6. Sodium street lamps emit a warm, yellow light (λ = 587.6 nm) due to electronic excitation of sodium vapor. Propose the electron configuration for sodium's 1st excited state. What is the molar energy required for this transition at room temperature? What would the temperature need to be to thermally induce these transitions?

6. Sodium street lamps emit a warm, yellow light (λ = 587.6 nm) due to electronic excitation of sodium vapor. Propose the electron configuration for sodium's 1st excited state. What is the molar energy required for this transition at room temperature? What would the temperature need to be to thermally induce these transitions?

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

If two wavefunctions, y(x) and ø(x), are orthogonal, this means that they have the following property: O ∞ S 88 y* (x) (x) dx = 1 8 8 S*~*\x{x}³² dx = S*®* [p{x}³² dx=1 |y(x) | (x) – 8 – 8 Soy 88 y* (x) Q(x) dx=0 y* (x) q (x) dx=1
How much energy in joules is required to change the energy state of the H-atom electron from n= 1 to n= 2? From n = 1 to n = 4? From n = 1 to inﬁnity? What are the wavelengths of these transitions? The frequencies?
Quantum numbers arise naturally from the mathematics used to describe the possible states of an electron in an atom. The four quantum numbers, the principal quantum number (n), the angular momentum quantum number ({), the magnetic quantum number (mp), and the spin quantum number (m,) have strict rules which govern the possible values. Identify all allowable combinations of quantum numbers for an electron. n = 4, l = 0, me = 1, m, = – n = 6, l = 6, me 1, mş = - п%3D 3, е %3D 2, те — — 1, m, — + n = 3, l = -2, mẹ = -1, m, = - 2 n = 5, l = 1, me = 0, m, = + O n = 2, € = 0, mẹ = 0, mş = –1
5. What is the maximum number of electrons that can occupy the orbitals with principal quantum mumber =4?
1. How many different spectral lines can electrons pro- duce that start in the n = 5 state and eventually end up in the groundstate? 2. An electron makes a transition from a 4f to a 1s state. What is the wavelength of the emitted photon? 3. Compute the magnitude of the angular momentum of hydrogen atoms in the 2p state (numercially).
Using the Bohr model of an electron orbiting a nucleus, the angular momentum of Earth's orbit around the Sun is about 2.67 x 1040 g m2 s−1. Using the Bohr quantization condition, what is the quantum number n for Earth's orbit? If the Earth transitions from this orbit to n-1 (emitting a graviton, which is the gravitational anagloue of the photon), how much energy would be released? Find the frequency of the graviton.
Most of the ultraviolet radiation reaching the surface of the earth is UV-A radiation, which has a wavelength range of 315 nm to 400 nm. UV-A radiation is a cause of skin aging and also contributes to development of skin cancer.Determine the energy of a mole of photons of UV-A radiation that have a wavelength of 325 nm
Assuming the wavelength for fluorescence is observed at 475 nm and the wavelength of the phosphorescence process occurs at 523 nm, find the energy released from 12.35 g of Calcium atoms. (Assume that there is 1 excited electron per calcium atom and every one of them relaxes via the processes above.) (Fluorescence occurs 2.45 times more frequently than phosphorescence)
In the hydrogen atom, the transition from the 2p state to the 1s state emits a photon with energy 16.2 x10-19 J. In an iron atom, the same transition emits X-rays with wave- length 0.193 nm. Calculate the energy difference between these two states in iron. Explain the difference in the 2p-1s energy level spacing in these two atoms.
A dye molecule has electrons that are free to travel up and down a chain of atoms, giving electron energy states that are given by the particle-in-a-box model, with En = (0.30 eV)n2.a. Sketch the energy levels that correspond to n = 1 to n = 4.b. What are the three longest wavelengths of visible light that the molecule will absorb?
Can you please help me with part C and D?
The iodine molecule can be photodissociated (broken apart with light) into iodine atoms in the gas phase with light of wavelengths shorter than about 792 nmnm. A glass tube contains 3.40×1017 iodine molecules. What minimum amount of light energy must be absorbed by the iodine in the tube to dissociate 15.0 %% of the molecules?