When excited electrons drop back down to their regular ground state, the distance they drop corresponds to a particular wavelength of light True False

**True**<br /><br />When excited electrons drop back down to their ground state, they release energy in the form of light. The amount of energy released corresponds to the difference between the energy levels involved in the transition. This energy determines the wavelength (and color) of the emitted light, as described by the equation:<br /><br />\[<br />E = h \cdot f<br />\]<br /><br />Where:<br />- \( E \) is the energy difference,<br />- \( h \) is Planck's constant (\( 6.626 \times 10^{-34} \, \text{J·s} \)),<br />- \( f \) is the frequency of the light.<br /><br />The wavelength (\( \lambda \)) is related to the frequency by:<br /><br />\[<br />\lambda = \frac{c}{f}<br />\]<br /><br />Where:<br />- \( c \) is the speed of light (\( 3.00 \times 10^8 \, \text{m/s} \)).<br /><br />Thus, the distance the electron "drops" between energy levels directly determines the wavelength of the emitted light.