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ChemT3
Chemistry Test
| Question | Answer |
|---|---|
| Two types of magnetism | Diamagnetic and Paramagnetic |
| Diamagnetic | All electrongs are paired up,down |
| Paramagnetic | Unpaired electrons |
| Values of S,P,D | 0,1,2 |
| 4 Quantum #'s | n,l,ml,ms |
| n | Primary quatum # deal w/ energy lvl |
| l | Deals w/ the shape of the orbital (s,p,d,f) |
| ml | Deals with the orientation 1s,3p,5d,7f |
| s | Deals with the spin +1/2 or -1/2 |
| Exceptions to AuFBau | Cr,Cu,Mo,Ag |
| Electron Affinity | x + e- --> x- Best for lvl 17. Peaks a 1,14,17. |
| Ionization Engery | M --> M+ + e Best for group 1. Minor peaks at 2,15 |
| Periodic Properties | Atomic Size, Ionic Size, Electron Affinity, and Ionization Energy |
| Bohr Harbor Cycle | Sublimation + Ionization energy + 1/2 bond energy + Electron Affinity + Lattice energy = Overall Delta H |
| Exception to Lewis 8e Rule | 6e, 10e, 12e, Odd #'s of e |
| Isoelectronic Series | -2,-1,0,+1,+2 |
| Calculating # Bonds | E have (8 X # Atoms) - ehave(Group #-10 & correct for charge) / 2 |
| Formal Charge | Group # - 10 - (# Bonds) - (# of electrons) |
| Electronegativity | Increase up and to the right. |
| Ionice size | Increase down and to the left. Postive ions are smaller than neutral ions. Negative ions are larger than neutral ion. |
| Ionic Bond | Greater than 1.5 |
| Polar Covalent Bond | Btwn .5 and 1.5 |
| Pure Covalent | Less than .5 |
| Schrodinger | Led to the theory of quantum physics |
| Lyman | 1 Ultraviolet |
| Balmer | 2 Visible and Untraviolet |
| Paschen | 3 Infrared |
| Brackett | 4 Infrared |
| JJ Thomson | Measured e/m ration of electron/proton |
| Millikan | Oil drop experiment measures e |
| Davisson & Germer | Mass of a nuetron AMU |
| Rutherfordy | Gold foil experiment. Led to planitary model. |
| Bohr | Model of e. Explain H. Calculates emission spectrum of H. |
| Einstein | Photoelectric effect light ---> pariticles and waves |
| Rydberg | Study emission spectrum of H. Led to Rydber constant. |
| C degree to Kelvin= | (C+ 273.15)=K |
| C to F | (1.8 x C)+ 32 F |
| Avagardo's Number | 6.022 x 10^23 |
| # of moles of an element | # grams have / AMU of element |
| Molecular weight | Atomic mass of each atom added together. |
| a b NI C | # of protons = b # of netrons = a-b # of electrons = b while correcting for C(the charge) |
| Group 1 , Group 2, Group 16, Group 17, Group 18 | 1 Alikali Metals, 2 Alkaline Earth, 16 Chalcogens, 17 Halogens, 18 Noble Gas |
| S, D, P, F | S(1,2); D(3-12); P(13-18); F(lower two) |
| Lanthanides | First row of F |
| Actinides | Second row of F |
| isotope | Same # of protons but different # of neutrons |
| nano- | 10^-9 |
| pico- | 10^-12 |
| micro- | 10^-6 |
| milli- | 10^-3 |
| centi- | 10^-2 |
| deci- | 10^-1 |
| tera- | 10^12 |
| giga- | 10^9 |
| mega- | 10^6 |
| kilo- | 10^3 |
| % yield | actual yield/ theoretical yield |
| Boyles Law | PV=nRT |
| Gas constant | R= .08206 |
| Titration | CV=CV |
| Molarity | Moles/Liter(M=n/V) |
| Charles Law | P1V1/T1 = P2V2/T2 |
| A gas is most ideal under... | High pressure and low temperature |
| Stoichiometry | moles of what u have x want/have x grams of what u want |
| Dalton's Law | Pi=XiPt |
| Endothermic reaction | absorbs heat, temperature decreases, sign is + |
| Exothermic reaction | gives off heat, temperature rises, sign is - |
| A bomb calorimeter measures | Delta E |
| A cup calorimeter measures | Delta H |
| Delta E = | q + w |
Created by:
hermis1986
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