• Stoichiometry Calculations Study Guide For Content Mastery Teacher Edition

The Chemistry 1210 Final Exam consists of 40 questions and covers Chapters 1-10 and 12 from the 12th Edition of “Chemistry the Central Science” by Brown, LeMay, Bursten, Murphy, and Woodward. To assist you on the exam you will be given the following information:. The following Practice Exams can serve as a starting point for your studying, but as you saw from the previous exams, the content will be the same, but the questions will be worded differently. (Chapters 1-10) (Chapters 1-10) Dr. Zellmer is teaching CHEM 1250 this semester and his first three exams cover the chapters on the final. The links to his web-site are shown below: The Following topics will be fair game on the exam: Section 1.5 Significant Figures Use significant figures, scientific notation, SI units and dimensional analysis in calculations. Section 1.6 Dimensional Analysis Know common metric unit and SI units and prefixes, and be able to convert between units in calculations.

Empirical Information you are expected to know: The volume relationship 1 cm 3 = 1 mL The meaning of the prefixes: kilo-, deci-, centi-, and milli- (Table 1.4) Empirical Information you are not expected to memorize: Conversions between metric and english units. Prefixes other than those listed above. Lab #1: Scientific Measurements Know definition of density and be able to calculate quantities using it. Know difference between accuracy and precision, and be able to distinguish between determinate and indeterminate errors and be able to apply these terms when analyzing a data set. Lab #2: Separation of the Components of a Mixture Distinguish among elements, compounds and mixtures (including separation methods for mixtures).

Distinguish between molecular substances and ionic substances in terms of their composition. Describe the organization of the periodic table including the locations of metals and nonmetals. Section 2.1-2.3 Atomic Structure Describe the structure of the atom in terms of protons, neutrons, and electrons. Describe the electric charge and relative masses of protons, neutrons, and electrons. Express the subatomic composition of isotopes/ions using chemical symbols together with atomic number and mass number.

Write the complete atomic symbol for ions (including atomic number, mass number, and charge). Section 2.4 Atomic Weight Relate atomic weights to the masses of individual atoms and to their natural abundances. Section 3.4 Avogadro’s Constant and the Mole Convert grams to moles and moles to grams using molar masses, and convert number of molecules to moles and moles to number of atoms or molecules using Avogadro’s number. Section 2.8 Common Cations and Anions Know all the ions and charges on Table 2.4 and 2.5 Use the periodic table to predict the charges of common ions. Section 2.8 Nomenclature Write the empirical formulas of ionic compounds, given the charges of their component ions. Write the name of an ion given its chemical formula, or write the chemical formula given its name. Write the name of an ionic compound given its chemical formula, or write the chemical formula given its name.

Name or write chemical formulas for binary inorganic compounds and for acids. Section 3.1 Chemical Equations Balance chemical equations. Section 3.1 Chemical and Physical Changes Distinguish between chemical and physical change. Section 3.2 Chemical Reactions Identify simple combination, decomposition, and combustion reactions, predict their products, and write their balanced chemical equations.

Law of Conservation of Mass in chemical reactions. Section 3.7 Limiting Reactants and Theoretical Yield Determine the limiting reactant in a reaction and use it to determine the amounts of products formed. Section 3.7% Yield Calculate the percent yield of a reaction. Section 3.5 Empirical and Molecular Formulas Calculate the empirical and molecular formula of a compound from percentage composition and molecular weight. Section 3.6 Quantitative Information From Chemical Equations Be able to relate particle level diagrams to a balanced chemical equation and vice-versa. Section 4.1 Electrolytes Classify substances as either strong electrolytes, weak electrolytes or non-electrolytes.

Demonstrate an understanding of the differences between the three. Recognize and differentiate between strong acids, weak acids, strong bases and weak bases. Section 4.2-4.3 Reactions in Aqueous Solution Identify simple acid-base, precipitation and redox reactions and be able to predict the products of such reactions.

Stoichiometry Calculations Study Guide For Content Mastery Teacher Edition

Interpreting the Solubility Guidelines You do not have to memorize these. They will be attached to the exam. Net Ionic Equations Given the molecular equation for a reaction be able to identify spectator ions and write the full ionic equation and/or the net ionic equation for the same reaction. Section 4.4 Oxidation-Reduction Reactions Assign oxidation numbers to individual atoms in neutral substances and ions, and use these assignments to determine which substance is reduced which substance oxidized in a redox reaction.

Interpreting the Activity Series You do not have to memorize this series. It will be attached to the exam. Reactions Involving Gaseous Products Be able to predict which reactions will produce a gaseous product. Section 4.5 Concentration Calculate the molarity of a solution, and be able to convert between molarity, the number of moles present in a solution, and the volume of the solution.

Dilution Know how to prepare a dilute solution with a specific concentration and volume from a more concentrated solution. Stoichiometry in Solution and Lab #3: Development of an Equation Determine limiting reactants and/or calculate theoretical yields of reactions involving aqueous solutions. Use the results of a titration to determine the concentration of an unknown solution. Section 4.6 Titrations Know what an equivalence point/end point of a titration is and be able to use it to perform calculations based on titration data. Section 5.2-5.3 Heat and Change in Enthalpy Express the relationships among the quantities heat and change in ethalpy. Learn their sign conventions, including how the signs of heat and change in enthalpy relate to whether a process is exothermic or endothermic. Section 5.2 The First Law of Thermodynamics State the first law of thermodynamics and understand how it is applied in chemical reactions.

Section 5.2 State Functions Understand the concept of a state function and be able to give examples of quantities that are and are not state functions. Section 5.4 Stoichiometry of Thermochemical Reactions Use thermochemical equations to relate the change in enthalpy to the amount of substance involved in the reaction. Section 5.5 Calorimetry Relate temperature measurements and heat transferred by using heat capacities or specific heats. Section 5.6 Hess’s Law Use Hess’s law to determine enthalpy changes for chemical reactions. Experiment #6: Calorimetry and Hess’s Law Section 5.7 Standard Enthalpy of Formation Use standard enthalpies of formation to calculate the standard enthalpy change for reactions.

Section 6.1 Photon Energy Explain what photons are, and be able to calculate their energies given either their frequency or wavelength. Calculate the wavelength of electromagnetic radiation given its frequency or its frequency given its wavelength. Order the common kinds of radiation in the electromagnetic spectrum according to their wavelengths or energy.

Section 6.2 Quantized Energy and Photons Use quantum theory to understand that energy is quantized and to explain the photoelectric effect. Section 6.3 The Bohr Hydrogen Atom Using the Bohr theory, explain how line spectra relate to the idea of quantized energy states of electrons in atoms. Be able to identify the limitations of the Bohr Model.

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Experiment #7: Emission of Light and Atomic Models Section 6.5 Quantum Numbers Relate the quantum numbers to the number and type of orbitals, and recognize the different orbital shapes. Section 6.6 Atomic Orbitals Interpret radial probability function graphs for the orbitals. Draw an energy-level diagram for the orbitals in a many-electron atom, and describe how electrons populate the orbitals in the ground-state of an atom, using the Pauli Exclusion Principle and Hund’s rule.

Section 6.7-6.9 Electron Configuration/Orbital Block Notation Use the periodic table to write condensed electron configurations and determine the number of unpaired electrons in an atom. Section 7.2 Effective Nuclear Charge Understand the meaning of effective nuclear charge and how the effective nuclear charge depends upon nuclear charge and electron configuration. Section 7.3-7.5 Periodic Trends Use the periodic table to predict the trends in atomic radii, ionic radii, ionization energy, and electron affinity. Section 7.3 Atomic Radii Explain how the radius of an atom changes upon losing electrons to form a cation or gaining electrons to form an anion. Section 7.4 Ionization Energy Explain how the ionization energy changes as we remove successive electrons. Recognize the jump in ionization energy that occurs when the ionization corresponds to removing a core electron.

Section 7.4 Electron Configuration of Ions Be able to write the electron configurations of ions. Section 7.5 Electron Affinity Understand how irregularities in the periodic trends for electron affinity can be related to electron configuration. Section 8.2 Lattice Energy Be able to understand how lattice energy is dependent upon the charge and size of ions. Be able to recognize how lattice energy relates to physical properties such as melting point and boiling point.