Unit 2-Notes 2-At structure-1-1

Unit 2-Notes 2-At structure-1-1 - = c/ E = h c/ What is (...

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Keywords Atomic radius Ionic radius Ionization energy Acidic oxides Basic oxides Amphoteric oxides Thompson’s model Proton Electron Neutron Velocity of light Frequency Wavelength Wave number Emission spectrum Hydrogen spectrum Visible spectrum Balmer series Rydberg’ constant
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Atomic Radii
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Atomic radii of the elements
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We can see that ………………………………………………………………………………………… ……. .
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Compare the……………………………………………………………………… …………………
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oxides
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Thompson’s model of the atom
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What is velocity? ………………………………………………………………………. What is frequency? ………………………………………………………………………………………. .
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Important equations to remember E = h but
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Unformatted text preview: = c/ E = h c/ What is ( new bar ) = 1/ It is the number of waves in 1 cm What is the visible series? Balmer Series Photoelectric Effect E=hv--- Metal Surface- K.E. =1/2mv^2e-E= B.E. + K.E. Incident light energy binding energy kinetic energy of electron to surface of ejected electron Hv = hvo + 1/2mv^2 PROBLEM Photons of minimum nrg-496 KJ/Mole are required to ionize Na atoms. Calculate the lowest frequency of light and the highest wavelength of light that will ionize Na atoms If light of 600 kJ/mol was used, what would be the velocity of the emitted electrons? 1J=1kg m^2s^-2 Bohr Model (1913) Bohr-circular orbits of electrons around central nucleus of protons; quantization of orbital angular momentum principal quantum #, n. Mvr=nh/2pi Mvr = mass/velocity/radius...
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Unit 2-Notes 2-At structure-1-1 - = c/ E = h c/ What is (...

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