Term
| If NH3 were to behave as an acid, its conjugate base would be NH2-. |
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Definition
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Term
| Delocalization of electron density is a stabilizing factor |
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Definition
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Term
| Amide ion, NH2-, is a Lewis base. |
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Definition
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Term
| H3O+ is a stronger acid than NH4+ and, therefore, NH3 is a stronger base than H2O. |
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Definition
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Term
| Inductive effects can be used to describe electron delocalization. |
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Definition
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Term
| The direction of equilibrium in an acid-base reaction favors the side containing the stronger acid and stronger base. |
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Definition
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Term
| The conjugate base of CH3CH2OH is CH3CH2O-. |
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Definition
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Term
| CH3+ and NH4+ are Lewis acids. |
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Definition
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Term
| Between a strong acid and a weak acid, the weak acid will give rise to the stronger conjugate base. |
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Definition
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Term
| H2O can function as an acid (proton donor) and as a base (proton acceptor). |
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Definition
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Term
| The strongest base that can exist in aqueous solution is OH-. |
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Definition
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Term
| A strong acid is one that completely ionizes in aqueous solution. |
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Definition
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Term
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Definition
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Term
| A Bronsted-Lowry acid is a proton donor. |
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Definition
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Term
| When comparing the relative strength of acids, the stronger acid has the smaller value of pKa. 2.3 |
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Definition
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Term
| When comparing the relative strengths of acids, the stronger acid has the smaller value of Ka. 2.3 |
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Definition
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Term
| The formulas of a conjugate acid-base pair differ only by a proton. 2.2 |
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Definition
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Term
| A Lewis base is an electron donor. 2.6 |
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Definition
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Term
| Acetic acid, CH3COOH, is a stronger acid than carbonic acid, H2CO3, and therefore, acetate ion, CH3COO-, is a stronger base then bicarbonate ion, HCO3-. 2.2 |
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Definition
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Term
| The strongest acid that can exist in aqueous solution is H3O+. 2.4 |
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Definition
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Term
| A Lewis acid-base reaction results in the formation of a new covalent bond between the Lewis acid and the Lewis base. 2.6 |
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Definition
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Term
| When a base accepts a proton in an acid-base reaction, it is converted into its conjugate base. 2.2 |
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Definition
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Term
| When a metal hydroxide, MOH, dissolves in water, the solution becomes basic because of the presence of hydroxide ions, OH-. 2.1 |
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Definition
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Term
| A Lewis acid is a proton acceptor. 2.6 |
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Definition
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Term
| If NH3 were to behave as a base, its conjugate acid would be NH4+. 2.2 |
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Definition
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Term
| Resonance effects can be used to describe electron delocalization. 2.5 |
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Definition
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Term
| All Lewis acid-base reactions involve transfer of a proton from the acid to the base. |
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Definition
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Term
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Definition
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Term
| When HCl dissolves in water, the major ions present are the H+ and Cl-. 2.3 |
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Definition
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Term
| Acid-base reactions take place only in aqueous solution. 2.6 |
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Definition
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Term
| The conjugate acid of HCO3- is H2CO3. 2.2 |
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Definition
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