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Unformatted text preview: Fundamentals of Micromachining Vacuum Systems Outline Vacuum principles Vacuum pumps Vacuum materials and components Vacuum instrumentation Vacuum systems Uses of Vacuum in Microfabrication Rough Vacuum High Vacuum UltraHigh Vacuum wafer chucks evaporation surface analysis load locks ion implantation molecular beam epitaxy (MBE) sputtering reactive ion etching (RIE) low pressure chemical vapor deposition (LPCVD) Units of Pressure Measurement 1 atmosphere = 760 mm Hg = 760 torr 760,000 millitorr or microns 29.9213 in. Hg 14.6959 psi 1.01325 bar 1013.25 millibar 101,325 pascals (Pa) 407.189 in. H 2 O 33.9324 ft. H 2 O 1 Pascal = 1 N/m 2 1 Torr = 1 mm Hg 1 micron = 1 m Hg 760 mm Hg 33.93 ft H 2 O Vacuum Ranges Low or Rough Vacuum (LV) 760 to 103 torr High Vacuum (HV) 103 to 108 torr UltraHigh Vacuum (UHV) 108 to 1012 torr Partial Pressures of Gases in Air at STP Gas Symbol Volume Percent Partial Pressure, Torr Nitrogen N 2 78 593 Oxygen O 2 21 159 Argon Ar 0.93 7.1 Carbon Dioxide CO 2 0.03 0.25 Neon Ne 0.0018 1.4 x 102 Helium He 0.0005 4.0 x 103 Krypton Kr 0.0001 8.7 x 104 Hydrogen H 2 0.00005 4.0 x 104 Xenon Xe 0.0000087 6.6 x 105 Water H 2 O Variable 5 to 50, typ. Ideal Gas Law  1 V = volume of enclosure N = number of molecules N m = number of moles = N/N A n = particle density = N/V P = pressure T = absolute temperature k B = Boltzmanns constant = 1.381 x 1023 J/K N A = Avogadros number = 6.022 x 10 23 particles/mole R = Gas constant = N A k B = 8.315 J/moleK T nk P T Nk PV RT N PV B B m = = = Ideal Gas Law  2 Historical Laws: Boyles Law: P 1 V 1 = P 2 V 2 at constant T Charles Law: V 1 /T 1 = V 2 /T 2 at constant P GayLussacs Law: V = V (1 + T/ 273) Kinetic Gas Theory Velocity of a molecule is Mean square velocity is Pressure exerted on a wall in the xdirection is If velocities for all directions are distributed uniformly, Thus, Each molecular DOF has an average excitation of k B T/2. z v y v x v v z y x + + = r 2 2 2 2 z y x v v v v + + = 2 x x v nm P = 2 2 3 x v v = T nk v nm P B = = 2 3 1 T k v m B 2 3 2 2 1 = Distribution Functions  1 Boltzmanns postulates for an ideal gas: The number of molecules with xcomponents of velocity in the range of v x to v x + dv x is proportional to some function of v x 2 only: The distribution function for speed v must be the product of the individual and identical distribution functions for each velocity component: z z vz y y vy x x vx dv v N dN dv v N dN dv v N dN ) ( ) ( ) ( 2 2 2 = = = z y x z y x z y x vz vy vx dv dv dv v v v dv dv dv v N dN ) ( ) ( ) ( ) ( 2 2 2 2 , , = = Distribution Functions  2 A mathematical solution to the above equations has the form of ( A and v m are constants): Normalization of the distribution functions: 2 2 / 2 ) ( m x v v x Ae v = N v NA dv NAe dN m x v v vx...
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This note was uploaded on 11/16/2011 for the course MSE 5960 taught by Professor Douglas during the Fall '04 term at University of Florida.
 Fall '04
 Douglas

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