How come light photons penetrate these solutions easily

In summary, light travels through a solution by interacting with the molecules in the solution. The appearance of a solution is determined by the size and concentration of particles, with smaller and evenly dispersed particles resulting in a clear solution. The concentration, size, and type of particles in a solution also affect how easily light can penetrate it. Light can penetrate different types of solutions to varying degrees, with transparent solutions like water allowing more light to pass through and opaque solutions like milk absorbing and scattering light. The interaction between light photons and molecules in a solution depends on the properties of the molecule, such as its size, shape, and composition, with some molecules absorbing specific wavelengths of light and others scattering light in all directions.
  • #1
g.l.
1
0
Hello,

I'm looking for an answer to the following question -

X-rays are attenuated by liquid iodine solutions (in fact, these solutions are used as medical imaging contrast agents). so far so good.
How come light photons penetrate these solutions easily ? (these solutions appear water like - transparent)

Thanks for an educated explanation.

Gadi.
 
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  • #2
The absorption of light by matter is frequency dependent.
This is related to the molecular structure of the material, and so is different for different materials. The absorption is greatest near a resonant frequency of the particular molecule.
 
  • #3


Hello Gadi,

Light photons penetrate liquid iodine solutions easily because they have a lower energy level compared to X-rays. X-rays have a much higher frequency and energy, which allows them to be easily absorbed by the iodine molecules in the solution. On the other hand, light photons have a lower frequency and energy, making them less likely to interact with the iodine molecules. This allows them to pass through the solution without being absorbed or attenuated as much. Additionally, the molecular structure of iodine allows for a higher degree of transparency compared to other substances, further allowing light to easily penetrate through the solution. I hope this helps to explain why light photons are able to easily penetrate liquid iodine solutions.
 

1. How does light travel through a solution?

Light travels through a solution by interacting with the molecules in the solution. When light encounters a molecule, it can be absorbed, scattered, or transmitted. In the case of transmission, the light is able to pass through the solution without being absorbed or scattered.

2. Why do some solutions appear clear while others appear cloudy?

The appearance of a solution depends on the size and concentration of the particles in the solution. If the particles are small and evenly dispersed, the solution will appear clear. However, if the particles are larger or more concentrated, they may scatter or absorb light, causing the solution to appear cloudy.

3. What properties of a solution affect how easily light can penetrate it?

The concentration, size, and type of particles in a solution all affect how easily light can pass through it. Solutions with smaller and less concentrated particles will allow more light to pass through, while solutions with larger and more concentrated particles will absorb or scatter more light.

4. Can light penetrate all types of solutions equally?

No, light can penetrate different types of solutions to varying degrees. For example, water is a transparent solution that allows a large amount of light to pass through, while milk is an opaque solution that absorbs and scatters light, making it more difficult for light to penetrate.

5. How do light photons interact with molecules in a solution?

When light photons encounter molecules in a solution, they can be absorbed, scattered, or transmitted. The specific interaction depends on the properties of the molecule, such as its size, shape, and composition. Some molecules may absorb specific wavelengths of light, while others may scatter light in all directions.

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