Skip To Main Content

Logo Image

Logo Title

Chemistry

Course Description

Chemistry: Chemistry is the study of matter and energy from a molecular point of view. Students will use laboratory experiences, classroom demonstrations, discussions, and practical application to investigate atomic structure and the periodic table, bonding, intermolecular forces, reactions and science practices.

Honors Chemistry: Compared to Chemistry, Honors Chemistry is a more analytical and in-depth study of matter and energy from a molecular point of view. Students will use laboratory experiences, classroom demonstrations, discussions, and practical application to investigate atomic structure and the periodic table, bonding, intermolecular forces, chemical, physical and nuclear processes and relevant science practices.

Grade Level(s): 10th Grade

Related Priority Standards (State &/or National): MLS Science Standards Grades 6-12 

Enduring Understandings/Big Ideas

  • All matter is comprised of atoms which can bond with one another to form molecules.
  • Changes in matter may or may not involve bonds between atoms breaking and/or forming.
  • Density is a derived measurement of how much matter is found in a given volume.
  • All measurements involve estimation, and as such, are not exact.
  • Manipulation of measurements requires attention to precision (significant figures).
  • Energy changes accompany every change and can be followed using Potential Energy(PE) diagrams.
  • Cause and effect-breaking bonds requires energy; forming bonds releases energy.
  • Chemical reactions can be classified.
  • Balanced chemical reactions demonstrate conservation of mass.
  • Amounts of matter can be expressed and calculated by mass, mole and particle.
  • Acids and bases neutralize each other.
  • Pressure, temperature, volume & moles of gases are interrelated.
  • Concentrations of solutions can be described using molarity.
  • Chemical reactions occur in both the forward and Big Ideas reverse directions.
  • The understanding of matter at the subatomic level developed over time with a progression of models based
    on increasing technology and scientific analysis. The current model is the orbital model.
  • Nuclear reactions involve changes in the nucleus, a subatomic part of the atom.
  • Light emission occurs due to interaction of the subatomic structure of the atom and energy.
  • The Periodic Table is based on a variety of patterns that allow chemists to predict properties and reactivity.
  • Atoms will lose, gain or share electrons in order to become more stable.
  • Electron dot structures depict how electrons are lost, gained or shared to form bonds.
  • Whether atoms lose, gain or share electrons can be determined from the Periodic Table.
  • Electron dot structures can be used to predict Big Ideas molecular shapes.
  • Hydrogen and carbon bond to form organic compounds.
  • Organic compounds contain recognizable functional groups.
  • Molecular shapes affect polarity.
  • Polar substances dissolve polar substances; nonpolar substances dissolve nonpolar substances.
  • Intermolecular attractions of hydrogen bonding, dipole-dipole forces, and dispersion forces can be predicted from molecular structure and polarity.
  • Intermolecular attractions give rise to predictable properties of materials.

Course-Level Scope & Sequence (Units &/or Skills)

Unit 1: Matter and Change

All matter is composed of atoms which can bond with one another to form molecules. Changes may or may not involve bonds between atoms breaking and/or forming. Phases describe the relative freedom of movement of the atoms and molecules in a sample.  Students will be able to:

  • Label the components of a chemical reaction (reactants, products, state/phase symbols[solid, liquid, gas, aqueous],
    coefficient, subscript, yield sign, chemical symbol, chemical formula).
  • Recognize hydrocarbon combustion reactions, and predict the products.
  • Distinguish among solids, liquids & gases and their properties.
  • Draw or interpret pictures of solids, liquids and gases at the particle level.
  • Identify/classify the components of a solution.
  • Identify correct application of lab safety rules, as well as possible consequential disabilities for not following safe practices.
  • Follow safety protocols when conducting a lab.
  • Distinguish between chemical and physical changes in matter at the symbolic, macroscopic, and sub-microscopic (particulate) levels.
  • Write common formulas for all the elements on the periodic table.
  • Identify metals and nonmetals by their position on the periodic table, and describe some of their characteristic properties.
  • Write formulas & names for binary compounds, both M-N (ionic) and N-N (covalent), given reference materials (except Roman numerals and polyatomics).
  • Distinguish among elements, compounds & mixtures.
  • Classify a substance as an element, compound, or mixture at the symbolic, macroscopic, and sub-microscopic (particulate) levels.
  • Distinguish between atoms and molecules at the symbolic, macroscopic, and sub-microscopic (particulate) levels.

Unit 2: Energy and Number Handling

Density is a derived measurement of how much matter is found in a given volume. All measurements involve estimation, and as such, are not exact. Manipulation of measurements requires attention to precision (significant figures). Energy changes accompany every change and can be followed using Potential Energy(PE) diagrams. Students will be able to:

  • Measure length, mass, volume, temperature, and time to the appropriate precision of the measuring device.
  • Collect data accurately and precisely (equipment scales, instrumental error).
  • Represent & analyze data accurately and precisely.
  • Relate the arrangement of particles in a substance to the intensive property of density and observable behavior.
  • Use the equation D=m/V.
  • Use measurements (mass & volume) and the mathematical definition of density to identify samples (regular & irregular solids, liquids and gases).
  • Explain using collision theory the effect of changing concentration and temperature, or addition of a catalyst, on the rate of reaction.
  • Given an energy diagram for a reaction or an equation, determine if the reaction is exothermic or endothermic.
  • Explain at the particle level how activation energy initiates a chemical reaction. Given an energy diagram, explain the effect of a catalyst on the activation energy needed to initiate a reaction.
  • Collect lab data to calculate heat using the equation: Q = mass x specific heat x temperature change.
  • Identify the possible effects of random and systematic errors on observations, measurements, and calculations.

Unit 3: Reactions and Stoichiometry

Chemical reactions can be classified. Balanced chemical reactions demonstrate conservation of mass. Amounts of matter can be expressed and calculated by mass, mole and particle. Students will be able to:

  • Classify reaction types (single/double replacement, composition, decomposition, combustion).
  • Predict the products of an oxidation (rusting) reaction.
  • Write formulas and names for compounds that contain polyatomic ions and Roman numerals.
  • Balance chemical equations, applying conservation of atoms/mass/matter.
  • Compare the mass of the reactants to the mass of the products in a chemical reaction as support for the Law of Conservation of Mass.
  • Recognize that the size of atoms necessitates the use of moles (1 mole = 6.022 x 1023; 1 g = 6.022 x 1023 amu).
  • Given a chemical formula, calculate its molar formula mass.
  • Given a chemical quantity, convert between mass, moles, and particles.
  • Using a balanced chemical equation and a given amount of a reactant/product, calculate the proportional amount of another reactant/product.

Unit 4: Solutions and Gasses

Acids and bases neutralize each other. Pressure, temperature, volume & moles of gases are interrelated. Concentrations of solutions can be described using molarity. Chemical reactions occur in both the forward and reverse directions. Students will be able to:

  • Distinguish between acids and bases based on chemical formulas.
  • Compare and contrast the properties of acidic, basic and neutral solutions.
  • Use pH scale to distinguish between acids and bases.
  • Identify a neutralization reaction.
  • Predict the products of a neutralization reaction.
  • Given two of the three variables: molarity, volume of solution or moles of solute, calculate the third.
  • Use the molarity and volume of solutions to calculate the proportional amount of another reactant/product.
  • Use the combined gas law to solve for an unknown quantity (volume, pressure, temperature).
  • Convert Celsius to Kelvin temperatures.
  • Given three of the four variables: pressure of a gas sample, volume of a gas sample, number of moles in a gas sample, temperature of a gas sample (and given R), solve for the fourth.
  • Use a balanced equation to calculate the proportional amount of gaseous reactant or product at STP. (1 mole = 22.4L)
  • Explain that some reactions proceed in both the forward and reverse directions.
  • Recognize that at equilibrium, the rates of forward and reverse reactions are the same.
  • Predict the shift (towards reactants or products) resulting when stress is applied to a gaseous system at equilibrium (i.e. change in pressure, temperature, add/remove reactants/products).

Unit 5: Atomic Structure and Light

The understanding of matter at the subatomic level has developed over time with a progression of models based on increasing technology and scientific analysis. The current model is the orbital model. Nuclear reactions involve changes in the nucleus, a subatomic part of the atom. Light emission occurs due to interaction of the subatomic structure of the atom and energy.  Students will be able to:

  • Identify and describe how atomic models have changed over time as a result of new evidence.
  • Calculate numbers of protons, electrons, and neutrons, given atomic number, mass number and charge.
  • Calculate average atomic mass using isotopic abundance data.
  • Determine one isotope mass given isotopic composition, average atomic mass and all other isotope masses.
  • Determine percent (isotope) composition given two isotope masses and average atomic mass.
  • Describe the process for light emission based on the interaction of the current model of the atom with electromagnetic spectrum energies.
  • Use the electromagnetic spectrum to predict relative wavelength, energy and frequency.
  • Describe the atom as having a dense, positive nucleus surrounded by a cloud of negative electrons.
  • Identify various nuclear reactions based on reaction patterns and calculate the subatomic particles involved.
  • Describe how changes in the nucleus of an atom during a nuclear reaction (i.e., nuclear decay, fusion, fission) result in emission of radiation.

Unit 6: The Periodic Table 

The Periodic Table is based on a variety of patterns that allow chemists to predict properties and reactivity. Students will be able to:

  • Explain the structure of the Periodic Table in terms of the elements with common properties (groups/families) and repeating properties (periods).
  • Classify elements as metals, nonmetals, metalloids (semi-conductors), and others (alkali, alkaline earth, transition, halogens, noble gases) according to their location on the Periodic Table.
  • Compare and contrast the properties of metals, nonmetals, metalloids (semi-conductors), and representative families.
  • Analyze graphs to discern periodic trends.
  • Predict properties across periods and within families.
  • Derive the long form and short form electron configurations for atoms/ions using the periodic table.
  • Derive orbital diagrams for atoms/ions using the periodic table.
  • Identify the number of valence electrons in a representative element based on Periodic Table location or electron configuration.
  • Determine the Lewis/electron dot structures for representative elements and ions from the Periodic Table or electron configuration.

Unit 7: Bonding

Atoms will lose, gain or share electrons in order to become more stable. Electron dot structures depict how electrons are lost, gained or shared to form bonds. Whether atoms lose, gain or share electrons can be determined from the Periodic Table. Electron dot structures can be used to predict molecular shapes. Students will be able to:

  • Predict stable ion charge based on family membership using the octet rule for any representative element.
  • Use Lewis/electron dot structures to depict bond formation (ionic and covalent) by applying the octet and duet rules.
  • Compare and contrast types of chemical bonds (i.e., ionic, covalent – polar & nonpolar).
  • Use the periodic table and/or electronegativity values to predict bonding type.
  • Determine molecular shapes (tetrahedral, trigonal pyramidal, trigonal planar, bent and linear) using valence shell electron pair repulsion (VSEPR) theory.

Unit 8: Organic and Intermolecular Forces

Hydrogen and carbon bond to form organic compounds. Organic compounds contain recognizable functional groups. Molecular shapes affect polarity. Polar substances dissolve polar substances; nonpolar substances dissolve nonpolar substances. Intermolecular attractions of hydrogen bonding, dipole-dipole forces, and dispersion forces can be predicted from molecular structure and polarity. Intermolecular attractions give rise to predictable properties of materials. Students will be able to:

  • Use shapes and bond polarity to predict molecular polarity.
  • Use molecular polarity to predict solubility.
  • Predict intermolecular attractions (hydrogen bonding, dipole-dipole or dispersion forces) of a substance from the structure and shape of the molecule.
  • Use intermolecular attractions to explain the macroscopic properties (melting point, solubility) of a substance.
  • Draw structural formulas to represent organic molecules.
  • Draw line structural formulas to represent organic molecules.
  • Identify common functional groups (alcohol, amine, aromatic, acid, ketone, aldehyde, ether, ester, amide) in organic compounds.

Course Resources & Materials: District and teacher-made resources

Date Last Revised/Approved:  May 2017