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4. An electron with a mass of 5.486 × 104 amu has an uncertainty in position of 0.28 nm. Calculate the electron's minimum uncertainty in velocity. 5. Label the variables from the Rydberg equation with the names and units. Discuss with your group what this equation means. Remember that n₂>ni. = 1.097 × 107 m²¹ (1-1) x m-1 λ

4. An electron with a mass of 5.486 × 104 amu has an uncertainty in position of 0.28 nm. Calculate the electron's minimum uncertainty in velocity. 5. Label the variables from the Rydberg equation with the names and units. Discuss with your group what this equation means. Remember that n₂>ni. = 1.097 × 107 m²¹ (1-1) x m-1 λ

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4. An electron with a mass of 5.486 × 104 amu has an uncertainty in position of 0.28 nm. Calculate the electron's minimum uncertainty in velocity. 5. Label the variables from the Rydberg equation with the names and units. Discuss with your group what this equation means. Remember that n₂ > ni. 1 = 1.097 × 107 m-¹ (1-1) λ
Transcribed Image Text:4. An electron with a mass of 5.486 × 104 amu has an uncertainty in position of 0.28 nm. Calculate the electron's minimum uncertainty in velocity. 5. Label the variables from the Rydberg equation with the names and units. Discuss with your group what this equation means. Remember that n₂ > ni. 1 = 1.097 × 107 m-¹ (1-1) λ
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