1. Chemical equations and solutions Chapter 6 and 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  Na + Cl 2  NaCl  To balance it  2 Na + Cl 2  2 NaCl

4. Subscript letters  The phase of substance is often denoted by subscript letters in parenthesis  solid –s, liquid-l, gas-g  Na (s) + Cl 2(g)  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) O H H positive side 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) -  MgF 2(s)  Mg (aq) 2+ + 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 F 2 and 2 F  F 2 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 + HCO 3 -  NaHCO 3 →Na + (aq) + HCO 3 - (aq)

9. Write the dissociation equation for  Chromium (III) chlorate  Potassium Oxide

10. Write the dissociation equation for  Nickel (II) phosphate  Calcium Chloride