Chapter 1 form chem 1303 – Flashcards
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| Chemistry |
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| The study of matter and changes it undergoes |
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| macroscopic |
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| things we can touch (seen by naked eye) |
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| microscopic |
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| things we can imagine and measure with modern technology (cannot be seen with only the naked eye) |
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| Scientific Method |
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| Systematic approach to research (to figuring things out) |
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| Law |
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| a concise verbal or mathematical study of the relationship between phenomena that are always the same under the same conditions |
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| Theory |
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| unifying principle that explains a body of facts and the laws that are based on those facts |
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| Hypothesis |
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| tentative explanation for a set of observations; leads to "if-when" questions; test of theory |
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| Matter |
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| anything that occupies space and has mass -->all matter is made up of chemicals |
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| mixture |
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| combination of 2 or more substances in which the substances retain distinct identities (air, milk, cement, tea, coffee) |
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| Homogeneous mixture |
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| same composition throughout (sugar in water, tea) |
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| Heterogeneous mixture |
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| non-uniform composition (sand + iron filings) |
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| substance |
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| form of matter that has a definite or constant composition and distinct properties (H2O, NH3, sugar, gold...) |
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| elements |
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| substance that cannot be separated into simpler elements by chemical means |
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| Al |
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| Aluminum |
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| As |
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| Arsenic |
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| Ba |
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| Barium |
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| Br |
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| Bromine |
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| Ca |
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| Calcium |
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| C |
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| carbon |
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| Cl |
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| Chlorine |
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| Cr |
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| Chromium |
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| Co |
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| cobalt |
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| Cu |
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| copper |
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| F |
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| Fluorine |
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| Au |
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| Gold |
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| H |
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| hydrogen |
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| I |
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| Iodine |
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| Fe |
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| iron |
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| Pb |
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| lead |
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| Mg |
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| Magnesium |
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| Mn |
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| manganese |
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| Hg |
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| mercury |
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| Ni |
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| nickel |
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| N |
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| nitrogen |
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| O |
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| oxygen |
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| P |
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| Phosphorus |
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| Pt |
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| platinum |
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| K |
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| potassium |
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| Si |
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| silicon |
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| Ag |
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| silver |
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| Na |
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| sodium |
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| S |
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| sulfer |
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| Sn |
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| Tin |
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| W |
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| Tungsten |
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| Zn |
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| zinc |
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| Compounds |
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| substance composed of atoms of 2 or more elements chemically united in fixed proportions |
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| Physical property |
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| can be measured and observed without changing the composition or identity of a substance |
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| Chemical Property |
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| requires a chemical change in order to be observed |
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| Extensive Property |
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| depends on the amount of material, Ex: mass and volume |
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| Intensive property |
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| does not depend on the amount, EX: temperature and density |
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| tera- |
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| T 1,000,000,000,000 10^12 1 terameter(Tm)= 1 X 10^12 m |
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| giga- |
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| G 1,000,000,000 10^9 1 gigameter (Gm)= 1 x 10^9 |
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| mega- |
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| M 1,000,000 10^6 1 megameter (Mm)= 1 x 10^6 |
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| kilo- |
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| k 1,000 10^3 1 kilometer (km)= 1 x 10^3 m |
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| deci- |
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| d 1/10 10^-1 1 decimeter (dm)= 0.1 m |
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| centi- |
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| c 1/100 10^-2 1 centimeter (cm)= 0.01 m |
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| milli- |
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| m 1/1000 10^-3 1 millimeter (mm)= 0.001 m |
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| micro- |
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| µ 1/1000,000 10^-6 1 micrometer (µm)= 1 x 10^-6 m |
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| nano- |
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| n 1/1,000,000,000 10^-9 1 nanometer (nm)= 1 x 10^-9 m |
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| pico- |
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| p 1/1,000,000,000,000 10^-12 1 picometer (pm) = 1 x 10^-12 m |
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| 1 inch = _____ cm |
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| 2.54 cm |
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| 1 m= ______ inches |
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| 39.37 inches |
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| 1 kg = ______ lb |
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| 2.205 lb |
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| 1 lb = _______ g |
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| 454 g |
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| 1 L = ______ qt |
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| 1.057 qt |
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| 1 gal = ____ L |
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| 3.786 L |
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| 1000 cm^3 = ______ mL |
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| 1000 |
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| 1000 mL= _______ dm^3 |
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| 1 |
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| 1 dm^3 = _______mL |
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| 1000 |
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| 1000 mL= _______ L |
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| 1 |
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| 1 cm^3 = ______ mL |
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| 1 |
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| density formula |
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| d= mass/volume usually g/cm^3 or g/mL |
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| specific gravity |
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| density of substance/ density of water a dimensionless quantity |
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| ?C---> ?F |
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| ?F= (9/5)?C +32 |
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| ?F---> ?C |
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| ?C= (5/9) (?F- 32) |
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| ?C---> K |
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| K= ?C + 273.15 |
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| boiling point of water a) Kelvin b) ?C c) ?F |
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| a) 373 K b) 100?C c) 212? F |
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| Body temperature a) Kelvin b)?C c)?F |
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| a) 310 K b) 37?C c) 98.6?F |
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| Room Temperature a) Kelvin b) ?C c) ?F |
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| a) 298 K b) 25?C c) 77?F |
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| Freezing point of water a) K b) ?C c) ?F |
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| a) 273 KK b) 0?C c) 32?F |
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| Sig Fig rule for multiplication and division |
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| look for factor with the fewest # of sig figs |
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| Sig Fig rule for addition and subtraction |
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| look for value with fewest # of decimal places |
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| Significant Figures |
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| # of "significant figures" shows degree of uncertainty in measurement |
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| accuracy |
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| how close to the "true" value? systematic errors |
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| precision |
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| how reproducible is the measurement? random errors |
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| Exact numbers |
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| values that are exactly counted or defined can be assumed to have an infinite number of sig figs, EX: 25 people or 1 foot= 12 inches |
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| 1 foot= _____ inches |
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| 12 |
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| 1 inch = _____ cm |
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| 2.54 |
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| 1 mi= ______ ft |
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| 5280 |
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| 1 gal= _____ L |
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| 3.786 |
