Question

How many wavelengths of light are represented in the diagram below?

a. 1
b. 6
c. 7
d. 8

Answer 1

The correct answer is (c) 7.

Step-by-step explanation:

In the diagram provided, we observe a spectrum displaying colors ranging from violet to red. The seven colors of the rainbow, commonly remembered using the acronym ROYGBIV, represent the different wavelengths of light. These colors, in order, are red, orange, yellow, green, blue, indigo, and violet. Each color corresponds to a specific wavelength within the electromagnetic spectrum.

The phenomenon responsible for this separation of colors is called dispersion, which occurs when light passes through a prism or a diffraction grating. As light travels through these mediums, it bends at different angles depending on its wavelength, resulting in the distinct colors we see in the spectrum. The fact that we can identify seven distinct colors in the diagram indicates that there are seven different wavelengths of light represented.

To calculate the number of wavelengths, one could consider the transition between adjacent colors. For instance, the transition from red to orange or from blue to indigo signifies a change in wavelength. Since there are six such transitions between the seven colors, we can conclude that there are seven distinct wavelengths of light.

In summary, the spectrum in the diagram represents seven wavelengths of light, corresponding to the seven colors of the rainbow.

Answer 2

There are 7 wavelengths of light represented in the diagram. Option c is correct.

Step-by-step explanation:

In the diagram below, there are 7 wavelengths of light represented. Option c is correct. Each peak and trough in the diagram corresponds to one complete wavelength of light. You can count the number of complete wavelengths present in the diagram to determine the answer.

To determine how many different wavelengths of light are emitted by these atoms as the electrons fall into lower-energy orbits, we would need to know the specific transitions being made by the electrons within the atoms. In a typical atomic spectrum, an electron can fall from a higher-energy orbit (n-higher) to a lower-energy orbit (n-lower), and this change in energy levels results in the emission of photons with specific wavelengths.

According to the Rydberg formula, the wavelength of the emitted photon can be calculated using the initial and final energy levels of the electron. The wavelengths of emitted light correspond to the differences in energy levels and can be represented in a diagram like a line spectrum. Without the diagram or specific information about the transitions, it's impossible to provide a numeric answer to the question.

The visible spectrum ranges from about 400 nm to 800 nm in wavelength, and these wavelengths correspond to different colors perceived by the human eye, with the lower wavelengths (around 400 nm) appearing violet and the higher wavelengths (around 700-800 nm) appearing red. The color of the emitted light from an atom depends on the energy of the photons, which is inversely related to the wavelength.