1) Calculate the energy change corresponding to the excitation of an electron from the n=1 to n=3 electronic state in the hydrogen atom.
2) Calculate the wavelength of electromagnetic radiation associated with the energy change above.
As we know
E = hcR*(1/n1^2 - 1/n2^2)
= (6.626*10^-34*3*10^8*10973731.6)*(1 - 1/9)
= 1.9389*10^-18 J
Wavelength = hc/Energy
= (6.626*10^-34*3*10^8)/(1.9389*10^-18)
= 1.025*10^-7 m
calculate the energy change corresponding to the excitation of an electron from the n=1 to n=3 electronic state in the hydrogen atom.
Calculate the energy of a photon required to excite a hydrogen
atom from the n = 1 state to the n = 2 state.
10. [1pt] Calculate the energy of a photon required to excite a hydrogen atom from the - 1 state to the n - 2 state, Answer: Submit All Answers 11. [1pt] An electron in a hydrogen atom falls to an energy level n = 2. If the wavelength of the emitted electromagnetic radiation is 4.86x10m, what...
11. For the electronic transition from n 3 to n 5 in the hydrogen atom, calculate the energy wavelength (in nm). 12. Calculate the energy of a photon of frequency 5.20x1o' s1.
11. For the electronic transition from n 3 to n 5 in the hydrogen atom, calculate the energy wavelength (in nm). 12. Calculate the energy of a photon of frequency 5.20x1o' s1.
The electron from a hydrogen atom drops from an excited state into the ground state. When an electron drops into a lower-energy orbital, energy is released in the form of electromagnetic radiation. How much energy does the electron have initially in the n=4 excited state?
a) A hydrogen atom undergoes an electronic transition from the n = 4 to the n-2 state. In the process the H atom emits a photon. This photon then strikes a cesium metal surface and ejects an electron. The binding energy for cesium is 3.23 x 10-19 Calculate a) the wavelength of the emitted photon; and b) the energy of the ejected electron.
For an electron in the n - 1 state of the hydrogen atom, calculate the total energy of the electron. (Express your answer to four significant figures.) times 10^-18J For an electron in the n - 1 state of the hydrogen atom, calculate the speed of the electron. (Express your answer to four significant figures.) times 10^6m/s For an electron in the n - 4 state of the hydrogen atom, calculate the angular moment. (Express your answer to four significant...
1. Finally, calculate the energy in kJ/mol corresponding to the removal of an electron from a hydrogen atom originally in the ground state (i.e., from n=1 to n=∞). Show all your work.
4. Calculate the energy, in kJ/mole associated with an electronic transition in a hydrogen atom from n = 3 to n = 1 orbitals. 18X10 Vom 5. Calculate the frequency and wavelength of a photon emitted in the n = 3 to n= 1 transition considered in question 4 un?
An electron in the Hydrogen atom is in the excited state with energy E2. a) According to the Bohr model, what is the radius of the atom in this state, in Angstroms? b) What is the wavelength le of the electron, in Angstroms? c) What is the momentum of the electron, in kg-m/s ? d) This atom decays from the excited state with energy E2 to the ground state with energy E1 . What is the energy of the emitted photon?...
For an electron transition in a hydrogen atom from n=1 to n=3, calculate the wavelength of this radiation. (Useful information: Rh=2.18x10^-18 J; h=6.63x10^-34 J-s; c=3.00x10^8 m/s)
Consider an electron transition from n 5 to n =3 of a hydrogen atom. 5. Use Bohr's H model to calculate the energy required to for this electron transition. Will the hydrogen atom absorb or emit energy during this transition? a) What wavelength of light will the hydrogen atom absorb or emit in this electron transition? b) A rifle bullet (mass-4.20 g) has a velocity of 2160 mph. What is the wavelength associated with this bullet? (1 km 0.62137 mil)...