CH 18(CH 10 Kaplan) Acids and Bases Flashcards
(37 cards)
1
Q
What is the definition or an Arrhenius Acid/Base?
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2
Q
What is the definition or an Arrhenius Acid/Base?
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3
Q
What is the definition of a Lewis Acid/Base?
A
Lewis Acid = Electron Acceptor, has a vacant orbital to accept a lone pair
Lewis Base= Electron Donor
Most comprehensive definition
4
Q
Lower the pKa the (stronger/weaker the acid)?
A
Lower the pKa the stronger the acid
5
Q
Higher the pKa the (stronger/weaker the acid)?
A
Higher the pKA = weaker acid
6
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Higher Ka = stronger or weaker acid?
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Higher Ka = stronger acid
7
Q
Lower Ka = stronger or weaker acid?
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Lower Ka = weaker acid
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16
Q
What is the definition of a Bronsted-Lowry Acid?
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17
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What is the definition of a Bronsted-Lowry Base?
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23
Q
What is the definition of a Lewis Acid?
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24
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What is a Lewis Base?
A
25
What is the definition of a Lewis Acid-Base reaction?
Donation and acceptance of a lone pair to form a covalent bond
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Which species are considered amphoteric? (3 answers)
1) Partially dissociated conjugated base of polyvalent acid
2)Hydroxides of certain metals (Al, Zn, Pb, and Cr)
3)Oxidizing and reducing agents
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True or false: Every Arrhenius acid is a Bronsted-Lowry acid and every Bronsted-Lowry Acid is a Lewis Acid?
True
30
Which acid/base definition is considered amphiprotic?
Bronsted-Lowry: can donate or accept a proton making it amphiprotic
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/(Electronegative elements positioned near an acidic proton ________ (increase/decrease) acid strength by__________________
Electronegative elements positioned near an acidic proton INCREASE acid strength by pulling electron density away from the bond holding the proton
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What are the approximate pH values for these reactions?
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Periodic Table trends: Acidity _________ across a period and down a group
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