Question | Answer |
acetic acid CH3COOH | strong acid |
carbonic acid H2CO3 | strong acid |
hydrogen sulfide H2S | weak acid |
dihydrogen phosphate ion H2PO4- | weak acid |
ammonium ion NH4+ | weak acid |
hydrocyanic acid HCN | weak acid |
phenol C6H5OH | weak acid |
bicarbonate ion HCO3- | weak acid |
hydrogen phosphate ion HPO4 2- | weak acid |
water H2O | weak acid |
ethanol C2H5OH | weak acid |
Iodide ion | Weak Base |
chloride ion | Weak Base |
hydgrogen sulfate ion | Weak Base |
nitrate ion | Weak Base |
water | Weak Base |
sulfate ion | Weak Base |
dihydrogen phosphate ion | Weak Base |
acetate ion | Weak Base |
bicarbonate ion | Strong Base |
hydrogen sulfide ion | Strong Base |
hydrogen phosphate ion | Strong Base |
ammonia | Strong Base |
cyanide ion | Strong Base |
phenoxide ion | Strong Base |
carbonate ion | Strong Base |
phosphate ion | Strong Base |
hydroxide ion | Strong Base |
ethoxide ion | Strong Base |
most important factor determining relative acidities of organic compounds | stability of molecular structure where the greater the electronegativity of anion formed when H is removed the more stable the more acidic |
how electronegativity, resonance, and inductive effect determine stability of anions | greater electrondegativity, more resonant structures, delocalized negative charge(neg side and pos side) make better acids that want to give up H+ or proton |
Hydroiiodic acid HI | strong acid |
hydrochloric acid HCl | strong acid |
Sulfuric Acid H2SO4 | strong acid |
Nitric Acid HNO3 | strong acid |
Hydronium ion H3O+ | strong acid |
Hydrogen sulfate ion | strong acid |
Phosporic Acid H3PO4 | strong acid |
Arrhenius Acid | dissociate in aqueous solution to form hydrogen ions (H+) |
Arrhenius Base | which dissociate in aqueous solution to form hydroxide (OH−) ions |
Bronsted-Lowry Acid | ability to "donate" hydrogen ions (H+) or protons |
Bronsted-Lowry Base | ability to "accept" hydrogen ions (H+) or protons |
Rules for using curved arrows | Show the change in position of electron pairs where tail is at electron pair and head shows new position showing bond formation or breaking |
1st Rule of writing acceptable Resonance Contributing Structures | must have the same number of valence electrons |
2nd Rule of writing acceptable Resonance Contributing Structures | must obey the rules of covalent bonding 2e- for H, 2nd Per. 8e- 3rd Per 12e- |
3rd Rule of writing acceptable Resonance Contributing Structures | positions of all nuclei must be the same with differences only in distribution of valence e- |
4th Rule of writing acceptable Resonance Contributing Structures | must have the same total number of unpaired and paired e- |
strong acid | an acid that ionises completely in an aqueous solution by losing one proton |
strong base | compound that is able to deprotonate very weak acids in an acid-base reaction |
1st step to determine position of acid-base equilibrium | identify two acids on each side of equation |
2nd step to determine position of acid-base equilibrium | determine which acid is the stronger |
3rd step to determine position of acid-base equilibrium | identify the stronger base knowing that the stronger acid gives a weaker base |
4th step to determine position of acid-base equilibrium | stronger acid and base react to give weaker acid and base therefore equilibrium goes toward the weaker acid and base |
Acidity of alcohols, water, and carboxylic acid | alcohols weaker than water and much weaker than carboxylic acids |