When an electron makes a transition from the n=3 to the n=2 hydrogen
atom bohr orbit, the energy difference between these two orbits
(3.0x10^-19 J) is given off in a photon of light. The relationship
...
between the energy of a photon and its wavelength is given by
E=hc/wavelength, where E is the energy of the photon J, h is planck’s
constant (6.626x10^-34 J x s), and c is the speed of light (3.00x10^8 m/s)
Find the wavelength of light emitted by hydrogen atoms when an electron makes this transition.
To find the wavelength of light emitted when an electron makes a transition from the n=3 to the n=2 orbit in a hydrogen atom, we can use the equation E = hc/λ, where E is the energy of the photon, h is Planck's constant, c is the speed of light, and λ is the wavelength of the photon.
Given information:
E = 3.0x10^-19 J (energy difference between the n=3 and n=2 orbits)
h = 6.626x10^-34 J·s (Planck's constant)
c = 3.00x10^8 m/s (speed of light)
We need to rearrange the equation to solve for the wavelength (λ):
λ = hc/E
Substitute the given values into the equation:
λ = ((6.626x10^-34 J·s) * (3.00x10^8 m/s)) / (3.0x10^-19 J)
= ((6.626 * 3.00) * (10^-34 * 10^8)) / (3.0 * 10^-19)
= (19.878 * 10^-26)/(3.0 * 10^-19)
= 6.626 * 10^-7 m (meters)
Therefore, the wavelength of light emitted by hydrogen atoms when an electron makes the transition from the n=3 to the n=2 orbit is approximately 6.626 x 10^-7 meters.
the energy from radiation can be used to cause the rupture of chemicals bonds. a minimum energy of 495 kj/mol is required to break the oxygen- oxygen bond in o2. what is the longest wavelength of radiation that possesses the necessary energy to break the bond?
All you need to do is to substitute the numbers in to E = hc/wavelength.
3 x 10^-19 = 6.626 x 10^-34 x 3 x 10^8/wavelength.
Solve for wavelength.