Atomic Structure and Periodicity
Quiz yourself by thinking what should be in
each of the black spaces below before clicking
on it to display the answer.
Help!
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| Light | electric and magnetic field through space.
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| Light | fields are perpendicular to each other and direction of the magnetic field is determined by the right hand rule
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| Visible light | 10^14
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| Microwaves | 10^9-10^12
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| Frequency Cycles | 10^6 -short waves,10^8-TV,infared,visible, UV=10^14, x ray=10^18, gamma rays
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| wavelength (upside down y) | distance on a wave from crest to crest
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| Frequency (v) | the number of complete waves passing through a point in a given amount of time. Higher frequency is higher energy.
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| Hertz | the unit of measure which is waves per second
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| Amplitude | the height or intensity of the wave
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| Nodes | point in the wave where the intensity is equal to zero over ever 1/2 (upside down y)
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| Traveling Waves | like at a football game
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| Transverse Wave | a compression wave = sound
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| Standing or Stationary Wave | similar to two people holding a jump rope in two stationary positions
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| Plank Equation (E=h v) | energy is quantized, energy comes in packets. A packet called a photon.
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| E = hv | E= hv=[(h)(c/wavelength)
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| Velocity | (frequency)(wavelength),,,,,C=v(wavelength)...c=2.9x10^8.
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| E= units (J sec) | h=6.62x10^-34
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| Atomic Line Spectra | Excitation of elements will give rise to line spectra or spectra of various ranges much like red is not observed in a sodium vapor lamp
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| (A)E =Efinal - Eintial | En=R(h)c/n^2....n is principal quantum number,shell...R=2.179e-18 J/atom
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| Quantum Mechanical Principle a. Heisenberg Uncertainty Principle | states that it is impossible to determine both the position and the momentum of the electron with comple accuracy
orbitals describe the probability of finging an electron in a particular region of space rather than its exact location
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| Quantum Mechanical Principle b. Pauli Exclusion Principle | States that no two electrons in an atom can have the same four quantum numbers
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| Quantum Mechanical Principle c. Hund's Rule | states that electrons prefer to occupy different orbitals and have a parallel spin rather than pair up in the same orbital and have opposite spins. Electrons will fill a subshell with parallel spins before pairing up
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| Hund's Rule | diamagnetism and paramagnetism
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| Atomic Radius | is equal to one-half the distance between the centers of two atoms of that element that are just touching each other. decreases from left to right, increases from top to bottom
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| Hybridization | formation of a set of hybrid orbitals with favorable directional characteristics by mixing together two or more valence orbitals of the same atom
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| Ionization Energy | energy required to completely remove an electron from a gases atom or ion
increases from left to right, decreases from top to bottom
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| Electron Affinity | energy change that occurs when an electron is added to a gaseous atom, and it represents the ease with which the atom can accept an electron. The stronger the attractive pull of the nucleus for electrons, the greater the electron affinity will be.
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| Electronegativity | measure of the attraction an atom has for the electrons in a chemical bond. THe greater the electronegativity, the greater its attraction to bonding elements.
Increases from left to right, decreases from top to bottom
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