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20 Cards in this Set
- Front
- Back
Describe a Bronsted acid.
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A Bronsted acid is a H+ donor.
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Describe a Bronsted base.
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A Bronsted base is a H+ acceptor.
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Describe a Lewis acid.
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A Lewis acid is also known as an electrophile--an e- pair acceptor.
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Define a Lewis base.
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A Lewis base is also known as a nucleophile--an e- pair donor.
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What is the general structural characteristic of an acid?
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A H+ bound to an electronegative atom.
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What is the general structural characteristic of a base?
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Presence of lone electron pairs which can bond with a proton.
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What is Ka?
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Ka =
1) The equilibrium constant for dissociation. 2) The acidity constant |
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List the two equations for Ka.
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1) Ka = [Conjugate base][Conjugate acid] / [Acid]
2) Ka = Keq[H2O] |
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True or false?
More bonds between two atoms make for a shorter bond length? |
False.
More bonds between two atoms make for longer bond lengths. |
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True or false?
Less bonds between two atoms make for stronger bonds. |
False.
More bonds between two atoms means greater bond strength. |
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What is the hierarchy of characteristics that determine which resonance structure the molecule looks like?
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1) More full shells
2) Has the most bonds 3) Least charge separation |
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What is the definition of Ka?
How is Ka calculated? |
Ka = the acid dissociation constant
Ka = {[H3O+] [A-]} / [HA] HA + H3O+ ---> (H3O+) + A- |
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What is the equation of pKa?
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- log (Ka) = pKa
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What is the relationship between Ka and pH?
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Higher Ka = more acidic
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What is the relationship between pKa and acidity?
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Lower pKa = more acidity
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What are the three properties of organic molecules mentioned in Chapter 2?
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1) Boiling point
2) Melting point 3) Solubility |
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Define boiling point.
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Boiling point
The amount of energy needed to separate molecules. |
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Define "dispersion forces".
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Dispersion forces
Momentary charge dispersion. |
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What characteristics of molecules determine dispersion forces? Explain each.
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- Size
Larger molecules elicit more dispersion forces. - Surface area More surface area elicit more dispersion forces. |
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List the hierarchy of bonds that determine boiling point.
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1) H-bonds between molecules
Why? H-bonds between molecules are strong. 2) Dipole moments 3) Dispersion forces |