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Reactions in aqueous solutions

This review focuses on chemical reactions in aqueous solutions, outlining the essential components of reactions, including reactants and products, as well as the role of the yields sign. Key examples, such as the reaction of sodium and chlorine gas to form table salt, are provided. The chapter explains how ionic compounds dissolve in water through dissociation, emphasizing the importance of water as a polar molecule in separating ions. The review also covers polyatomic ions and offers homework exercises on dissociation equations for various ionic compounds.

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Reactions in aqueous solutions

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  1. Reactions in aqueous solutions Chapter 6 moving into chapter 7

  2. Review • Two parts to a reaction • reactants (what you start with) and products (what you make) • In the middle is always a “” (yields sign), this separates the products and reactants

  3. An example • Sodium and chlorine gas react to form table salt • 2 Na + Cl2 2 NaCl

  4. Subscript letters • The phase of substance is often denoted by subscript letters in parenthesis • solid –s, liquid-l, gas-g • 2 Na(s) + Cl2(g)2 NaCl(s) • Some ionic compounds tend to dissolve in water • Ions dissolved in water get the subscript- (aq) • it stands for aqueous (water-like)

  5. Why it dissolves in water Water is a polar molecule (meaning it has a positive and negative side) positive side H H O negative side The positive side attaches itself to anions and the negative side attaches to cations, water then rips the ions away from each other, allowing the ions to float freely in the water.

  6. Dissociation Equations • dissociation- separating of ionic compounds into free ions in a solution • for NaCl in water • NaCl(s)  Na+(aq)+ Cl-(aq) • MgF2(s)  Mg2+(aq)+ 2 F-(aq) • Why did you need 2 in front of F? • Because there are two F’s on the reactant side

  7. Where to draw that 2 • there is a difference between F2 and 2 F • F2 means the Fluorine molecules are bonded together • 2 F implies there are 2 fluorine atoms NOT bonded together floating around

  8. Polyatomic Ions • In this chapter we do NOT break apart polyatomic ions • Sodium hydrogen carbonate • Na+ HCO3- • NaHCO3→Na+(aq)+ HCO3-(aq)

  9. Homework • give the formula and show the dissociation equation for: • cobalt (II) iodide • potassium sulfate

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