ch231hchapter5
Chapter 5 Learning Goals
- You understand that when water is a solvent, both dipolar interactions and hydrogen bonding can play a role in stabilizing the (solvated) solute.
- You understand that ionic compounds dissolve in water to form solvated ions. The electron-rich oxygen points to the cation; the electron-poor hydrogens point to the anion.
- You understand that an ionic solution will contain a balanced number of dissolved ions moving freely through the medium.
- You understand that the ability of dissolved ions to move is the basis for such solutions to conduct electricity as positively charged ions (cations) move to the negatively-charged cathode, and negatively charged ions (anions) move to the positively-charged anode.
- You know that mixing different ionic solutions can create a precipitate of an insoluble or poorly-soluble ionic compound. You can write the net ionic reaction for such a case, and recognize the role of nonreacting "spectator ions" in the mixed solutions.
- You can recognize the core reaction type of acid-base neutralization and if given a balanced acid-base reaction, identify the acid, the base, and the salt produced.
- You know how acids lead to formation of H3O+ in water, and how bases lead to formation of OH- in water (each with an appropriate counterion). You further recognize that any use of the term "H+(aq.)" should be interpreted as meaning the H3O+ ion.
- You can recognize oxidation/reduction ("redox") reactions based on changes in oxidation state of the reactants.
- You can identify the oxidizing agent and the reducing agent in any redox reaction.
- You can balance redox reactions by analyzing the two balanced half-reactions involved.
Note: Weak acid chemistry and titration will be left to Chapter 16, covered in a later course in the sequence.
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