1.The only electron in a hydrogen atom moved from n=3.0 to n=6.0. What is the wa

Question

1.The only electron in a hydrogen atom moved from n=3.0 to n=6.0. What is the wavelength of photon (in nm) being associated with this transition? Use whole numbers of nm without any decimal places, such as "415", "1125"

2. A student obtained the Rydberg constant to be 2.0*10-18 J. What is the % error of the measurement? Answer as percentage and keep one decimal place.

3. A 100-mL sample of Pb initially has a concentration of 15.8 ppm. If this sample was diluted to 5.000 mL, what is the new concentration in ppm? Keep one decimal place for your answer.

4.

Which of the following orbitals of H has the highest energy?

1s

5.

The only electron in a hydrogen atom moved from n=3.0 to n=6.0. What is the wavelength of photon (in nm) being associated with this transition? Use whole numbers of nm without any decimal places, such as "415", "1125".

Explanation / Answer

1. Using,

dE = -2.18 x 10^-18(1/n2^2 - 1/n1^2)

with,

n1 = 3

n2 = 6

we get,

dE = -2.18 x 10^-18(1/36 - 1/9) = 1.816 x 10^-19 J

dE = hc/l with l = wavelength of transition.

l = 6.6626 x 10^-34 x 3 x 10^8/1.816 x 10^-19 = 1.09 x 10^-6 m = 1094 nm

2. with found value for Rydberg constant = 2.0 x 10^-18

% error = (2 x 10^-18 - 2.18 x 10^-18) x 100/2.18 x 10^-18 = 8.257% (ignore the -ve sign)

3. 100 ml of 15.8 ppm Pb diluted to 5 ml

New concentration of Pb = 15.8 ppm x 100/5 = 316 ppm

4. The hydrogen orbital with highest energy would be, 3d orbital

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