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The electron in the lowest (n = 1) orbit in hydrogen atom has energy - 13.6 e V. How much energy is required to ionize a hydrogen atom which is already in the first excited level.
- a)3.4 e V
- b)10.2 e V
- c)13.6 e V
- d)1.9 e V
Correct answer is option 'A'. Can you explain this answer?
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Most Upvoted Answer
The electron in the lowest (n = 1) orbit in hydrogen atom has energy -...
E=13.6 × z^2/n^2
E1/E2=n2^2 /n1^2
13.6/E2=2^2/1^2
E2=3.4 ev
E1/E2=n2^2 /n1^2
13.6/E2=2^2/1^2
E2=3.4 ev
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Community Answer
The electron in the lowest (n = 1) orbit in hydrogen atom has energy -...
Explanation:
To find the energy required to ionize a hydrogen atom that is already in the first excited level, we need to consider the energy difference between the two levels.
Step 1:
The energy of an electron in the nth orbit of a hydrogen atom is given by the formula:
E = -13.6/n^2 eV
Given that the electron is in the lowest (n = 1) orbit, the energy is:
E1 = -13.6/1^2 = -13.6 eV
Step 2:
The energy required to ionize a hydrogen atom is the difference between the energy of the final state (when the electron is completely removed) and the initial state.
In this case, the initial state is when the electron is in the first excited level (n = 2). The energy of this state is given by:
E2 = -13.6/2^2 = -13.6/4 = -3.4 eV
Step 3:
To find the energy required to ionize the atom, we subtract the energy of the initial state from the energy of the final state:
Eionization = E2 - E1
Eionization = -3.4 eV - (-13.6 eV)
Eionization = -3.4 eV + 13.6 eV
Eionization = 10.2 eV
Therefore, the energy required to ionize a hydrogen atom that is already in the first excited level is 10.2 eV.
Conclusion:
The correct answer is option A) 3.4 eV.
To find the energy required to ionize a hydrogen atom that is already in the first excited level, we need to consider the energy difference between the two levels.
Step 1:
The energy of an electron in the nth orbit of a hydrogen atom is given by the formula:
E = -13.6/n^2 eV
Given that the electron is in the lowest (n = 1) orbit, the energy is:
E1 = -13.6/1^2 = -13.6 eV
Step 2:
The energy required to ionize a hydrogen atom is the difference between the energy of the final state (when the electron is completely removed) and the initial state.
In this case, the initial state is when the electron is in the first excited level (n = 2). The energy of this state is given by:
E2 = -13.6/2^2 = -13.6/4 = -3.4 eV
Step 3:
To find the energy required to ionize the atom, we subtract the energy of the initial state from the energy of the final state:
Eionization = E2 - E1
Eionization = -3.4 eV - (-13.6 eV)
Eionization = -3.4 eV + 13.6 eV
Eionization = 10.2 eV
Therefore, the energy required to ionize a hydrogen atom that is already in the first excited level is 10.2 eV.
Conclusion:
The correct answer is option A) 3.4 eV.
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The electron in the lowest (n = 1) orbit in hydrogen atom has energy - 13.6 e V. How much energy is required to ionize a hydrogen atom which is already in the first excited level.a)3.4 e Vb)10.2 e Vc)13.6 e Vd)1.9 e VCorrect answer is option 'A'. Can you explain this answer?
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