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Transcript
Chemistry I PAP (2010) – Semester I Final Review All students will complete a semester exam review regardless of exemption status. The student should be able to do the following: Chapter 1 (Matter) & 2 (Measurements) - interpret a correctly made graph from laboratory data - list and define common metric base units and prefixes - construct conversion factors from equivalent measurements and apply techniques of dimensional analysis (factor-label method) in problem solving - report measurements to the correct number of significant digits - express large and small numbers in scientific and standard notation - demonstrate safe laboratory procedures and attire - identify common laboratory equipment and know their uses - classify a sample of matter as an element, compound, or mixture (homogeneous vs. heterogeneous) - classify properties as either physical or chemical (physical: color, odor, shape, mass solubility, malleability, ductility, melting and boiling points, density, conductivity, chemical reactivity, flammability) - distinguish between physical and chemical changes (states) and know the three states of matter - Practice: Sketch the tree map on page 15 - p. 18 2 p. 24 3 p. 42 2,3,5 p. 57 2,3,4,6,7,8 VOCAB: chemical and physical change, homogeneous and heterogeneous mixtures, compound, element Chapter 3 (Atoms) Define and apply the Law of Conservation of Mass - define atom, nucleus, electron, neutron, isotope, proton (including relative size and charge of subatomic particles, average atomic mass, cation, anion, atomic number, atomic mass - discuss the evolution of atomic theory to the present electron cloud model emphasizing that the atom is mostly empty space. (Rutherford, Thompson, Bohr, quantum mechanical model) - use the mass number and atomic number to determine the element and its number of protons, electrons, and neutrons - determine the atomic number and mass number of an element when the number of protons, neutrons, and electrons is specified - know how isotopes of an atom differ and understand how relative abundance of isotopes determine atomic mass VOCAB: isotope, average atomic mass, atom, electron, nucleus, neutron, proton, isotope, cation, anion, atomic number, atomic mass 1. Practice Problems: p. 74 2 (a, b), 3 Additional Questions: p. 85 1-7 Write the chemical configuration, including atomic number & mass number, for the following isotopes. a. carbon-14 c. nickel-63 b. chromium-53 d. zirconium-92 2. 3. 4. 5. Complete the table for the following isotopes. Zn Symbol Atomic # 20 Mass # 65 74 40 # of protons 34 # of 21 neutrons # of 18 electrons Calculate the average atomic mass of copper if 69.17% of the copper atoms occurring in nature are 63Cu and 30.83% are 65Cu. What is the charge of an ion that has 26 protons, 30 neutrons, and 24 electrons? What is the charge of an ion that has 15 protons, 16 neutrons, and 18 electrons? Chapter 4 (Electrons in Atoms) & 5 (Periodic Law) - write electron configurations and orbital filling diagrams (including energy level, sublevels, and orbitals for any element) - recognize the difference between excited state and ground state configuration and everyday applications (fireworks, neon light) - understand the periodic properties due to repeating outer electron configurations and the properties of the representative elements (s and p block) - understand the organizing principles of the periodic table to include: atomic number, placement of metals, non-metals, and metalloids (semi-metals), and names of and location of groups (families) and periods - define and describe the following trends: atomic radius, electronegativity, ionization energy, and ionic radius - Be able to apply the Aufbau principle, the Pauli exclusion principle, and Hund’s rule when writing electron configuration and orbital notation - Calculate various wave problems - Know the mathematical relationship between wavelength and frequency VOCAB: ground state, electron configuration, quantum numbers, orbital filling diagrams, dot diagram, valence electrons, energy level - Practice Problems: p. 104 1,3 p. 116 3-5 p.118 8 p.154 1 - Additional Questions - Calculate the wavelength if the frequency is 2.5 x 10 5 Hz. Find the energy of a photon if frequency is 7.31 x 10 14 Hz. Fill in the table for the following elements. Electron configuration Symbol Atomic # Orbital Diagram Quantum numbers F V Chapter 7 (Formulas and Compounds) - convert between moles, mass, and number of particles given a chemical formula calculate empirical and molecular formulas solve hydrate problems determine the percent composition of a substance use cations and anions to write chemical formulas given the formula for a compound, write its name interpret the information conveyed in a chemical formula determine the formula / molecular mass of a substance VOCAB: moles, atoms, molecule, formula unit, empirical and molecular formulas, percent composition, alkanes, alkenes, alkynes, hydrocarbons, alcohols, acids, hydrates - Practice Problems: p. 215 2-4 p.219 1,2 p. 228 3,5,6 p.233 1-5 Dot diagram - P.237 35, 42 Additional Questions 1. Draw the structural formula of 2,2-dimethyl octane. 2. Write formulas for the following compounds (HINT: First determine ionic/acid/covalent). a. calcium bromide d. octane b. iron(III) sulfate e. dinitrogen tetroxide c. hydrofluoric acid f. sulfurous acid Chapter 8 (Rxns) - identify the reactants and products in a chemical equation and the following symbols used in equation writing – s, l, g, aq, , - Understand and apply the activity series in predicting reactions - write a balanced equation and predict the products when given names of formulas of all products and reactants in a chemical reaction - classify reactions as double replacement (ionic), single replacement, synthesis (combination / composition), decomposition (analysis), and combustion. - Define the terms precipitate, activity series, exothermic, and endothermic, and identify a reaction as to the change in energy involved - Practice Problems: 264 2-4