Honors Chemistry Final ExamName: ______

Study Guide 2013-2014Period: ______

Exam Date: Thursday, June 12th

The final exam will consist of a series of calculations/ concepts worth 100 points. The exam questions will mimic each unit test that you have taken during semester two. This review is worth 10% of final exam score.

Given information on the Exam- The blue packet which includes:

Periodic Table

Electronegativity Chart

Solubility Chart

Activity Series

STP conditions

R (ideal gas law constant)

Part A.

Mathematics of Chemistry- This section involves simple conversations through the mole. You can anticipate conversions between grams, volume, particles, and moles.

A 2.5 L of carbon dioxide gas contains how many molecules of carbon dioxide?

What is the percentage of oxygen that is present in the above carbon dioxide sample?

Part B.

Chemical Equations- This section will involve identifying the type of chemical reaction (synthesis, decomposition, single replacement, double replacement, and combustion) and write the balanced chemical reaction.

Butane (C4H10) is burned in air.

Solutions of nitric acid and lithium hydroxide are mixed.

Part C.

Atomic Theory and Structure- This section is an assessment of 1st semester material. You’ll be asked to identify the atomic number, atomic mass, number of protons, number of neutrons, and number of electrons. You’ll also be asked to determine the electron configuration of an element, indicate a possible ion, and distinguish between ions and isotopes.

Determine the electron configuration of chlorine.

What is the most common ion for chlorine.

Indicate two possible isotopes of chlorine.

Chemistry Calculations and Concepts-

5 questions with multiple parts you select one stoichiometry problem and two others to answer completely.

  1. Stoichiometry Problem
  2. Stoichiometry Problem
  3. Gas Laws – Ideal Gas Law, Combined Gas Law, Dalton’s Law
  4. Solution Stoichiometry involving dilutions
  5. IMFs and Organic Chemistry

Stoichiometry- What mass of lead (II) iodide will be produced when 16.4g of lead (II) nitrate is added to 28.5g of potassium iodide?

Solutions- Formalin is an aqueous solution of formaldehyde, HCHO, used as a preservative for biological specimens. How many grams of formaldehyde must be used to prepare 2.5 L of 12.3 M formalin?

Solution Stoichiometry- Acid rain results from the reaction of nitrogen dioxide with water in the air.

3NO2 (g) + H2O (l)  2HNO3 (aq) + NO(g)

At STP, how many liters of NO2 gas are required to produce 0.275 L of 0.400 M HNO3?

Gas Laws

a. Chlorine gas, Cl2, is used to purify the water in swimming pools. How many moles of chlorine gas are in a 7.00 L tank if the gas has a pressure of 865 mmHg and a temperature of 240C?

b. What is the molar mass of a gas if a 2.21 g sample occupies a volume of 0.425 L at STP?

c. Limestone (CaCO3) reacts with HCl to produce aqueous calcium chloride and carbon dioxide gas.

i. Determine the balanced chemical reaction.

ii. How many liters of carbon dioxide are produced at 752 mmHg and 240C from a 25.0 g

sample of limestone?

IMFs and Organic Chemistry

  1. Determine the structure of the following organic compounds:

i.Methyl propane

ii.1-chloro 2- pentene

iii.2-hexanol

  1. Draw the structure for the following compounds:

i.Propane

ii. Propanal

  1. Indicate on the two structures above the possible intermolecular forces.
  1. Which of the two structures above is likely to have the higher boiling point? Why?