A hydrogen atom in the ground state absorbs 13.6 eV of energy. What change does the energy cause to the atom\'s structure? Let Planck's constant h = 4.136 x 10 eV s, the speed of light %3D c = 3.00 x 10° m/s, and the Rydberg constant R= 1.097 × 10' m. O The atom is completely ionized O The electron transitions to the n 2 state. O The electron transitions to the n= 5 state. O The electron is captured by the nucleus.

An electron characterized by energy level 1 (n=1)  for the hydrogen atom has an energy of E = – 2.18 x 10–18 J. Which of the following is the energy associated with an electron characterized by energy level 4 ( n=4) of the hydrogen atom?

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The threshold frequency vo describes the smallest light frequency capable of ejecting electrons from a metal. Determine the minimum energy Eo of a photon capable of ejecting electrons from a metal with vo = 2.66 x 10¹4 s-¹. Eo = What is the maximum kinetic energy KEclection of electrons ejected from this metal by light with a wavelength of 255 nm? KEclectron =

Using the Rydberg equation for hydrogen (equation 3.8 in your textbook), what is the energy of the electromagnetic radiation released when an electron in hydrogen starts in the n = 6 excited state and falls to the n = 1 final ground state?

For the hydrogen atom, which statement is true   The transition from n = 5 to n = 3 involves greater energy than one from n = 4 to n = 2   A transition from n = 2 to some large value of n corresponds to the ionization energy of the H atom   The transition from n = 4 to n = 2 emits radiation of longer wavelength than the transition from n = 5 to n = 1   All transitions from states for which n > 1 to the n = 1 state involve the absorption of energy by the atom

The energy E of the electron in a hydrogen atom can be calculated from the Bohr formula: E=-Ry/n2 In this equation Ry stands for the Rydberg energy, and n stands for the principal quantum number of the orbital that holds the electron.  Calculate the wavelength of the line in the absorption line spectrum of hydrogen caused by the transition of the electron from an orbital with n=5 to an orbital with n=9.

What is the wavelength of light that has a frequency of 7.155 x 1014 s-1? Note that - 1 nm = 1 x 10-9 m Note: In problems dealing with frequencies, wavelengths, photon energies, or electron transitons in hydrogen atoms, you may need some of the following equations: 1 v = c where c = 2.99792458 x 108 m s1 Ep = h v where h = 6.6260755 x 1034 J s En = -RH / n2 where RH 2.1798741 x 10-18 j %3D

The electron in an (unbound) hydrogen atom (H(g)) is excited from the ground state to the n=3 state.Which of the following statements are true and which are false. 1. it takes less energy to ionize the electron from n=3 than it does from the ground state.2. The wavelength of the light emitted when the electron returns to the ground state from n=3 is the same as the wavelength of light absorbed to go from n=1 to n=3.3. the electron is farther from the nucleus on average in the n=3 state than in the ground state.4. The first excited state corresponds to n=3.5. The wavelength of light emitted when the electron drops from n=3 to n=2 is shorter than the wavelength of light emitted if the electron falls from n=3 to n=1.

A hydrogen atom absorbs a photon with a wavelength of 1094 nm and causes an electron to make a transition from an unknown n1 to a final n2 = 6.   Part A Calculate frequency of the absorbed photon in units of s-1.       Part B Calculate the energy change in the atom (ΔEatom in J) upon absorption of the photon.     Part C Calculate the value of n1