Presentation is loading. Please wait.

Presentation is loading. Please wait.

Reactions in aqueous solutions

Similar presentations


Presentation on theme: "Reactions in aqueous solutions"— Presentation transcript:

1 Reactions in aqueous solutions

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

7

8 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

9 Where to draw that 2 there is a difference between MF2 and Mg2+ + 2 F-
MgF2 means the Fluorine ions are bonded to the magnesium ion. Everything is clumped together in an ionic crystalline structure Mg F- implies there is a magnesium and 2 fluoride ions NOT bonded together floating around

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

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


Download ppt "Reactions in aqueous solutions"

Similar presentations


Ads by Google