Atoms and Atomic Structure
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1 Atoms and Atomic Structure 101 Week 13 2
2 A remarkable fact, which is important to science and technology: Nature is simple. 101 Week 13 3
3 What is matter? Physics is a reductionist science. Beneath the surface, nature is simple! All matter is composed of elements. There are 91 stable elements, and about 20 other unstable elements which decay by radioactive processes. 101 Week 13 4
4 Ancient ideas about matter from the philosophers of ancient Greece Elements. They had the idea that all matter is composed of a few basic forms of matter air, earth, fire and water. Atoms. They had the idea that matter has smallest particles; matter is not infinitely divisible. Democritus ( BC) The word Atom comes from Greek, meaning cannot be cut. 101 Week 13 5
5 Democritus of Abdera ( BC) A + tome cannot be cut the laughing philosopher 101 Week 13 6
6 The Elements 101 Week 13 7
7 101 Week 13 8
8 Periodic properties of the elements: Elements in the same column have similar chemical and physical properties. Noble gases Alkali metals Halogen gases Precious metals Semiconductors 101 Week 13 9
9 What is an element? These are not the elements of ancient Greece (air, earth, fire, water). There are 91 stable elements, plus some unstable ones. Each element has a unique atom. Atomic number of an element = the number of electrons in an atom of the element Examples of materials that are not elements: compounds and mixtures. A chemical compound has a complex molecule (a bound state of different atoms) as its basic particle. 101 Week 13 10
10 The Atomic Theory Link 101 Week 13 11
11 Atomic Structure 101 Week 13 12
12 Atomic Orbitals 101 Week 13 13
13 Chemistry Atoms combine in molecules, by sharing electrons 101 Week 13 14
14 How big is an atom? 101 Week 13 15
15 The Atom How large is an atom? How can we measure the size of an atom? What fundamental factors determine the size of an atom? 101 Week 13 16
16 Amedeo Avogadro define a standard number of atoms or molecules, to use in the interpretation of chemical reactions by the atomic theory. N But how do we know that atoms and molecules even exist? 101 Week 13 17
17 When does a theory become accepted as true? Atoms and molecules are much too small to be seen. An atom is only 1 / 5000 times as large as one wavelength of visible light. If we cannot see an atom, can the atomic theory be accepted as true? The truth of atoms was not generally accepted until the 20 th century. But how? 101 Week 13 18
18 Brownian motion Brownian motion is the random jittery motion of a small particle suspended in a fluid, due to collisions with the molecules of the fluid. Picture from Atoms by Jean Baptiste Perrin Brownian motion is direct evidence of atoms. 101 Week 13 19
19 First Solvay Congress, 1911; Brussels; L-R seated at table: Nernst; Brillouin; Solvay; Lorentz; Warburg; Perrin; Wien; Curie; Poincare. L-R Standing: Goldschmidt; Planck; Rubens; Sommerfeld; Lindemann; De Broglie; Knudsen; Hasenohrl; Hostelet; Herzen; Jeans; Rutherford; Kamerlingh-Onnes; Einstein; Langevin 101 Week 13 20
20 Jean Baptiste Perrin and Avogadro s number N Perrin used Brownian motion to measure Avogadro s number, in The theory had been worked out in 1905 by Einstein. The properties of the motion depend on temperature, molecular weight, and number density. From the observations Perrin could deduce the value of N. He got the Nobel prize in Today N is determined most accurately by X- ray scattering. N = 6.02 x atoms 101 Week 13 21
21 How large is an atom? (1) The mass density of solid carbon (diamond) is 3.52 g/cm 3 ; so the volume of 12 grams of carbon is V 12 g g / cm cm 3 (2) Therefore the volume of a single carbon atom (from N) is V N cm (3) Convert V a to an atomic radius (V a = 4/3 p r 3 ) r 3 1/ 3 8 V 110 a 4 cm 101 Week 13 22
22 Result: The typical order of magnitude of an atomic radius is m = 0.1 nm. What determines this size? 101 Week 13 23
23 Atomic structure How do we know that an atom has this structure? 101 Week 13 24
24 101 Week 13 25
25 The typical order of magnitude of an atomic radius is m = 0.1 nm. Why? What determines this size? quantum dynamics of the electron potential kinetic energy energy V ( r) 101 Week K 2 p 2m 2 e 4 r 0 1 2m h 2 r Heisenberg uncertainty principle The state with lowest energy has mean radius = h 2 me Bohr radius m 2
26 Democritus of Abdera ( BC) 101 Week 13 27
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