South Pasadena • AP Chemistry



( AP Chemistry Name ____________________________________

Mod ___ Date ___/___/___

Chapter 1 - Chapter 3 ( Chemistry Basics

Ch1- Ch 3 STUDY QUESTIONS and PROBLEMS

Test will be 20 MC (1 points each) and 2 Free Response (12 and 13 points)= total 45 points

1. Name the polyatomic ions:

C2H3O2-

IO4-

OH-

HCO3-

Cr2O72-

ClO3-

2. What are the formulas of the polyatomic ions:

phosphate nitrite

sulfate cyanide

sulfite chlorite

3. Write the ions present in the following salts and predict their formulas:

potassium bromide

calcium carbonate

magnesium iodide

lithium oxide

aluminum sulfate

4. Name the following ionic salts:

| (NH4)2SO4 | Co2(SO4)3 |

|KHCO3 |NiSO4 |

|Ca(NO3)2 |AlPO4 |

RbOH Ca(OH)2

5. Name the following binary compounds of the nonmetals:

CS2

SF6

IF5

N2H4

PCl5

Cl2O7

HIO3 H2C2O4

HI H2S

6. What are the formulas for the following binary compounds?

| silicon dioxide | phosphorus tribromide |

|boron trifluoride |disulfur dichloride |

|dinitrogen pentoxide |hydrogen selenide |

7. a. How many moles are present in 128 grams of sulfur dioxide?

b. What is the mass of 3 moles of oxygen molecules?

c. If 5 moles of a metallic element have a mass of 200 grams, which element is it?

d. What is the molar mass of methane CH4?

e. How many moles of nitrogen atoms are there in 6 moles of TNT (trinitrotoluene CH3C6H2(NO2)3)?

8. What is the percent by mass of nitrogen in ammonium nitrate?

9. The hydrocarbons ethylene (molar mass 28 g/mol), cyclobutane (molar mass 56 g/mol), pentene (molar mass 70 g/mol), and cyclohexane (molar mass 84 g/mol), all have the same empirical formula. What is it? Write the molecular formulas for these four compounds.

10. Given the following reaction: NaBH4 + BF3 ( NaBF4 + B2H6

If you begin with 18.9g of NaBH4 and you isolate 7.50g of B2H6 gas, what is the percent yield of this reaction?

11. The reaction of methane and water is one way to prepare hydrogen:

CH4(g) + H2O(g) ( CO(g) + 3 H2(g)

If you begin with 995 g of CH4 and 2510 g of water, what is the maximum possible yield of H2?

12. Disulfur dichloride, S2Cl2, is used to vulcanize rubber. It can be made by treating molten sulfur with gaseous chlorine:

S8(l) + 4 Cl2(g) ( 4 S2Cl2(l)

Starting with a mixture of 32.0 g of sulfur and 71.0 g of Cl2, which is the limiting reactant? What mass of S2Cl2 (in grams) can be produced? What mass of the excess reactant remains when the limiting reactant is consumed?

13. Ethyl butyrate is a compound that contains C, H, and O. When .00278g of ethyl butyrate is combusted it forms .00632g CO2 and .00258g of water. What is the empirical formula? If the molecular mass is 116g/mol, what is the molecular formula?

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