Question

In: Chemistry

1) If the electron drops down from the n=5 level to n=2, and then to the...

1) If the electron drops down from the n=5 level to n=2, and then to the ground state of hydrogen, what colors (wavelengths) of light will be emitted?

2) What color of light is this?

3) Photon color for n=2 to ground

4) What color of light is this?

Solutions

Expert Solution

Apply Rydberg Formula

E = R*(1/nf^2 – 1/ni ^2)

R = -2.178*10^-18 J

Nf = final stage/level

Ni = initial stage/level

E = Energy per unit (i.e. J/photon)

E = (-2.178*10^-18)*(1/5^2 – 1/2^2)

E = 4.573*10^-19

For the wavelength:

WL = h c / E

h = Planck Constant = 6.626*10^-34 J s

c = speed of particle (i.e. light) = 3*10^8 m/s

WL = (6.626*10^-34)(3*10^8)/( 4.573*10^-19 )

WL = 4.34681*10^-7 m

WL (in nm) = 4.34681*10^-7 *109 = 434 nm (this is violet/purple)

the color of light is violet/purple

now for n= 2 to n = 1

Apply Rydberg Formula

E = R*(1/nf^2 – 1/ni ^2)

R = -2.178*10^-18 J

Nf = final stage/level

Ni = initial stage/level

E = Energy per unit (i.e. J/photon)

E = (-2.178*10^-18)*(1/2^2 – 1/1^2)

E = 1.6335*10^-18

For the wavelength:

WL = h c / E

h = Planck Constant = 6.626*10^-34 J s

c = speed of particle (i.e. light) = 3*10^8 m/s

WL = (6.626*10^-34)(3*10^8)/( 1.6335*10^-18)

WL = 1.21689*10^-7 m

WL (in nm) = 4.34681*10^-7 *109 = 121 nm this is ultaviolet lgith

no visible light to human eye

queen_honey_blossom answered 1 year ago

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