Subjective Type

Energy of an electron in the ground state of the hydrogen atom is $$-2.18\displaystyle \times 10^{-18}J$$. Calculate the ionization enthalpy of atomic hydrogen in terms of J mol$$\displaystyle ^{-1}$$.

Solution

The ionization enthalpy is the amount of energy required to remove an electron from ground state to infinity. The energy of electron in the ground state is $$\displaystyle -2.18 \times 10^{-18} J $$.
The energy of electron at infity is zero.

The energy required to remove electron is $$\displaystyle 0-(-21.8 \times 10^{-18} J )= 2.18 \times 10^{-18} J $$.

To remove 1 mole of electrons, the amount of energy required is $$\displaystyle 2.18\times 10^{-18} \times 6.023\times 10^{23} = 13.130\times 10^{5} J/mol $$. This is the ionization enthalpy of hydrogen.

SIMILAR QUESTIONS

Periodic Classification of Elements

Green house effect is caused by :

Periodic Classification of Elements

Ionization energy of gaseous $$Na$$ atoms is $$495.5$$ kJ mol$$^{-1}$$. The lowest possible frequency of light that ionizes a sodium atom is: $$[h=6.626\times 10^{-34} \ Js, N_A=6.022\times 10^{23} \ mol^{-1}]$$

Periodic Classification of Elements

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Periodic Classification of Elements

Ionizing radiation is:

Periodic Classification of Elements

Would you expect the first ionization enthalpies for two isotopes of the same element to be the same or different? Justify your answer.

Periodic Classification of Elements

Which of the following can most easily form unipositive gaseous ion?

Periodic Classification of Elements

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Periodic Classification of Elements

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Periodic Classification of Elements

The electronic states $$X$$ and $$Y$$ of an atom are depeicted below: $$X : 1s^{2} 2s^{2} 2p^{6} 3s^{1}$$ $$Y: 1s^{2} 2s^{2} 2p^{6} 3s^{2} 3p^{6} 4s^{1}$$ Which of the following statements is not correct?

Periodic Classification of Elements

Which of the following elements will have highest ionisation energy?

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