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27 Cards in this Set
- Front
- Back
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Measurement & Significant Figures
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Tells how accurate the measuring instrument was.
NUMBERS >1: All numbers are significant, except trailing zeros with NO decimal. (if there is a dec--> significant) NUMBERS <1: All numbers after first non-zero is significant. |
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Calculating with Significant Figures
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MULTIPLYING and DIVIDING:
Limit & round to the least number of Significant Figures. ADDING and SUBTRACTING: Limit & round to least number of decimal places. |
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Precision vs. Accuracy
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Precision: How close your measurements are to eachother.
Accuracy: How close your measurements are to the standard. |
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Percent Error
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% ERROR= (ACCEPTED VALUE-EXPERIMENTAL VALUE/ ACCEPTED VALUE) x 100
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Basic Lab Equiptment
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Scoopula, Sparker, Graduated cylinder, Test tube, Test tube rack, Test tube holder, Evaporating dish, Flask, Watch glass, Spatula, Wire gauze, Clay triangle, Beaker, Etc.
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SI Units:
Length Mass Time Amount Temperature Energy Volume |
LENGTH- Meter
MASS- Gram TIME- Second AMOUNT- Mole TEMP.- Kelvin ENERGY- Joule VOLUME- Liter |
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Metric Prefixes
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kilo- 1000
deci- .1 (10^-1) centi- .01 (10^-2) milli- .001 (10^-3) micro- .000001 (10^-6) nano- .000000001 (10^-9) pico- .000000000001 (10^-12) |
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Exponential Form
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ALL sigfigs will be in the MANTISSA-->
when multiplying/dividing 2 exponential numbers, limit to least number of sig figs (if adding/subtracting, least decimal places) |
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Dimensional Analysis
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FACTOR LABEL METHOD
Measurement x Conversion Fraction (conversion fraction- ORIGINAL UNIT/ amount it is equal to in DESIRED UNIT) |
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Types of Matter
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Substances & Mixtures
Substances- Elements and Compounds Mixtures- Homogeneous and Heterogeneous |
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Three Phases of Matter and Their Properties
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SOLID- Locked in place
Definite Shape Definite Volume Retain Shape Most dense phase of an Element (except: H2O) Highest intermolecular attraction LIQUID- Atoms free to move around No definite volume Take shape of container Less dense than solids (Still high density) GAS- No definite volume No definite shape Will fill container completley Lowest density of phases Lowest intermolecular attractions *Can be affected by pressure changes |
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Elements, Compounds & Mixtures
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Element- Cannot be broken down any further. 1 type of atom.
Compounds- 2+ elements chemically bonded. Mixtures- Combination of Elements and/or compounds mixed together, but seperable by physical means. Components retain properties. |
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Symbols for Various Elements
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TRICKY ELEMENTS:
Na- Sodium K- Potassium Cu- Copper Co- Cobalt Hg- Mercury Pb- Lead Au- Gold Ag- Silver Sn- Tin Sb- Antimony As- Arsenic |
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Heterogeneous vs. Homogeneous Mixtures
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Homogeneous- Solution. Uniform throughout.
Heterogeneous- Suspension. NOT Uniform throughout. --> Colloids: Look uniform, but eventually settle. |
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Ways to Seperate Mixtures
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FILTRATION- Used for heterogeneous mixtures. Use filter paper, etc.
DISTILLATION- Use apparatus or hot container. Substance with lower BP vaporizes first and is collected. EVAPORATION-Liquid evaporates out. CHROMATOGRAPHY- Pigments seperate out on special paper. CRYSTALLIZATION- Force solids to form crystalls. |
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Physical Vs. Chemical Properties of Matter
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PHYSICAL PROPERTIES- Observed with senses, determined without chemically altering the object. Shape, mass, length, odor.
CHEMICAL PROPERTIES- How a substance reacts with something else. Can be observed only when something is chemically reacting. |
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Differences Between Physical and Chemical Changes
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PHYSICAL CHANGES- Substance retains its chemical identity
CHEMICAL CHANGE- New products are created as substance reacts. |
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Density Problems
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Density= Mass/ Volume
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Forms of Energy
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Kinetic Energy & Potential Energy
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Law of Conservation of Energy
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Energy cannot be created or destroyed, but it CAN be converted from one form to another.
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Potential Energy Vs. Kinetic Energy
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KINETIC ENERGY: Associated with moving matter.
POTENTIAL ENERGY: Stored in matter |
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Heat
-Properties |
Transfer of Energy
Flows from HIGH-->LOW temperature When heat is added, motion of particles increases. When heat is taken away, motion of particles decreases. |
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Temperature
-function -Converting: K<->C -Absolute Zero |
Measurement of AVERAGE KINETIC ENERGY
K=C+273 C=K-273 Absolute zero: No motion of particles |
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Endothermic Changes vs. Exothermic Changes
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Endothermic: Require heat
Exothermic: Give off heat Solid Liquid Gas Solid > Liquid> Gas: Endothermic Gas > Liquid > Solid: Exothermic |
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Phase Changes of Matter
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Melting/ Fusion (s > l)
Boiling/ Vaporization (l > g) Condensation (g > l) Freezing/ Solidification (l > s) Sublimation (s > g) DepositioN (g > s) |
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Heating and Cooling Curves
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Study Phase Change Diagrams
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Heat Equations
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Heat energy during temp (KE) changes:
q=mc^T Heat energy during phase (PE) changes: q=mHv, q=mHf |
