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How is an electron able to change energy levels? Day 1 1-7 Objective / Essential Question How do we define / describe an electron’s location in the atom? Notes Revisiting the Electron Cloud Page 7 Electron Position: probability orbitals uncertainty Electron Distribution element Properties of How can the whereabouts of an electron compare to an apartment building? Floor/story of building Energy level Sublevel Suite/apartment Orbital for e- couple Bedroom Spin Female / Male The Address of the Electrons Just like people in an apartment, electrons have an address. The most probable location of an electron is described using quantum numbers. Each electron has 4 quantum numbers which each relays a different piece of information about the electron’s possible whereabouts in the atom. The Address of the Electrons Pauli exclusion- no 2 electrons can have the same address!!! – same 4 quantum numbers Describing Atomic Structure Energy level – regions of space where there is a high probability of finding electrons Energy levels - break into - Sublevels - break into Orbitals Describing Atomic Structure Sublevels 3 2 1 First sublevel – 2 electrons Second sublevel – 6 electrons Third sublevel – 10 electrons Describing Atomic Structure – Building an Address Energy levels – designated by - # 1st Level = 1, 2nd Level = 2, etc. … Sublevels – designated by – letter (s, p, d, f) 1st Sublevel = s 2nd Sublevel = p 3rd Sublevel = d 4th Sublevel = f Describing Atomic Structure # of energy level = # of sublevels in that energy level Energy level 1 = 1 sublevel Energy level 2 = 2 sublevels Energy level 3 = 3 sublevels … Describing Atomic Structure E n e r g y Sublevels f d p s Energy still Increases away from the nucleus Day 2 1-8 1. Why is it impossible to determine the speed and location of an electron at the same time? The New Atom? Do you think Bohr was right or wrong? Pauli exclusion? Energy levels - break into Sublevels - break into - Orbitals Electron Arrangement Energy level 1, sublevel s, orbital 1s 2 1 3 Energy level 2, has two sublevels s and p, 2s orbital and 2p orbitals Energy level 3, 3 sublevels s, p, and d, 3s orbital, 3p orbitals, and 3d orbitals Electron Arrangement Quantum #s – specify the properties of atomic orbitals and the properties of electrons in those orbitals Principle quantum # (n) – main energy level = 1, 2, 3… Angular momentum quantum # (l) – shape of the orbital = 0, 1, 2… (n-1) 0 = s, 1 = p, 2 = d, 3 = f Magnetic quantum # (ml) – orientation of the orbital around the nucleus Electron Arrangement Quantum #s – specify the properties of atomic orbitals and the properties of electrons in those orbitals Magnetic quantum # (ml) – orientation of the orbital around the nucleus Spin quantum # – indicate the two possible spin states (+1/2, -1/2) Electron Arrangement Energy levels – designated by - # (n the principle quantum #) s=0 p=1 d=2 f=3 E n e r g y Sublevels – designated by – letter (s, p, d, f) (l the angular momentum quantum #) Energy still Increases away from the nucleus Electron Arrangement How many electrons in an orbital? 2 electrons fit in an orbital one spinning in the +1/2 orientation and one spinning in the -1/2 orientation 1. What is an atomic emission spectra (use your lab handout if necessary)? Day 3 1-11 NO ATB today. Sit with your partner(s) for lab and get out your lab. Wait for instructions. Day 5 1-13 LAB Day 3 111 Day 4 112 Day 6 113 Quantum Theory Quanta’s Ability: Light energy hits the electrons in metal- the light must be powerful enough. Electrons in the metal absorb the energy. The electrons become excited, and they jump out of the metal. Quantum Theory The electrons become excited, and they jump out of the metal. The electrons fall down again, and create a spark or current. Examples: The luster of a shiny metal, Photoelectric cells (solar power) Q of the Day 1. How many electrons fit in an orbital? How is their movement different (from each other)? Day 1 1-15 Q of the Day 1. How many sig figs: 4020 4020.00 0.004020 Day 2 1-19 Q of the Day 1. There are 4 quantum numbers for each electron. Each one tells you something about the electron’s location within the atom. What do they tell you? Energy level, sublevel, orbital, spin Day 4 1-21 Electron Arrangement How many orbitals in each sublevel? s=1 p=3 d=5 f=7 Electron Arrangement How many sublevels in each energy level? 1 = _____ (__) 3 2 = _____ (____) 3 = _____ (______) 4 = _____ (__________) 2 1 Electron Arrangement 4 xx xx xx xx xx xx xx xx xx 3 xx xx xx xx xx xx xx xx xx 2 xx xx xx xx d xx xx xx xx xx xx xx f p 1 xx s Each x = an electron Each xx = an orbital Review Energy levels number Sublevel letter s, p, d, f Taking a Look at Orbitals S D P Notes Page 10 Taking a Look at Orbitals Taking a Look at Orbitals p – orbitals always occur in 3’s (one for each dimension) Q of the Day 1. Get out your electron acrostic from yesterday. You have 2 minutes to finish!!! Today’s ATB = What shape is an s sublevel? What shape is a p sublevel? Day 5 1-22 Electron Acrostic E L E C T R O N Electron Arrangement Recall that atoms like to stay in their most stable (lowest energy) state. - Sublevels fill from the nucleus outward 3 2 1 Electron Arrangement Recall that atoms like to stay in their most stable (lowest energy) state = electron configuration electron configuration – notation used to show electron placement within sublevels Electron Arrangement electron configuration – notation used to show electron placement within orbitals electron Configuration for: Si 1s22s22p63s23p2 C 1s22s22p2 Electron Configurations Practice: S 1s22s22p63s23p4 F 1s22s22p5 1s22s22p63s23p3 P http://www.youtube.com/watch?v=Vb6kAxwSWgU http://www.youtube.com/watch?v=rcKilE9CdaA The most likely location of an electron is described by a wave of probability. This type of wave is actually a set pattern that forms a 3-D shape within the space of the atom. This wave pattern does not overlap itself and is known as a standing wave. http://www.youtube.com/watch?v=-gr7KmTOrx0 http://www.youtube.com/watch?v=3BN5-JSsu_4 http://www.youtube.com/watch?v=18BL7MKjtZM Define: quantized Plank’s constant wavelength Bohr electron cloud model excited state radiant energy electromagnetic radiation Speed of light Objective / Essential Question How do we define / describe an electron’s location in the atom? Quick Talk Ground state radiant energy Bohr photon frequency Compton quanta excited state continuous particle or wave Electron Acrostic E L E C T R O N Electron Acrostic E L E C T R O N Element Mn C Electron Configuration Noble Gas Notation # of Valence electrons