The ionization potential of an atom is defined as the energy required to completely remove an electron . using Bohr's theory , calculate the ionization potential of the hydrogen atom?

Question

The ionization potential of an atom is defined as the energy required to completely remove an electron . using Bohr's theory , calculate the ionization potential of the hydrogen atom?

1 Answer

Impact of this question

2739 views around the world

You can reuse this answer
Creative Commons License

Answer 1 · 2018-02-01T04:09:56

See the calculation in the explanation below...

Explanation:

The stationary state energies for a hydrogen atom, in Bohr's model are calculated from the formula

$E_{n} = \frac{- 1311}{n^{2}} \frac{k J}{mol}$ $E_n=(-1311)/n^2 (kJ)/"mol"$

where -1311 kJ/mol is a constant that Bohr objected in his calculations. Its value depends only on physical constants such as the mass and charge of the electron (and Planck's constant), and $n$ $n$ is the number of the energy level (or orbit).

The ground state corresponds to $n = 1$ $n=1$ , the lowest possible energy, and the orbit closest to the nucleus.

$E_{1} = \frac{- 1311}{1^{2}} = - 1311 \frac{k J}{mol}$ $E_1 = (-1311)/1^2 = -1311 (kJ)/"mol"$

The ion state, where the electron has been removed from the atom corresponds to $n \to \infty$ $nrarroo$ , at which point $E = 0$ $E=0$ .

The ionization energy is the difference between these two levels:

$I E = 0 - (- 1331) = 1311 k \frac{J}{mol}$ $IE= 0 - (-1331) = 1311 kJ/"mol"$

Science

Math

Humanities

... and beyond

The ionization potential of an atom is defined as the energy required to completely remove an electron . using Bohr's theory , calculate the ionization potential of the hydrogen atom?

1 Answer

Explanation:

Related questions

Impact of this question