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Chemistry 221
Mt. Hood Chemistry course
| Question | Answer |
|---|---|
| Metric System: Giga | 10 to the 9th power |
| Metric System: Mega | 10 to the 6th power |
| Metric System: Kilo | 10 to the 3rd power |
| Metric System: Deci | 10 to the -1st power |
| Metric System: Centi | 10 to the -2nd power |
| Metric System: Milli | 10 to the -3rd power |
| Metric System: Micro | 10 to the -6th power |
| Metric System: Nano | 10 to the -9th power |
| Metric System: Pico | 10 to the -12th power |
| Metric System: Femto | 10 to the -15th power |
| American Metric Conversion | 2.54cm=1in, 1.06qt=1L, 454g=1LB, 39.37in=1m, 2.21LB=1kg, 1.609km=1mi |
| American Mass | 1LB=16mass oz, 1ton=2000LBs |
| American Volume | 1c=8fl.oz, 1pt=2c, 1qt=2pt, 1gal=4qt |
| American Length | 1ft=12in, 1yd=3ft, 1mi=5280ft |
| Polyatomic Ions: chlorate | ClO3, -1 Charge |
| Polyatomic Ions: Permanganate | MnO4, -1 Charge |
| Polyatomic Ions: acetate | CH3COO, -1 Charge |
| Polyatomic Ions: hydroxide | OH, -1 Charge |
| Polyatomic Ions: cyanide | CN, -1 Charge |
| Polyatomic Ions: thiocyanide | SCN, -1 Charge |
| Polyatomic Ions: ammonium | NH4, +1 Charge |
| Polyatomic Ions: sulfate | SO4, -2 Charge |
| Polyatomic Ions: carbonate | CO3, -2 Charge |
| Polyatomic Ions: phosphate | PO4, -3 Charge |
| Polyatomic Ions: nitrate | NO3, -1 Charge |
| Polyatomic Ions: chromate | CrO4, -2 Charge |
| Polyatomic Ions: dichromate | Cro7, -2 Charge |
| Polyatomic Ions: oxalate | C2O4, -2 Charge |
| Polyatomic Ions: thiosulfate | S2O3, -2 Charge |
| Element | One type of atom only |
| Atom | The smallest representative particle of an element |
| Matter | Anything that has a mass and takes up space (Atom, Element, Compounds, and Molecules) |
| Chemistry | Study of matter and changes it undergoes |
| Macro | Big |
| Micro | Small |
| Atomic Theory | Atoms are the smallest particles of an element |
| Law of Constant Composition | Observation that the elemental composition of a pure compound is always the same |
| Law of Conservation Mass | Total mass present after a chemical reaction is the same as the total mass present before the reaction |
| Law of Multiple Proportions | states that when elements combine, they do so in the ratio of small whole numbers |
| Empirical Formula | The formula of a compound showing the simplest ratio of the atoms present (ie. B2F6>BF3) |
| Compounds | contains atoms of two or more chemical elements held together by chemical bonds |
| Molecules | Smallest physical unit of a substance that can exist independently, consisting of one or more atoms held together by chemical forces |
| States of Matter | Gas,Liquid,and Crystalline solid |
| Homogeneous | Completely uniform at macroscopic level (Air) |
| Mixture | Two or more different elements, compounds, and/or states of matter in a container |
| Heterogeneous | Uneven at Macroscopic level (Granite) |
| Pure Substance | Only one pure element or compound (not physically divisible) |
| Diatomics: hydrogen | H2 |
| Diatomics: oxygen | O2 |
| Diatomics: nitrogen | N2 |
| Diatomics: chlorine | Cl2 |
| Diatomics: bromine | Br2 |
| Diatomics: iodine | I2 |
| Diatomics: flourine | F2 |
| Polyatomics: sulfur | S8 |
| Polyatomics: phosphorous | P4 |
| Matter Chart | Heterogeneous Mixture< Homogeneous Matter< Element Pure Substance < Compound |
| Physical Properties | Properties that can be observed or measured without changing the composition of a substance (boiling, melting, color, and conductivity) |
| Chemical Properties | Can only be observes when a substance is changes into another substance (flammability,and reactivity to acid) |
| Chemical Reactions | In the course of a chemical reaction, the reacting substances are converted to new substances |
| Methods of Seperation: Distilation | Uses differences in the BP of substances to seperate homogeneous mixtures into its components |
| Methods of Seperation: Filtration | Solid subtances are seperated from liquids and solutions |
| Methods of Seperation: Chromatography | Seperates subtances on the basis of the differences in solubity in a solvent and attraction to the chromatography paper |
| Qualitative Information | Non-numerical experimental observations (Descriptions) |
| Quantitative Information | Numerical experimental data (measurements in mass or volume) |
| Celsius | 0-100*C *C=(5/9)(F-32) |
| Kelvin | 273-373K K=C+273.15 |
| Fahrenheit | 32-212*F *F=(9/5)(*C)+32 |
| Density | Ratio of mass of object to it volume D=(M/V) |
| Specific Gravity | Density of Liquid/Density of Water (the density without units) |
| Temperature | Is a measure of kinetic energy |
| Significant Figures | -All non zero digits are sig-figs -0 between numbers are sig-figs -0 before number not sig-figs -0 before and after decimals are sig-figs -ignore 1 in conversions |
| Scientific Method (Thought Process) | Observation & Experiments> >Finding patterns trends and laws> >Formulate & test hypthesis> >Theory |
| Coulombs Law | F=((kQ1Q2)/D2) Q=magnitude of the ion charge D=distance betweem ion center k=konstant |
| Coulombs Law | -Opposite charges attract;Same charges repel -Strength of force is determined -change increases attractive force increases -distance increases attractive force decreases |
| Periodic Table: Group 1A | Alkali Metals -very reactive |
| Periodic Table: Group 2A | Alkaline Earth Metals -react w/HOH to produce alkaline soln. Except Be |
| Periodic Table: Group 6A | Chalogens |
| Periodic Table: Group 7A | Halogens -very reactive -react violently w/Alkali Metals |
| Periodic Table: Group 8A | Noble Gases -rare gases -inert gases -not reactive |
| Periodic Table: | Groups/Family: Columns Periods: Rows Main Elements: A Group Transition Metals: B Group |
| Percent Abundance | Percent of a specific isotope that occurs in a natural sample of an element A.W.=((%isotope1)/100)(MassIsotope1)+... |
| Isotopes | Atoms with the same atomic # but different mass # |
| AMU | AMU=atomic mass 1 AMU=1.661*10^-24g |
| Atomic Mass | Atomic weight, the average mass of an atom in a natural sample element |
| Mass Number (A) | Number of protons and neutrons |
| Nuclear Strong Force | Holds protons together |
| Positive & Negative | Cation=Positive Anion=Negative |
| Subatomic Particles | Proton(p):positive +1 Charge Electron(e):negative -1 Charge Neutron(n):nuetral 0 Charge |
| Alpha | =positive charges particles |
| Naming Acids: Hydro-,-ic | If anion has -ide then change it to hydro-,-ic acid (ie. HCl= hydrochloric acid) |
| Naming Acids: Hypo-,-ous | If anion has hypo-,-ite then change it to hypo-,-ous acid (ie. HClO= hypochlorous acid) |
| Naming Acids: -ous | If anion has -ite then change it to -ous acid (ie. HClO2= chlorous acid) |
| Naming Acids: -ic | If anion has -ate then chenge it to -ic acid (ie. HClO3= chloric acid) |
| Naming Acids: per-,-ic | If anion has per-,-ate then change it to per-,-ic acid (ie. HClO4= perchloric acid) |
| Naming Bases | Add hydroxide(OH)to formula (ie. NaOH= sodium hydroxide) |
| Acid | A compound that produces hydrogen ions when dissolved in water. Chemical Formula usually HX(X = monatomic or polyatomic ion). Chemical formula = H+ |
| Base | A compound that produces hydroxide ions when dissolved in water. Bases are named as if they were ionic compounds (the name of the cation followed by the name of the anion). |
| Naming Polyatomics: -ide | No oxygen (ie. Cl= chloride) |
| Naming Polyatomics: hypo-,-ite | -2 oxygens (ie. ClO= hypochlorite) |
| Naming Polyatomics: -ite | -1 oxygen (ie.ClO2= chlorite) |
| Naming Polyatomics: -ate | Common or representative oxyanion (ie. ClO3= chlorate) |
| Naming Polyatomics: per-,-ate | +1 oxygen (ie. ClO4= perchlorate) |
| Monatomic Ions | Single atoms that have lost or gained an electron |
| Polyatomic Ions | Group of atoms tat have an electrical charge |
| Fixed Charge | Al +3 Charge, Ga +3 Charge, In +3 Charge, Zn +2 Charge, Cd +2 Charge, Ag +1 Charge |
| Ambiguous Number | No decimal point to symbolize that that was the real value. |
| Ionic Compound Properties | -high metling points -hard and brittle -cleaves cleanly along sharp boundary |
| Atomic Number(Z) | Number of protons |
| Electrostatic Force | Attracts cation and anion |
| Molecular Covalent Bond | Nonmetal bonds to nonmetal |
| Ionic Bonds | Metals bonds to nonmetal (cation bonds to anion) |
| Condensed Structure | Atoms are written in such a way that the structures can be determined |
| Metalloids | Properties somewhere between metals and nonmetals |
| Nonmetals | -solid,liquid,and gas -do not conduct electricity |
| Metal | -solid -conducts easily -ductile(drawn into wires) -malleable(rolled into sheet) |
| Nuclear Symbol | Symbol of element, mass#, and atomic # |
| Percent Error Formula | %error= (|true value-average|/true value)*100 Find average of data taken and plug in. |
| Extensive Property | Depends on the amount of substance (mass,and volume) |
| Intensive Property | Independent of the amount of substance (density,and boiling point) |
| Accuracy | Refers to how closely individual measurements agree with the correct or true value -percent error formula |
| Precision | Measure of how closely individual measurements agree with one another -finding averages of results (ie. Student A: 77.4 79.1 78.0 78.3 (77.4+79.1+78.0+78.3)/4=78.2 (77.4-78.2=.8,79.1-78.2=.9,78.0-78.2=.2, 78.3-78.2=.1)=2.0/4=.5 .5 is precision) |
| Structural Formula | Shows connections among atoms by using lines to represent covalent bonds |
| Conversion ie. | . |
| Molecular Formula | Shows the numbers and kind of atoms in one molecule of a compound |
| Chemical Equations | They are a concise representations of chemical reactions |
| Law of Conservation of Matter | Matter can be neither created nor destroyed Mass of Reactants=Mass of Products |
| Balancing Equations | 1. Write unbalanced equation using correct formula for R & P 2.Add appropriate coefficients to balance 3.Check (Equal#of same atoms) 4.Reduce coefficients to lowest whole # value |
| Reaction Types: Combination Reaction | This type of reaction two or more substances react to form one product |
| Reaction Types: Decomposition Reaction | Decomposition of one substance breaks down into two or more substances |
| Reaction Types: Combustion Reaction | -rapid reaction that produces a flame -mostly involve hydrocarbons reacting with oxygen in the air |
| Mole | Amount of a substance that contains many elementary entities (atoms,molecules,and other particles. -1mole=6.022*10^23 -Conversion factor |
| Avogadro's Number | 6.022*10^23 |
| Molar Mass | Mass in grams of one mole of any element or molecule |
| Bridges From Grams to Particles | GRAMS<MolarMass>MOLES<Avogadro's#>PARTICLES |
| Percent Composition | Mass%=(MolarMassOfElement/MolarMassOfCompound)*100 |
| Percent Composition ie. | . |
| Bridges For Emprical Formula | MASS%X>assume.100g>GRAMS X>molar mass>MOLES X> >mol to mol.ratio>EMPIRICAL.FORMULA (x=element) |
| Empirical Formula ie. | . |
| Finding Subscript for E.F. | Integral Factor=(Molecular Mass/E.F.Mass) |
| Stoichiometry | Provides the quantitative relationship between reactants and products in a chemical reaction |
| Stoichiometry ie. | . |
| Limiting Reactant | The reactant that is used up. It limits the amount of product produced |
| Reactant in Excess | Often heavily in excess to ensure limiting reactant is completely used up |
| Theoretical Yield | The mass of product that could theoretically be produced assuming 100% efficiency |
| Actual Yield | The actual amount of product produced |
| Percent Yield | (Actual/Theoretical)*100= percent yield |
| Limiting Reactant ie. | . |
| Strong Electrolyte | 100% Dissociation -good conductor of electricity* |
| Weak Electrolyte | Partially dissociation -poor conductors of electricity* |
| Non-Electrolyte | Dissolve in HOH but don't ionize -dont conduct electricity (ie.Sugar) |
| Solution | Homogeneous mixture of two or more substances (soln.) |
| Homogeneous | Uniform all through out |
| Solvent | The medium in which a solute is dissolved in to form a solution (greatest quantity) |
| Solute | The substance dissolved in a solvent to form a solution (smallest quantity) |
| Electrolyte | Compounds whose aqueous solutions conduct electricity |
| Solvates/Dissociation | general process in which ionic compounds separate or split into smaller molecules, ions |
| Strong Acids: hydrochloric acid | HCl |
| Strong Acids: hydrobromic acid | HBr |
| Strong Acids: hydroiodic acid | HI |
| Strong Acids: Chloric acid | HClO3 |
| Strong Acids: perchloric acid | HClO4 |
| Strong Acids: nitric acid | HNO3 |
| Strong Acids: sulfuric acid | H2SO4 |
| Strong Bases: Group 1A Metals with OH | LiOH,NaOH,KOH,RbOH,CaOH |
| Strong Bases: Group 2A Metals with OH | Ca(OH)2,Sr(OH)2,Ba(OH)2 |
| Solubility Exceptions: Alkali Metals, NH4 ;NO3 ;C2H3O2 | None |
| Solubility Exceptions: Cl`,Br`,I` | Ag ,Hg2 ,Pb |
| Solubility Exceptions: SO4 | Sr ,Ba, Hg2 ,Pb |
| Insolubility Exceptions: CO3 ,PO4 | Alkali Metals, NH4 |
| Insolubility Exceptions: S ,OH` | Alkali Metals, NH4 ,Ca ,Sr ,Ba |
| Precipitation | Formation of an insoluble compound (solid) |
| Acid-Base(Neutralization) | Formation of a salt and water. Proton(H+)Transfer |
| Gas-Forming | Evolution of a water-insoluble gas "effervescence" |
| Oxidation-Reduction | Electron transfer. |
| Exchange Reaction | Found when precipitation, acid-base, and gas-forming reactions occur. * |
| Metathesis Reactions | Metathesis in Greek mean "to transpose" Also known as -Double replacement reactions -Double displacement reaction -Exchange reactions |
| Molecular Equation | All reactants and prosuct written in molecular formulas |
| Total Ionic Equation | All soluble reactants and products written as ions |
| Net Ionic Equations | Total ionic equation without the spetator ions |
| Spectator Ions | Ions present before and after the reaction |
| Writing Net Ionic Equations | 1.Write a balanced Molec. Equation 2.Dissociate all strong electrolytes 3.Cross out any remaining unchanged ions from left and right 4.Wrote the net ionic equation with the species that remain. |
| Net Ionic Equation ie. | . |
| Characteristics of Acids | Acid gives away protons,Taste sour, inorganic acids have H in front, organic acids have H at the end, Strong acids completely dissociate -Single arrow Weak Acids partially dissociate -double arrow |
| Characteristics of Bases | Base is a proton acceptor, taste bitter, inorganic bases soluble metal hydroxides Strong Base complete dissociation Weak Base partial dissociation |
| Neutralization Reaction | Reaction between strong acid and strong base -Produces HOH and salt. Creates the Net Ionic Equation |
| Gases Produced In a Gas-Forming Reaction | H2,N2,O2,F2,Cl2 H2S H2O(Assume its a liquid unless told otherwise) |
| Known Gas-Forming Reaction Compounds | H2CO3>H2O+CO2 H2SO3>H2O+SO2 NH4OH>H2O+NH3 |
| Oxidation | Is when an atom or ion loses an electron * |
| Reduction | Is when an atom or ion gains an electron * |
| Pnemonics For Redox | LEO the lion says GER Loss e` Oxidation Gain e` Reduction |
| Redox Reactions | Reactions that involve oxidation and reduction, where e` are transferred from one reactant to another |
| Oxidizing Agent | The reactant in a redox that causes oxidation |
| Reducing Agent | The reactant in a redox reaction that causes reduction |
| Redox Reaction ie. | . |
| Oxidation Number | Indicates whether the atom is nuetral, e` rich, or e` poor |
| Single Replacement | A BC->AC B A BC->BA C Metals replace metals, nonmetal replace nonmetals |
| Concentration | The amount of solute diluted in a given amount of solution |
| Molarity | Molarity=(amountofsolute[mol]/volumeofsolution[liters]) Molar Units: mol/L or M |
Created by:
rozakhodak
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