An electron moves from the n = 27 to the n = 15 shell in hydrogen. Is this emiss

Question

An electron moves from the n = 27 to the n = 15 shell in hydrogen. Is this emission or absorption? Determine the wavelength of the photon emitted or absorbed (in nm)? What is the frequency of this photon (in Hz)? What is the energy of this photon (in eV) Write the condensed electron configurations for Mo and Mo^4+ Mo: [Kr] 4d^5 5s^1 Mo^4+: [Kr] 4d^2 5s^0 The following is the orbital diagram for a certain element. Is this diagram as written correct? yes No. Based in this diagram is this element is paramagnetic, diamagnetic? What element does this orbital diagram represent? What is the maximum number of electrons that can be placed into each of the following? Then n = 3 shell? A 3d orbital

Explanation / Answer

a.

this must be emission, since energy will be released (high energy level to low energy level)

b.

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)*(1/72^2 – 1/15^2)

E = 9.259*10^-21

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

E = energy per particle J/photon

WL = (6.626*10^-34)(3*10^8)/(9.259*10^-21

WL = 0.00002146884 m --> 0.00002146884*10^9 = 21468.84 nm

c.

v = c/WL = (3*10^8)/(0.00002146884 = 1.39737*10^13 Hz

d.

energy to eV

1 eV = 1.602677·10-19 J

(9.259*10^-21)/(1.60*10^-19) = 0.05786875 eV

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