2. A pair of substances undergoes a change. This change is observed in the form of a difference in energy. Substance A falls from energy level M to energy level N and gives off infrared radiation. Substance B also undergoes a change and has energy that is given off and falls from energy level O to energy level P and gives off ultraviolet radiation. Which transition, from M to N or from O to P, has a greater energy difference? Explain your answer. Use a diagram of the electromagnetic spectrum if necessary. Answer: 10 16 10:14 Gamma rays 400 (violet) 10 12 AL 10 10 Xrays 500 10 UV Wavelength in meters (m) 10* 10 109 1 Visible ght IR 600 Wavelength in nanometers (nm) 1 10² 10" 10⁰ 10² 700 fredl Radio waves

2. A pair of substances undergoes a change. This change is observed in the form of a difference in energy. Substance A falls from energy level M to energy level N and gives off infrared radiation. Substance B also undergoes a change and has energy that is given off and falls from energy level O to energy level P and gives off ultraviolet radiation. Which transition, from M to N or from O to P, has a greater energy difference? Explain your answer. Use a diagram of the electromagnetic spectrum if necessary. Answer: 10 16 10:14 Gamma rays 400 (violet) 10 12 AL 10 10 Xrays 500 10 UV Wavelength in meters (m) 10* 10 109 1 Visible ght IR 600 Wavelength in nanometers (nm) 1 10² 10" 10⁰ 10² 700 fredl Radio waves

Chemistry

9th Edition

ISBN:9781133611097

Author:Steven S. Zumdahl

Publisher:Steven S. Zumdahl

Chapter7: Atomic Structure And Periodicity

Section: Chapter Questions

Problem 137AE: Photogray lenses incorporate small amounts of silver chloride in the glass of the lens. When light...

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Similar questions

Which of the following electron configurations correspond to an excited state? Identify the atoms and write the ground-state electron configuration where appropriate. a. 1s22s23p1 b. 1s22s22p6 c. 1s22s22p43s1 d. [Ar]4s23d54p1 How many unpaired electrons are present in each of these species?
What does wave-particle duality mean? What are its implications in our modem view of atomic structure?
Characterize the Bohr model of the atom. In the Bohr model, what do we mean when we say something is quantized? How does the Bohr model of the hydrogen atom explain the hydrogen emission spectrum? Why is the Bohr model fundamentally incorrect?
Which of the following statements is(are) true? a. The 2s orbital in the hydrogen atom is larger than the 3s orbital also in the hydrogen atom. b. The Bohr model of the hydrogen atom has been found to be incorrect. c. The hydrogen atom has quantized energy levels. d. An orbital is the same as a Bohr orbit. e. The third energy level has three sublevels, the s, p, and d sublevels.
Determine whether each statement that follows is true or false: a Electron energies are quantized in excited states but not in the ground state. b Line spectra of the elements are experimental evidence of the quantization of electron energies. c Energy is released as an electron passes from ground state to an excited state. d The energy of an electron may be between two quantized energy levels. e The Bohr model explanation of line spectra is still thought to be correct. f The quantum mechanical model of the atom describes orbitals in which electrons travel around the nucleus. g Orbitals are regions in which there is a high probability of finding an electron. h All energy sublevels have the same number of orbitals. i The 3p orbitals of an atom are larger than its 2p orbitals but smaller than its 4p orbitals. j At a given sublevel, the maximum number of d electrons is 5. k The halogens are found in Group 7A/17 of the periodic table. l The dot structure of the alkaline earths is X, where X is the symbol of element in the family. m Stable ions formed by alkaline earth metals are isoelectronic with noble gas atoms. n Atomic numbers 23 and 45 both belong to transition elements. o Atomic number 52, 35, and 18 are arranged in order of increasing atomic size. p Atomic number 7, 16, and 35 are all nonmetals.
Answer the following questions as a summary quiz on the chapter. (a) The quantum number n describes the ______ of an atomic orbital. (b) The shape of an atomic orbital is given by the quantum number _______. (c) A photon of green light has _______ (less or more) energy than a photon of orange light. (d) The maximum number of orbitals that may be associated with the set of quantum numbers n = 4 and = 3 is ________. (e) The maximum number of orbitals that may be associated with the quantum number set n = 3, = 2, and m = 2 is _______. (f) Label each of the following orbital pictures with the appropriate letter: (g) When n = 5, the possible values of are _________. (h) The number of orbitals in the n = 4 shell is _______.
Planck originated the idea that energies can be quantized. What does the term quantized mean? What was Planck trying to explain when he was led to the concept of quantization of energy? Give the formula he arrived at and explain each of the terms in the formula.
Consider the transition from the energy levels n=5 to n=3. (a) What is the frequency of light associated with this transition? (b) In what spectral region does the transition occur? (c) Is energy absorbed?
Photogray lenses incorporate small amounts of silver chloride in the glass of the lens. When light hits the AgCl particles, me following reaction occurs: AgClhvAg+Cl The silver metal that is formed causes the lenses to darken. The energy change for this reaction is 3.10 102 kJ/mol. Assuming all this energy must be supplied by light, what is the maximum wavelength of light that can cause this reaction?

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