Download Honors Chemistry Syllabus Instructor: Julie Stansberry email

Honors Chemistry Syllabus
Instructor: Julie Stansberry
phone (423)581-1600 ext 1170
email: [email protected] Text: Modern Chemistry (Holt)
website: mhhsw.hcboe.net
words listed in italics will be covered in a different chapter
Unit 1 Atomic Structure
Week 1-Atomic Structure (Chapter 3)
3.1 Defining the atom
3.2 Structure of the atom
3.3 Distinguishing among atoms (omit relating mass to number of atoms)
Demo: Cathode ray tube
Lab: Law of Definite Composition
Timeline: Scientists who contributed to Model of the Atom
vocabulary: Democritus, Dalton’s atomic theory, Thomson, Rutherford, Chadwick, Planck, Bohr, quantum
mechanical model, nucleus, proton, neutron, electron, orbit, energy levels, probability, atomic number, mass
number, isotope, ion, oxidation number, cation , anion, and neutral atom
Ch. 3.1-3.3 test
spi 3221
1.1 Compare and contrast the major models of the atom (eg. Democritus, Thomson, Rutherford, Bohr, and the
Quantum Mechanical model.
1.2 Interpret the periodic table to describe an element’s atomic makeup
Week 2-Nuclear Chemistry (Chapter 21)
21.1 The Nucleus
21.2 Radioactive decay
21.3 Nuclear radiation
21.4 Nuclear fission and fusion
vocabulary: radioactivity ,electromagnetic radiation spectrum, carbon-14 dating, radioisotopes, alpha, beta,
positron, gamma, half-life, transmutation, transuranium elements, parent nuclide, daughter, chain reaction,
decay series, fission, fusion, moderator, control rod, Geiger counter, film badge, scintillation counter, and film
badge
Ch. 21 Test
spi 3221
t/e.1 Distinguish among tools and procedures best suited to conduct a specified scientific inquiry
math.3 Interpret graphs that depict real-world phenomena
2.4 Classify a property of change of matter as (physical, chemical, or) nuclear
3.8 Describe radioactive decay through a balanced nuclear equation and through the analysis of half-life
3.9 Compare and contrast nuclear fusion and fission
Week 3-Electrons in the Atom (Chapter 4)
4.1 A New Atomic Model
4.2 Quantum Model of the atom
4.3 Electron configuration
Lab: Flame Test
vocabulary: valence electron, core electrons, electron configuration, noble gas configuration, orbital notation,
core configuration, valence configuration, atomic orbital, Aufbau principle, energy levels, Hund’s rule, Pauli’s
exclusion principle, photons, and quantum
ch 19 Oxidation-reduction reactions
19.1 oxidation and reduction
Ch. 4,19.1 Test
spi 3221
1.5 represent an electron’s location in the quantum mechanical model of an atom in terms of the shape of
electron clouds (s and p orbitals in particular), relative energies of orbitals, and the number of electrons possible
in the s,p,d, and f orbitals
Week 4-The Periodic Table (Chapter 5)
5.1 History
5.2 Electron configuration and the periodic table
5.3 Periodic properties
Demo: Reactivity of Group I Metals (Sodium and Calcium)
Lab: Mini Hindenburgs/ Properties of Hydrogen
vocabulary: alkali metals, alkali earth metals, atomic radius, electronegativity, halogens, noble gas, maingroup, inner transition metal, lanthanide series, actinide series, transition metal, representative element, metal,
nonmetal, metalloid, and periodic law
Ch. 5 Test
spi 3221.
1.3 Describe the trends found in the periodic table with respect to atomic size, ionization energy, electron
affinity, or electronegativity
Week 5- Chemical Bonding (Chapter 6)
6.1 Intro
6.2 Covalent and molecular compounds
6.3 Ionic bonding
6.4 Metallic bonding
6.5 Molecular geometry
Lab: Saponification
vocabulary: chemical formula, electron dot structure (Lewis dot structure), formula unit, ionic bond, ionic
compound, metallic bond, octet rule, valence electron, covalent bond, dipole, dispersion forces, double covalent
bond, hydrogen bonds, molecular compound, molecule, nonpolar covalent bond, polar covalent bond,
polyatomic ion, single covalent bond, triple covalent bond, unshared pair (nonbonding electrons), van der Waals
forces, (intermolecular forces), hybridization, VSEPR
Ch. 6 test
spi 3221
1.4 determine the Lewis electron-dot structure or number of valence electrons for an atom of any main-group
element from its atomic number or position on the periodic table
3.1 Analyze ionic and covalent compounds in terms of how they form, (names), chemical formulas, (percent
composition and molar mass)
Unit 1 Exam (¼)
Unit 2 Interactions of Matter Unit A:
Week 6-Hydrocarbon Compounds (Chapter 22)
22.1 Organic compounds
22.2 Hydrocarbons
22.3 Functional Groups
22.4 Organic reactions
Lab(dry): organic models
vocabulary: hydrocarbon, alkane, alkene, alkyne, straight-chain, branched-chain, condensed structural formula,
alkyl group, unsaturated compounds, saturated compounds, isomers, polymerization, alcohol, aldehyde, ester,
ether, carboxylic acid, amine, and ketone
Ch. 22 test
spi 3221
3.1 Analyze (ionic and) covalent compounds in terms of(how they form), name, chemical formula, (percent
composition and molar mass)
Week 7-Chemical names and formulas (Chapter 7)
7.1 Chemical names and formulas
Activity: naming tournament
vocabulary: acid, binary compound, monatomic ion, and polyatomic ion, subscript
Project: Research a compound
Ch. 7.1 test
spi 3221
3.1 Analyze ionic and covalent compounds in terms of how they form, names, chemical formulas, (percent
composition, and molar mass)
Week 8-Chemical Reactions (Chapter 8)
8.1 Describing chemical reactions
8.2 Types of chemical reactions
8.3 Activity series
Lab: Observing Chemical changes
vocabulary: chemical equation, coefficient, balanced equation, combustion, combination (composition,
synthesis), decomposition, single-replacement, double replacement, soluble (aqueous), and precipitate
Ch. 8 test
spi 3221
3.2 Identify the reactants, products, and types of different chemical reactions: composition (synthesis,
combination), decomposition, double replacement, single replacement, and combustion
3.3 Predict the products of a chemical reaction
3.4 Balance a chemical equation (to determine molar ratios)
Unit 2A Exam (½) Unit B:
Week 9-Scientific measurement (Chapters 2, 3, and 7)
2.2 Units of measurement
2.3 Using scientific measurements
Lab: Density and graphing
vocabulary: measurement, scientific notation, accuracy, precision, accepted value, experimental value, error,
percent error, dimensional analysis, conversion factor, density, and significant figures
-Chemical quantities
3.3 Counting atoms (relating mass to number of atoms only)
Mole-mass and mole-volume relationship
7.3,7.4 Percent composition and Chemical formulas
Lab: % composition of Aspirin
vocabulary: Avogadros number, representative particle, molar mass, molar ratio, STP, molar volume, percent
composition, percent yield
Ch.2.2,2.3,3.3, 7.3,7.4 test
spi 3221
Inq.4 evaluate the accuracy and precision of data
Math.4 Apply measurement unit relationships including Avogadro’s number, (molarity, molality), volume, and
mass to balance chemical equations
Math.5 Use concepts of mass, length, area, and volume to estimate and solve real-world problems
3.1 Analyze ionic and covalent compounds in terms of how they form, names, chemical formulas, percent
composition, and molar mass.
3.5 Convert among the following quantities of a substance: mass, number of moles, number of particles, molar
volume at STP
3.6 Identify and solve stoichiometry problems: volume at STP to mass, moles to mass, (and molarity)
Week 10-Stoichiometry (Chapter 9)
9.1 The arithmetic of equations
9.2 Chemical calculations
9.3 Limiting reagent and percent yield
Lab: Stoichiometry- Limiting Reactant and Rice Krispie
vocabulary: actual yield, excess reagent, limiting reagent, mole ratio, stoichiometry, and theoretical yield
Ch 9 test
spi 3221
3.4 balance a chemical equation to determine molar ratios.
3.6 Identify and solve stoichiometry problems: volume at STP to mass, moles to mass, (and molarity)
Week 11-Acids, Bases, and Salts (Chapters 14 and 15)
14.1 Properties of acids and bases
14.2 Acid-base theories
14.3 Acid and base reactions
15.1 pH
15.2 Titrations
18.3 Buffers (only)
Activity: Acidic and Basic properties of household items
Lab: Analysis of vinegar
vocabulary acidic solution, basic (alkaline) solution, amphoteric, buffers, monoprotic acid, diprotic acid,
triprotic acid, end point, hydronium ion, neutral solution, neutralization reaction, pH, strong acid, strong base,
weak acid, weak base, strong elctrolyte, weak electrolyte, nonelectrolyte, titration, Arrhenius acids and bases,
Bronsted-Lowry Acids and bases, Lewis Acids and bases, conjugate acids and bases
Ch. 14 and 15 test
spi 3221
t/e.1 distinguish among tools and procedures best suited to conduct a specified scientific inquiry
Math.2 Perform operations on algebraic expression (logarithms)
3.2 Identify the reactants, products, and types of chemical reactions (double replacement)
3.7 Classify substances as acids or bases based on their formulas and how they react with various indicators
Unit 2B Exam (3/4)
Unit 3 Matter and Energy
week 12 – Intro to Chemistry (ch 1,2)
1.1 Chemistry is a physical science
2.1 Scientific method
Activity: scientific method
Project: Apply the engineering design process to a current or new product from inception to product.
vocabulary matter, chemistry, organic chemistry, inorganic chemistry, biochemistry, technology,
biotechnology, pollutant, biodiesel, agriculture, scientific method, observation, hypothesis, experiment,
manipulated variable, responding variable, theory, scientific law, numeric word problem, engineering design
cycle (process)
-Matter and its properties
1.2 Properties of matter
Activity: Classifying matter
vocabulary: element, diatomic element, compound, mixture, homogeneous mixture, heterogeneous mixture,
solution, alloy, colloid, suspension, atom, molecule, pure substance phase change, physical property, chemical
change, chemical property, product, reactant, chemical symbol, shape, volume, mass, definite, indefinite,
energy, compress, expand, melt, freeze, boil, vaporize, evaporate, condense, sublime, and depose
Ch.1.1,1.2,2.1 Test
spi 3221
Inq1 Select a description or scenario that reevaluates and/or extends a scientific finding
Inq2 Analyze the components of a properly designed scientific investigation
Inq5 Defend a conclusion based on scientific evidence
Inq6 Determine why a conclusion is free of bias
Inq7 Compare conclusions that offer different, but acceptable explanation for the same set of experimental data
t/e1 Distinguish among tools and procedures best suited to conduct a specified scientific inquiry
t/e.2 Evaluate a protocol to determine the degree to which an engineering design process was successfully
applied.
2.1 Distinguish among elements, compounds, solutions, colloids, and suspensions
2.4 Classify a property of change of matter as physical, chemical, (or nuclear)
2.6 Investigate similarities and differences among solids, liquids, and gases in terms of energy and particle
spacing
week 13-Thermochemistry (ch 16)
16.1 Thermochemistry
Lab Specific heat of a metal
vocabulary: heat of fusion, heat of vaporization, phase change, temperature change, thermochemistry, heat, law
of conservation of energy, surroundings, system, endothermic, exothermic, joule, calorie, specific heat,
calorimeter
Ch. 16 test
spi 3221
3.10 Relate the laws of conservation of mass/energy to thermal changes that occur during physical,
chemical, or nuclear processes
Week 14-The Behavior of Gases (Chapters 10 and 11)
10.1 Kinetic Theory
11.1 Gases and pressure
11.2 The Gas Laws
11.3 Ideal gases
11.4 Diffusion and Effusion
Lab: Bicarbonate in Antacid
Demo: Boyle’s Law/Charles Law
vocabulary: Barometer, Boyle’s law, Charles’s law, Avogadro’s law, combined gas law, Dalton’s law of
partial pressure, diffusion, Gay Lussac’s law, ideal gas law, ideal gas law constant, partial pressure, kinetic
theory
Ch. 10 and 11 test
spi 3221
math.1 use real numbers to represent real-world applications (eg slope, rate of change, probability and
proportionality)
math.2 perform operations on algebraic expressions and informally justify the selected procedures
2.7 predict how changes in volume, temperature, and pressure affect the behavior of a gas
Week 15-Solutions
12.1 Types of mixtures
12.2 The solution process
12.3 Concentration of solutions
13.2 colligative properties of solution
Demo: making a supersaturated solution
Lab: Colligative Properties- Making ice cream
vocabulary: boiling point elevation, concentrated solution, concentration, colligative property, dilute solution,
freezing point depression, immiscible, miscible, molality, molal constants, molarity, dissociation, molecular
solvation, saturated solution, unsaturated solution, super saturated solution, solubility, seed crystal, surface
area, vapor pressure, agitation, ppm, ppb, percentage m/m or v/v, solute, and solvent
Ch. 12,13 test
spi 3221
2.2 Identify properties of a solution: solute and solvent in a solid, liquid, or gaseous solution; procedure to make
or determine the concentration of a solution in units of ppm, ppb, molarity, molality, percent composition;
factors that affect the rate of solution; and colligative properties
Unit 3 Exam
Week 16-Project: Use the engineering design cycle to improve or create a product that would improve
everyday life.
Week 17-Review
*if time permits: The Chemistry of life Ch. 24
Final Exam (20% of semester grade)