AP Chemistry – Fall Final Exam

Exam Details

• The exam will consist of three (3) questions that are AP-style in formatting
• Each question will have multiple parts and require calculations
• You will be permitted to use the AP periodic table and the AP formula sheets
• The exam is designed to require one hour to complete but you will have 90 minutes to do so
• The exam could pull from any of the first 10 chapters of the textbook
• Note: PRACTICE exams are made available for those wishing to try extra problems

Exam Objectives

• Use experimental data to draw a conclusion from an experiment (1.4 – 1.6)
• Use the rules of scientific notation and significant figures to appropriate express measurements (1.6 – 1.6)
• Explain the structure of atoms and the particle that comprise atoms (2.1 – 2.5)
• Write formulas and names of chemical compounds (2.6 – 2.8)
• Use the concept of the mole to calculate the composition of a compound (3.3 – 3.5)
• Balance chemical reactions (3.6)
• Use mole-mass relationships to relate the reactants and products in a reaction (3.6 – 3.7)
• Predict the products of reactions in aqueous solutions (4.1 – 4.4)
• Use the concept of molarity to compare quantities of compounds in solutions (4.5 – 4.6)
• Use the First Law of Thermodynamics to relate energy changes in a process (5.1 – 5.3)
• Use calorimetry and enthalpy to determine the energy change in a reaction (5.4 – 5.7)
• Use emission spectra as evidence of the electronic structure of an atom (6.1 – 6.4)
• Write electron configurations of atoms and ions and connect these to electron orbitals (6.5 – 6.9)
• Use the periodic table to compare electronic properties of atoms (7.1 – 7.8)
• Draw the Lewis dot structures for chemical compounds and ions (8.1 – 8.7)
• Identify the polarity of a bond and the overall polarity of a molecule (8.4, 9.3)
• Predict the 3D shape of a molecule (9.1 – 9.2)
• Identify the bonding being used by an atom in a compound (9.4 – 9.6)
• Use gas laws to determine the changes in properties of gases in a process (10.1 – 10.6)
• Use Kinetic Molecular Theory to relate the micro properties of a gas to the macro properties of a gas (10.7 – 10.8)