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Exam 3 Chem
| Term | Definition |
|---|---|
| Definition of entropy | Measure of disorder or energy dispersion in a system |
| Definition of (Gibbs') free energy | Energy available to do work at constant temperature and pressure |
| Determining the relative molar entropy of different species | Relative molar entropy increases with higher molecular complexity, mass, number of atoms, and flexibility in structure or motion |
| Determining the standard free energy change of a reaction | ΔG ∘ =∑ΔG f∘(products)−∑ΔG f∘(reactants) or ΔG ∘=−RTlnK |
| Determining the temperature at which a reaction becomes spontaneous | T= ΔH/ΔS |
| Predicting reaction spontaneity (vs. non-spontaneity vs. @ EQ) | ΔG<0: Spontaneous ΔG>0: Non-spontaneous ΔG=0: At equilibrium |
| Determining the relative values of ΔH° & ΔS° from a chemical reaction | Gas formation increases Δ𝑆∘ Condensation or solidification decreases Δ𝑆^o Breaking bonds absorbs energy (+ΔH ∘ ). Forming bonds releases energy (−ΔH ∘) |
| Calculating ΔS° for a reaction given S° | 1. Multiply the standard molar entropy (S ∘ ) of each species by its stoichiometric coefficient in the balanced reaction. 2. Sum these values for products and reactants separately. 3. Subtract the sum for reactants from the sum for products. |
| Calculating ΔG from ΔG°; significant of ΔG vs. ΔG° | ΔG=ΔG ∘+RTlnQ |
| Determining ΔH° & ΔS° from a Van't Hoff Plot | ΔH ∘=−m⋅R ΔS ∘ =b⋅R |
| Calculating Keq/ΔG°/Ɛ° (via Power Triangle) | ΔG ∘=−RTlnK eq ΔG ∘ =−nFE ∘ E ∘ = 0.0592/n x logKeq |
| Determining the total # of electrons transferred in a redox reaction | Balance chem equation |
| Identifying the characteristics ( Keq, ΔG°, or Ɛ°) of a spontaneous or non-spontaneous reaction | Non-spontaneous reaction: ΔG ∘ >0 E ∘ <0 𝐾eq<1 Spontaneous reaction: ΔG ∘ <0 E ∘ >0 𝐾eq>1 |
| Calculating Ɛ from Ɛ° (Nernst Equation) | E=E ∘ − (0.0592/n) logQ |
| Determining spontaneous direction of a galvanic cell, and calculating its overall cell potential | Ecell∘>0: Spontaneous. Ecell∘<0: Non-spontaneous. Reduction at cathode, oxidation at anode |
| Solving for Q in a galvanic cell | Q=[product at anode]/[product at cathode] |
| Process of iron oxidation; preventative measures against iron oxidation | Oxidation: Fe=Fe2+ + 2e- Reduction: O2+4e-+2H2O=4OH- -Attach a sacrificial anode (zinc or magnesium) to corrode instead of iron. -Use corrosion-resistant alloys -Coatings |
| Determining the products of an electrolytic cell involving a molten salt | Cathode: Na++e-=Na(s) Anode: 2Cl-=Cl2(g)+2e- Overall: 2Nacl(l)=2Na(s)+Cl2(g) Cations produce the metal. Anions produce a non-metal gas or liquid |
| Characteristics of ligands within a coordination compound, including type of dentition (mono-, bi-, polydentate) | Monodentate: One donor atom Bidentate: Two donor atoms Polydentate: Three or more donor atoms Bidentate and polydentate ligands form stable chelate complexes by binding to the metal at multiple sites |
| Drawing Lewis structures of linkage isomers, cis/trans isomers, and fac/mer isomers | Cis: Identical ligands are adjacent. Trans: Identical ligands are opposite. Fac: Three identical ligands form a triangular face Mer: Three identical ligands are in a plane passing through the meta |
| Identifying transition metal present within biological coordination complexes (e.g. - chlorophyll, hemoglobin, etc.) | Chlorophyll: Magnesium (Mg) Hemoglobin/Myoglobin: Iron (Fe) Vitamin B12: Cobalt (Co) |
| Calculating crystal field splitting energy for an octahedral complex | Δ o=hc/λ |
| Drawing a crystal field diagram (number of electrons to use, and where they go); effect of high-field vs. low-field ligands; identifying high-spin vs. low-spin complexes) | High field = low spin, max unpaired electrons Low field = high spin, minimum unpaired electrons |
| MATCHING SECTION: Identifying the 5 different types of coordination compound isomerism (linkage, coordination, cis/trans, fac/mer, and optical/enantiomeric) from a coordination compound (or complex ion) formula | Optical isomerism: Occurs when a complex has non-superimposable mirror images (chiral) Coordination Isomerism: How to Identify: Identify complexes with the same formula but different coordination arrangements between the metal and the ligands |
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