Keeping Balancing Equations Cool Like They're Going Out of Style

During Friday's class, we went even deeper into balancing equations. So deep that many people would consider it impossible in anyway shape or form. Specifically, we discussed Molecular Equations, Complete Ionic Equations, and Net Ionic Equations.

Molecular Equations

• Molecular Equations show the overall stoichiometry of the equation, but not the actual forms of the substances
• (Example): KCl+AgNO3------------>KNO3+AgCl

Complete Ionic Equations

• Complete Ionic Equations represent, as ions, all substances that are strong electrolytes
• Ionic Compounds dissociate in water
• Spectator Ions are ions that don't react; spectator ions are still included in Complete Ionic Equations
• (Example): K(^+)+ Cl(^-)+NO3(^-)------------>AgCl+K(^+)+NO3(^-)

Net Ionic Equations

• Includes only those ions undergoing a charge (spectator ions are NOT included)
• Net Ionic Equations are only written if a solid is formed
• (Example): Cl(^-)+Ag(^+)------------->AgCl(s)

NOTE: Molecular Equations, Complete Ionic Equations, and Net Ionic Equations are all Double Replacement Reactions

After we deciphered Molecular Equations, Complete Ionic Equations, and Net Ionic Equations, we proceeded to work on our newest worksheet (Net Ionic Equation Worksheet). Here are some tips in completing this worksheet:

1. To find the Molecular Equation, balance the equation given
2. To find the Complete Ionic Equation, seperate ions from compounds (include charges)
3. If a reaction isn't seen, or there is no solid, a Net Ionic Equation isn't needed

We proceeded to work on the Net Ionic Equation Worksheet for the rest of class.

On Monday, we will be doing a series of 48 reactions. The reactions will help establish rules regarding what we talked about on Friday. Furthermore, there is a WebAssign due Monday, on section 4.2 (Precipitation Reactions).

Stay thursty, my friends.