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STAAR Ladder to Success

STAAR Ladder to Success. Rung 10. Arrhenius Definition. Savante Arrhenius, Swedish chemist who by 1890 formulated the first useful theory for acids. Acids contain hydrogen ions. Bases contain hydroxide ions (OH - ). Bronsted -Lowry Definition. Acids are proton (H + ) donors.

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STAAR Ladder to Success

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  1. STAAR Ladder to Success Rung 10

  2. Arrhenius Definition Savante Arrhenius, Swedish chemist who by 1890 formulated the first useful theory for acids. • Acidscontain hydrogen ions • Basescontain hydroxide ions (OH-)

  3. Bronsted-Lowry Definition • Acidsare proton (H+) donors. • Bases are proton (H+) acceptors. • Conjugate acid-base pairs are formed.

  4. conjugate base conjugate acid Bronsted-Lowry Definition Pairs identifies the particles formed when H+ ions are donated and accepted when an acid or a base is dissolved in water. Base gains H+  conjugate acid formed Particle that remains  conjugate base HCl + H2O  Cl– + H3O+ acid base

  5. pH = -log[H3O+] pOH = -log[OH-] pH + pOH = 14

  6. - + Strength • Strong Acid/Base • 100% ionized in water • many ions produced • strong electrolyte HCl HNO3 H2SO4 HBr HI HClO4 NaOH KOH Ca(OH)2 Ba(OH)2

  7. - + Strength • Weak Acid/Base • does not ionize completely • few ions produced • weak electrolyte HF CH3COOH H3PO4 H2CO3 HCN NH3

  8. Determining Types of Reactions

  9. Neutralization • Chemical reaction between an acid and a base. • Products are a salt (ionic compound) and water. ACID + BASE  SALT + WATER HCl + NaOH NaCl + H2O • Salts can be neutral, acidic, or basic. • Neutralization does not mean pH = 7.

  10. Single Replacement A + BC  B + AC • Whether one metal will replace another metal from a compound is determined by the reactivities of the two metals. • To help us determine this, an activity series of metals arranges metals in order of decreasing reactivity. • A reactive metal will replace any metal listed below it in the activity series.

  11. Precipitation Reactions • Double replacement reaction where a precipitate is formed due to the insolubility of the compound that is formed. • Refer to the solubility rules.

  12. Oxidation numbers • The apparent charge assigned to an atom of an element • Metal: positive charge • Nonmetal: negative charge • Key points to remember: • The sum of the oxidation numbers of the elements in any compound is 0. • The sum of the oxidation numbers of the elements in any ion (polyatomic) is equal to the charge on the ion.

  13. Reduction-oxidation reactions (redox) • Any chemical reaction in which changes in oxidation numbers occur • Has two parts: • Oxidation: one reactant is losing electrons or increases in oxidation number • The reactant losing electrons or increasing in oxidation number is known as the reducing agent • Reduction: other reactant is gaining electrons or decreases in oxidation number • The reactant gaining electrons or decreasing in oxidation number is known as the oxidizing agent

  14. Using oxidation numbers • If there are changes in atomic oxidation numbers in the reaction, meaning loss and gain of electrons, then the reaction ISredox. • If there are no changes in atomic oxidation numbers then the reaction IS NOT redox.

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