Chemistry
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| 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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Created by:
aperez48
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