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by: Maya Silver-Isenstadt
Maya Silver-Isenstadt

GPA 4.0

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About this Document

These notes cover lecture notes AND notes from the textbook that were not directly touched on in discussion or lecture class.
Chemistry I - Fundamentals of General Chemistry
John Ondov
Class Notes
General Chemistry
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This 2 page Class Notes was uploaded by Maya Silver-Isenstadt on Friday September 9, 2016. The Class Notes belongs to CHEM131 at University of Maryland - College Park taught by John Ondov in Fall 2016. Since its upload, it has received 134 views. For similar materials see Chemistry I - Fundamentals of General Chemistry in Chemistry at University of Maryland - College Park.


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Date Created: 09/09/16
Chapter Two Continued   Significant Fi​ gures→ In multiplication/division, use the smallest number of significant figures in  the original problem for final answer rounding. In addition/subtraction, use fewest number of  decimal places given in original problem for final answer rounding.   ● Final answers MUST include 1) a sign 2) an amount 3) a unit 4) a label  ● Treat ALL units as separate entities​ and perform operations on them as any other number  ​ Mole→ ​Avogadro’s Number​. SI unit of substance. A mol contains approximately  6.02214*10^23 pieces.   Chapter Three  Properties of Light and Electrons  1) Both light and electrons have wave­like and particle­like properties  2) The Bohr model shows noncontinuous energy levels “orbitals”  3) Heisenberg Uncertainty principle states that one can know only the position of an  electron but not the speed or only the speed but not the position **Because atoms are  quantized, they simply appear on one energy level and then jump to another.​ There is no  inbetween state where an experimenter can track their movement.   4) Electromagnetic Radiation moves through space like kinetic energy. It uses waves. A  magnetic vector crosses an electric vector to transfer energy in a direction. ​**Waves  transfer energy NOT mass  ENERGY IS PROPORTIONAL TO FREQUENCY      Important Units!  1) Wavelength, λ , meters  2) Frequency , v, seconds  3) Velocity, C (constant) , meters/seconds ​*speed of light = 3.00e8 (m/s)  4)  Energy, E, Joules  Important Equations and Constants!  1) V=c/λ   2) E=hv *h is Plank’s constant = 6.626e­34(J*sec)  3) (1/λ )=R[(1/Nfinal^2)­(1/Ninital^2)] ​*R=1.0974e­7m​  ​Gives energy of emitted photon of  light when an electron switched orbitals.  4) E of emitted photon = ­hcR[(1/Nfinal^2)­(1/Ninital^2)]  5) mu^2=hu/λ ​*Gives wavelength of an electron­sized particle  Important Principles!  ● Heisenberg Uncertainty→ Th​e experimenter canNOT know both velocity and position of  an electron. One can NOT predict the trajectory of an electron.   ● Principal Quantum Number → determines size and energy of the orbital (n=1,2,3,...etc)  ● Angular Quantum Number → determines shape (any value of n­1) ex. n=2, l=1,0  ● Magnetic Quantum Number→ orientation of orbital  ● Spin → Electrons can only spin up or down and only with the value  .5  + −  


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