Final exam

The final exam will have 45 multiple choice questions, and it is suggested to review quizzes, practice tests, and tests from the semester. Below is a list of potential topics:

Chapter 2: Measurement and Problem Solving

  • Be able to convert any number into scientific notation (powers of ten).

  • Significant figures: know both +/- and x/divide rules; be able to combine the rules.

  • Be able to convert from one unit to another using dimensional analysis.

  • Be able to convert volumes and densities using dimensional analysis.

Chapter 3: Matter and Energy

  • Be able to determine whether a process is a physical or chemical change.

  • Understand the conservation of mass during a chemical reaction.

  • Be able to convert temperature units given F=95C+32F = \frac{9}{5} C + 32.

  • Be able to convert energy units using given conversion factors.

  • Solve heat flow problems using q=(mass)×(sp.ht.capacity)×(ΔT)q = (mass) \times (sp. ht. capacity) \times (\Delta T).

Chapter 4: Atoms and Energy

  • Determine protons, neutrons, and electrons in any isotope or ion.

  • Determine likely charges on Main Group elements of the Periodic Table when forming ions.

  • Know the names of select groups (chemical families) in the Periodic Table.

  • Know the trends in chemical behavior of the elements in the Periodic Table.

  • Understand how the atomic mass of each element is determined (weighted average of isotopes).

Chapter 5: Molecules and Compounds

  • Decide whether a compound is ionic or molecular based on its formula or name.

  • Name a compound given its formula or write its formula from the name for:

    1. Binary ionic compounds made from predictable ions.

    2. Binary ionic compounds made from variable charge metal ions.

    3. Polyatomic ionic compounds.

    4. Diatomic molecular compounds.

    5. Molecular compounds.

    6. Acids.

  • Calculate the formula weight of the compounds listed above.

Chapter 6: Chemical Composition

  • Determine the molar mass of any element, molecular, or ionic compound.

  • Convert back and forth from grams to moles to Avogadro’s number of atoms, ions, or molecules.

  • Determine % by mass of an element in any compound.

  • Determine the empirical formula from % composition.

  • Determine the molecular formula from empirical formula and molar mass.

Chapter 7: Chemical Reactions

  • Balance chemical equations.

  • Understand the behavior of ionic and molecular compounds in aqueous solutions.

  • Predict the precipitate formed when mixing two aqueous solutions based on solubility.

  • Identify an oxidation/reduction reaction.

  • Write a net ionic equation for various reactions.

  • Know combustion reactions and the products formed from carbon/hydrogen compounds.

Chapter 8: Quantities in Chemical Reactions

  • Use balanced chemical equations to calculate grams or moles of reactants/products.

  • Determine the limiting reactant given the quantities of all reactants.

  • Calculate % yield from starting quantities and actual yield.

Chapter 10: Chemical Bonding

  • Draw Lewis structures for atoms, ions, and molecules.

  • Predict bond polarity based on electronegativity.

  • Predict molecular polarity based on molecule shape.

Chapter 12: Intermolecular Forces (IMF)

  • Determine existing IMF’s in a substance.

  • Predict relative melting/boiling points based on the strength of IMF.

  • Identify different types of crystalline solids.

Chapter 13: Solutions

  • Perform calculations with concentration units % by mass and molarity (M).

  • Carry out calculations with dilutions of stock solutions.

  • Solve stoichiometry problems involving solutions.

  • Determine miscibility based on the polarity of liquids.

  • Understand concepts of osmosis, freezing point depression, and boiling point elevation.

Chapter 14: Acids and Bases

  • Recognize the differences between strong and weak acids.

  • Identify conjugate acid/base pairs.

  • Calculate pH using concentrations of H3O+ and OH- in solutions.

  • Understand how buffers work and their components.

Chapter 15: Chemical Equilibrium

  • Know factors affecting reaction rates and collision theory principles.

  • Understand what it means for a chemical reaction to be at equilibrium.

  • Recognize how system changes affect the equilibrium position and calculate equilibrium constants.

Chapter 2: Measurement and Problem Solving

  • Lesson 1: Scientific Notation

    • Understand how to convert any number into scientific notation (powers of ten).

  • Lesson 2: Significant Figures

    • Learn the rules for significant figures: addition/subtraction and multiplication/division.

    • Practice combining the rules.

  • Lesson 3: Dimensional Analysis

    • Convert between units and apply dimensional analysis in different contexts.

    • Use dimensional analysis for volume and density conversions.

Chapter 3: Matter and Energy

  • Lesson 4: Physical vs. Chemical Changes

    • Identify processes as physical or chemical changes.

  • Lesson 5: Conservation of Mass

    • Discuss the conservation of mass during chemical reactions.

  • Lesson 6: Temperature Conversion

    • Convert temperature units using the formula F=95C+32F = \frac{9}{5} C + 32.

  • Lesson 7: Energy Conversion

    • Use conversion factors for energy units.

  • Lesson 8: Heat Flow Problems

    • Solve problems involving heat flow using the equation q=(mass)×(sp.ht.capacity)×(ΔT)q = (mass) \times (sp. ht. capacity) \times (\Delta T).

Chapter 4: Atoms and Energy

  • Lesson 9: Isotopes and Ions

    • Determine protons, neutrons, and electrons in isotopes or ions.

  • Lesson 10: Charges of Main Group Elements

    • Identify likely charges on Main Group elements when forming ions.

  • Lesson 11: Periodic Table Groups

    • Know the names of select groups (chemical families) in the Periodic Table and their trends in chemical behavior.

  • Lesson 12: Atomic Mass

    • Understand how atomic mass is determined (weighted average of isotopes).

Chapter 5: Molecules and Compounds

  • Lesson 13: Ionic vs. Molecular Compounds

    • Decide whether a compound is ionic or molecular based on its formula or name.

  • Lesson 14: Naming and Formulating Compounds

    • Practice naming and writing formulas for:

    1. Binary ionic compounds made from predictable ions.

    2. Binary ionic compounds with variable charge metal ions.

    3. Polyatomic ionic compounds.

    4. Diatomic molecular compounds.

    5. Molecular compounds.

    6. Acids.

  • Lesson 15: Formula Weight Calculation

    • Calculate the formula weight of the listed compounds.

Chapter 6: Chemical Composition

  • Lesson 16: Molar Mass

    • Learn to determine molar mass of elements and compounds.

  • Lesson 17: Conversions

    • Convert between grams, moles, and Avogadro’s number.

  • Lesson 18: Percent by Mass

    • Determine the % by mass of elements in compounds.

  • Lesson 19: Empirical and Molecular Formulas

    • Find empirical formulas from % composition and molecular formulas from empirical formula and molar mass.

Chapter 7: Chemical Reactions

  • Lesson 20: Balancing Equations

    • Learn to balance chemical equations.

  • Lesson 21: Ionic and Molecular Behavior

    • Understand the behavior of ionic and molecular compounds in aqueous solutions.

  • Lesson 22: Precipitation Reactions

    • Predict precipitates when mixing aqueous solutions based on solubility.

  • Lesson 23: Oxidation/Reduction Reactions

    • Identify oxidation/reduction reactions and write net ionic equations.

  • Lesson 24: Combustion Reactions

    • Know combustion reactions and the products from carbon/hydrogen compounds.

Chapter 8: Quantities in Chemical Reactions

  • Lesson 25: Using Balanced Equations

    • Calculate grams or moles of reactants/products using balanced chemical equations.

  • Lesson 26: Limiting Reactant

    • Determine the limiting reactant and calculate % yield from starting quantities and actual yield.

Chapter 10: Chemical Bonding

  • Lesson 27: Lewis Structures

    • Draw Lewis structures for atoms, ions, and molecules.

  • Lesson 28: Bond Polarity

    • Predict bond polarity based on electronegativity.

  • Lesson 29: Molecular Polarity

    • Predict molecular polarity based on shape.

Chapter 12: Intermolecular Forces (IMF)

  • Lesson 30: Identifying IMF

    • Determine existing intermolecular forces in substances.

  • Lesson 31: Melting/Boiling Points

    • Predict relative melting/boiling points based on IMF strength.

  • Lesson 32: Crystalline Solids

    • Identify different types of crystalline solids.

Chapter 13: Solutions

  • Lesson 33: Concentration Calculations

    • Perform calculations with concentration units: % by mass and molarity (M).

  • Lesson 34: Diluptions

    • Carry out calculations involving dilutions of stock solutions.

  • Lesson 35: Stoichiometry with Solutions

    • Solve stoichiometry problems involving solutions.

  • Lesson 36: Miscibility

    • Determine miscibility based on liquid polarity.

  • Lesson 37: Osmosis and Boiling/Freezing Point Changes

    • Understand osmosis, freezing point depression, and boiling point elevation concepts.

Chapter 14: Acids and Bases

  • Lesson 38: Strong vs. Weak Acids

    • Recognize differences between strong and weak acids.

  • Lesson 39: Conjugate Pairs

    • Identify conjugate acid/base pairs.

  • Lesson 40: pH Calculations

    • Calculate pH using concentrations of H3O+H_3O^+ and OH−OH^- in solutions.

  • Lesson 41: Buffers

    • Understand how buffers work and their components.

Chapter 15: Chemical Equilibrium

  • Lesson 42: Reaction Rates and Collision Theory

    • Discuss factors affecting reaction rates and principles of collision theory.

  • Lesson 43: Equilibrium

    • Understand chemical reaction equilibrium concepts.

  • Lesson 44: System Changes and Equilibrium Position

    • Recognize how system changes affect equilibrium position and calculate equilibrium constants.

Term 1: What are the steps to convert a number into scientific notation?
Definition 1: Convert any number into powers of ten, ensuring only one non-zero digit is to the left of the decimal point.
Term 2: What are the rules for significant figures in addition/subtraction and multiplication/division?
Definition 2: For addition/subtraction, the answer should have the same number of decimal places as the measurement with the least. For multiplication/division, the answer should have the same number of significant figures as the measurement with the least significant figures.
Term 3: How do you determine if a process is a physical or chemical change?
Definition 3: A physical change alters the form of a substance without changing its identity, while a chemical change transforms a substance into different substances.
Term 4: What is the conservation of mass, and how does it apply to chemical reactions?
Definition 4: The conservation of mass states that mass is neither created nor destroyed in a chemical reaction; the total mass of reactants equals the total mass of products.
Term 5: How do you convert temperature from Celsius to Fahrenheit?
Definition 5: Use the formula F=95C+32F = \frac{9}{5} C + 32 for conversion.
Term 6: What is the formula for calculating heat flow in a substance?
Definition 6: The formula is q=(mass)×(sp.ht.capacity)×(ΔT)q = (mass) \times (sp. ht. capacity) \times (\Delta T).
Term 7: How can you find the number of protons, neutrons, and electrons in an isotope?
Definition 7: Use the atomic number for protons (same as the element), the mass number minus the atomic number for neutrons, and for ions, add or subtract electrons based on the ion's charge.
Term 8: How do you determine if a compound is ionic or molecular based on its formula?
Definition 8: Ionic compounds typically consist of metals and nonmetals; if the formula has metal and nonmetal or a polyatomic ion, it is ionic. Molecular compounds consist of nonmetals only.
Term 9: What is the process to calculate the formula weight of a compound?
Definition 9: Sum the molar masses of all atoms in the compound's formula.
Term 10: How do you find the empirical formula from percent composition?
Definition 10: Convert the percent composition to grams, then to moles, divide by the smallest number of moles to find the ratio of elements.
Term 11: How do you identify an oxidation/reduction reaction?
Definition 11: Look for changes in oxidation states: oxidation is an increase while reduction is a decrease in oxidation number.
Term 12: What are the differences between strong and weak acids?
Definition 12: Strong acids completely dissociate in solution, while weak acids only partially dissociate.

Term 1: What are the differences between strong and weak acids?
Definition 1: Strong acids completely dissociate in solution, while weak acids only partially dissociate.
Term 2: How do you identify conjugate acid/base pairs?
Definition 2: A conjugate acid/base pair consists of two species that differ by one proton (H+).
Term 3: How do you calculate pH using concentrations of H<em>3O+H<em>3O^+ and OH−OH^- in solutions? Definition 3: Use the formula pH=−extlog([H</em>3O+])pH = - ext{log}([H</em>3O^+]); for OH−OH^-, use pOH=−extlog([OH−])pOH = - ext{log}([OH^-]) and pH+pOH=14pH + pOH = 14.
Term 4: What is the role of a buffer solution?
Definition 4: A buffer solution maintains a relatively constant pH upon the addition of small amounts of acid or base; it consists of a weak acid and its conjugate base or a weak base and its conjugate acid.
Term 5: How do factors affect reaction rates in chemical reactions?
Definition 5: Factors include concentration of reactants, temperature, presence of catalysts, and surface area of reactants which can all influence the speed of a chemical reaction.
Term 6: What does it mean for a chemical reaction to be at equilibrium?
Definition 6: At equilibrium, the rates of the forward and reverse reactions are equal, and the concentrations of reactants and products remain constant over time.
Term 7: How do system changes affect equilibrium position?
Definition 7: According to Le Chatelier's principle, if a system at equilibrium is subjected to a change in concentration, temperature, or pressure, the equilibrium position shifts to counteract that change.
Term 8: How do you calculate equilibrium constants?
Definition 8: The equilibrium constant (K) is calculated using the concentrations of products over reactants, each raised to the power of their coefficients in the balanced chemical equation: K=rac[products][reactants]K = rac{[products]}{[reactants]}.