Which transition would result in a photon with the longest wavelength and why?? a. n=2 to n=1 b. n=4 to n=1 c. n=5 to n=3 d. n=7 to n=6

An electron in a hydrogen atom transitions from n = 3 to n = 5. Which of the following statements is true? A. There is not enough information B.  a photon of wavelength 1.28 nm is emitted C.  a photon of wavelength 1.28 nm is absorbed D. a photon of wavelength 1.28 um is emitted E. a photon of wavelength 1.28 um is absorbed

An excited hydrogen atom emits light with a wavelength of 410.4 nm to reach the energy level for which n = 2. In which principal quantum level did the electron begin? n = HINT(s)

when an electron in excited energy level drops to a lower energy level, a photon is emitted.    if the electron is deopping to n=1, which transition will emit the longest wavelength? n=_____ to n=1

Which of the following electron transitions in the hydrogen atom is associated with radiation having the longest wavelength? You can do four different calculations, but that might take you awhile.  You should be able to do this problem without performing a single calculation. Select one: a. from n = 4 to n = 1 b. from n = 5 to n = 3 c. from n = 3 to n = 1 d. from n = 6 to n = 3

The minimum frequency of light needed to eject electrons from a metal is called the threshold frequency, vo. Find the minimum energy needed to eject electrons from a metal with a threshold frequency of 3.09 x 1014 s-. Eo = J With what maximum kinetic energy will electrons be ejected when this metal is exposed to light with a wavelength of 285 nm? KEelectron J %3D 1 A étv W MacBook Air 80 DO0 D00 DI DD F3 F4 F5 F6 F7 F8 F9 F10 F11 F12 %24 & 25

An electron transitions from n = 7 to n = 3 in a hydrogen atom. Calculate the energy of the photon emitted during this transition. A) 8.12x10−17 J B) 1.98x10−19 J C) 3.57x10−20 J D) 7.44x10−18 J

When an electron in excited energy level drops to a lower energy level, a photon is emitted. If the electron is dropping to n=1, which transition will emit the longest wavelength? n=______ to n=1.

Which transition of an electron in the hydrogen atom emits a photon with the smallest amount of energy?  a. n = 6 to n = 1 b. n = 7 to n = 1 c. n = 2 to n = 1 d. n = 7 to n = 6 e. n = 1 to n = 7

Sa 1 points An electron completes a transition from the n = 1 energy level where it has energy E1 =-2.18 x 10-18 Joules to the n=3 energy level where it has energy E3-2.42 x 10-19 Joules by absorbing 1018 Joules (essentially the difference between these two values). Calculate the wavelength (A) of a photon that would need to be absorbed to cause the n=1 to n 3 transition. energy E= 1.94 X hc where Plank's constant h 6.626 x 1034JS