Phases of Matter

Students will:

• Understand that different phases of matter have different properties.
• Explain how the heating curve conveys information about phases of matter, phase changes, and the energy involved in those changes.
• Use models and observations to draw conclusions about the heating curve and phase changes demonstrates the nature of science.

The Atom

Students will:

• Understand that atoms are the smallest building blocks of matter, and advancements in technology have changed knowledge of the atom over time.
• Understand an atom’s subatomic structure can be altered causing the formation of ions and isotopes.
• Explain that electron configurations show the most likely location of an electron in its lowest energy (ground) state, including valence electrons.
• Explain how when atoms absorb energy, electrons jump to an excited state and become unstable. When electrons return to ground state, energy is released as electromagnetic radiation.

Periodic Table and Trends

Students will:

• Use the periodic table as an organizational tool that allows for the prediction of chemical and physical properties of elements.
• Describe the periodic trends that are determined by principal energy levels and number of protons in an atom.

Introduction to Avogadro’s Number

Students will:

• Explain how the mole is the fundamental unit for counting particles in a substance.
• Use scientific notation and significant figures to convey information about numbers.
• Use dimensional analysis as a mathematical method to perform mole conversions.
• Understand how mathematical models allow scientists to represent quantities that cannot be directly observed, demonstrating the nature of science.

Mass and Moles

Students will:

• Explain how the mole is a fundamental unit for the amount of particles and is related to the mass of a substance via the molar mass found on the periodic table.
• Understand that the Law of Multiple Proportions states that different compounds can contain the same elements in different ratios and will have different properties. (ex. H ₂ O vs. H ₂ O ₂ ).
• Explain that chemical compounds have distinct ratios of elements by mass which can be used to determine empirical and molecular formulas.

Ionic Compounds

Students will:

• Understand that ionic compounds are composed of ions held together by electrostatic attractions.
• Explore how many substances with ionic bonds dissociate when added to a polar solvent.
• Understand that binary ionic bonds are formed by the transfer of electrons between metals and nonmetals.
• Explore how elements and ions behave in predictable patterns when bonding, allowing scientists to write standardized names and formulas, reflecting the nature of science.

Covalent Compounds

Students will:

• Explore how atoms combine to form covalent compounds in order to obey the octet rule and achieve stability.
• Explain that bonded and non-bonded pairs of electrons can be used to predict molecular geometry.
• Understand that the physical properties of covalent compounds can be predicted based on their structures, including the unique property of carbon to form organic compounds.
• Explain that elements behave in predictable patterns when bonding, allowing scientists to write standardized names and formulas, reflecting the nature of science.

Reactions and Introduction to Stoichiometry

Students will:

• Understand that atoms will rearrange through chemical reactions in specific ratios that balance the equation to follow the law of conservation of matter.
• Explore how chemical reactions demonstrate the nature of science in that they follow predictable patterns.
• Conduct stoichiometry calculations using mole ratio are performed to quantify the amount of reactants and products in a chemical reaction.

Solutions

Students will:

• Conduct experiments to explain solutions result from the interactions between a solute and solvent, and can be described through different models including concentration.
• Understand that properties of solutions are dependent upon different factors, including concentration, temperature, and the forces of attraction between particles.
• Explore the characteristic properties of acids and bases and the way that they react in predictable ways.

Kinetics

Students will:

• Understand that in a closed system, total energy is a conserved quantity that allows us to predict the chemical and physical behavior of the system.
• Explore the energy changes in reactions that occur as bonds are broken and formed.
• Collision theory relates matter and energy to predict the rate and progress of reactions.
• Experimental data provides evidence for constructing and evaluating models of molecular interactions, demonstrating the nature of science.

Thermodynamics

Students will:

• Explain that in a closed system, when heat energy is exchanged between the system and its surroundings, the energy is conserved overall.
• Explain how energy changes can be determined experimentally and theoretically for physical or chemical processes.

Stoichiometry

Students will:

• Understand that chemical reactions can be investigated and understood quantitatively and qualitatively from both macroscopic and molecular levels.
• Explain that the mole is the fundamental unit for counting quantities in a chemical reaction.
• Understand that the quantities of substances used or produced in a chemical reaction can be calculated theoretically and compared to experimental data, demonstrating the nature of science.

Gas Laws and Phase Diagrams

Students will:

• Understand that the Kinetic Molecular Theory relates matter and energy to predict the behavior of gases, reflecting the nature of science.
• Explore that gases and their properties can be modeled through mathematical relationships.
• Understand that the state of matter of a substance is determined by the temperature and pressure of the substance.