light associated with transitions between energy levels An electronic transition occurs from n = 5 to n = 2 in a hydrogen atom. What is the wavelength and frequency of light associated with this transition? %3D

light associated with transitions between energy levels An electronic transition occurs from n = 5 to n = 2 in a hydrogen atom. What is the wavelength and frequency of light associated with this transition? %3D

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter7: Atomic Structure And Periodicity

Section: Chapter Questions

Problem 175CP: The figure below represents part of the emission spectrum for a one-electron ion in lhe gas phase....

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The energy needed to ionize an atom of element X when it is in its most stable state is 500kJmol1 . However, if an atom of X is in its lowest excited state, only 120kJmol1 is needed to ionize it. What is the wavelength of the radiation emitted when an atom of X undergoes a transition from the lowest excited state to the ground state?
6.105 When we say that the existence of atomic spectra tells us that atoms have specific energy levels, are we using deductive or inductive reasoning?
Why was Schrodinger not able to describe exactly the pathway an electron takes as it moves through the space of an atom?
What does it mean to say that the energy of the electrons in an atom is quantized?
6.23 Describe how the Bohr model of the atom accounts for the spectrum of the hydrogen atom.
One bit of evidence that the quantum mechanical model is correct lies in the magnetic properties of matter. Atoms with unpaired electrons are attracted by magnetic fields and thus are said to exhibit pararamagnetism. The degree to which this effect is observed is directly related to the number of unpaired electrons present in the atom. Consider the ground-state electron configurations for Li, N, Ni, Te, Ba, and Hg. Which of these atoms would be expected to be paramagnetic, and how many unpaired electrons are present in each paramagnetic atom?
6.106 When Bohr devised his model for the atom, was he using deductive or inductive reasoning? Explain your answer.
Consider the bright line spectrum of hydrogen shown in Fig. 11.10 . Which line in the spectrum represents photons with the highest energy? With the lowest energy?
According to a relationship developed by Niels Bohr, for an atom or ion that has a single electron, the total energy, En, of an electron in a stable orbit of quantum number n is En = [Z2/n2] (2.179 1018 J) where Z is the atomic number. Calculate the ionization energy for the electron in a ground-state He+ ion.
(a) Give the complete electron configuration (1s22s22p) of aluminum in the ground state. (b) The wavelength of the radiation emitted when the outermost electron of aluminum falls from the 4s state to the ground state is about 395 nm. Calculate the energy separation (in joules) between these two states in the Al atom. (c) When the outermost electron in aluminum falls from the 3d state to the ground state, the radiation emitted has a wavelength of about 310 nm. Draw an energylevel diagram of the states and transitions discussed here and in (b). Calculate the separation (in joules) between the 3d and 4s states in aluminum. Indicate clearly which has higher energy.
Heated lithium atoms emit photons of light with an energy of 2.9611019 J. Calculate the frequency and wavelength of one of these photons. What is the total energy in 1 mole of these photons? What is the color of the emitted light?
6.11 Define the term photon.