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Chemistry

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Question
Answer
show 6.022X10^23  
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show protons+neutrons  
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charge of electron   show
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show # protons=#electrons unless it's charged  
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show #neutrons change so mass changes but atomic #same  
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show - charge, closer to nucleus the lower energy level, less interaction w/environment  
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cation   show
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anion   show
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valence e-   show
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Plancks quantum theory   show
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Bohr Model   show
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show E=-Rh/n^2=-Rh(1/n^2initial-1/n^2final) E=- absorption E=+ emission E↑ negativity↓ n↑ e- goes from lower level to higher they AHED: Absorb light, Higher potential, Excited, Distant from nucleus  
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show E=hf=hc/wavelength  
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Lyman Series   show
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Balmer Series   show
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Paschen Series   show
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Absorption   show
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show uncertainty of position of a particle and it's momentum. You can know position but not momentum and vice versa ▲x▲p≥h/2  
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show No two e- in the same atom can have same four quantum #'s  
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show #1 principle (n) (1,2,3..) shell (energy level, # of period # on periodic table) #2 azimuthal (l) (0,1..(n-1)) subshell: s L=0; p L=1; d L=2; f L=3 #3 magnetic (ml) (-L to L) orbital: px;py;pz #4 spin (ms) (-1/2, +1/2) spin (↑↓)  
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Quantum number equation   show
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show each new proton added creates new element and each new e- occupies lowest energy level (n) BOWLOW stability ↑ fill lowest n level with n+l if same pick lowest n  
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Electron configuration   show
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show Exception: Half & completely filled subshell preferred Ex: Cr: [Ar]4s23d4→[Ar]4s3d5 Anion: move toward RIGHT of element Cation: move toward LEFT of element Ex: [Br-]: [Ar]4s2 3d10 4p6  
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Hund's Rule   show
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Paramagnetic   show
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Diamagnetic   show
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Periodic table trends   show
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Chemical properties of Periodic Table   show
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Atomic Radius   show
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Electrostatic force   show
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show Amount of charge felt by most recently added e- ↑Zeff←(L to R) ↓Top to bottom ↓shielding  
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show Energy required to detach an e- from atom ↑IE→(L to R)↑Bottom to top Why? e- are closer to nucleus  
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First vs Second IE   show
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show Tendency of atom to attract e- shared in covalent bond The LARGER the diff b/w electronegativities the LARGER the polarity so ↑attraction  
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Electron Affinity   show
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octet rule   show
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show 1) Find total # of valence e- for all atoms 2)Use pair of e- to form single bonds 3) arrange remaining e- into lone pairs &double or triple bond to satisfy duet/octet rule Total # e-=Σvalence e-  
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show VE-(Nnonbonding (dots)+ 1/2Nbonding (sticks))  
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Bond ranking   show
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show -covalent bond where valence e- are transferred to one atom (unequal sharing) creating polarity -most enegative atom attracts e- -b/w metal &nonmetal -High melting pt -soluble in H2O & insoluble in nonpolar conducts electricity in aqueous soln  
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show -valence e- are shared equally -similar enegativities -soluble in nonpolar -insoluble in H2O -low melting pt and boiling pt -nonconductor of heat & electricity  
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show occur when (+) charge center is not same as (-) charge so e- are pulled to one side  
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show -determined by geometry of molecule (due to dipole orientation)  
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Intermolecular attraction Types   show
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London Forces   show
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Hydrogen bond   show
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Dipole-Dipole   show
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Induced Dipole   show
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show arise spontaneously in non-polar molecule Why? -e- move around & become uneven create dipole in neighboring atoms  
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Bond Length   show
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Bond Energy (Bond Dissociation Energy   show
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show Bond Length: single bond >double bond>triple bond Bond Strength: single<double<triple Bond Energy: single<double<triple  
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show sigma bond: bounding pair of e- found in space b/w bonding atoms Lowest Energy; Strongest Most Stable pi bond: overlapping p orbitals, More Reactive ↑s character↓bond length↑bond strength↑bond energy↑stability sp (50:50)>sp2(33:66)>sp3(25:75)  
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Aromaticity &Huckel Rule   show
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Resonance Structure   show
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Fisher Projection   show
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Newman Projection   show
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Valence Shell Electron Pair Repulsion(VSEPR) Geometry Linear (sp) & Trigonal planar (sp2)   show
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show [#bonds=4][#lone pairs=0] tetrahedral AX4 [#bonds=3][#lone pairs=1] trigonal pyramidal AX3E1 [#bonds=2][#lone pairs=2] bent AX2E2  
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Valence Shell Electron Pair Repulsion(VSEPR) Geometry Trigonal bipyramidal (sp3d)   show
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show [#bonds=6][#lone pairs=0] octahedral AX6E0 [#bonds=5][#lone pairs=1] square pyramidal AX5E1 [#bonds=4][#lone pairs=2] square planar AX4E2 [#bonds=3][#lone pairs=3] Tshaped AX3E3 [#bonds=2][#lone pairs=4] linear AX2E4  
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