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HOBr is a weaker acid than HBrO3. Account for this fact.

HOBr is a weaker acid than HBrO3. Account for this fact. Strong Acid/Weak Acid. The number of oxygen atoms will effect the strength of the acid. HOBr has a single oxygen atom while HBrO3 contains three.

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HOBr is a weaker acid than HBrO3. Account for this fact.

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  1. HOBr is a weaker acid than HBrO3. Account for this fact.

  2. Strong Acid/Weak Acid • The number of oxygen atoms will effect the strength of the acid. HOBr has a single oxygen atom while HBrO3 contains three. • Oxygen is a very electro negative atom and will draw electrons away from the H-Br bond thus weakening the bond making it easier to dissociate when in dissolved in water. The more oxygen atoms the weaker the H-Br bond. • Charge of X • The charge on the X which in this case is the Br atom has a different charge in HOBr (+1) than in HBrO3 (+5) • Strength of O-H Bond • Strength of X-O Bond

  3. Arrhenius Acid Base Concept Arrhenius Acid/Base Concept • Acids produce Hydrogen ions (H+) within an aqueous solution • Bases produce Hydroxide Ions (OH-) in solution • Definition is limited because it applies only to acids and bases that can dissociate OH- and H+ ions • Examples: • NaOH will dissociate into Na+ and OH- • HCl will dissociate into H+ and Cl-

  4. Bronsted-Lowry Model • The model definition of Acid/Base • Bronsted Acid – A proton “donor” • Bronsted Base – A proton “acceptor” • The definition applies to many more molecules that may exhibit Acid/Base qualities but do not directly produce OH- or H+ ions. • Every Acid and Base has a conjugate Acid or Base • Water can act as an acid and a base • H3O+ (Hydronium ion) (acid) and OH- (Base)

  5. Bronsted-Lowry Model • Example of Bronsted Base • NH3(aq) + H2O(l) NH4+(aq) + OH-(aq) • Example of Bronsted Acid • HC2H3O2(aq) + H2O(l) H3O+(aq) + C2H3O2-(aq) Base Acid Conjugate Acid Conjugate Base Weak Acid Base Conjugate Acid Conjugate Base

  6. Lewis Acid/Base Definition • Lewis Acid/Base Definition • Lewis Acid – Electron Pair Acceptor • Lewis Base – Electron Pair Donor • Encompasses an even wider variety of molecules (Bronsted and Arrhenius) even ones that do not donate protons or produce OH- ions. • Must be aware of the Lewis structure of a particular molecule to determine whether it is a Lewis Acid or Base.

  7. Lewis Acid/Base Definition • Examples • BF3(g) + NH3(g)  F3BNH3(g) • BF3 is the Lewis Acid because it has no free unpaired electrons with only has 6 electrons around the central atom (Boron will require one more pair of electrons to complete the valence shell) • NH3 is the Lewis Base because the molecule has a completed octet valence shell with free unpaired electrons on the central atom. The BF3 will accept these unpaired electrons and form a covalent bond.

  8. Lewis Acid/Base Definition • Example • Ni2+(aq) + 6NH3(aq)  [Ni(NH3)6]2+(aq) • Ni2+ is the Lewis Acid because it is a cation which will attract negatively charged electrons to toward itself. • The NH3 is the Lewis Base because it provides the free unpaired electrons for the Ni2+

  9. Lewis Acid/Base Definition • Example • Even earlier definitions are encompassed in the Lewis Acid Model • H+ + H2O  H3O+

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