An electron transitions from n = 5 to n = 3 in a hydrogen atom. What is the energy required for this transition? Is energy emitted or absorbed in the transition?
To calculate the energy required for the electron transition in a hydrogen atom, you can use the formula for the energy of an electron in a hydrogen atom:
E = -13.6 eV * (1/n^2),
where E is the energy in electron-volts (eV), and n represents the principal quantum number.
In this case, the electron is transitioning from n = 5 to n = 3. Plugging these values into the formula:
E1 = -13.6 eV * (1/5^2) = -13.6 eV * (1/25) = -0.544 eV,
E2 = -13.6 eV * (1/3^2) = -13.6 eV * (1/9) = -1.511 eV.
The energy required for the transition is the difference between the initial and final energy states:
ΔE = E2 - E1 = -1.511 eV - (-0.544 eV) = -0.967 eV.
Now, to determine if energy is emitted or absorbed in the transition, we look at the sign of ΔE. If ΔE is negative, then energy is emitted. If ΔE is positive, then energy is absorbed.
In this case, ΔE is negative (-0.967 eV), indicating that energy is emitted in the transition.
En=− 13.6/(n^2) eV. is the energy in each level.
so figure for n=5, then n=3
subtract the n=5 energy from the n=3 level.