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# Energy Change in Hydrogen & Energy of Photons (College)

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## Energy Change in Hydrogen & Energy of Photons

1.
Which of the following equations can be used to calculate changes in energy in a hydrogen atom?
1. $∆E=2.178xx10^-18 J (1/n_f^2 - 1/n_i^2)$
2. $∆E=2.178xx10^-18 J (1/n_i^2 - 1/n_f^2)$
3. $∆E=-2.178xx10^-18 J (1/n_i^2 - 1/n_f^2)$
4. $∆E=-2.178xx10^-18 J (1/n_f^2 - 1/n_i^2)$
2.
Which of the following equations can be used to calculate the wavelength of an emitted photon?
1. $lambda={∆E}/{hc}$
2. $lambda={∆E xx h}/{c}$
3. $lambda={hc}/{∆E}$
4. $lambda={∆E xx c}/{h}$
3.
What is the energy change involved in moving from n=6 to n=2?
1. $4.84xx10^-19 J$
2. $-4.84 xx 10^-19 J$
3. $2.42 xx 10^-19 J$
4. $-2.42 xx 10^-19 J$
4.
What is the energy change involved in moving from n=3 to n=5?
1. $1.549 xx 10^-19 J$
2. $-1.549 xx 10^-19 J$
3. $7.75 xx 10^-20 J$
4. $-7.75 xx 10^-20 J$
5.
What is the energy change involved in moving from n=1 to n=7?
1. $-2.13 xx 10^-18 J$
2. $1.07 xx 10^-17 J$
3. $2.13 xx 10^-18 J$
4. $-1.07 xx 10^-17 J$
6.
What is the wavelength of an emitted photon, if the energy change associated with it is $2.1336xx10^-18 J$?
1. $1.07xx10^8 m$
2. $1.07xx10^7 m$
3. $5.035 xx 10^6 m$
4. $5.035 xx 10^7 m$
7.
What is the wavelength of an emitted photon, if the associated energy change is $4.84 xx 10^-19 J$?
1. $2.43 xx 10^6 m$
2. $2.43 xx 10^7 m$
3. $1.215 xx 10^6 m$
4. $1.216 xx 10^7 m$
8.
What is the wavelength of an emitted photon, if the associated energy change is $1.36xx10^-17 J$?
1. $6.84 xx 10^8 m$
2. $3.41 xx 10^7 m$
3. $6.84 xx 10^7 m$
4. $3.41 xx 10^8 m$
9.
Describe one limitation associated with the Bohr model, as is portrayed here for a hydrogen atom.

10.
Explain what is implied by the sign (positive or negative) of the energy change, ∆E, involved in hydrogen atoms. Be sure to explain your answer, in terms of n.

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