Problem 2. a. If an atom has an electron in the n= 5 state with m=3,...
Problem 2. a. If an atom has an electron in the n= 5 state with m= 3, what are the possible values of I? b. Find the wavelength of the third line (n=4 to n=1) in the Lyman series (hydrogen atom), and identify the type of EM radiation
A hydrogen atom has an excited electron in the n = 5 state. The electron descends to the n = 2 state. What is the energy level of the n = 5 state? What is the energy level of the n = 2 state? What is the wavelength of the emitted photon (3 sigfigs please)?
When an electron of an excited hydrogen atom descends, from an initial energy level (ni) to a lower (nf), characteristic electromagnetic radiation is emitted. The Bohr model of the H-atom allows the calculation of ?E for any pair of energy levels. ?E is related to the wavelength (?) of the radiation according to Einstein's equation ( ?E = [(hc)/?]). Distinct series of spectral lines have been classified according to nf: Lyman series:nf=1 (91<?<123 nm; near-UV). Balmer series:nf=2 (365<?<658 nm; visible)....
Find the wavelength of the third line in the Lyman series, and identify the type of EM radiation. I need to know what the governing principles are for this equation.
e) A hydrogen atom is in its ground state (n = 1). Using the Bohr theory of the atom, calculate (e) the energy gained by moving to a state where n = 5. g) A hydrogen atom is in its ground state (n = 1). Using the Bohr theory of the atom, calculate (g) the wavelength, λ, of the EM waved adsorbed in the process of moving the electron to a state where n = 5. Hint: There are two...
6. How many unpaired electrons does an atom of phosphorous have in its ground state? (3) 3 (4)5 (1) 1 (2) 2 7. A possible set of quantum numbers for the last electron added to complete an atom of silicon (Si) in its ground state is m eo m, A. 4 0 +% -% В. 3 0 +1 C. 4 1 -1 +% D. 3 1 +1 -% (1) A (2) B (3) C (4) D 8. A possible set...
1) Calculate the energy change corresponding to the excitation of an electron from the n=1 to n=3 electronic state in the hydrogen atom.2) Calculate the wavelength of electromagnetic radiation associated with the energy change above.
14. Consider the hydrogen atom. (a) What value of wavelength is associated with the Lyman series for n = 2? (Rydberg constant RH = 1.097 x 10^7 m^-1). (b) An electron in a hydrogen atom makes a transition from the n = 4 to the n = 3 energy state. Determine the energy (in eV) of the emitted photon. (c) Calculate the radius, speed. linear momentum. and de Broglie wavelength of the electron in the first Bohr orbit. (me =...
Consider an electron transition from n 5 to n =3 of a hydrogen atom. 5. Use Bohr's H model to calculate the energy required to for this electron transition. Will the hydrogen atom absorb or emit energy during this transition? a) What wavelength of light will the hydrogen atom absorb or emit in this electron transition? b) A rifle bullet (mass-4.20 g) has a velocity of 2160 mph. What is the wavelength associated with this bullet? (1 km 0.62137 mil)...
A hydrogen atom that has an electron in the n=1state absorbs a photon. What wavelength must the photon possess to send the electron to the n=4 state? wavelength: nm What possible wavelengths would be detected in the spectral lines that result from the deexcitation of the atom as it returns from n=4\ to the ground state? Classify each wavelength as either possible or not possible. Answer Bank: 821nm 656nm 1460nm 103nm 365nm 122nm 486nm 1880nm 91.2nm 97.3nm Possible: Not possible: