(a) The energy required to remove the electron of the hydrogen atom at an unknown energy level (n = x) is 328.0 kJ/mol. (i) Determine the initial energy level (n = x). (ii) Was the hydrogen atom in the ground state or excited state before the electron was removed? (iii) Determine the wavelength (in nm) of the radiation required to remove the electron from the hydrogen atom (where electron is at n = x).
(a) The energy required to remove the electron of the hydrogen atom at an unknown energy level (n = x) is 328.0 kJ/mol. (i) Determine the initial energy level (n = x). (ii) Was the hydrogen atom in the ground state or excited state before the electron was removed? (iii) Determine the wavelength (in nm) of the radiation required to remove the electron from the hydrogen atom (where electron is at n = x).
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Chapter7: Quantum Theory Of The Atom
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Transcribed Image Text:QUESTION 2
(a) The energy required to remove the electron of the hydrogen atom at an unknown energy level
(n = x) is 328.0 kJ/mol.
(i) Determine the initial energy level (n = x).
(ii) Was the hydrogen atom in the ground state or excited state before the electron was
removed?
(iii) Determine the wavelength (in nm) of the radiation required to remove the electron from the
hydrogen atom (where electron is at n = x).
(b) What is the maximum number of electrons in an atom that can have the following set of
quantum numbers?
(i)
n = 3, t = 2, me =-2, ms = +½
(ii)
n = 2, ms = -½
(ii)
n = 5, { = -1, me = 1
(iv)
n = 4, m= 1
(v)
n= 6, { = 3, m; = +½
(c) Give the ground-state electron configuration for each of following substances:
(i) Phosphorus
(ii) Cr(II) ion
(ii) Sulfide ion
(iv) Ti(IV) ion
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