Textbook Question
Use Coulomb's law to calculate the ionization energy in kJ>mol of an atom composed of a proton and an electron separated by 100.00 pm. What wavelength of light has sufficient energy to ionize the atom?
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Ch.8 - Periodic Properties of the Elements
Chapter 8, Problem 114
Consider the elements: Na, Mg, Al, Si, P. a. Which element has the highest second ionization energy?
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Identify the elements given: Na, Mg, Al, Si, P.
Understand that the second ionization energy is the energy required to remove the second electron after the first has already been removed.
Consider the electronic configurations of the elements after the first electron is removed: Na^+, Mg^+, Al^+, Si^+, P^+.
Recognize that the second ionization energy is highest for the element that achieves a stable electron configuration after the first ionization.
Determine which element, after losing one electron, has a stable noble gas configuration or a half-filled or fully filled subshell, making it difficult to remove the second electron.
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