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Chapter 5 Review Wave Nature of Light WavelengthThe distance between two consecutive peaks or troughs. FrequencyThe number of waves that pass a point each second (the unit is the Hertz, Hz). One complete wave or cycle per. second = 1 Hz. VelocityDistance a peak moves in a unit of time. Particle Nature of Light PHOTOELECTRIC EFFECT When light shines on certain metals an electric current is produced (electrons are emitted from the metal). Not explained by the wave theory of light… Light is thought of as a stream of particles called… Bohr’s Model absorbs energy electron ‘jumps’ to a higher energy level (orbit). Atom Electron ‘jumps’ to a lower orbit energy released (photon). Energy difference between the two orbits energy of the photon The color (frequency) of light produced E = h f Bohr’s Shortcomings Quantized energy levels were not immediately accepted by other scientists (though correct) Worked for hydrogen but not for other elements with more electrons. Heisenberg Uncertainty Principle It is impossible to determine simultaneously the position and velocity of an electron or any other particle. Orbital A three dimensional region around the nucleus that indicates the most probable location of the electron. Quantum Numbers Describe the properties of atomic orbitals and the electrons that occupy them… Quantum Number Describes Principle main E. level Angular Momentum - shape of Orbital Magnetic orientation of orbital Spin orientation of electron Rules for Writing e- configurations An electron occupies the lowest energy orbital that can receive it…(like filling a glass) If two electrons occupy the same orbital they must have opposite spins! Orbitals of equal energy are each occupied by one electron before any orbital is occupied by a second electron. 1S2 2S2 2P2 What do the symbols represent? Write Orbital notation for Nitrogen Electron configuration for: Ne 1S2 2S22P6 Nobel Gas Notation for: Aluminum Al [Ne] 3S2 3P1 How does the arrangement of electrons relate to an elements position on the periodic table? ….where would find an element with an outermost energy level like this 4S24P4 ? Calculate Frequency and energy Wavelength = 4.5 x 10-7 meters Region outside of nucleus where an electron can most probably be found Orbital An electron in the lowest possible energy level said to be in it’s Ground state When an electron absorbs energy it will be in… An excited state A photon is released when an electron moves from Excited state to ground state A quantum of electromagnetic energy is a Photon How does an orbit differ from an orbital? Orbitals do not show the exact location or path of an electron… only the probable location It is not possible to know the precise location and velocity of an electron or other small particle (“what is…”) Heisenberg uncertainty principle Indicates the main energy level of an orbital or electron Principle quantum number An electron at main energy level 5 has more ___ than an electron at main energy level 2 Energy Dumbell-shaped set of 3 orbitals P ORBITALS Indicates the orientation of the orbital with regard to a three dimensional axis Magnetic quantum number A spherical electron cloud S orbital The difference between a 2S orbital and a 3S orbital Distance from nucleus or energy level An electron occupies the lowest energy orbital that can receive it Aufbau principle Orbitals of equal energy are each occupied by one electron before any is occupied by a second electron. Hund’s Rule Two electrons in the same orbital must have opposite spins Pauli exclusion principle The Bohr model was an attempt to explain what about hydrogen Bright line or line emission spectrum The number of electrons in the highest occupied energy level of argon (a noble gas) 8 The distance between successive peaks on a wave wavelength