Light causes the excitation of electrons in various molecules, which leads the molecules to eject an electron. The energy of the ejected electron, in joules (J), depends on the type of molecule and the frequency of the light. Figure 1 shows how electron energy varies with light frequency for several different molecules. Figure 2 shows how the number of ejected electrons varies with light intensity, and Figure 3 shows the maximum energy of an ejected electron at a given light intensity for a given molecule.
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Question 1 of 5
1. Question
Question 1:
The x-axis of Figure 3 represents which of the following data?
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Question 2 of 5
2. Question
Question 2:
The hypothesis that increasing the amount of light directed at a molecule will increase the number of electrons emitted per second is supported by which figures?
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Question 3 of 5
3. Question
Question 3:
If the data in Figure 3 were produced by a light with a frequency of 10.5×1014 Hz, which molecule was most likely used?
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Question 4 of 5
4. Question
Question 4:
Is the statement “The maximum energy of electrons increases with increasing light intensity” supported by the data in Figure 3?
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Question 5 of 5
5. Question
Question 5:
According to the data presented, which of the following statements best compares the frequencies of light required for both Molecules W and T to produce an electron with a maximum energy of 3?
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