Chapter 6 Part 1 Structure of the atom
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1 Chapter 6 Part 1 Structure of the atom What IS the structure of an atom? What are the properties of atoms? REMEMBER: structure affects function! Important questions: Where are the electrons? What is the energy of an electron? Chapter 6 Part 1 Dual Nature of Light λν=c E = hν Line Spectrum Bohr Model of Hydrogen Atom Mary J. Bojan Chem 110 1
2 Why do we start with Chapter 6? Overview of Chem 110 Key themes: structure effects function (properties). How do we know about atoms, etc.? Structure of atom Ch. 6 Properties of Atom Ch. 7 How atoms bond to form molecules Ch. 8 Structure of molecules Ch. 9 Properties of molecules Ch. 10, 11, 13 Molecules REACT! Ch. 3, 4, 10 Rules that govern reactions Thermodynamics (think energy) Ch. 5 Equilibrium Ch. 15 Mary J. Bojan Chem 110 2
3 What is the structure of an ATOM? COMPONENTS OF ATOMS proton p electron e neutron n mass (a.m.u.) charge (a.u.) Neutral Ion 19 F 9 39 K 19 + Mary J. Bojan Chem 110 3
4 ISOTOPES Isotopes: atomic number =??? DEFINES identity of element For a given element, number of protons is fixed, but number of neutrons can vary. 35 Cl 37 Cl Mary J. Bojan Chem 110 4
5 We define: The Atomic Mass Scale mass of 12 C = exactly 12 amu. Use ISOTOPE RATIOS to find Average Atomic Masses Mary J. Bojan Chem 110 5
6 Another definition: The Atomic Mass Scale Problem: no one can see (or weigh) an atom 1 mole of 12 C has a mass of 12 g What is a mole? 1 mole of anything (atoms, molecules, green peas) = Avogadro s number of them How BIG is a mole? Mary J. Bojan Chem 110 6
7 The Mole and Avogadro s Number Mole: connection between microscopic (what we don t see: atoms) and macroscopic (what we see) Mary J. Bojan Chem 110 7
8 Back to the atom Mary J. Bojan Chem 110 8
9 Structure of Atom ~1910 Earnest Rutherford tested Thompson s plum pudding Model Rutherford concludes: massive nucleus with electrons orbiting around it. Mary J. Bojan Chem 110 9
10 Modern View of atom An atom is almost entirely empty space. 1nm = 10-9 m 10Å = 1nm Å= angstrom Atom Diameter = nm Nuclear diameter = 10-5 nm Atom diameter = 10,000 x nuclear diameter Mary J. Bojan Chem
11 study of light interacting with matter WHAT IS LIGHT???? Mary J. Bojan Chem
12 Electromagnetic radiation What KIND of energy? kinetic or potential What is moving? What are the units of energy????? Mary J. Bojan Chem
13 Electromagnetic radiation (light) Light behaves as a wave! c = 3.00x10 +8 m/s for light λ = wavelength ν = frequency c = λν Mary J. Bojan Chem
14 Electromagnetic radiation What is the range (wavelengths) of visible light? Does uv light have longer or shorter λ than visible? Rank the following ranges of light in order of increasing λ. uv, ir, visible, microwave What is the frequency of light if λ = 450nm? c = λν c = 3.00x10 +8 m/s for light What has a higher frequency? a) visible light (λ = 640nm) b) microwaves (λ = 600cm) Mary J. Bojan Chem
15 Electromagnetic Spectrum Regions of EM spectrum gamma X-Ray ultraviolet visible infrared microwave radio Common use? Dangerous or not??? Mary J. Bojan Chem
16 Light behaves as a wave! Or does it??? Several phenomena were inconsistent with the wave nature of light. Blackbody radiation Photoelectric effect Line spectrum of atoms Black body radiation Planck shows: E= nhν n = integer ν = frequency of emitted light h = Planck s constant = J-s Energy = hν photon energy frequency of photon Mary J. Bojan Chem
17 Photon energy What is the energy of a green photon (wavelength equal to 523 nm)? J J J J J Mary J. Bojan Chem
18 Spectroscopy: light interacting with matter λ Energy Interaction with matter gamma X-Ray ultraviolet visible infrared microwave radio Mary J. Bojan Chem
19 Is light emitted or absorbed? How do I know? We need a brief excursion into Chapter 5 Mary J. Bojan Chem
20 First Law of Thermodynamics Energy can be converted from one form to another, but the total energy Law of conservation of energy all energy lost by a system under observation must be gained by the surroundings (and vice versa) *during energy conversion, some heat is always produced" Mary J. Bojan Chem
21 Internal Energy Internal energy: total energy (E) associated with a system; the sum of all sources of kinetic & potential energy. " The capacity to do work or transfer heat.! Quantitative definition:" ΔE = E final E initial " ΔE = q + w" Mary J. Bojan Chem
22 Which has more energy? E is a state function (path independent)" Mary J. Bojan Chem
23 Exothermic and Endothermic ENTHALPY: Heat transferred when P is constant ΔH (=q p ) Usually run chemical reactions at constant pressure (atmospheric). Exothermic: heat System Surroundings ΔH = Endothermic heat Surroundings System ΔH = + Mary J. Bojan Chem
24 What you need to know from Chapter 5 Difference between kinetic and potential energy (can you make up your own examples?) Know units of energy and order of magnitude of different kinds of energies (photon energy, etc.) Be watching for electronic energy, i.e., the energy of an electron. What is the First Law of Thermodynamics? Watch for how the potential energy of electrons gets converted to kinetic energy (a photon). What is meant by the system? The surroundings? What does the sign of energy mean? + means energy into the system (endothermic) means energy out of the system (exothermic) Notice State functions (like P, T V) as we encounter them and keep the definition of state function in mind. Why is it useful to know that these are state functions? Remember that Enthalpy is another word for heat: specifically it is an heat measured when the system is at constant pressure, but for now, just know that it is a form of energy (heat). Mary J. Bojan Chem
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Particle nature of light & Quantization A quantity is quantized if its possible values are limited to a discrete set. An example from classical physics is the allowed frequencies of standing waves on a