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Quarter 3: Post Test Review
A. Chemical Formulas and Equations
Write the following chemical formulas:
1. Calcium chloride
2. Chromium (II) sulfate
3. Zinc phosphate
4. Disulfur tetraoxide
5. Magnesium iodide
6. Hydrobromic acid
Write the following names of the chemical formulas:
6. BeF2
7. Hg2(OH)2
8. H3PO3
9. NaClO3
10. NaCl
11. Cu(NO3)2
Balance the following equations:
12. ___Al + ___Pb(NO3)2  ___Pb + ____Al(NO3)3
13. ___Mg(OH)2 + ___HCl  ___H2O + ___MgCl2
14. ___Al2(SO4)3  ____Al2O3 + _____SO3
Chemical Reactions Types:
15. What are the products of a combustion reaction ________________ and _______________
16. NaBr + Ca(OH)2  CaBr2 + NaOH
Type of reaction: ____________
17. C5H9O + O2  CO2 + H2O
Type of reaction: ____________
18. Pb + H3PO4  H2 + Pb3(PO4)2
Type of reaction: ____________
19. NH4OH  NH3 + H2O
Type of reaction: ____________
20. HBr + Al(OH)3  H2O + AlBr3
Type of reaction:_____________
B. Quantifying Matter
What is the molar mass of H2SO4? _________
b. CoCl2? _________ c. Ni3(PO4)2?_____
Determine the mass in grams of 40.0 moles of sodium
Calculate the moles in 510.0 g of aluminum sulfide
Calculate the number of moles in 1.00 grams of barium hydroxide
The octane present in gasoline burns according to the equation: 2 C8H18 + 25 O2 → 16 CO2 + 18 H2O
a. What is the mol to mol ratio of oxygen to water? _____: _____
26. When completing the above reaction (in number 28), the reaction runs out of the propane reactant before it runs
out of the oxygen reactant. Therefore, propane is called the ___________ ____________
27. What is the oxidation number of Manganese in KMnO4?
C. Bonding and Electron Configurations
28. Besides metallic, what are the other two types of bonding. _____________ and __________
b. define the relationship between electrons in these two types of bonds
c. a _______ bond is between a metal and a non-metal
d. a ________ bond is between two non-metals
29. What are the main differences between the Bohr model of an atom, a Lewis dot structure and the modern model of
the atom?
30. Draw the Lewis dot diagram for the following compounds:
a. CCl4 b. O2
c. NF3 d. H2O e. Br2
f. SO2
g. COF2
Which compounds have at least one double bond?
31. Fill in the following information
Orbital name
Max number of electrons
32. Write the full AND noble gas electron configuration for the following
a. sodium
b. neon
c. bromine
d. calcium
e. oxygen
33. How many more electrons do the following need to satisfy the octet rule?
a. [Ne] 3s23p3
b. 1s2,2s2, 2p4
D. Gas Laws
34. What is the kinetic molecular theory?
35. What is Boyle’s law? _______________________________
b. What is the relationship between pressure and volume?
36. What is Charles’s law? _______________________________
b. What is the relationship between volume and temperature?
37. What is the ideal gas law? ______________________________
38. When using the ideal gas law what are the units for the following?
Temperature = Pressure =
Volume =
39. What is STP?
40. ________ mmHg = __________torr = _________atm = __________kilopascals
Convert 2983.4 mmHg into torr. ___________________ convert in Pascals ________________
41. The volume of a balloon is 300. mL and has a pressure of 1.5 atm. If the pressure is increased to 3.0 atm, what is the
new volume?
42. What is the volume of a 2.0 mol sample of gas at 800 mm Hg and 5.0 0 C?
E. Acids and Bases
Define acid and base.
How is water both an acid and a base?
What is the expression for pOH? pH?
In the reaction, HCl + H2O ↔ H3O+ + Cl-, what are the conjugate base pairs?
Discuss each diagram in terms of precision and accuracy.