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The energy required to remove both electrons from the helium atom in its ground state is 79.0 eV. How much energy is required to ionize helium? (i.e. to remove single electron)
- a)54.4 eV
- b)39.5 eV
- c)65.4 eV
- d)24.6 eV
Correct answer is option 'D'. Can you explain this answer?
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Verified Answer
The energy required to remove both electrons from the helium atom in i...
Consider He+ which is a hydrogen like atom. We can apply the Bohr theory to see that energy required to go from
What we need is
Given is the total energy required to get He2+ from He.
What we need is
Given is the total energy required to get He2+ from He.
We cannot apply Bohr theory directly to Helium because it is not a hydrogen like atom.
The correct answer is: 24.6 eV
Most Upvoted Answer
The energy required to remove both electrons from the helium atom in i...
To find the energy required to ionize helium, we need to calculate the energy required to remove a single electron from the helium atom.
First, let's determine the energy required to remove both electrons from the helium atom in its ground state, which is given as 79.0 eV.
The energy required to remove the first electron is given by the ionization energy of helium, denoted as I1. The energy required to remove the second electron is given by the second ionization energy of helium, denoted as I2.
To find the energy required to remove a single electron, we subtract the second ionization energy from the total energy required to remove both electrons:
Energy required to ionize helium (I1) = Total energy - Second ionization energy
I1 = 79.0 eV - I2
Since the question asks for the energy required to ionize helium, we need to find I1. To do this, we need to know the value of the second ionization energy, which is not given in the question.
However, we can make use of a known relationship between the first and second ionization energies. The second ionization energy is always greater than the first ionization energy. In the case of helium, the first ionization energy is known to be 24.6 eV.
Therefore, we can substitute this value into our equation:
I1 = 79.0 eV - 24.6 eV
I1 = 54.4 eV
Hence, the energy required to ionize helium (i.e., remove a single electron) is 54.4 eV.
Therefore, option D, 24.6 eV, is not the correct answer.
First, let's determine the energy required to remove both electrons from the helium atom in its ground state, which is given as 79.0 eV.
The energy required to remove the first electron is given by the ionization energy of helium, denoted as I1. The energy required to remove the second electron is given by the second ionization energy of helium, denoted as I2.
To find the energy required to remove a single electron, we subtract the second ionization energy from the total energy required to remove both electrons:
Energy required to ionize helium (I1) = Total energy - Second ionization energy
I1 = 79.0 eV - I2
Since the question asks for the energy required to ionize helium, we need to find I1. To do this, we need to know the value of the second ionization energy, which is not given in the question.
However, we can make use of a known relationship between the first and second ionization energies. The second ionization energy is always greater than the first ionization energy. In the case of helium, the first ionization energy is known to be 24.6 eV.
Therefore, we can substitute this value into our equation:
I1 = 79.0 eV - 24.6 eV
I1 = 54.4 eV
Hence, the energy required to ionize helium (i.e., remove a single electron) is 54.4 eV.
Therefore, option D, 24.6 eV, is not the correct answer.
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The energy required to remove both electrons from the helium atom in its ground state is 79.0eV. How much energy is required to ionize helium? (i.e. to remove single electron)a)54.4eVb)39.5eVc)65.4eVd)24.6eVCorrect answer is option 'D'. Can you explain this answer?
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