1) There are two forces holding the particles of different solids together. How are these forces different?

 

2) In a water solution, Sodium chloride dissociates into what?

 

3) Assuming complete dissociation (like our book does), how many ions will these chemicals procduce in solution? (answers will be whole numbers)

NaCl=___ CaCl2=___ ZnSO4=___
K2SO4=___ Ba(OH)2=___ (NH4)2SO4=___

4) If you dissolve 2 moles of CaCl2 in water, how many moles of Ca+ ions do you get?____ How many moles of Cl- ions?
 

5) For each of the six chemicals in the table above, write the equations showing their dissociation into ions. Don't forget coefficients if needed.

 

 

 

 

 


6) If you mix solutions of Ammonium sulfide and Cadmium nitrate, what products do you get?

 

7) What's the difference between an "overall" ionic equation and a "net" ionic equation?

 

8) Write the overall ionic equation for the reaction mentioned in #6 above. (please try it on your own before peeking on page 429)

 

9) Which of the ions from #8 above are the "spectator" ions?
 

10) Ionic compounds, like NaCl, are already made of ions. What do you call it when a molecule (which are non-ionic) creates an ion?

 

11) What's the difference between ionization and dissociation?

 

12) Take a second look back at figure 13-9 on page 405. Specifically, look at the two green "hydrated Cl-" ions. Based on this picture, make up a definition of hydration and write it here:

 

13) Hydrogen chloride is a molecule... it is not ionic. Yet it ionizes in water. Why?

 

14) H3O? What sort of madness is this? Where does come H3O come from?

 

15) If a molecule dissolved in water only weakly conducts electricity, what sort of electrolyte is it?

 

16) Does a molecule have to dissolve completely to be considered a strong electrolyte?

 

17) Why is HF considered a weak electrolyte?

 

18) The last paragraph in section 14-1 gives an important idea. What is this idea?