Final Exam Study Guide PDF

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Chemistry 105 Final Exam Study Guide 1. Properties of Matter: Describe matter in terms of phases, physical and chemical properties, and physical and chemical changes, using symbolic, macroscopic, and microscopic notation. 1. Define chemistry and matter 2. Describe phases of matter and phase changes according to energy and particle motion 3. Classify different forms of matter as elements, compounds, mixtures, etc. 4. Distinguish between physical and chemical properties, physical processes and chemical reactions 5. Apply the laws of conservation of mass, definite proportions, and multiple proportions 6. Use standard representations to describe molecules 2. Quantitative Reasoning: Perform scientific calculations while attending to precision, accuracy, units, and significant figures. 1. Analyze data to determine if it is accurate and/or precise 2. Perform simple arithmetic calculations using significant figures 3. Assign appropriate units to all measurements 4. Use metric prefixes to report measurements more conveniently 5. Use dimensional analysis to convert simple and compound units 3. History of the Atom: Explain how scientific discoveries have shaped our understanding of the atom over time. 1. Describe the contributions of Dalton, Thompson, Millikan and Curie to our understanding of atoms. 2. Define atomic number, atomic mass, and mass number in terms of subatomic particles 3. Explain the concept of and calculate the average atomic mass 4. Explain how atomic spectra led to insights about the structure of atoms 5. Describe the Bohr Model of the atom, and calculate energies of electronic transitions 6. Understand the limitations of Bohr’s Model 4. Light: Describe properties of light and the relationships between them. 1. Describe properties of light including wavelength, frequency, energy, and intensity 2. Relate wavelength, frequency, and energy of light both qualitatively and quantitatively (using equations). 3. Describe the problem of blackbody radiation and the solution proposed by Planck 4. Explain how changing the wavelength, frequency, energy, or intensity of light would affect the output of electrons in the photoelectric effect 5. Explain the photoelectric effect and use it to calculate work functions or kinetic energies of escaped electrons.

6. Calculate deBroglie wavelengths 5. Modern Atomic Theory: Use modern atomic theory to describe the probability of finding an electron in a particular location. 1. Distinguish between orbits and orbitals 2. Define  and 2 3. Use quantum numbers n, l, and ml to describe the size, shape, orientation and energy of orbitals including angular and radial nodes 4. Use quantum numbers to describe electrons 5. Write the electron configuration for an element or ion, following the Aufbau Principle 6. Define the term isoelectronic and identify an isoelectronic series 7. Draw an orbital diagram for an element or ion, also following the Pauli Exclusion Principle and Hund’s Rule 8. Identify diamagnetic and paramagnetic electron configurations 9. Identify the most stable monatomic ion for main group elements 10. Classify ground vs. excited state electron configurations 6. Periodic Table and Trends: Use the periodic table to identify important chemical properties of the elements. 1. Use the periodic table to identify groups of elements (alkali metals, alkaline earth metals, halogens, noble gases, metals, nonmetals, metalloids) or periods on the periodic table and to describe reactivity 2. Define the term mole, as used in chemistry 3. Calculate molecular mass/formula mass for a chemical compound 4. Use mole-based conversion factors in dimensional analysis 5. Define atomic or ionic radius, ionization energy, electron affinity, and electronegativity 6. Explain trends in these periodic properties using Zeff and quantum numbers 7. Explain anomalies in ionization energy and electron affinity based on orbital filling patterns 8. Compare first, second, and third ionization energies 7. Bonding: Use the periodic table and Coulomb's law to classify substances by type of bonds. Use valence bond theory and molecular orbital theory to describe covalent bonding patterns. 1. Compare and contrast types of bonding including ionic, covalent, and metallic 2. Predict trends in lattice energy for ionic compounds based on ion charge and size (Coulomb's Law). 3. Explain the differences between valence bond theory and molecular orbital theory 4. Identify, draw, and describe sigma and pi bonds using valence bond theory. 5. Identify hybridization of orbitals and relate it to molecular geometries 6. Know the difference between atomic and molecular orbitals

7. Recognize or draw sigma and pi bonding and antibonding orbitals 8. Fill molecular orbital diagrams to predict bonding and magnetic properties 9. Describe bonding in metals and semiconductors 8. Representations as Models: Given a chemical formula, draw an appropriate Lewis structure, including resonance forms, and use that structure to predict properties including bond order, geometry, and polarity. 1. Draw Lewis Dot Structures for elements and monatomic ions 2. Draw Lewis Dot Structures for ionic compounds 3. Draw Lewis Dot Structures for small molecules 4. Define bond order and identify single, double and triple bonds from Lewis Dot Structures 5. Assign formal charges in Lewis Dot Structure 6. Explain the concept of resonance and draw correct resonance structures 7. Identify the most stable resonance forms for a molecule 8. Draw Lewis dot structures for exceptions to the octet rule 9. Describe the relationship between bond order, length, and strength and predict trends based on structure. 10. Use Lewis Structures to identify common electron group geometries 11. Use Lewis Structures to identify common molecular geometries 12. Explain exceptions to idealized bond angles 13. Analyze a molecular structure to determine if the molecule is polar or nonpolar 9. Nomenclature: Communicate about chemicals using standard naming conventions for covalent and ionic inorganic compounds, acids, and simple organic compounds. 1. Name ionic compounds or write their formulas from names 2. Name acids or write their formulas from names 3. Name covalent compounds or write their formulas from names 4. Name and draw the structure given the name of alkanes, alkenes, and alkynes. 10. Organic Chemistry: Create and use line-bond diagrams of organic molecules, including recognizing common functional groups and isomers. 1. Draw and interpret line notation diagrams of molecules. 2. Recognize functional groups including alkenes, alkynes, aromatics, alcohols, ethers, aldehydes, ketones, esters, carboxylic acids, amines, amides 3. Recognize structural, geometric, and optical isomers. a. Draw structural isomers for a given molecular formula. b. Identify chiral/stereo centers in optical isomers 11. Gas Laws: Use the kinetic molecular theory and variables P, V, n, and T to describe the behavior of gases, and calculate changes under new experimental conditions.

1. Use Kinetic-Molecular Theory to explain the behaviors of gases. 2. Explain Effusion and Diffusion. 3. Describe the four variables used to characterize a gas. 4. Identify the relationships between pressure, temperature, volume, and number of moles and use the combined gas law to calculate how changes in certain variables will affect other variables. 5. Use the ideal gas law to calculate the pressure, temperature, volume, or number of moles of gas given the other values. 6. Find molar mass and density of a gas using the ideal gas law. 7. Use stoichiometry to calculate outcomes of gas phase reactions. 8. Perform calculations using Dalton's Law of Partial Pressures. 9. Explain principles that govern solubility of gases. 10. Understand the deviations of real gases from ideal gases. 12. Intermolecular Forces: Identify predominant intermolecular forces in pure substances or mixtures, and use the classification to predict physical properties. 1. Compare and contrast intermolecular forces and intramolecular forces. 2. Describe dispersion forces, dipole-dipole interactions, hydrogen bonding, iondipole, and ionic interactions in terms of electrostatic attraction. 3. Identify the predominant intermolecular force in a sample of a substance, given the substance’s molecular formula. 4. Relate Intermolecular Forces to solubility, miscibility, melting or boiling points, heat of vaporization or heat of fusion, vapor pressure, and surface tension. 5. Describe special properties of water due to hydrogen bonding 6. Interpret Phase Diagrams 13. Stoichiometry: Use molar relationships to predict how much product will form in a chemical reaction and compare actual quantities to expected values. 1. Write correct formulas for chemicals given their names. 2. Balance simple chemical equations using whole number coefficients. 3. Use stoichiometric ratios to convert between quantities of reactants and products. 4. Use a balanced chemical equation to perform mole conversions. 5. Identify the limiting reactant in a chemical reaction. 6. Calculate the predicted mass of product in a chemical reaction. 7. Calculate the % yield in a chemical reaction. 8. Calculate % composition. 9. Given % composition, determine empirical formulas. 10. Given empirical formulas and molar mass, determine molecular formulas. 11. Use combustion analysis data to find the empirical formulas of compounds. 14. First Law of Thermodynamics: Describe how changes in heat and work affect the total energy of a system and calculate quantities of heat transfer associated with phase changes, calorimetry, standard enthalpies of formation, Hess' Law, and

bond enthalpies 1. State the First Law of Thermodynamics. 2. Relate the change in internal energy of a system to changes in heat and work. 3. Recognize situations where H and q are similar or different. 4. Identify endothermic and exothermic reactions. 5. Recognize state functions. 6. Calculate heat related to heating/cooling a substance. 7. Calculate and compare enthalpy changes associated with phase changes. 8. Interpret heating/cooling curves. 9. Analyze calorimetric data to find the enthalpy of a reaction, the heat capacity of a substance or calorimeter, or the initial or final temperature of the system. 10. Calculate Hrxn using Hess’ Law. 11. Calculate Hrxn using standard enthalpies of formation. 12. Calculate Hrxn using bond enthalpies. 13. Make decisions about fuel choices based on thermodynamic and chemical data. 14. Be able to explain the carbon cycle and the influence of fossil fuels. 15. Describe ways in which individuals can reduce their carbon footprint. 15. Second and Third Laws of Thermodynamics: Describe entropy and free energy and calculate changes in these quantities associated with physical and chemical changes. Relate free energy to spntaneity. 1. State the Second Law of Thermodynamics. 2. Identify changes associated with increased or decreased entropy. 3. Calculate changes in entropy for reactions, given S° values. 4. State the third law of thermodynamics. 5. Calculate entropy and enthalpy changes associated with phase transitions. 6. Classify processes as always spontaneous, always non-spontaneous, or spontaneous at only high or low temperatures and explain your reasoning. 7. Calculate Gibbs Free Energy, G, for a reaction based on enthalpy, entropy, and temperature. 8. Calculate Gibbs Free Energy, G, for a reaction based on Gf°. 9. Describe how biological systems use coupled reactions....