We’re being asked to determine which transition represents the emission of a photon with the highest energy.
Which electronic transition in a hydrogen atom would emit the highest energy photon?
The transition that represents the emission of a photon with the highest frequency is n = 3 → n = 1.
Which of the following electronic transitions of hydrogen has the highest largest frequency?
The transition with the greatest distance is 5p → 1s, which is n = 5 going to n = 1. This means this transition also has the largest energy and frequency. The answer is d. 5p → 1s.
Which electron transition emits energy of the longest wavelength?
Longest wavelength goes with lowest energy: Thus transition between n = 1 and n = 2 corresponds to the longest wavelength. Likewise, the transition between n = 1 and n = 4 (highest energy) corresponds to the shortest wavelength. 9.
Which of the following electronic transitions of hydrogen has the highest largest frequency and thus releases the largest amount of energy?
Which of the following transition has highest frequency?
Therefore n=2 to n=1 transition produces highest frequency.
Which transition in the hydrogen atom has the longest wavelength?
The red light has the longest wavelength, lowest energy, and lowest frequency.
Which of the following transitions in the hydrogen atom emits the least energy?
Complete answer: The lowest energy is for n=4 to n=3 transition.
Which of the following transition in a hydrogen atom emits the photon of highest frequency?
i.e., Photon of higher frequency will be emitted if transition takes place from n=2 to 1.
Which of the following transition gives the highest frequency for electron emission?
Which of the following transitions give the highest frequency for electron emission? Lower the value of the lower quantum number to which electron is jumping, higher will be the frequency. Therefore n=2 to n=1 transition produces highest frequency.
Which of the following transition in hydrogen atom emits photon of lowest frequency?
(i) n = 2 to n = 1. (ii) n = 4 to n = 3. As n increases, the energy levels gradually gets more closer. And, as a result hydrogen atom emits photon of lowest frequency in the transition.
Which of the following transition will have highest emission frequency?
Explanation: To obtain emission frequency the e lectron must transit from higher to lower energy level. Hence, transitions from n = 1 to n = 3 and n = 2 to n = 5 does not contribute to emission of radiations. Hence, for transition from n = 2 to n = 1 the frequency emitted will be highest.
What is the energy change during the transition of an electron?
Transition of an Electron and Spectral Lines. The energy change during the transition of an electron from n = n1 to n = n2 is ΔE = E2 −E1 = 13.6× ( 1 n2 1 − 1 n2 2) eV. () Obviously, a positive energy change means that the electron absorbs energy, while a negative energy change implies a release of energy from the electron.
What is the potential energy of an electron in EV?
Bohr modeled the potential energy of an electron at the n -th principal energy level of a hydrogen atom with the equation where k = 13.6 ⋅ eV, which is numerically equal to the energy required to move an electron from the principal energy level n = 1 of a hydrogen atom to an infinite separation from the nucleus.
Why is the wavelength of light emitted from a hydrogen atom quantized?
Since the energy level of the electron of a hydrogen atom is quantized instead of continuous, the spectrum of the lights emitted by the electron via transition is also quantized. In other words, the wavelength are integers.
What is the energy of the electron of a monoelectronic atom?
The energy of the electron of a monoelectronic atom depends only on which shell the electron orbits in. The energy level of the electron of a hydrogen atom is given by the following formula, where n n n denotes the principal quantum number: E n = − 1312 n 2 kJ/mol. E_n=-\\frac{1312}{n^2}\ext{ kJ/mol}. E n = − n 2 1 3 1 2 kJ/mol.
