Test Answers on Exam 1 – Chemistry – Flashcards
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| Speed of Light |
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| c= 3.00*108m/s |
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| C=lambda*frequency |
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| wavelength*frequency=speed |
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| Gamma Rays |
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| 400mm and violet |
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| Radio Waves |
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| 700mm and red |
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| Nanometers |
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| 10-9 |
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| Blackbody Radiation |
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| when a solid is heated it emits electromagnetic radiation |
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| E=hv |
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| amount of energy emitted. planks constant and the frequency. |
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| Ephoton=hv |
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| Einstein's theory photoelectric effect |
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| Rydberg equation |
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1/lambda=Rinifinity(1/nf2-1/ni2) Rinifinity=1.097*107m-1 |
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| Ground State |
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| lowest energyt state of an atom |
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| ;E=Ef-Ei |
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Ef=-2.18*10-18J(1/nf2) same for Ei |
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| ;=h/mu |
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| wavelength =6.63*10-34 divide by (mass*velocity) |
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| Principal Quantum Number |
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| Designates the size of the particular orbital. The larger the "n" is the greater the average distance of an electron in the orbital from the nucleus. |
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| Angular Momentum Quantum Number |
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describes the shape of the atomic orbital. L=n-1 Ex. N=2 L=1,0 |
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| Magnetic Quantum Number |
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describes the orientation of the orbital in space. Within a subshell the value of ml depends on the value of L. ml=(2l+1) Ex. L=2 ;ml=-1,0,1 |
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| Pauli Exclusion Principle |
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| No two electrons in an atom can have the same four quantum numbers! |
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| The Aufbau Principle |
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| fill lowest shells first. |
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| Hund's Rule |
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| fill across with same charge. |
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| Quantum L |
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L=0=s L=1=p L=2=d L=3=f |
