Chemistry – Goshen High School
Calendar
st
3rd Quarter
1 Quarter
Mathematics & Measurements
Atoms
Reactions
Pure Substances & Mixtures
2nd Quarter
4th Quarter
Atoms [cont’d]
Compounds
Pure Substances & Mixtures [cont’d]
Kinetics
Learning Targets
1. Mathematics and Measurement in Chemistry
A. Standard: Quantify the properties of matter.
1.
Students will use the appropriate units when making measurements.
2.
Students will utilize the metric system.
3.
Students will record measurements with the correct number of significant digits.
4.
Students will determine the number of significant digits in a number.
5.
Students will round numbers to a specified number of significant figures.
6.
Students will apply the correct number of significant digits to answers when performing calculations.
7.
Students will implement appropriate qualitative and quantitative error analysis (percent error).
B. Standard: Use specific mathematical techniques to solve problems [dimensional analysis].
1.
Students will develop conversion factors from equality statements.
2.
Students will convert between units using dimensional analysis.
3.
Students will calculate density of objects using dimensional analysis.
4.
Students will use scientific notation when performing calculations.
5.
Students will calculate the number of moles given the number of particles.
2. Atoms
A. Standard: Summarize the historical development of the atomic theory.
1.
Students will describe the importance of models in science.
2.
Students will explain each of the following atomic models: Dalton, Thomson, and Rutherford.
3.
Students will use Thomson’s and Rutherford’s models to describe locations of subatomic particles.
4.
Students will draw representations for each model of the atom.
5.
Students will use mass number and atomic number to describe various isotopes.
6.
Students will calculate the average atomic mass for an element.
7.
Students will calculate the mass given the number of moles or particles.
8.
Students will calculate the number of particles given the number of moles or grams.
9.
Students will calculate the number of moles given the number of particles or grams.
B. Standard: Summarize types of radioactive decay and applications of nuclear reactions.
1.
Students will describe alpha, beta, gamma, and positron decay of the nucleus.
2.
Students will write balanced nuclear equations.
3.
Students will differentiate between fission and fusion.
4.
Students will evaluate applications of fission and fusion.
C. Standard: Summarize the current modeling of the atom.
1.
Students will explain each of the following atomic models: Bohr and quantum mechanical model.
2.
Students will use an atomic spectrum to explain discrete energy levels.
3.
Students will explain the photoelectric effect.
4.
Students will summarize the number and energy level of electrons using s, p, d and f sublevels.
5.
Students will model the s and p sublevels.
6.
Students will write the orbital notation of the elements in the first three periods.
7.
Students will write the electron configuration of the elements in the first three periods.
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Chemistry – Goshen High School
D. Standard: Describe relationships within the periodic table.
1.
Students will identify the number of valence electrons based on an element’s group.
2.
Students will locate metals, nonmetals and metalloids on the periodic table.
3.
Students will compare properties in groups based on valence electron configuration.
4.
Students will describe and analyze the following periodic trends: atomic radii, ionic radii, first ionization
energies, and electronegativity.
3. Compounds
A. Standard: Define the types of chemical bonds holding atoms together.
1.
Students will explain why atoms form chemical bonds.
2.
Students will define a polar-covalent bond, nonpolar-covalent bond, and an ionic bond.
3.
Students will classify a bond based on electronegativity difference.
B. Standard: Explain the formation, nomenclature and properties of covalent compounds.
1.
Students will explain that an atom will share electrons to obtain a stable configuration.
2.
Students will describe the properties of molecular compounds.
3.
Students will describe the properties of covalent networks.
4.
Students will name binary covalent compounds using ten prefixes.
5.
Students will name binary acids.
6.
Students will name oxyacids.
7.
Students will write formulas for binary covalent compounds using ten prefixes.
8.
Students will write formulas for binary acids.
9.
Students will write formulas for oxyacids.
10. Students will draw a Lewis structure for compounds/polyatomic ions containing hydrogen, carbon, oxygen,
nitrogen, phosphorus, sulfur and/or the halogens.
11. Students will utilize VSEPR to classify the three dimensional shape of the molecules/polyatomic ions
containing hydrogen, carbon, oxygen, nitrogen, phosphorus, sulfur and/or the halogens.
12. Students will classify a molecule as polar or nonpolar.
C. Standard: Explain the formation, nomenclature, and properties of ionic compounds.
1.
Students will explain that metals will lose electrons to obtain a stable configuration forming a cation.
2.
Students will explain that nonmetals will gain electrons to obtain a stable configuration forming an anion.
3.
Students will analyze how an ionic bond gives the various properties of ionic compounds including brittleness,
high melting/boiling points, conductivity, and state of matter.
4.
Students will draw/sketch a representation of the formation of an ionic bond.
5.
Students will name binary ionic compounds.
6.
Students will name binary ionic compounds containing a transition metal.
7.
Students will name ionic compounds containing polyatomic ions.
8.
Students will write formula for binary ionic compounds.
9.
Students will write formulas for binary ionic compounds containing a transition metal.
10. Students will write formulas for ionic compounds containing polyatomic ions.
D. Standard: Explain formation and properties of metallic bonds.
1.
Students will draw/sketch a representation of a metallic bond.
2.
Students will define a metallic bond and explain what is happening to the electrons in one.
3.
Students will summarize how a metallic bond gives luster, conductivity, malleability and ductility.
E. Standard: Perform calculations regarding chemical compounds.
1.
Students will calculate the molar mass of a compound.
2.
Students will convert among particles, moles and mass for a compound.
3.
Students will calculate the percent composition of a compound.
4.
Students will determine the empirical formula given mass or percent data.
5.
Students will determine the molecular formula given the molar mass of the compound and the empirical
formula.
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Chemistry – Goshen High School
4. Reactions
A. Standard: Write and balance chemical equations.
1.
Students will write a balanced chemical equation from words.
2.
Students will classify chemical reactions as: synthesis, decomposition, single-replacement, double-replacement,
or combustion.
3.
Students will recognize oxidation-reduction reactions.
4.
Students will identify which substance is reduced and which is oxidized in an oxidation-reduction reaction.
5.
Students will write/predict the products of various chemical reactions given the reactants.
6.
Students will explain that precipitates form because of changes in forces between ions.
B. Standard: Perform stoichiometric calculations.
1.
Students will list the molar ratio(s) in a given equation.
2.
Students will calculate the theoretical yield in moles.
3.
Students will calculate the theoretical yield in grams.
4.
Students will calculate the percent yield of a reaction.
5.
Students will conceptually describe the idea of limiting reactants.
5. Pure Substances and Mixtures
A. Standard: Use intermolecular forces to explain properties in various states of matter.
1. Students will describe the five states of matter.
2. Students will draw pictures to represent the five states of matter.
3. Students will differentiate between intermolecular and intramolecular forces.
4. Students will explain London dispersion forces (Van der Waals).
5. Students will explain dipole-dipole forces.
6. Students will explain hydrogen bonding.
7. Students will explain that physical properties (solubility, evaporation rates, boiling point, and melting point) are
the result of intermolecular forces.
B. Standard: Perform solution stoichiometric calculations.
1.
Students will explain why a substance will dissolve in a solvent.
2.
Students will describe factors that affect how quickly a solute will dissolve in a solvent.
3.
Students will calculate the molarity of a solution.
4.
Students will calculate the theoretical yield of a reaction given the molarity.
5.
Students will dilute stock solutions to a specified molarity.
C. Standard: Describe acid-base reactions qualitatively and quantitatively.
1.
Students will describe Arrhenius acids and bases.
2.
Students will calculate the pH of a solution given the hydrogen ion [hydronium ion] concentration or hydroxide
ion concentration.
3.
Students will write an acid-base reaction.
4.
Students will perform a titration experiment.
5.
Students will calculate the molarity of an acid or base in a titration experiment.
6. Kinetics
A. Standard: Perform calculations in the Real World using properties of gases.
1.
Students will describe the physical properties of a gas using KMT.
2.
Students will use the combined gas law to calculate physical properties of a gas.
3.
Students will describe Avogadro’s Law.
4.
Students will use the ideal gas law to calculate physical properties of a gas, with different values of R.
5.
Students will combine the principles of the gas laws, stoichiometry, and problem solving skills to solve all of
the world’s problems.
6.
Students will explain why real gases are not ideal.
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Chemistry – Goshen High School
B. Standard: Describe energy changes in chemical reactions.
1.
Students will explain a chemical reaction in terms of collision theory.
2.
Students will describe the factors that affect the rate of chemical reactions.
3.
Students will predict the direction of an equilibrium reaction using Le Chatelier’s Principle.
4.
Students will describe the action of catalysts.
5.
Students will draw and interpret graphic representations to represent the energy changes during a reaction,
including the activation energy.
6.
Students will describe a reaction as endothermic or exothermic.
7.
Students will describe specific heat capacity.
8.
Students will calculate the energy released or absorbed in calorimetry.
9.
Students will analyze energy changes that occur during changes of state.
10. Students will analyze the roles of energy and entropy in determining the spontaneity of chemical reactions.
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