1. Iron (remember electron configuration)
Chemistry
Tutoring this afternoon
Agenda –
Bellringer (5 min)
Finish Activity Series if not complete
Finish Net Ionic Equations if not complete
Begin precipitate section
Draw a Bohr model for each of the following atoms and be able to explain why you drew it the way you did.
Iron (remember electron configuration)

2. Objectives

3. Reaction Type: Single Replacement
An activity series  helps us predict when one metal will replace another.
The element farther up the list will replace one lower on the list.
Also, a halogen can replace a different halogen only if it (the halogen to do the replacing) is above it (the halogen to be replaced) on the periodic table
This reaction will happen, while the one below will not.
Reaction Type: Single Replacement

6. Objectives

7. This is the way that we have done balanced reactions so far
However, in aqueous solutions (in water) most ionic compounds dissociate (separate into cations and anions)
We can now show a complete ionic equation by showing each dissolved (aqueous) ionic compounds as being free ions (split them apart and show the charges & (aq)).
Net Ionic Equations

8. Notice that the NO3- does not change (stays aqueous)
Notice that the NO3- does not change (stays aqueous). Since the nitrate ion and the sodium ion appear on both sides of the equation and they do not seem to do anything in this reaction, they are called a spectator ions. We will actually not even show them in the reaction (cross them out).
This new equation is called a net ionic equation (net as in after everything that is not important is removed).
Net Ionic Equations

9. In the previous reaction, both sides of the equation are balanced (neutral on both sides)
In any net ionic equation the charge on the reactant side must equal the charge on the product side.
In this reaction, nitrate is the spectator ion again.
Net Ionic Equations

10. In this net ionic reaction, there is a +1 charge on the reactant side and a +2 charge on the product side. This is unacceptable.
Net Ionic Equations

11. Chemistry Tutoring this afternoon Agenda – Bellringer (5 min)
Finish Net Ionic Equations if not complete
Begin precipitate section

12. Process: 1. If a substance is ______, separate it into ions. 2
Process: 1. If a substance is ______, separate it into ions. 2. Any ions that are still _____ are eliminated because they are spectators. 3. Determine _______ of each ion left. 4. balance equation so that both ______ and ______ are equal on both sides.

14. Predicting a Precipitate
A precipitate (ppt) is a solid that is sometimes formed when combining two non-solid reactants.
The only way to know if it will form a ppt is to look at its solubility.
If it is insoluble, then it will form a ppt.
AgCl? , H3PO4?, Mg(NO3)2?
Predicting a Precipitate

15. Predicting a Precipitate
For this we have to look at the chart to the left.
This should be a double displacement reaction forming sodium nitrate (soluble) and barium carbonate (insoluble)
After we determine the solubility of the products, we can now find the net ionic equation.
2Na+(aq)+CO32-(aq)+Ba2+(aq)+2(NO3)-(aq) 2Na+(aq) +2(NO3)-(aq)+Ba(CO3)(s)
Predicting a Precipitate

16. Predicting a Precipitate
This leaves us the above reaction as our net ionic reaction
Predicting a Precipitate

17. Solutions of iron (II) sulfate and barium hydroxide are mixed.
For each of the following combinations of reactants, do the following:
• Predict possible products with phase labels
• Write the balanced chemical equation. If no visible reaction occurs, write NR. If a
precipitate forms, give the formula and name of the precipitate.
• Write the complete ionic equation and net ionic equation for all reactions
(whether or not a visible reaction occurs)
Solutions of iron (II) sulfate and barium hydroxide are mixed.
Solutions of calcium chloride and potassium phosphate are mixed.
Solutions of calcium nitrate and sodium chloride are mixed.
Solutions of potassium chloride and silver nitrate are mixed.
Solutions of sodium sulfide and nickel (II) sulfate are mixed.