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CHEM 1A Lecture Notes - Lecture 5: Radiant Energy, Photon, Niels Bohr

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11 Oct 2015

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CHEM 1A Full Course Notes

CHEM 1A Full Course Notes

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Photoelectric effect: observation that metals emit electrons when light shines upon them. Amount of energy transferred from light to object must exceed binding energy (energy that keeps electron to the object) Depends on intensity of the light and not the wavelength. If intensity low, lag time is the time between initial light and the emission of electrons. No electrons emitted unless frequency v (nu) is above a certain threshold frequency v, regardless of the light intensity. Energy of photon = hv = hc/ . H = planck"s constant = 6. 626 * 10^-34 j*s. Photon: a packet of light/ a quantum of light. Energy pulse / energy of photon = number of photons. Ke of emitted electrons = hv - . Interference is not electrons interfering with another, but rather by each electron interfering with itself. Can"t simultaneously observe both particle nature of the electron and the wave nature of the electron emission spectrum: series of bright lights.

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LIGHT LAB SPRING 2018 CHEM 1430 Ill. Quantization of Electromagnetic Radiation In 1894, the German physidist, Max Plank, was working for a utility company to maximize visible light output from incandescent lamps using minimum power. Based on theoretical considerations, Planck postulated that electromagnetic energy could only be emitted at discrete values, rather than the continuum of predicted by classical physics, as multiples of the frequency of the radiation. Planck's Postulate took the mathematical form: EÂ·hv where the energy emitted, in Joules, is the product of a constant, h, known as Planck's Constant, and the frequency of the radiation, v. Planck's Postulate was experimentally verified and h found to have the value of 6.626 x 1034 Js(Joule seconds). The idea that electromagnetic radiation energy had specific frequency dependent energy was termed a "quantum of action," a distressing finding for the dlassically trained Planck. Despite his objections, Planck adopted this quantization of energy as a last resort to reconcile experiment with theory. This discovery set the stage for the early understanding of atomic structure, led to the term "photon" to describe the packet of energy carried by light waves, led to an understanding of the photoelectric effect, eventually leading to the development of general quantum theory Planck's Relationship, in combination with the tight equation, c the energy of a photon from frequency or wavelength. Î» w, allow expressions to be written to calculate ACTIVITY 4: QUANTIZATION OF THE ENERGY OF RADIATION To practice cakculations with Planck's Relationship, complete the following table, showing work with units in the right mest column, Convert given frequency to energy or given wavelength to energy. Take the value for Planck's Constant, h, to be 6.626 x 10"Js, show a calculation string include dimensions, reporting the final value to the proper number of significant figures Spectral Region Wavelength Frequency Energy in J/photon Show Calculation String Î» in meters v in s or cps X-ray 6.0 x 10"m Blue light 4.5 x 10m Infrared 4.1 x 10" cps Microwave 7.3 x 101 cps Radio Wave 3.0x 10 m IV. Bohr's Quantum Model for the Hydrogen Atom Ernest Rutherford's Gold Foil Experiment of 1911 demonstrated the nuclear structure of the atom. Questions remained as to how electrons were arranged in the atom. The most common belief called for the negatively charged the late 19h century recognized a particle (an electron) traveling around a body (the positively charged nucleus) would continuously radiate energy, slowing over time, eventually falling into the nucleus. Matter would collapse. Page 8 of 12

A suspect is apprehended in an assault case and is found to have smears of makeup on his clothing. The victim was known to have been wearing a distinctive pearl-white makeup. The pearl effect in cosmetics is from an ionic bismuth compound, BiOCl (bismuth has a 3+ charge).(a) What is the Lewis Structure of this compound (draw it the best you can by typing--if you have trouble with the dots, type out the explanation regarding where they should be)? Explain how you arrived at this structure. In other words, don't just give me the structure, but walk me through and explain to me how exxactly you arrived at your answer.(b) We also discussed wavelength and frequency in this Lesson. They are actually mathematically related: v = c / (lambda), where v is the frequency, c is the speed of light (see below), and (lambda) is wavelength. The particle nature of light was first proposed by Einstein, who suggested that light could be described as a stream of particles called photons. A photon of a certain wavelength (lambda) has an energy (E) given by the equation: E = hc / lambda, where E is the energy of the photon in J, h is Planck's constant (6.626 x 10^-34 J*s), and c is the speed of light (3.00 x 10^8 m/s). If we use a fancy instrument called an inductively coupled plasma-optical emission spectrophotometer (ICP-OES) to detect bismuth by monitoring light emitted at a wavelength of 223.1 nm, what is the energy and frequency that corresponds to this wavelength? (HINT: 1 nm = 1 x 10^-9 m; be sure all units are able to cancel out as necessary). You must show all work to receive credit.

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