Summary
Summary Physical Organic Chemistry
- Course
- Institution
- Book
Complete summary of the book and lecture notes
[Show more]
Connected book
Book Title:
Author(s):
- Edition:
- ISBN:
- Edition:
More summaries for
-
Samenvatting Modern Physical Organic Chemistry - Reaction Mechanism (WMCH006-05)
-
Summary Physical Organic Chemistry
6 reviews
By: yvettejacobs1 • 3 year ago
By: cillianmacailin • 3 year ago
By: user12426 • 4 year ago
Does not start from the beginning of the book
By: karima_bahida • 6 year ago
Summary is not entirely relevant to me. Have not learned all these chapters. Good for the rest
By: sadaharutje • 7 year ago
By: yousif4_m12 • 7 year ago
Seller
Follow
ScheikundeRU
Reviews received
Content preview
Summary Physical Organic Chemistry4.1 Thermodynamic Analyses of Binding
Solute-solute interactions: one is the host and the other the guest
- The host (H) is the larger molecule, and it encompasses the smaller guest (G) molecule
Knowledge of thermodynamics of binding is essential for designing of synthetic systems that perform
functions and tasks
- Often the goal: to bind a desired molecule from solution and interact with it in some manner
(performing a reaction, giving of a signal)
[HG]
- Ka : association constant = [H][G]
[H][G]
- Kd : dissociation constant =
[HG]
- Ka and Kd are reciprocals
- ΔG° = -RT ln(Ka)
ΔG reflects the change in Gibbs free energy for the conversion of
one mole of H and G to one mole of HG if H and G started in their
standard states and HG ended in its standard state
Low and high concentrations that make H and G or HG dominant
- When the initial concentrations of H and G are the same
and are both below kd, free H and G will dominate the equilibrium
- When the initial concentrations of H and G are above kd, then HG will dominate
- When the concentrations of free H and G equal kd, [HG] = kd
- The entropy of a solution of H, G and HG will increase more rapidly upon dilution when
creating free H and G, because there are two species that are leading to an entropic
stabilization relative to the one HG
- Upon dilution, an HG complex will continually dissociate to H and G due to the favourable
entropy of the entire solution
Standard state:
- When the entropy of a solution of reactants becomes more favourable faster than the
entropy of a solution of products upon dilution it means that the Gibbs free energy of the
solution is changing upon dilution
- To compare different systems: the entropy resulting from dissolution in a solvent is the same
for any solute, regardless of its identity (not when comparing reactions)
- The potential for a spontaneous change in composition to occur is the difference in the Gibbs
free energies of H, G and HG in their standard states plus a term that reflects the mismatch
between the experimental ratios of H, G and HG and their intrinsic rations at standard state
- μH = μoH + RT ln(aH)
- When a ΔG* diagram would show HG higher in energy than H and G, it means that given this
reference state, free H and G are preferred
The influence of change in heat capacity:
- ΔHo and ΔSo won’t change with temperature
- This is often not true for many types of binding interaction a clear indication that the heat
capacities of the reactants and products are different
- Heat capacity: amount of energy that a substance absorbs as a function of temperature
- HA° = HA°’ + (T – 298) CP(A)°
T
- SA°(Tf) = SA°(Ti) + CP(A)° lnTf
i
The benefits of buying summaries with Stuvia:
Guaranteed quality through customer reviews
Stuvia customers have reviewed more than 700,000 summaries. This how you know that you are buying the best documents.
Quick and easy check-out
You can quickly pay through credit card or Stuvia-credit for the summaries. There is no membership needed.
Focus on what matters
Your fellow students write the study notes themselves, which is why the documents are always reliable and up-to-date. This ensures you quickly get to the core!
Frequently asked questions
What do I get when I buy this document?
You get a PDF, available immediately after your purchase. The purchased document is accessible anytime, anywhere and indefinitely through your profile.
Satisfaction guarantee: how does it work?
Our satisfaction guarantee ensures that you always find a study document that suits you well. You fill out a form, and our customer service team takes care of the rest.
Who am I buying these notes from?
Stuvia is a marketplace, so you are not buying this document from us, but from seller ScheikundeRU. Stuvia facilitates payment to the seller.
Will I be stuck with a subscription?
No, you only buy these notes for $4.33. You're not tied to anything after your purchase.
Can Stuvia be trusted?
4.6 stars on Google & Trustpilot (+1000 reviews)
79373 documents were sold in the last 30 days
Founded in 2010, the go-to place to buy study notes for 14 years now