Consider the element vanadium (Z=23)a) There is a line in the vanadium spectrum at 318.5nm.i. What is the frequency of the line?ii. What is the energy difference between the two levels responsible for this line in kJ per mole?iv. The ionization energy of vanadium from the ground state is 650.2 kJ/mol. Assume that the transition in (3) is from the ground state to an excited state. If that is the case, calculate the ionization energy from the excited state.
Consider the element vanadium (Z=23)a) There is a line in the vanadium spectrum at 318.5nm.i. What is the frequency of the line?ii. What is the energy difference between the two levels responsible for this line in kJ per mole?iv. The ionization energy of vanadium from the ground state is 650.2 kJ/mol. Assume that the transition in (3) is from the ground state to an excited state. If that is the case, calculate the ionization energy from the excited state.
Chemistry & Chemical Reactivity
10th Edition
ISBN:9781337399074
Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Chapter6: The Structure Of Atoms
Section: Chapter Questions
Problem 8PS: The most prominent line in the emission spectrum of magnesium is 285.2 nm. Other lines are found at...
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Consider the element vanadium (Z=23)
a) There is a line in the vanadium spectrum at 318.5nm.
i. What is the frequency of the line?
ii. What is the energy difference between the two levels responsible for this line in kJ per mole?
iv. The ionization energy of vanadium from the ground state is 650.2 kJ/mol. Assume that the transition in (3) is from the ground state to an excited state. If that is the case, calculate the ionization energy from the excited state.
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