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23 Cards in this Set
- Front
- Back
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Delta G should be __________ for a favorable reaction |
negative |
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Delta G = _______ - ________ |
Delta H - T*Delta S |
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DeltaG = -______________ |
-RTlnKeq |
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Cations are _________ whereas anions are _________ |
Positive, negative |
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When a compound donates H it is considered a Bronsted-Lowry _______________ |
Base |
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When a compound accepts H it is considered a Bronsted-Lowry __________________ |
Acid |
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A proton is ___________ |
H+ |
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A lewis acid is an ______________________ |
electron pair acceptor |
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A lewis base is an ________________ |
electron pair donor |
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All Lewis __________ are electrophiles |
acids |
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_______________ Ka values are more acidic |
Larger |
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Ka = ?/? |
= [H3O+][A-]/[HA] |
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______________ pKa values are more acidic |
Lower |
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pKa = _________ |
=-logKa |
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Ka = 10^? |
-pKa |
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pH=_____________ |
-log[H30+] |
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The stronger the acid, the ___________ its conjugate base |
weaker |
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The larger the pKa of the conjugate acid, the _________________ its conjugated base |
stronger |
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Acidity increases within a given row by the _________________ effect |
electronegativity (left to right) |
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Acidity increases within a given column by the _______________________ effect |
bond strength (top to botttom) |
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The stronger the bond the _____________ the acid is |
weaker |
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The __________ the electronegativity of an atom, the easier it will acquire a negative charge |
higher |
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Generally, the presence of very strong base in a reaction requires the use of aprotic solvents, i.e. the solvents without _____________ protons like in -OH groups |
acidic (dissociable) |
