what are the wavelengths, in nanometers of the ,bright line of the hydrogen emission spectrum corresponding to the transition : n=6 to n=2
show work and answer please. The other question like this did not help me i keep getting incorrect answers.
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E = Rh ( 1/n^2 - 1/n2^2) = 2.18x10^-18 J ( 1/36 - 1/4) = 4.84x10^-19 J
(Ignore the negative sign, energy is absolute value)
E = h v
c = λ v
v = c / λ
E = h c / λ
h, planck's constant
c, speed of light
λ = h c / E = 6.626x10^-34 J s x 3.00x10^8 m/s / 4.84x10^-19 J = 4.1x10^-7 m
1 nm = 1.0x10^-9 m
Divide by 1.0x10^-9 to convert from m to nm
4.1x10^-7 m x ( 1 nm / 1.0x10^-9 m ) = 410 nm