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64 Cards in this Set
- Front
- Back
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Alkaline Metals
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Li, Na, K, Rb, Cs
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Alkaline Earth Metals
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Mg, Ca, Sr, Ba
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Noble Gases
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He, Ne, Ar, Kr, Xe, Rn
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Halogens
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F, Cl, Br, I, At
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cation
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positive ions, have same name as metal (for metal catoins)
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anion
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negative ions, formed by replacing end of name of elemend with ide
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Ammonium ion
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NH4+
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hydronium ion
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H30+
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hydride ion
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H-
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Nitride ion
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N(-3)
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hydroxide ion
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OH-
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cyanide ion
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CN-
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peroxide ion
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O2(-2)
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magnesium ion
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Mg(+2)
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calcium ion
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Ca(+2)
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strontium ion
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Sr(+2)
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barium ion
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Ba(+2)
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zinc ion
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Zn(+2)
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cadmium ion
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Cd(+2)
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Aluminum ion
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Al(+3)
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Carbonate ion
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CO3(-2)
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Nitrate ion
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NO3(-)
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Phosphate ion
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PO4(-3)
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Sulfate ion
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SO4(-2)
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Chlorate ion
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ClO3(-)
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per___ate
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(+O atom)
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adding H to oxyanions
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prefix hydrogen or dihydrogen etc, and reduces the charge by however many H added
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Acetate ion
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C2H3O2(-)
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perchlorate ion
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ClO4(-)
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Permangantate ion
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MnO4(-)
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acid nomenclature
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ate-->ic, ite-->ous, keep per or hypo prefixes where appropriate
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greek prefixes
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mono, di, tri, tetra, penta, hexa, hepta, octa, nona, deca
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naming binary molecular compounds
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1) name of element farther left usually writen first. cept compounds containing oxygen (always last except when w/ flourine)
2)elements of same group, one with higher atomic number named first 3)name of second element given ide ending 4)use greek prefixes, just dont say mono for the first element named |
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combustion reactions def
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rapid reactions producing a flame. involve O2 as a reactant. combustion of hydrocarbon compounds --produce CO2 and H2O
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percent composition
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%element = ((number of atoms of that element)(atomic weight of element))/formula weight of compound
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mole
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number of atoms, ions or molecules in a sample
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avogadros number
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6.02x10^23
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molar mass
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mass in grams of oen mole of a substance (g/mol)
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converting between g moles and formula weight
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grams<-use molar mass->moles<-use avogadro's number->formula units
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finding empirical formulas
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mass%elements--assume 100g sample-->grams of each element---use molar mass-->moles of each element---calculate mole ratio--->empirical formula
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limiting reacting/reagent
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the reactant that is completely consumed in a reaction
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aqueous solution
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solutions in which water is the dissolving medium
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solution
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a homogeneous mixtrure of two or more substances
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solvent
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substance in a solution present in greatest quantity
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solute
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substances in a solution in less quantity
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electrolyte
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a substance whose aqueous solutions contain an electrolyte
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soluble ionic compounds
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NO3(-)
C2H3O2(-) Cl(-) minus Ag+, Hg2(+2), Pb(+2) Br(-) minusAg+, Hg2(+2), Pb(+2) I(-) minus Ag+, Hg2(+2), Pb(+2) SO4(-2) minus Sr(+2) Ba(+2) Hg2(+2) and Pb(+2) |
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insoluble ionic compounds
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S(-2) minus NH4(+), alkali metal cations, Ca(+2), Sr(+2) and Ba(+2)
CO3(-2) minus NH4+ alkali metal cations PO4(-3) mius NH4+ and alkali metal cations OH(-) minus alkali metal cations, NH4+, Ca(+2) Sr(+2) and Ba(+2) |
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acids
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ionize in aqueous solutions to form hydrogen ions. proton donors (H+ a proton)
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bases
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accept (react with) H+ ions and produce hydroxide ions when dissolve in water
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strong acidsa dn bases
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are strong electrolytes (completely ionized in solution). more reactive than weak
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weak acides and bases
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are weak electrolytes (partly ionized in solution), less reactive than strong
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chalcogens
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O, S, Se, Te, Po
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to find grams of sub B given grams sub A
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grams sub A ---> moles sub A --use coefficients of A and B from balanecd equation --. moles of sub B---> grams sub B
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theoretical yield
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the quantity of product that is calculated to form when all fo tthe limiting reactant reacts .
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percent yield
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actual yield/theoretical yield
x100 |
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metathesis or exchange reactions
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AX + BY ---> AY + BX
many precipitation reactions and acid base reactions |
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molecular equation
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chemical formulas of reactants and products without indicating ionic character
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complete ionic equation
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shows all soluble strong electrolytes shown as ions
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spectator ion
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ions that appear in identical forms among both the reactants and products ina complete ionic equation. play no direct role in the reaction.
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net ionic equation
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complete ionic equation - spectator ions
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Strong Acid examples
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HCl, HBr, HI, HClO3, HClO4, HNO3, H2SO4
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Strong Bases examples
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alkaline metal hydroxides, and Ca(OH)2, Sr(OH)2, Ba(OH)2
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is NH3 a strong or weak base?
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weak
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