SEMESTER II MIDTERM EXAM REVIEW
Complete the practice problems on a separate sheet of paper.
Chapter 7: Chemical Reactions
 Write a balanced chemical equation given a word equation and vice versa
 Classify the 5 types of reactions
 Use activity series of the elements to predict products
 Use solubility chart to predict the formation of a precipitate
 Practice problems:
4. Write a balanced equation from this word equation. aqueous silver nitrate + copper metal  silver metal + aqueous copper nitrate
5. Write the balanced equation for the reaction between iron (III) chloride and sodium hydroxide. The products are iron (III) hydroxide and sodium chloride.
6. Use the activity series of metals and your knowledge of the relative reactivity of the halogens to predict the products for the reactions below. If no reaction occurs, just write “No Reaction”.
Write balanced equations for those reactions that do occur. a. Br
2
(g) + NaCl(aq)  b. Ca(s) + Mg(NO
3
)
2
(aq)  c. K(s) + H
2
SO
4
(aq)  d.
Zn(s) + NaOH(aq) 
7. Predict the products for the reactions below. Identify the precipitate formed and the aqueous product. If no precipitate is formed, write no precipitate. a. Zn(NO
3
)
2
+ SnCl
2
 b. KCl + AgNO
3
 c. Cu(NO
3
)
2
+ Na
2
S  d. Al
2
(SO
4
)
3
+ 3Mg(OH)
2

Chapter 9: Stoichiometry
 Understand what a mole ratio is and how it is used
 Mole to mole conversions mol A | mol B = mol B
| mol A
 Mass to mole conversions mass A | 1 mol A | mol B = mol B
| molar mass A | mol A
 Mole to mass conversions mol A | mol B | molar mass B = mass B
| mol A | 1 mol B
 Mass to mass conversions mass A | 1 mol A | mol B | molar mass B = mass B
| molar mass A | mol A | 1 mol B
 Theoretical vs. actual yield
 Percent yield: Actual . x 100
Theoretical
 Practice problems:
8. Two moles of potassium chloride and three moles of oxygen are produced from the decomposition of two moles of potassium chlorate, KClO3(s). Write the balanced equation. How many moles of oxygen are produced from 12 moles of potassium chlorate?
9. Given: H
2
(g) + Cl
2
(g)  2HCl(g), calculate the number of moles of hydrogen chloride produced from
10 moles of hydrogen.
10. Given: 2NO(g) + O
2
(g)  2NO
2
(g) , calculate the number of grams of nitrogen dioxide that are produced from 4 moles of nitric oxide.
11. Given: 2KClO
3
(s)  2KCl(s) + 3O
2
(g), calculate the mass of oxygen produced from the decomposition of 75.0 g of potassium chlorate.
12. In the reaction, 2Mg(s) + CO
2
(g)  2MgO(s) + C(s), 57.9 grams of magnesium oxide is actually produced when excess carbon dioxide reacts with magnesium metal. The theoretical yield of magnesium oxide is 70.9 grams. Find the percent yield of magnesium oxide.

1. H
2. Na
3. K
4. Rb
5. Be
How many orbitals are in the following sublevels: a. 1s b. 4d d. 5s e. 4f c. 6d f. 3p
What are the types of sublevels and number of orbitals in the following energy levels? a. n = 1 b. n = 4 d. n = 3 e. n = 2 c. n = 5
Write out the electron configuration for each of the following elements.

9. O
10. S
11. Cl
12. Br
13. I
14. Kr
15. Xe
16. Fe
6. Mg
7. Ca
8. Sr