need to convert the energy from electron volts (eV) to joules. The conversion factor is:
So:
For :
For :
Final Answers:
- For : The maximum wavelength is approximately 91.2 nm.
- For : The maximum wavelength is approximately 364.7 nm.
These wavelengths correspond to the ultraviolet region of the electromagnetic spectrum.
Would you like more details on any part of this process, or do you have any further questions?
Related Questions:
- What is the significance of the Rydberg constant in these calculations?
- How does the ionization energy change for higher energy levels (n > 2)?
- What is the relationship between energy levels and the emission spectrum of hydrogen?
- How can we calculate the wavelength for transitions between two energy levels?
- What are the practical applications of knowing the ionization energies for different elements?
Tip:
Remember that shorter wavelengths correspond to higher energy photons, which are capable of ionizing atoms more effectively.
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Math Problem Analysis
Mathematical Concepts
Quantum Physics
Photon Energy
Ionization Energy
Wavelength-Energy Relationship
Formulas
E_n = -13.6 eV / n^2
E = hc / λ
1 eV = 1.602 x 10^-19 J
Theorems
Bohr's Model of the Atom
Energy-Wavelength Relationship
Suitable Grade Level
College/University
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