Chem 103 - End of Chapter Problems & Clicker Questions
End of Chapter Problems
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Clicker Questions
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Chem 103 - Study Guide for Exam 1
| Chapter | Sections | |
Problems |
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| 1 | 1.1-1.8 | 8, 12, 14, 20, 22, 26, 30, 34, 38, 42 | ||
| 2 | 2.1-2.7 | 14, 20, 22, 26, 28, 30, 32, 42, 46, 62 | ||
| 3 | 3.1-3.7 | 12, 14, 20, 22, 28, 30, 32, 34, 40, 52, 56, 60 |
Note: Most of these problems will be worked in the SLC EI sessions, and some will appear on quizzes and exams (albeit with different compounds, chemical equations, or values).
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Objectives:
The student should be able to:
- Describe the scientific process. [Intro]
- Define the terms hypothesis, law, and theory. [Intro]
- Describe the nature of gases, liquids, and solids and interpret them according to the kinetic-molecular theory. [1.1]
- Recognize whether a substance is a pure substance or a mixture, and whether a mixture is homogeneous or heterogeneous. [1.1]
- Define the terms atom, element, molecule and compound. [1.2, 1.3]
- Carry out calculations involving density. [1.4]
- Convert between Celsius and Kelvin temperature. [1.4]
- Determine whether a property of a substance is an intensive property or an extensive property. [1.4]
- Recognize whether a change is a physical change or a chemical change. [1.5]
- Carry out calculations using the base SI Units in Table 1.2 and the prefixes in Table 1.3. [1.6]
- Define precision and accuracy. [1.7]
- Determine the number of significant figures in a measurement and use the correct number of significant figures in a calculation. [1.8]
- Perform calculations using dimensional analysis. [1.8]
- Carry out calculations involving percent. [1.8]
- State the postulates of Dalton's atomic theory and describe how they explain the laws of chemical composition. [lecture]
- Define the terms proton, neutron, electron, and describe the structure of the atom. [2.1]
- Define atomic number, mass number, and isotope, and determine the number of neutrons for a given isotope. [2.2, 2.3]
- Calculate average atomic masses (atomic weights) from isotopic abundances. [2.4]
- Define the mole, Avogadro's number, and molar mass. [2.5]
- Interconvert between masses, moles, and numbers of particles. [2.5]
- Classify elements in the periodic table as being main group or transition elements and whether they are metals, nonmetals or metalloids. [2.6]
- Recognize alkali metals, alkaline earth metals, chalcogens, halogens, and noble gases, and describe their chemical properties. [2.7]
- Understand molecular formulas and structural formulas, and molecular models. [3.1, 3.2]
- Predict the charges of ions of the elements on the left and right sides of the periodic table. [3.3]
- Write the formulas for ionic compounds by combining ions in the proper ratio. [3.3]
- Given a formula, write the name, or given a name, write the formula, for ionic compounds and binary molecular compounds. [3.3, 3.4]
- Determine the molar mass (formula weight or molecular weight) of a compound from its formula. [3.5]
- Perform calculations using the mole ratios of elements or ions in formulas as conversion factors. [3.5]
- Calculate percent composition from chemical formulas. [3.6]
- Understand the difference between empirical formulas and molecular formulas. [3.6]
- Determine empirical formulas from percent composition. [3.6]
- Calculate the number of water molecules in a hydrated compound from experimental data. [3.7]
Chem 103 - Study Guide for Exam 2
| Chapter | Sections | |
Problems |
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| 4 | 4.1-4.6 | 6, 8, 14, 18, 20, 22, 28, 30, 38 | ||
| 5 | 5.1-5.10 | 8, 12, 20, 26, 28, 36, 40, 44, 46, 50, 52, 62, 68, 72, 76 | ||
| 6 | 6.1-6.8 | 10, 24, 28, 32, 40, 46, 48, 52, 58 |
Note: Most of these problems will be worked in the SLC EI sessions, and some will appear on quizzes and exams (albeit with different compounds, chemical equations, or values).
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Objectives:
The student should be able to:
- Balance chemical equations. [4.2]
- Do stoichiometric calculations from balanced equations. [4.3]
- Determine the limiting reactant in a reaction. [4.4]
- Calculate the theoretical yield and percent yield in a reaction. [4.5]
- Use stoichiometric calculations in chemical analysis. [4.6]
- Define solution, solvent, solute; electrolytes, strong electrolytes, weak electrolytes, and nonelectrolytes, and be able to categorize compounds by these definitions. [5.1]
- Determine whether or not an ionic compound will be soluble in water and recognize what ions are formed when it is. [5.1]
- Predict the products of precipitation reactions; write balanced chemical equations and net ionic equations for them. [5.2]
- Define acids and bases; identify substances as acids or bases. [5.3]
- Write balanced and net ionic equations for acid-base neutralization reactions. [5.4]
- Predict the products of gas-forming reactions. [5.5]
- Define oxidation and reduction. [5.7]
- Recognize redox reactions, determine oxidation numbers, and identify the oxidizing agent and reducing agent. [5.7]
- Define molarity; do calculations involving molar concentrations, preparing solutions of known concentration, and dilution. [5.8]
- Define pH, and calculate the pH of a solution from its hydrogen ion concentration and vice versa. [5.9]
- Do stoichiometric calculations for reactions in aqueous solution and titrations. [5.10]
- Define kinetic and potential energy and the law of energy conservation. Convert between energy units. [6.1]
- Describe what is meant by a system and its surroundings, and the concept of exothermic and endothermic energy transfer between them. [6.1]
- Define heat capacity, and specific heat capacity; do problems involving heat capacity and energy transfer. [6.2]
- Use heat of fusion and heat of vaporization to determine energy quantities involved in changes of state. [6.3]
- Describe the first law of thermodynamics and how it relates to heat and work. [6.4]
- Define enthalpy change and describe how it relates to energy changes in chemical reactions. [6.5]
- Calculate heats of reaction from calorimetry data. [6.6]
- Explain how Hess’s Law relates to the law of energy conservation and use it to calculate enthalpy changes in chemical reactions. [6.7]
- Define standard state and standard molar enthalpies of formation. Use standard molar enthalpies of formation to calculate enthalpy changes in chemical reactions. [6.8]
Chem 103 - Study Guide for Exam 3
| Chapter | Sections | |
Problems |
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| 7 | 7.1-7.6 | 6, 18, 22, 24, 28, 34, 36, 54, 66 | ||
| 8 | 8.1-8.7 | 6, 14, 28, 32, 34, 44, 48, 62 | ||
| 9 | 9.1-9.10 | 16, 20, 22, 24, 26, 30, 32, 44, 48, 80 | ||
| 10 | 10.1-10.3 | 4, 8, 18, 28, 34, 42, 46, 52 |
Note: Most of these problems will be worked in the SLC EI sessions, and some will appear on quizzes and exams (albeit with different compounds, chemical equations, or values).
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Objectives:
The student should be able to:
- Describe the wave properties of light. Convert between wavelength and frequency. [7.1]
- Calculate the energy of a photon using Planck’s equation. [7.2]
- Describe the Bohr model of the atom, and calculate energy differences between any two allowed energy states of the hydrogen atom. [7.3]
- Calculate the wavelength of a particle using de Broglie's equation. [7.4]
- Define the uncertainty principle, wave functions, electron density, and orbitals, and understand the role they play in quantum mechanics. [7.5]
- Describe the quantum numbers n, l, and ml and list correct combinations of them. [7.5]
- Recognize the shapes of s, p, d and f orbitals. [7.6]
- Describe the electron spin quantum number ms, and how electron spin gives rise to diamagnetic and paramagnetic properties of substances. [8.1]
- Understand how the Pauli exclusion principle limits the number of electrons that can exist in a given orbital to two. [8.2]
- Know the relative energies of orbitals and the order in which they are filled by electrons. [8.3]
- Write the electron configuration, using orbital box diagrams, spectroscopic notation or noble gas notation, for any element or ion. [8.4, 8.5]
- Recognize core electrons and valence electrons. [8.4]
- Rank elements according to atomic radius, ionization energy, and electron affinity, and explain the trends. [8.6]
- Describe how periodic trends affect the chemical properties of the elements. [8.7]
- Draw Lewis symbols for atoms and ions. [9.1]
- Predict relative lattice energies for ionic compounds. [9.3]
- Draw Lewis structures for molecules and polyatomic ions, including formal charges. Use formal charge to determine which of several Lewis structures is more stable. [9.4, 9.8]
- Draw resonance structures for species that cannot be adequately described by a single Lewis structure. [9.5]
- Recognize when a species is an exception to the octet rule. [9.6]
- Predict electron-pair geometries and molecular geometries from the VSEPR model. [9.7]
- Predict bond polarities from electronegativities. [9.8]
- Predict whether a molecule will be polar or nonpolar. [9.9]
- Calculate enthalpies of reaction from bond dissociation energies. [9.10]
- Determine the hybridization used by each atom in molecules and polyatomic ions. [10.2]
- Describe the bonding in multiple bonds: sigma and pi bonds. [10.2]
- Draw molecular orbital diagrams for second-row diatomics and use them to determine bond orders and magnetic properties. [10.3]
Chem 103 - Study Guide for Final Exam
For Part 1, New material:
| Chapter | Sections | |
Problems |
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| 12 | 12.1-12.7 | 6, 12, 16, 22, 26, 28, 36, 40, 42, 92 | ||
| 13 | 13.1-13.10 | 4, 6, 8, 20, 34, 44, 50, 52, 54, 56 | ||
| 14 | 14.1-14.4 | 2, 6, 8, 24, 26, 30, 38, 40, 44, 50, 60, 66 |
Note: Most of these problems will be worked in the SLC EI sessions, and some will appear on quizzes and exams (albeit with different compounds, chemical equations, or values).
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For Part 2, Comprehensive: Problems from the first three exams.
Objectives:
The student should be able to:
For Part 1, New Material:
- Define pressure and interconvert units of atmosphere, torr (mm Hg), pascal and bar. [12.1]
- State the relationships between pressure, volume, and temperature of a gas, and work problems involving Boyle's law, Charles' law, Gay-Lussac's law, and Avogadro's law. [12.2]
- Carry out calculations involving the ideal-gas equation and standard molar volume. [12.3]
- Determine the molar mass of a gas from its density or from P, V, T data. [12.3]
- Work stoichiometry problems involving gas-phase reactions. [12.4]
- State Dalton's law of partial pressures and work problems involving partial pressures, mole fraction, and collecting gases over water. [12.5]
- State the postulates of the kinetic-molecular theory of gases. [12.6]
- Work problems involving root-mean-square speed and Graham's law of effusion. [12.6, 12.7]
- Define the various types of intermolecular forces (London dispersion, dipole-dipole, ion-dipole and H-bonding) and predict the relative boiling points of molecules. [13.2-13.4]
- Work problems involving heats of vaporization and heats of fusion. [13.5]
- Explain the relationship between vapor pressure, volatility, temperature and boiling point. [13.5]
- Perform calculations involving atomic and ionic radii and the dimensions of the unit cell for simple cubic, body-centered cubic, and face-centered cubic crystal structures. [13.6]
- Predict the types of bonding in solids and describe the resulting properties. [13.7-13.9]
- Interpret phase diagrams. [13.10]
- Interconvert between the concentration units mass percentage, parts per million, mole fraction, molarity, and molality. [14.1]
- Describe the solution process in terms of the intermolecular forces involved and the energy changes that occur. [14.2]
- Describe the factors affecting solubility: solute-solvent interactions, pressure effects (Henry's law), and temperature effects. [14.3]
- Define colligative properties and calculate vapor pressures of solutions from Raoult's law. [14.4]
- Calculate boiling-point elevation, freezing-point depression, and osmotic pressure for solutions, and determine molar masses of solutes from any of these three properties. [14.4]
For Part 2, Comprehensive:
Be able to do problems similar to those on the first three exams.
