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(B) white hot solid emits a continuous spectrum containing all wavelengths of visible light.When this light passes through a sodium flame (sodium vapo

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Two dark lines in the yellow region

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(B) white hot solid emits a continuous spectrum containing all wavelengths of visible light.When this light passes through a sodium flame (sodium vapour),the sodium atoms absorb specific wavelengths corresponding to their characteristic emission lines ($D_1$ and $D_2$ lines).As a result,these specific wavelengths are removed from the continuous spectrum,appearing as two dark lines in the yellow region of the otherwise continuous spectrum.This phenomenon is known as an absorption spectrum.

List-$I$	List-$II$
$1$. Nitrogen molecules	$(A)$ Continuous spectrum
$2$. Incandescent solids	$(B)$ Absorption spectrum
$3$. Fraunhofer lines	$(C)$ Band spectrum
$4$. Electric arc between iron rods	$(D)$ Emission spectrum

When light emitted by a white hot solid is passed through a sodium flame,the spectrum of the emergent light will show

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