Chemistry Help! (Rydberg Equation)
 👍 0
 👎 0
 👁 608

 👍 0
 👎 0
posted by DrBob222
Respond to this Question
Similar Questions

Chemistry 1
In the spectrum of a specific element, there is a line with a wavelength of 486 nm. Use the Rydberg equation to calculate the value of n for the higher energy Bohr orbit involved in the emission of this light. Assume the value for
asked by Sarah on July 1, 2014 
Chemistry
In the spectrum of a specific element, there is a line with a wavelength of 656 nm. Use the Rydberg equation to calculate the value of n for the higher energy Bohr orbit involved in the emission of this light. Assume the value for
asked by James on March 31, 2014 
Chemistry
In the spectrum of a specific element, there is a line with a wavelength of 656 nm. Use the Rydberg equation to calculate the value of n for the higher energy Bohr orbit involved in the emission of this light. Assume the value for
asked by Luke on June 29, 2014 
chemistry
If our eyes could see a slightly wider region of the electromagnetic spectrum, we would see a fifth line in the Balmer series emission spectrum. Calculate the wavelength λ associated with the fifth line. Express your answer with
asked by myah on November 1, 2016 
analytical chemistry
Any help is greatly appreciated 5mL of a solution A (unknown concentration) was transferred into sic 25mL volumetric flask. The following volumes of a standard solution of A with with a concentration 75ppm were added to the flask:
asked by Katy on May 8, 2015 
chem
λ for one line of the hydrogen spectrum is .4118 x 104 cm. Use this value in the Rydberg equation to calculate the RH value using n1 = 2, and n2 = 5. change the line spectrum to meters you know the equation is Et= EfEi (i think
asked by Mary on October 2, 2006 
chemistry
Atoms of ionized lithium gas (Li2+) are struck by neutrons moving at a velocity of 1.46e5 m/s. Calculate the shortest wavelength in the emission spectrum of Li2+ under these circumstances. You can assume that all electrons start
asked by schoolgirl on March 23, 2013 
chemistry
An electron of wavelength 1.74*1010m strikes an atom of ionized helium (He+). What is the wavelength (m) of the light corresponding to the line in the emission spectrum with the smallest energy transition?
asked by James on March 25, 2013 
chemistry
An electron of wavelength 1.74*1010m strikes an atom of ionized helium (He+). What is the wavelength (m) of the light corresponding to the line in the emission spectrum with the smallest energy transition?
asked by Maikol on March 23, 2013 
Physical Chemistry
An electron of wavelength 1.74*1010m strikes an atom of ionized helium (He+). What is the wavelength (m) of the light corresponding to the line in the emission spectrum with the smallest energy transition?
asked by Echoes on March 23, 2013