Final Exam Exam Test – Flashcards
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| 2 Types of Matter |
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| Pure & Mixtures |
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| 2 Types of Pure Substances |
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| Elements & Compounds |
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| 2 Types of Mixtures |
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| Homogenous & Heterogenous |
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| Physical Properties |
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| Anything observed without changing the substance or forming new substance |
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| Chemical Properties |
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| Observed through forming new substances |
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| A glass of milk souring is a _____ change? |
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| Chemical change |
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| A ice cube melting is a _____ change? |
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| physical |
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| Kilo- |
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| 10^3 |
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| Centi- |
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| 10^-2 |
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| Nano- |
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| 10^-9 |
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| Deci- |
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| 10^-1 |
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| Milli- |
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| 10^-3 |
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| Founder of Modern Atomic Theory. formed the atomic theory, which states that all matter is composed of tiny, indestructible particles called atoms that are all alike and have the same atomic weight. |
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| John Dalton |
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| JJ Thompson |
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| discovered the electron and developed the plum-pudding model of the atom. |
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| used the results of his gold-foil experiment to state that all the mass of an atom were in a small positively-charged ball at the center of the atom. |
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| Ernest Rutherford |
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| Father of modern chemistry. Law of Conservation of matter. |
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| Antoine Levoisier |
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| Aristotle's Atomic Theory |
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| Everything made of 4 elements: fire, water, earth and air |
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| Bond Involving electron sharing |
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| Covalent |
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| Bond involving electron transfer |
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| Ionic Bond |
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| Molar Mass |
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| Add g/mol |
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| Atomic weight |
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| amu |
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| % Composition |
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| Part/Whole * 100= ___% |
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| Empirical formula |
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| Simplest whole # ratio |
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| Steps of Stoichiometry |
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| 1. Bal Eqn 2. Convert moles (divide g by mm) 3. Compare moles given to moles unknown( unknown/given) 4. Convert to whatever |
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| (g)->moles |
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| Divide by mm |
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| moles->particles |
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| Multiply by Avogadro's # |
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| Precipitate Reaction |
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| Often involve Ionic Compounds X (aq)+ y(aq) -> Z(s)+A(aq) Z is precipitate Anions Pair with Cations Unsoluble is precipitate (see rules) |
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| Acid Base Rxn |
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| Forms salt and water |
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| LEO THE LION SAYS GER |
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| Loss electrons oxidation Gain electrons reduced |
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| Redox Rxns |
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| Electron transfer...follow oxidation rules given (not in a compound # is 0) |
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| Pressure |
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| =F/A |
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| Boyles Law |
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| As P increases V decreases (INVERSE) |
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| Charles Law |
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| as temp increases V increases |
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| Gay-Lusaac's Law |
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| As Temp increases P increases |
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| Ideal Gas Law |
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| PV=nRT P= Pressure, V=volume, T=Temp (Kelvins only), n=moles, R=0.0821 liter·atm/mol·K |
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| 1st Law of Thermodynamics |
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| ?E=work+heat loss |
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| Enthalpy |
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| Heat(Q) at constant P |
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| Calorimetry |
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| q=m.s?T q=heat, m=mass, s=specefic heat, ?T |
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| Wavelength Eqn |
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| c = ? ? f c=speed of light,?=wavelength, f=frequency |
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| Max Plank |
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| Said energy is Quantized |
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| Einstein |
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| e=mc^2 and photoelectric effect |
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| Neils Bohr |
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| Electrons orbit the nucleus |
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| Molarity |
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| moles of solute/L of solution or m=n/V (in L) |
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| Dilution |
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| Decreases concentration not moles |
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| Acid |
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| Proton Donator |
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| Base |
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| Proton Acceptor |
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| Salts |
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| Ionic compound of cation (NOT H) and anion (NOT OH- or O2-) |
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| Net Ionic Equation |
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| Then, you break apart the soluble molecules into the two ions that are formed (one positive and one negative). You will have to use the solubility rules to do this, they can be found online. If something is insoluble, it should not be broken apart. Write the reaction out with all of the separated ions. This is called the Total Ionic Equation. Then, you simplify by canceling things out if they appear on both sides of the reaction, resulting in the Net Ionic Equation. |
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| Ionic Compounds do/do not exist as gases |
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| Do not |
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| Normal Atmospheric Conditions |
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| 25 degrees C & 1 atm pressure |
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| Force |
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| Mass x Acceleration |
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| Pressure |
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| Force/ Area |
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| Manometer |
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| Used to measure pressure of gases other than atmospheres |
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| Plasma V Gas |
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| Charged / Not charged vol is not def / vol not definate compress / compress Move in straight lines like pong |
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| Molar Mass |
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| mass/mole M=m/n or rewritten as n=m/M |
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| PV=mRT/M |
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| Density= |
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| M/V |
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| m/v=PM/RT |
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| D=PM/RT |
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| 1 Mol of Gas at Rm Temp |
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| 22.4L |
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| Ideal Gas V Real |
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| M but not v / m & v dont attract or repulse / at high temps do not exhibit ideal behavior same as above/hi Pressure real gases attract |
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| Heat |
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| transfer of energy btw bodies |
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| Temperature |
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| Measure of av KE |
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| 1st law |
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| change in E equals work plus heat loss |
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| DeBroglie |
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| Waves can act like particles and particles like waves (Wave particle duality) |
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| Heisenberg |
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| Uncertainty of the position of a particle in time-photon can bump into it |
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| Schrodinger |
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| showed how particles transition from different waves, assigned quantum #s |
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| Quantum #s |
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| 1st tells main level, 2nd sub, 3rd Orbital, 4th Spin |
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| Mendelev |
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| varied rows with similar prop. in different lengths, leaving blanks for undiscovered elements. |
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| Newlands |
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| Created a 7x7 periodic table based on atomic mass not atomic # |
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| Alkaline elements |
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| 1st column except H |
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| Alkaline Earth |
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| Second column |
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| Halogens |
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| Second to last column 7a |
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| Noble Gas |
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| Last column |
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| Atomic # |
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| increases L to Right top to bottom |
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| Atomic radius |
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| Increases right to left top to bottom |
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| Ionization energy |
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| increases bottom to top and left to right |
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| Electronegativity |
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| Increases bottom to top and left to right |
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| Lattice energy |
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| Increases with charge (small distance is akin to higher lattive energy also) |
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| Single Covalent Bond |
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| Longest weakest |
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| Triple covalent bond |
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| shortest and strongest |
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| ABE |
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| A: Central B: Bond E: Lone pair |
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| Exceptions to the Octet Rule |
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| Having too few valence electrons to ever obtain an octet. Hydrogen, Beryllium and Boron have two few valence electrons to ever obtain a full octet. See this. Hydrogen can have at most 2 valence electrons after it shares its electron with another atom. Beryllium will have 4 valence electrons after it has finished bonding. Boron will have 6 valence electrons after it shares its valence electrons with other atoms. 2. Expanding the octet to have 10, 12 or 14 valence electrons instead of 8. elements in periods 3, 4, 5, 6 and 7 can expand their octet to have 10, 12, or 14 valence electrons. |
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| Nuclear Reactors |
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| Fission |
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| Hydrocarbons |
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| Hydrogen and carbon (exceptions: CO2, CO, CN-1, Carbonates, Bicarbonates, CO3-2, HCO3-) |
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| Alliphatic Hydrocarbons |
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| Alkanes, alkynes, cycloalkanes, alkenes |
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| Aromatic Hydrocarbons |
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| Moth balls (napthalene). Atleast 1 benzene ring C6H6 |
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| Alkanes |
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| single bond between C. CnH2n+2 |
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| Alkynes |
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| 1 triple bond btw carbon atoms. CnH2n-2 |
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| Cycloalkanes |
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| single bond between C atoms. CnH2n. ex butane in a ring is cyclobutane. |
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| Alkenes |
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| at least one dbl bond btw c. CnH2n |
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| Naming Alkanes |
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| Location-#of C+yl-Parent Name |
