The ionization energy of a certain element is 352 kJ/mol. (Ionization energy is the minimum energy...

The ionization energy of a certain element is 352 kJ/mol. (Ionization energy is the minimum energy required to remove an electron from an atom. It is usually expressed in units of kJ/mol; that is, it is the energy in kilojoules required to remove one mole of electrons from one mole of atoms.) However, when the atoms of this element are in the first excited state, the ionization energy is only 166 kJ/mol. Based on this information, calculate the wavelength of light emitted in a transition from the first excited state to the ground state.

λ = × 10 nm

(Enter your answer in scientific notation.)

Solutions

Expert Solution

Formula: E = hc/

Where E is the change in energy = Ionization energy in ground state - ionization energy in excited state

'h' is the Planck's constant = 6.626*10^-34 J.s

'c' is the velocity of light = 3*10⁸ m/s

'' is the wavelength of light emitted in the transition.

i.e. (352 - 166)*10³ J/6.022*10²³ atom = 6.626*10^-34 J.s * 3*10⁸ m.s^-1/

Therefore, = 643.6*10^-9 m

Here, 1 nm = 10^-9 m

Hence, = 6.436*10² nm

queen_honey_blossom answered 1 year ago

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