Complete Ionic amp Net Ionic Equations

>> YOUR LINK HERE: ___ http://youtube.com/watch?v=nzGaMKBYqAg

In this video we'll look at the difference between molecular equations, complete ionic equations, and net ionic equations. • The Molecular equation is made up of compound or single element and does not include ions. For example: • AgNO3 + NaCl = AgCl + NaNO3 • We balance molecular equations by changing the coefficients in front of the compounds (the above equation is already balanced). • • In the Complete Ionic Equation the strong electrolytes are split into their ions. Note that solids, liquids, and gases are not split into ions - they stay together. For example: • Ag+ + NO3- + Na+ + Cl- = AgCl + Na+ + Cl- • Note AgCl is insoluble and is therefore a solid, which we do not split apart. • • In the Net Ionic Equation we remove the ions that are the same on both sides. These are called the spectator ions. They haven't changed. We end up with: • Ag+ + Cl- = AgCl • for the Net ionic equation. • ----------- • If you are unsure if a compound is soluble when writing net ionic equations you should consult a solubility table for the compound. • General Steps for writing Net Ionic equations: • 1. Write the balanced molecular equation. • 2. Write the state (s, l, g, aq) for each substance. • 3. Split soluble compounds into ions (the complete ionic equation). • 4. Cross out the spectator ions on both sides of complete ionic equation. • 5. Write the remaining substances as the net ionic equation. • Writing and balancing net ionic equations is an important skill in chemistry and is essential for understanding solubility, electrochemistry, and focusing on the substances and ions involved in the chemical reaction and ignoring those that don’t (the spectator ions). • More chemistry help at http://www.Breslyn.org

#############################

New on site