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Electrochemical cell: A device which converts chemical energy into electrical energy.

Electrode: A conductor at which a half-cell reaction occurs.

Anode: The electrode at which oxidation occurs Cathode: The electrode at which reduction occurs.

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I can analyze strengths of reducing and oxidizing agents, and balance redox equations

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Redox reactions can be broken up into oxidation and reduction half-reactions

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Oxidation: a species undergoing oxidation loses electrons

Reduction: a species undergoing reduction gains electrons

Oxidizing agent: The species being reduced

Reducing agent: The species being oxidized

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Ka = [H₃O][Ind] ÷ [HInd]

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HInd + H₂O = Ind + H₃O

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Reaction between a salt (ion or ions in a salt) and water to produce an acidic or basic solution.

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Kb = base ionization constant

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Ka = acid ionization constant

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2H2O(l) + 59kJ = H3O+(aq) + OH(aq)
at high temperatures, products are favoured, and so Kw is large
because  Kw = [H3O+] [OH]
and at low temperatures, reactants are favoured, and so Kw is small

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At 250C only: [H3O+] [OH] = 1.00 x 10⁻¹⁴

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equilibrium favours the side with the weaker acid

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a base which is less than 100% ionized (most molecules dont ionize)

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a base which is 100% ionized in a water solution (goes to completion)

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strength of acid does not effect how high or low the concentration is

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strength of acid does not effect how high or low the concentration is

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an acid which is less than 100% ionized (most molecules dont ionize)

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an acid which is 100% ionized in a water solution (goes to completion)

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A base is any substance which accepts a proton from another substance.

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An acid is any substance which donates a proton (H+) to another substance.

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tastes bitter
turns litmus paper blue
slippery
conducts electricity
reacts with acids

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tastes sour
turns litmus paper red
reacts with bases
conducts electricity

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base = an ionic species who's formula ends with OH

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acid = an ionic species who's formula starts with H

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I can find the concentration of a specific ion, and perform calculations involving solubility equilibrium concepts

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C1V1=C2V2

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determining the relative solubility of a substance

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determining the relative solubility of a substance

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want = have x know

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when particles return to the surface of a solid at the same rate as which they leave, chemical equilibrium is reached and the system is fully saturated

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if trial Keq is less than Keq then the system will shift right in order to reach equilibrium, and vice versa

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(initial, change, equilibrium)

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N2(g) + 3H2(g) 2NH3(g)

Keq = [NH3]2 ÷ [N2] [H2]3 = 626

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large Keq = lots of product = close to completion

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large Keq = big numerator
small Keq = big denominator

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solids and liquids are not included in the  Keq equation because they remain relatively constant

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the only  thing that changes Keq is temperature

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= [products] ÷ [reactants]

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If the total pressure of a system is increased, the system will shift towards the side with fewer moles of gas

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(same as temperature in a sense)

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when the temperature is increased the system shifts away from the heat term, and vice versa

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If a system at equilibrium is changed in some way, then the system will do things to counteract that change.

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4PCl5(g) ↔ Cl2(g) + PCl3(g) ∆H = 92.5 kJ

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PCl5(g) ↔ Cl2(g) + PCl3(g) ∆H = -92.5 kJ

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PCl5(g) ↔ Cl2(g) + PCl3(g) ∆H = 92.5 kJ

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when the two tendencies oppose each other the system will reach equilibrium

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when a solid dissolves in water the aqueous solution has greater entropy

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entropy favors the side which contains more moles of gas

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disorder
(maximum entropy favoured)

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Hola

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change in PE = change in enthalpy
(minimum enthalpy favoured)

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forward rate = reverse rate

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I can apply collision theory to explain how reaction rates can be manipulated

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I can apply collision theory to explain how reaction rates can be manipulated

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∆ colour intensity ÷ ∆time
(used for coloured ions only)
∆ temperature ÷ ∆time
(works for all)
∆ pressure ÷ ∆time
(when gases are present)
∆ volume ÷ ∆time
(when gases are present)
∆ mass ÷ ∆time
(solids, entire system if gas escapes)
∆ [ion] ÷ ∆time
[aqueous (don't include spectators)]

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bond breaking

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bond making

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In an exothermic reaction the ∆H is negative, which means it is giving off energy, and so the energy is placed on the products side of the reaction.

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∆H = change in enthalpy

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The total kinetic and potential energy of a substance

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Molecules must collide in order to react

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I can describe the energies associated with reactants becoming products

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I can describe the energies associated with reactants becoming products

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Reaction Rates

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(could also have calculated instantaneous rate)

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Average Rate Calculations (between 4.5 and 8 seconds)

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Average Rate Calculations (between 4.5 and 8 seconds)

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∆ amount = 0.12 – 0.09 = 0.03mol/L
∆ time = 8s – 4.5s = 3.5s
Rate = 0.03mol/L ÷ 3.5s = 8.6 x 10^-3

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Rate =  ∆ Amount ÷ ∆ Time Time =  ∆ amount ÷ Rate
∆ Amount = Rate x  ∆ Time

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I can monitor and Calculate the rate of a Reaction

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I can monitor and Calculate the rate of a Reaction

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In an endothermic reaction the ∆H is positive, which means it is gaining energy, and so the energy is placed on the reactants side of the reaction.