Chemistry Chapter 1 Test Questions – Flashcards
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| solid |
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| rigid, incompressible (can't manipulate volume), fixed shape and volume ex: ice |
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| liquid |
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| relatively incompressible fluid (fluid: no fixed shape, flows), fixed volume, no fixed shape ex: water |
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| gas |
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| easily compressible (compressible: volume can be manipulated) fluid (fluid: no fixed shape, flows), sample will fit into container of any size or shape; no fixed volume or shape ex: steam |
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| physical change/ change of state |
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| change in the form of matter but not in the chemical identity ex: change of state (melt ice, boil water) dissolution (dissolving kool aid powder in water) distillation (moon shine; boil mixture, it vaporizes, encounters a condensor, condenses back to liquid, is collected in a receiver) |
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| chemical change/reaction |
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| change in which one or more kinds or matter are transformed into a new kind of matter or several new kinds of matter ex: 2Na+ Cl --> 2NaCl |
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| test for chemical versus physical change |
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| original components cannot be reclaimed by physical means (chemical reaction; ex: bake a cake, if you freeze it, it wont turn back into the chocolate, flour, ect. you put in) original components can be reclaimed by physical means (physical change; ex: had ice, melted it, can freeze it to restore it to original state) |
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| substances |
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| cannot use physical means to separate into other kinds of matter possesses definitie intensive (independent of amount) physical and chemical properties ex: color |
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| elements |
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| cannot be decomposed by any chemical means into simpler substances; building blocks of matter ex: K, Cl, Na, O, ect. |
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| Who receives credit for the periodic table? |
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| Dmitri Mendeleev (1869) |
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| how did Mendeleev arrange the periodic table |
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| increasing atomic weight |
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| how is the periodic table arranged today? |
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| increasing atomic number |
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| atomic number |
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| number of protons in nucleus; chemical identity is linked to the number of protons ex: add a proton to Na and it becomes Mg |
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| symbol: H |
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| hydrogen |
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| symbol: He |
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| Helium |
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| symbol: Li |
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| Lithium |
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| Symbol: Be |
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| Beryllium |
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| symbol: B |
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| Boron |
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| Symbol: C |
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| Carbon |
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| symbol: N |
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| nitrogen |
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| symbol: O |
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| oxygen |
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| symbol: F |
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| Fluorine |
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| symbol: Ne |
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| neon |
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| symbol: Na |
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| sodium |
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| symbol: Mg |
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| magnesium |
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| symbol: K |
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| potassium |
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| symbol: Ca |
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| calcium |
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| symbol: Sc |
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| scandium |
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| symbol: Ti |
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| titanium |
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| symbol: V |
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| vanadium |
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| symbol: Cr |
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| chromium |
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| symbol: Mn |
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| manganese |
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| symbol: Fe |
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| iron |
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| symbol: Co |
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| cobalt |
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| Ni |
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| nickel |
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| Cu |
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| copper |
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| Zn |
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| zinc |
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| Ga |
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| gallium |
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| Ge |
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| Germanium |
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| As |
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| arsenic |
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| Se |
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| Selenium |
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| Br |
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| bromine |
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| Kr |
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| krypton |
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| Rb |
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| Rubidium |
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| Sr |
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| Strontium |
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| Cd |
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| cadmium |
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| In |
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| Indium |
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| Sn |
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| Tin |
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| Sb |
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| Antimony |
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| Te |
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| Tellurium |
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| I |
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| iodine |
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| Xe |
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| Xenon |
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| Cs |
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| Caesium |
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| Ba |
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| Barium |
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| Hg |
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| mercury |
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| Ti |
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| Thallium |
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| Pb |
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| lead |
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| Bi |
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| Bismuth |
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| Po |
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| Polonium |
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| At |
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| Astatine |
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| Rn |
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| Radon |
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| Fr |
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| Francium |
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| Ra |
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| Radium |
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| metals |
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| substance or mixture characterized by luster (shine) and generally a good conductor of heat and electricity most solid at room temp, except for Hg malleable ( hammered into a shape; changable) and ductile (drawn into wire; not brittle) |
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| nonmetals |
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| element that doesn't exhibit characteristics of a metal most are gases (ex: N, O) or solids (ex: P, S) solids are hard and brittle (shatter when hit) only liquid nonmetal at room temperature is Br) |
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| metalloids/ semimetals |
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| elements possessing both metallic and nonmetallic properties; properties depend on what they react with (react w/ metal, acts as nonmetal, vice versa) ex: Si and Ge (semiconductors) when pure, poor conductors of electricity; when doped (impure), or at high temps, become good conductors of electricity |
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| properties of matter (4) |
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| physical, extensive, intensive, chemical |
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| physical property |
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| characteristic of material that can be observed without altering its chemical identity (ex: color, mass, density, state) |
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| extensive property |
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| dependent on amount ex: mass |
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| intensive property |
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| independent of amount ex: color |
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| chemical property |
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| characteristic of material involving its chemical change reactivity (how much it reacts) |
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| le systeme international d'unites |
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| SI units common/ standard units |
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| SI base units: quantity: Length unit? symbol? |
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| meter m |
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| mass |
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| kilogram (often use gram) kg (g) |
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| time |
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| second s |
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| temperature |
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| kelvin K |
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| amount of substance |
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| mole mol |
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| SI Prefixes: Multiple: 10^6 prefix? symbol? |
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| mega M |
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| 10^3 |
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| kilo k |
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| 10^-1 |
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| deci d |
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| 10^-2 |
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| centi c |
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| 10^-3 |
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| milli m |
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| 10^-6 |
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| micro U (mu) |
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| 10^-9 |
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| nano n |
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| 10^-12 |
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| pico p |
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| how do you use SI prefixes? what do they indicate? |
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| augment base units with prefixes prefixes indicate the power of 10 that you multiply the base unti by ex: kg= 10^3g= 1,000g |
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| celsius scale: bp of water? fp of water? |
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| bp: 100 C fp: 0 C |
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| Kelvin scale: lowest theoretical temp? h2O fp? h2O bp? |
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| lowest: 0 K fp: 273 K bp: 373 K |
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| fahrenheit scale h2O fp? h2o bp? |
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| fp: 32 F bp: 212 F |
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| temp conversions celsius to Kelvin |
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| tk = tc + 273.15 |
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| temp conversion: C to F |
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| tf = (9/5) tc -32 |
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| temp conversion: F to C |
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| tc = (5/9) tf -32 |
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| temp conversion: K to C |
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| tc= tk - 273.15 |
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| volume units length x length x length |
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| m^3 = 1,000 L 1L = dm^3 = 10^3 cm^3 1 cm^3 = cc= 1 mL |
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| units of speed |
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| m/sec |
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| density formula? density formula units? |
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| d= m/V units: g/cm^3 ex: H2O d=1g/cm^3 |
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| relative densities: density generally ______ as you change from solid to liquid to gas exception? |
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| density generally DECREASES as you change from solid to liquid to gas exception: H2O; ice (0.92 g/cm^3), water (1 g/cm^3), gas (6x10^-4 g/cm^3) |
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| what's energy? |
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| "the potential or capacity to do work or heat transfer" |
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| formula for work |
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| w=F x d work = force x distance |
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| units of energy? (unit of energy, work, heat) |
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| the Joule: 1J = (1kg*m^2)/s^2 |
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| whats a calorie? |
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| the energy required to raise the temperature of 1g of H2O by 1 degree C 1 cal = 4.184 J |
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| types of energy KE |
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| Kinetic energy = 1/2 mass * velocity squared KE = 1/2 mv^2 energy of an object by virtue of its motion |
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| Potential energy |
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| potential energy of an object by virtue of its position in a field of force ex: gravity --> PE=mgh |
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| internal energy |
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| U = KE + PE |
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| total energy |
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| Etotal = KE + PE= U |
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| all types of energy (KE,PE,U,E total) are relative values based on______ |
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| a reference point ex: the floor for PE; 0 velocity for KE |
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| Deriver units: Area |
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| m^2 |
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| volume |
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| m^3 |
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| density |
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| kg/m^3 |
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