Enter your answer in the provided box. Consider the following energy levels of a hypothetical atom:...
Consider the following energy levels of a hypothetical atom: E4 -1.41 x 10-19 J Ez-5.01 x 10-19 J E2 -1.15 x 10-18 J E1 -1.75 x 10-18 (a) What is the wavelength of the photon needed to excite an electron from Ey to E4? *10 m (b) What is the energy in joules) a photon must have in order to excite an electron from E, to Ez? *10 J (c) When an electron drops from the Ez level to the...
Be sure to answer all parts. Consider the following energy levels of a hypothetical atom: E4 −2.11 × 10−19 J E3 −5.61 × 10−19 J E2 −1.05 × 10−18 J E1 −1.85 × 10−18 J (a) What is the wavelength of the photon needed to excite an electron from E1 to E4? × 10 m (b) What is the energy (in joules) a photon must have in order to excite an electron from E2 to E3? × 10 J (c)...
Consider the following energy levels of a hypothetical atom: E4 −2.21 × 10−19 J E3 −6.41 × 10−19 J E2 −1.15 × 10−18 J E1 −1.65 × 10−18 J (a) What is the wavelength of the photon needed to excite an electron from E1 to E4? × 10 m (b) What is the energy (in joules) a photon must have in order to excite an electron from E2 to E3? × 10 J (c) When an electron drops from the...
please answer quesiton 1,1a,1b 1. Consider the following energy levels of a hypothetical atom: E -1.0 x 10-19 -5.0 x 10-19 _-10 x 10-19 _-15 x 10-19 a. What is the wavelength of the photon needed to excite an electron from E, to Ex? (Use the Energies given in the problem) b. When an electron drops from the E3 to the E, level, the atom is said to undergo emission. Calculate the wavelength of the photon emitted in this process.
Enter your answer in the provided box. How much more energy per photon is there in green light of wavelength 536 nm than in red light of wavelength 622 nm? __× 10 __ J (Enter your answer in scientific notation.)
37 3 attempts left Check my work points Be sure to answer all parts. Enter your answers in scientific notation. The following values are the only allowable energy levels of a hypothetical one-electron atom: E = -2.0 * 10-19 Ex = -7.0 * 10-19 eBook E4--11.0*10-13 Print References E, --15.0 x 10-19 E, --17.0 10-19 E; --20.0 x 10-19, () Ir the electron were in the level, what would be the highest frequency (and minimum wavelength) of radiation that could...
Enter your answer in the provided box. What is the wavelength (in nanometers) of a photon emitted during a transition from n = 7 to ne=3 state in the H atom? x 10
A H atom emitts a photon with a wavelength of 6.57 × 102 nm. If the energy of the initial state of the H atom was -2.42 × 10(-19) J, calculate the energy of the final state. Express answer in scientific notation.
6. The first ionization energy of Au (IE1) is 890.1 kJ/mol. Is light with a wavelength of 225 nm capable of ionizing a gold atom in the gas phase? Justify your answer with a calculation. 7. The energy of an electron in a hydrogen atom is -4.45 x 100 J. What energy level (n) does it occupy? Is there another valid energy level at -2.69 x 1020 ? If so, what is this other energy level? 8. What is the...
6. The first ionization energy of Au (IE1) is 890.1 kJ/mol. Is light with a wavelength of 225 nm capable of ionizing a gold atom in the gas phase? Justify your answer with a calculation. 7. The energy of an electron in a hydrogen atom is -4.45 x 100 J. What energy level (n) does it occupy? Is there another valid energy level at -2.69 x 1020 ? If so, what is this other energy level? 8. What is the...