Popular in Chemistry I - Fundamentals of General Chemistry
Popular in Chemistry
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→ The 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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