The Structure of the Atom Review
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1 The Structure of the Atom Review
2 Atoms are composed of PROTONS + positively charged mass = x kg NEUTRONS neutral mass = x kg ELECTRONS negatively charged mass = x kg
3 + positive and negative charges - every object normally has both kinds of charges in equal amounts - objects with an equal amount of positive and negative charge are said to be electrically neutral
4 Forces between charges Electrostatic Force - objects with like charge repel + +
5 Forces between charges Electrostatic Force - objects with like charge repel objects with opposite charge attract +
6 In a sense chemistry amounts to asking the following questions What energies do individual electrons possess? Where in an atom can electrons be found?
7 Our Current Model of the Atom + + He
8 In a sense chemistry amounts to asking the following questions How many electrons are present in a particular atom? What energies do individual electrons possess? Where in an atom can electrons be found?
9 From Classical Physics to Quantum Theory
10 The properties of atoms are not governed by the same laws of physics as larger objects Quantum Mechanics: the physics of the very small
11 To understand the electron structure of atoms, one must understand the nature of light
12 The Players Erwin Schrodinger Werner Heisenberg Louis Victor De Broglie Neils Bohr Albert Einstein Max Planck James Clerk Maxwell
13 James Clerk Maxwell Proposed that visible light consists of electromagnetic waves. waves A vibrating disturbance by which energy is transmitted.
14 Electromagnetic radiation is energy propagated at the speed of light c = 3 x 10 8 m/sec Consists of electric and magnetic fields that simultaneously oscillate in planes mutually perpendicular to each other.
15 Electromagnetic radiation
16 Properties of Waves wavelength, λ = m Frequency ν = 1/s = Hz (Hertz) c = ν λ
17 Frequency and wavelength are inversely proportional c = ν λ low frequency-long wavelength high frequency-short wavelength
18 Types of electromagnetic radiation high frequency low frequency gamma rays X-rays ultraviolet light visible light infrared radiation microwaves radio waves short wavelength long wavelength
19
20 The Nature of Energy The wave nature of light does not explain how an object can glow when its temperature increases Pearson Education, Inc. Electronic Structure of Atoms
21 The Players Erwin Schrodinger Werner Heisenberg Louis Victor De Broglie Neils Bohr Albert Einstein Max Planck James Clerk Maxwell
22 An Observable Fact hot bodies radiate electromagnetic energy classical physics assumed that radiating energy was continuous, due to its wavelike nature.
23
24
25 iron bar
26 Red Hot
27 Blue Hot Classical physics what wave lengths are allowed? an infinite amount of energy could be released in a radiation process!
28 Max Planck the energy of the emitted electromagnetic radiation is proportional to frequency ΔE = hν where h = x J s h is called Planck s constant
29 Max Planck ΔE = n hν Energy is always emitted in multiples of hν. n is a whole number (integer)
30 Blue Hot hν hν hν Max Planck energy emitted as electromagnetic radiation by an object (such as a hot iron bar) can have only certain discrete values,
31 Energy of electromagnetic radiation comes in hν-sized packets bundles discrete units The energy of electromagnetic radiation is quantized. quanta
32 The Players Erwin Schrodinger Werner Heisenberg Louis Victor De Broglie Neils Bohr Albert Einstein Max Planck James Clerk Maxwell
33 Another Mystery in Physics: The Photoelectric Effect Experiments showed that electrons were ejected from the surface of certain metals exposed to light at a minimum threshold frequency.
34 Albert Einstein 1905 Accounted for the photoelectric effect by treating light as though it were a stream of particles -- photons. quantization of electromagnetic radiation h ν = kinetic energy e - + binding energy
35 The Photoelectric Effect Photon = hν threshold frequency for ejection of electrons
36 The Photoelectric Effect + KE = hν - BE
37 The Photoelectric Effect Kinetic energy of electron does not depend upon intensity of light + it depends on the frequency
38
39 ΔE = hν 700 nm 1.77 ev 550 nm 2.25 ev 400 nm 3.1 ev Vmax = 2.96 x 10 5 m/s Vmax = 6.22 x 10 5 m/s no electrons - - potassium ev needed to eject an electron Photoelectric Effect
40 Mass of a Photon E = hν E = mc 2 m = h c λ c 2 mc 2 = hν c λ = ν m = c h λ Mass of a Photon is relativistic
41 Depending on the experiment: light behaves either as a wave or as a stream of particles wave /particle duality
42 Example Calculate the energy(in joules)of a photon with a wavelength 5.00 x 10 4 nm (infrared region). ΔE = hc λ ΔE = hν c ν = λ ΔE = (6.63 x J. s ) 5.00 x 10 4 nm x (3.00 x 10 8 m/s) 1 x 10-9 m 1 nm = 3.98 x J
43 43
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