Which of the following statements about emission spectra is correct?
All the lines are evenly spaced.
All noble gases have the same spectra.
Each line corresponds to a series of wavelengths.
All the lines result from discrete energy differences
I have to say D) Each line corresponds to a series of wavelengths.
The correct statement about emission spectra is: "All the lines result from discrete energy differences."
To determine which statement about emission spectra is correct, let's break down each statement one by one and explain how to find the answer.
1. All the lines are evenly spaced: To verify this statement, you need to observe the emission spectrum of an element or a gas. Emission spectra are produced by sending light through or exciting a sample of a substance. The emitted light is then dispersed into its various wavelengths using a prism or a spectrometer. By examining the resulting spectrum, you can determine if the lines are evenly spaced. To find actual emission spectra, you can search online databases or consult scientific literature.
2. All noble gases have the same spectra: To check this statement, you need to compare the emission spectra of various noble gases. Noble gases are a group of elements on the periodic table that includes helium, neon, argon, krypton, xenon, and radon. Once you obtain the spectra for each noble gas, compare them to see if they share the same pattern of lines. Again, you can find these spectra through online sources or scientific references.
3. Each line corresponds to a series of wavelengths: This statement is generally correct. In an emission spectrum, each line represents a specific wavelength of light emitted by the sample. Different elements or gases produce distinct patterns of lines in their spectra, allowing scientists to identify them. So, if the statement suggests that each line corresponds to a unique wavelength, it is accurate.
4. All the lines result from discrete energy differences: This statement is correct. In an emission spectrum, the lines are a consequence of electrons transitioning from higher energy levels to lower energy levels within an atom or molecule. Each transition corresponds to a specific energy difference, which is why the lines appear at distinct locations in the spectrum.
Based on the explanations above, the statement that is generally correct and consistent with the properties of an emission spectrum is: "All the lines result from discrete energy differences."