Calculate the radius of second Bohr orbit in hydrogen atom from the given data. Mass of electron = 9.1 × 10 " kg %3D Charge on the electron = 1.6 × 101º C %3D Plank's constant = 6.63 × 10" J.S. Permitivity of free space = 8.85 x 1012 C²/Nm²
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- O 36 Sulfur (S) has an atomic number of 16. What is its electron configuration? O 1s 2s 2p°3s-3p O 1s°25-2p°3s°3p O 1s252p 3s²3d* O 1s°252p°3s²3p²(c) Consider the semi-classical model for a two-electron atom illustrated in the diagram below. This model attempts to extend the Bohr model to a two-electron system by assuming both electrons follow a circular orbit around the nucleus while remaining diametrically opposite to each other. electron nucleus, electron (i) Carefully explain why, for the ground state of helium, this semi-classical model predicts that both electrons would experience an effective nuclear charge Zeff %3D (ii) Assuming that each electron's angular momentum is quantized in the same manner as the usual Bohr model for single-electron atoms, calculate the total binding energy of the ground state of helium according to this semi classical model.Consider a hydrogen atom in its 1s state (ground state) and assume (for simplicity) that the electron and the proton are separated by a constant distance a, = 5.292 × 10–1'm (called the Bohr radius). (a) Calculate the gravitational force between these two charges. (use: Fg = G"m2) (b) Calculate the electric force between these two charges. (use: Fe = k«l&i[IQzl) (c) Calculate the ratio of these two forces to appreciate the strength of the electric force in comparison to the gravitational force.
- An electron is excited from the n=1 ground state to the n=3 state in a hydrogen atom. Which of the following statements are true? Correct the false statements to make them true. (It may help to draw the Bohr model of the atom with the corresponding electron orbits.)a. It takes more energy to ionize (completely remove) the electron from n = 3 than from the ground state.b. The electron is farther from the nucleus on average in the n = 3 state than in the n = 1 state.c. The wavelength of light emitted if the electron drops from n = 3 to n = 2 will be shorter than the wavelength of light emitted if the electron falls from n = 3 to n = 1.d. The wavelength of light emitted when the electron returns to the ground state from n = 3 will be the same as the wavelength of light absorbed to go from n = 1 to n = 3.e. For n = 3, the electron is in the first excited state.In the picture are two diagrams of the first five orbits in the Bohr model labeled A - E. The dot in an orbit is the electron. The nucleus is not shown. Shown is a BEFORE and AFTER state of the atom. An energy level diagram for the Bohr hydrogen atom is shown. Which of these events has occurred in going from the BEFORE to the AFTER state? a. a photon of energy 0.97 eV has been emitted b. a photon of energy 1.51 eV has been absorbed c. a photon of energy 1.51 eV has been emitted d. an electron of energy 1.51 eV has been emitted e. a photon of energy 0.97 eV has been absorbedWhat wavelength of light is emitted by a hydrogen atom in which an electron makes a transition from the n = 5 to the n = 2 state? Enter this wavelength expressed in nanometers to one decimal place. 1 nm = 1 x 10-9 m Assume the Bohr model.
- The Balmer series in hydrogen includes the Paschen series. has four lines in the ultraviolet. O includes both the Paschen series and the Lyman series. O has four lines in the visible. O includes the Lyman series.Which of the following would be closer to the nucleus? a. The ground state (n = 1) of an electron in a singly-charged helium atom. That is, a helium atom with only one electron instead of two. b. Both of these are the same distance from the nucleus c. The ground state electron for the hydrogen.What wavelength of light is emitted by a hydrogen atom in which an electron makes a transition from the n = 8 to the n = 5 state? Enter this wavelength expressed in nanometers. 1 nm = 1 x 10-9 m Assume the Bohr model.