Acids and Bases Review

Acids and Bases Review - “Hypo” “ite” “Ite”...

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Unformatted text preview: “Hypo” “ite” “Ite” “Ate” “Per” “ate” n. Base n. Acid mphiprotic/Amphoteric (either acid or base) HI HNO 3 H 2 SO 4 HClO 4 HClO 3 c ept F Andrew Rosen Naming Acids Binary Acids: Hydrogen and a nonmetal. “Hydro --- IC” HBr – Hydrobromic acid H 2 S – Hydrosulfuric acid *charges must have a net of 0* Ternary Acids: Hydrogen and polyatomic ion. “Ate” “Ic” “Ite” “Ous” HNO 3 – Nitrate – Nitric acid HNO 2 – Nitrite – Nitrous acid *Atoms in the same group have the same pattern as another element in the same group* Arrhenius’ Theory of Acids-Bases Acids: Produce H + ions (protons or H 3 O + ) as only positive ion in solution Bases: Produce hydroxide ions (OH- ) as only negative ion in solution Ionization: Ions produced from a molecular compound in solution HCl (l) H + (aq) + Cl- (aq) Dissociation: Ions produced from an ionic compound in solution NaOH (s) Na + (aq) + OH- (aq) Brønsted-Lowry Theory of Acids-Bases Acids: Proton (H + ) donor Bases: Proton acceptor NH 3 + H 2 O ↔ NH 4 + + OH- HCl + H 2 O ↔ H 3 O + + Cl- NH 2- + H 2 O ↔ NH 3 + OH- H 3 O + + OH- ↔ H 2 O + H 2 O N H 3 + N H 3 ↔ NH 4 + + NH 2- * The conjugates are always the opposites Lewis’ Theory of Acids-Bases Acids: Electron pair acceptor Bases: Electron pair donor NH 3 – Lewis Base BF 3 – Lewis Acid Anhydrides (must get rid of hydrogens) Acid Anhydride (without H...
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This note was uploaded on 02/17/2011 for the course CHEM 101 taught by Professor Me during the Spring '11 term at Bellarmine.

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Acids and Bases Review - “Hypo” “ite” “Ite”...

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