CHEM 1110: Chapters 5 and 6
33 Cards in this Set
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Limiting Reactant
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substance that limits the amount of product that can be formed in a reaction the first species that is completely consumed in a reaction limiting reactant quantity determines the maximum amount of a product that can be produced
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Excess Reactant
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species left over at the end of a reaction after stoichiometric amount of it reacted with limiting reactant
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Theoretical Yield
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amount of product calculated to form if the limiting reagent is completely reacted - virtually impossible to collect the amount product equal to the theoretical yield
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Actual Yield
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quantity of product obtained from a chemical reaction
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Actual Yield is less than what is theoretically possible:
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1. many reactions are reversible - don't go to completion. reversible reactions esult when the products formed are not very stable and react with themselves to regenerate the reactants 2. competing reactions may occur - reduce amount of product formed 3. experimental error - contributes t…
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Percent Yield
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actual weight recovered divided by theoretical weight * 100%
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Redox reaction
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reaction in which one or more electrons are transferred between reactant species aka oxidation-reduction reactions oxidation and reduction must occur simultaneously oxidation numbers of two or more atoms change during the course of the reaction
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Oxidation
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loss of electrons Na --> Na+ + e-
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Reduction
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gain of electron Cl(2) + 2e- --> 2Cl-
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Rules for Assigning Oxidation Numbers
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1. oxidation number of an element in elemental state is 0 2. oxidation number of hydrogen in compounds is +1 3. O# of oxygen in compounds is -2 except in hydrogen peroxide H2O2 (-1) 4. monatomic ions in compounds have O#s equal to their charges (S^2- = -2) 5. binary compound: more electro…
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more O# rules
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8. oxidation numbers of groups IA and IIA metals are always +1 and +2 respectively 9. O#s are assigned on per atom basis. in CL2Om sum of O#s for Cl is +2 (O is -2). since there are two chlorine atoms, each chlorine has a +1 O#
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Combination and Decomposition reactions
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combination: reaction of two substances that produces new compound A + B -> C decomposition: reaction in which a compound decomposes into two or more substances AB -> A+B decomposition rxns usually require external energy source (heat) to initiate rxn
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Single replacement reactions
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reaction in which a more reactive element replaces another element from a compound A +BC -> AC + B
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Precipitation reactions aka double replacement or metathesis
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Reaction in which a solid forms when 2 aqueous solutions are mixed The driving force for a precipitation rxn is the removal of ions from solution must know solubility rules AB + CD -> AD + CB (soluble+soluble -> soluble+insoluble) AB exists are A+ &B- ions and CD exists as C+ & D- ions in…
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Acid-Base reactions also metathesis rxns
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Bronstead-Lowry Acid: proton (H+) donor: an acid donates a proton to a base in acid-base rxn Bronstead-Lowry Base: proton (H+) acceptor: base accepts proton from acid in rxn HA + B -> HB+ + A base has unshared pair of electrons that form a bond with H+ - coordinate covalent bond
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Net Ionic Equations
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chemical equation that is written with spectator ions removed
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Solubility Rules for ionic compounds
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+ - 1. (groupIA)+, NH4+ | NO3-, CH3COO-, ClO3-,ClO4- 2. Pb^2+, Hg2^2+, Ag+ | CO3^2-, PO4^3-, S^2-, 3. | Cl-, Br-, I- 4. Ba^2+ | OH- (except BA^2+, Sr^2+, Ca^2+ 5. | So4^2 (except Sr^2+, Ca^2+ sol, insol, sol, insol, sol order of rules takes precedence
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Activity series for metals for replacement reactions
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most active least active Li K Ca Na Mg Al Zn Cr Fe Cd Co Ni Sn Pb H Cu Hg Ag Pt Au
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solubility rules
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Group I and NH4+ compounds carbonates (except Group I, NH4+ and uranyl compounds) nitrates sulfites (except Group I and NH4+ compounds) acetates (ethanoates) (except Ag+ compounds) phosphates (except Group I and NH4+ compounds) chlorides, bromides and iodides (except Ag+, Pb2+, Cu+ and Hg…
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Strong acids
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acid that is nearly 100% ionized (separated into ions) in dilute aqueous solution HCl - hydrochloric acid HBr - hydrobromic acid HI - hydroionic acid HNO3 - nitric acid H2SO4 - sulfuric acid HClO3 - chloric acid HClO4 - perchloric acid
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Strong Bases
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water soluble base that is 100% dissociate in water LiOH - lithium hydroxide NaOH - sodium hydroxide KOH - potassium hydroxide RbOH - rubidium hydroxide CsOH - cesium hydroxide Sr(OH)2 - strontium oxide Ba(OH)2 - barium hydroxide
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end ch 5
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end ch 5
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solvent
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does the dissolving
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saturated solution
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solution containing the max amount of solute that will dissolve at a given temperature
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unsaturated solution
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solution containing less than the max amount of solute that will dissolve at a given temperature
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supersaturated solution
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solution containing more than the max amount of solute that will dissolve this results in precipitation
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electrolyte
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if a solution produces ions upon dissolution in water, the solution will conduct electricity and the solute is classified as an electrolyte compund that ionizes/dissociates into ions when dissolved in water and produces a solution that conducts electricity
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strong electrolytes vs weak electrolytes
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strong: produces a large quantity of ions and conducts electricity well when dissolved in solution ex. ionic compounds, strong acids, strong bases weal: produces relatively few ions and is a poor conductor
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dissociation
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process in which an ionic compound separates into ions wehn dissoved in solution
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ionization
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molecular compound produces ion swhen dissolved in aqueous solution strong electrolytes completely (of nearly 100%) dissociate or ionize in aqueous soitin
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mass by volume
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(m/v)% = grams of solute/mL soln *100%
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mass by mass
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(m/m) = grams of solute/grams of solution *100%
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molarity
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moles of solute/1L of soln = moles of solute/1000mL of soln molarity x liters of soln = moles moles x (1/M) = L moles x (L of soln/moles) = L moles x (1ooomL soln/moles) = mL
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CHEM 1110: Elements of Periodic Table