  Chapter 11: Quantum Mechanics and Atomic Structuretron drops from n 4 to n 1 is longer than that from uncertainty in 4 to n 2. (e) The wavelength the atom absorbs in the diametergoing from n = 1 to n = 4 is the same as that emitted asit goes from n 4 to n 111.48 The ionization energy of a certain element is412 kJ mol-1. When the atoms of this element are inthe first excited state, however, the ionization energy is to break uponly 126 kJ mol-1. Based on this information, calculate electrons frthe wavelength of light emitted in a transition from the able to estinfirst excited state to the ground state.11.49 The UV light responsible for sun tanning falls in For exampthe 320- to 400-nm region. Calculate the total energy (in been recordjoules) absorbed by a person exposed to this radiation 3. x 10" kfor 2.0 hours, given that there are 2.0 x 1016 photons the temperahitting Earth's surface per square centimeter per second kinetic enenover an 80-nm (320-nm to 400-nm) range and that the 11.55 Consexposed body area is 0.45 m2. Assume that only half of shown belothe radiation is absorbed, and the other half is reflectedby the body. (Hint: Use an average wavelength of360 nm to calculate the energy of a photon.)11.50 In 1996, physicists created an antiatom of hydro-gen. In such an atom, which is the antimatter equivalentof an ordinary atom, the electrical charges of all thecomponent particles are reversed. Thus, the nucleus ofan antiatom is made of an antiproton, which has thesame mass as a proton but bears a negative charge, andthe electron is replaced by an antielectron (also calledpositron) with the same mass as an electron but bearing11.54 The seous materiduring a totcorona is instudying the

Question

11.48 help_outlineImage TranscriptioncloseChapter 11: Quantum Mechanics and Atomic Structure tron drops from n 4 to n 1 is longer than that from uncertainty i n 4 to n 2. (e) The wavelength the atom absorbs in the diameter going from n = 1 to n = 4 is the same as that emitted as it goes from n 4 to n 1 11.48 The ionization energy of a certain element is 412 kJ mol-1. When the atoms of this element are in the first excited state, however, the ionization energy is to break up only 126 kJ mol-1. Based on this information, calculate electrons fr the wavelength of light emitted in a transition from the able to estin first excited state to the ground state. 11.49 The UV light responsible for sun tanning falls in For examp the 320- to 400-nm region. Calculate the total energy (in been record joules) absorbed by a person exposed to this radiation 3. x 10" k for 2.0 hours, given that there are 2.0 x 1016 photons the tempera hitting Earth's surface per square centimeter per second kinetic enen over an 80-nm (320-nm to 400-nm) range and that the 11.55 Cons exposed body area is 0.45 m2. Assume that only half of shown belo the radiation is absorbed, and the other half is reflected by the body. (Hint: Use an average wavelength of 360 nm to calculate the energy of a photon.) 11.50 In 1996, physicists created an antiatom of hydro- gen. In such an atom, which is the antimatter equivalent of an ordinary atom, the electrical charges of all the component particles are reversed. Thus, the nucleus of an antiatom is made of an antiproton, which has the same mass as a proton but bears a negative charge, and the electron is replaced by an antielectron (also called positron) with the same mass as an electron but bearing 11.54 The s eous materi during a tot corona is in studying the fullscreen
Step 1

Whenever there is transition of electron from a higher energy level to lower energy level, some amount of energy is released in the form of radiations, and this amount of energy released is equal to difference in energy in those two-energy level.

Step 2

According to question,

Energy of excited state = 412 KJmol-1 = 412000 Jmol-1

Energy of ground state = 126 KJmol-1 = 126000Jmol-1

Now, electron does a transition from excited state to ground state and this transition will release some radiation having energy equal to difference of energy in these two-energy level.

Step 3

Thus,

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