This correlation lists the recommended Gizmos for this state's curriculum standards. Click any Gizmo title below for more information.
CHEM2.PS1: : Matter and Its Interactions
CHEM2.PS1.1: : Illustrate and explain the arrangement of electrons surrounding atoms and ions (electron configurations and orbital notation of a specific electron in an element) and relate the arrangement of electrons with observed periodic trends.
Electron Configuration
Create the electron configuration of any element by filling electron orbitals. Determine the relationship between electron configuration and atomic radius. Discover trends in atomic radii across periods and down families/groups of the periodic table.
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CHEM2.PS1.3: : Compare and contrast crystalline and amorphous solids with respect to particle arrangement, strength of bonds, melting and boiling points, bulk density, and conductivity; provide examples of each type.
Melting Points
Every substance has unique transition points, or temperatures at which one phase (solid, liquid, or gas) transitions to another. Use a realistic melting point apparatus to measure the melting points, boiling points, and/or sublimation points of different substances and observe what these phase changes look like at the microscopic level. Based on the transition points, make inferences about the relative strengths of the forces holding these substances together.
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CHEM2.PS1.4: : Investigate and use mathematical representations to support Dalton’s law of partial pressures and to compare and contrast diffusion and effusion.
Diffusion
Explore the motion of particles as they bounce around from one side of a room to the other through an adjustable gap or partition. The mass of the particles can be adjusted, as well as the temperature of the room and the initial number of particles. In a real-world context, this can be used to learn about how odors travel, fluids move through gaps, the thermodynamics of gases, and statistical probability.
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Observe how reactants and products interact in reversible reactions. The amounts of each substance can be manipulated, as well as the pressure on the chamber. This lesson focuses on partial pressures, Dalton's law, and Le Chatelier's principle.
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CHEM2.PS1.5: : Obtain data and solve combined and ideal gas law problems and stoichiometry problems at STP and non STP conditions to quantitatively explain the behavior of gases.
Boyle's Law and Charles's Law
Investigate the properties of an ideal gas by performing experiments in which the temperature is held constant (Boyle's Law), and others in which the pressure remains fixed (Charles's Law). The pressure is controlled through the placement of masses on the lid of the container, and temperature is controlled with an adjustable heat source. Gay-Lussac's law relating pressure to temperature can also be explored by keeping the volume constant.
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Explore relationships between amount, temperature, pressure, and volume for an ideal gas in a chamber with a moveable piston. Discover rules of proportionality contained in Boyle's law, Charles's law, Avogadro's law, and Gay-Lussac's law. Use these relationships to derive the ideal gas law and calculate the value of the ideal gas constant.
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CHEM2.PS1.7: : Investigate, describe, and mathematically determine the effect of solute concentration on vapor pressure using Raoult’s Law and of the solute’s van ’t Hoff factor on freezing point depression and boiling point elevation.
Freezing Point of Salt Water
Control the temperature of a beaker of water. As the temperature drops below the freezing point, a transformation of state will occur that can be viewed on a molecular level. Salt can be added to the water to see its effect on the freezing point of water.
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CHEM2.PS1.8: : Develop models to show how different types of polymers, such as proteins, nucleic acids, and starches, are formed by repetitive combinations of simple subunits by condensation and addition reactions and to show the diverse bonding characteristics of carbon.
Covalent Bonds
Choose a substance, and then move electrons between atoms to form covalent bonds and build molecules. Observe the orbits of shared electrons in single, double, and triple covalent bonds. Compare the completed molecules to the corresponding Lewis diagrams.
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Simulate ionic bonds between a variety of metals and nonmetals. Select a metal and a nonmetal atom, and transfer electrons from one to the other. Observe the effect of gaining and losing electrons on charge, and rearrange the atoms to represent the molecular structure. Additional metal and nonmetal atoms can be added to the screen, and the resulting chemical formula can be displayed.
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CHEM2.PS1.11: : Conduct a qualitative analysis lab to determine the solubility rules. Use solubility rules to identify spectator ions and write net ionic equations for precipitation reactions.
Solubility and Temperature
Add varying amounts of a chemical to a beaker of water to create a solution, observe that the chemical dissolves in the water at first, and then measure the concentration of the solution at the saturation point. Either potassium nitrate or sodium chloride can be added to the water, and the temperature of the water can be adjusted.
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CHEM2.PS1.14: : Conduct titrations with standard solutions (monoprotic and diprotic) and an appropriate indicator and/or a pH probe to determine the concentration of an unknown acid or base, and with a weak acid or weak base to determine the Ka or Kb and the pH at the equivalence point.
Titration
Measure the quantity of a known solution needed to neutralize an acid or base of unknown concentration. Use this information to calculate the unknown concentration. A variety of indicators can be used to show the pH of the solution.
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CHEM2.PS1.15: : Explain common chemical reactions, including those found in biological systems, using qualitative and quantitative information.
Cell Energy Cycle
Explore the processes of photosynthesis and respiration that occur within plant and animal cells. The cyclical nature of the two processes can be constructed visually, and the simplified photosynthesis and respiration formulae can be balanced.
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CHEM2.PS1.16: : Create a model of the atomic substructure including electrons, protons, neutrons, quarks, and gluons.
Bohr Model of Hydrogen
Shoot a stream of photons through a container of hydrogen gas. Observe how photons of certain energies are absorbed, causing the electron to move to different orbits. Build the spectrum of hydrogen based on photons that are absorbed and emitted.
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Fire photons to determine the spectrum of a gas. Observe how an absorbed photon changes the orbit of an electron and how a photon is emitted from an excited electron. Calculate the energies of absorbed and emitted photons based on energy level diagrams. The light energy produced by the laser can be modulated, and a lamp can be used to view the entire absorption spectrum at once.
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Use protons, neutrons, and electrons to build elements. As the number of protons, neutrons, and electrons changes, information such as the name and symbol of the element, the Z, N, and A numbers, the electron dot diagram, and the group and period from the periodic table are shown. Each element is classified as a metal, metalloid, or nonmetal, and its state at room temperature is also given.
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CHEM2.PS2: : Motion and Stability: Forces and Interactions
CHEM2.PS2.1: : Plan and conduct an investigation to compare the properties of the different types of intermolecular forces in pure substances and in components of a mixture.
Melting Points
Every substance has unique transition points, or temperatures at which one phase (solid, liquid, or gas) transitions to another. Use a realistic melting point apparatus to measure the melting points, boiling points, and/or sublimation points of different substances and observe what these phase changes look like at the microscopic level. Based on the transition points, make inferences about the relative strengths of the forces holding these substances together.
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Combine various metal and nonmetal atoms to observe how the electronegativity difference determines the polarity of chemical bonds. Place molecules into an electric field to experimentally determine if they are polar or nonpolar. Create different mixtures of polar and nonpolar molecules to explore the intermolecular forces that arise between them.
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Learn about molecular polarity and how polarity gives rise to intermolecular forces. Measure four macroscopic properties of liquids (cohesion, adhesion, surface tension, and capillary rise). Compare these properties for different liquids and relate them to whether the substances are polar or nonpolar.
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CHEM2.PS2.3: : Investigate and use mathematical evidence to support that rates of chemical reactions are determined by details of the molecular collisions.
Collision Theory
Observe a chemical reaction with and without a catalyst. Determine the effects of concentration, temperature, surface area, and catalysts on reaction rates. Reactant and product concentrations through time are recorded, and the speed of the simulation can be adjusted by the user.
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CHEM2.PS2.5: : Investigate the parameters of chemical equilibria in the laboratory by
Equilibrium and Concentration
Observe how reactants and products interact in reversible reactions. The initial amount of each substance can be manipulated, as well as the pressure on the chamber. The amounts, concentrations, and partial pressures of each reactant and product can be tracked over time as the reaction proceeds toward equilibrium.
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Observe how reactants and products interact in reversible reactions. The amounts of each substance can be manipulated, as well as the pressure on the chamber. This lesson focuses on partial pressures, Dalton's law, and Le Chatelier's principle.
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CHEM2.PS2.5.a: : writing and calculating equilibrium expressions (Kc, Kp, Ksp, Ka, Kb);
Equilibrium and Concentration
Observe how reactants and products interact in reversible reactions. The initial amount of each substance can be manipulated, as well as the pressure on the chamber. The amounts, concentrations, and partial pressures of each reactant and product can be tracked over time as the reaction proceeds toward equilibrium.
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Observe how reactants and products interact in reversible reactions. The amounts of each substance can be manipulated, as well as the pressure on the chamber. This lesson focuses on partial pressures, Dalton's law, and Le Chatelier's principle.
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CHEM2.PS2.5.b: : calculating Q and determining the direction the reaction will proceed; and
Equilibrium and Concentration
Observe how reactants and products interact in reversible reactions. The initial amount of each substance can be manipulated, as well as the pressure on the chamber. The amounts, concentrations, and partial pressures of each reactant and product can be tracked over time as the reaction proceeds toward equilibrium.
5 Minute Preview
Observe how reactants and products interact in reversible reactions. The amounts of each substance can be manipulated, as well as the pressure on the chamber. This lesson focuses on partial pressures, Dalton's law, and Le Chatelier's principle.
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CHEM2.PS2.5.c: : calculating equilibrium concentrations given an equilibrium constant and starting amounts.
Equilibrium and Concentration
Observe how reactants and products interact in reversible reactions. The initial amount of each substance can be manipulated, as well as the pressure on the chamber. The amounts, concentrations, and partial pressures of each reactant and product can be tracked over time as the reaction proceeds toward equilibrium.
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Observe how reactants and products interact in reversible reactions. The amounts of each substance can be manipulated, as well as the pressure on the chamber. This lesson focuses on partial pressures, Dalton's law, and Le Chatelier's principle.
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CHEM2.PS3.1: : Mathematically determine the enthalpy change for a given reaction using Hess’s Law, standard enthalpies of formation, or a given mass of a reactant.
Reaction Energy
Exothermic chemical reactions release energy, while endothermic reactions absorb energy. But what causes some reactions to be exothermic, and others to be endothermic? In this simulation, compare the energy absorbed in breaking bonds to the energy released in forming bonds to determine if a reaction will be exothermic or endothermic.
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CHEM2.PS3.5: : Use Coulomb’s law and patterns of valence electron configurations to explain trends in ionization energies and reactivity of pure elements.
Periodic Trends
Explore trends in atomic radius, ionization energy, and electron affinity in the periodic table. Measure atomic radius with a ruler and model ionization energy and electron affinity by exploring how easy it is to remove electrons and how strongly atoms attract additional electrons. View these properties on the whole periodic table to see how they vary across periods and down groups.
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CHEM2.PS3.7: : Investigate and explain the energy changes in biological systems (such as the combustion of sugar and photosynthesis) both qualitatively and quantitatively.
Cell Energy Cycle
Explore the processes of photosynthesis and respiration that occur within plant and animal cells. The cyclical nature of the two processes can be constructed visually, and the simplified photosynthesis and respiration formulae can be balanced.
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As a marine biologist students learn about photosynthesis to help scientists in Australia determine why the coral in the Great Barrier Reef is bleaching.
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CHEM2.PS4: : Waves and Their Applications in Technologies for Information Transfer
CHEM2.PS4.1: : Investigate and contrast the mechanism of energy changes and the appearance of absorption and emission spectra.
Bohr Model of Hydrogen
Shoot a stream of photons through a container of hydrogen gas. Observe how photons of certain energies are absorbed, causing the electron to move to different orbits. Build the spectrum of hydrogen based on photons that are absorbed and emitted.
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Fire photons to determine the spectrum of a gas. Observe how an absorbed photon changes the orbit of an electron and how a photon is emitted from an excited electron. Calculate the energies of absorbed and emitted photons based on energy level diagrams. The light energy produced by the laser can be modulated, and a lamp can be used to view the entire absorption spectrum at once.
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Analyze the spectra of a variety of stars. Determine the elements that are represented in each spectrum, and use this information to infer the temperature and classification of the star. Look for unusual features such as redshifted stars, nebulae, and stars with large planets.
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CHEM2.PS4.2: : Apply scientific principles and mathematical representations (C = (lambda)v and E = hv) to explain that spectral lines are the result of and correspond to transitions between energy levels.
Bohr Model of Hydrogen
Shoot a stream of photons through a container of hydrogen gas. Observe how photons of certain energies are absorbed, causing the electron to move to different orbits. Build the spectrum of hydrogen based on photons that are absorbed and emitted.
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Fire photons to determine the spectrum of a gas. Observe how an absorbed photon changes the orbit of an electron and how a photon is emitted from an excited electron. Calculate the energies of absorbed and emitted photons based on energy level diagrams. The light energy produced by the laser can be modulated, and a lamp can be used to view the entire absorption spectrum at once.
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Students assume the role of a scientist trying to solve a real world problem. They use scientific practices to collect and analyze data, and form and test a hypothesis as they solve the problems.
