C.1.1 Differentiate between pure substances and mixtures based on physical and chemical properties. Identify and explain why a sample that has multiple elements (water) can be pure (depending on the sample, not tap water). Students are able to identify physical and chemical properties in the laboratory. Separate mixtures using physical and chemical properties. Pure substance – composed of only one type of particle (compound or element) Mixture – sample of two or more pure substances where each material maintains its own properties Physical property – aspect of matter that can be observed or measured without changing the chemical composition of the sample Chemical property – any property of matter that may only be observed and measured by performing a chemical change or chemical reaction. Patterns Structure and Function C.1.2 Use chemical properties, extensive, and intensive physical properties to identify substances. Identifying various compounds and elements based on their chemical properties (flammable, oxidizer, etc.) extensive (mass, volume, etc.) and intensive physical properties (density, hardness, color, melting point, odor, etc.). Extensive properties of mass and volume can be used to calculate density (intensive) to help identify the substance. Extensive properties alone are not useful in the identification of a substance. Chemical properties – any property of matter that may only be observed and measured by performing a chemical change or chemical reaction. Extensive properties – dependent on the amount of matter that is present in a sample Intensive properties – do not depend on the amount of matter present in a sample Physical properties – aspect of matter that can be observed or measured without changing the chemical composition of the sample Substances – a material with a definite chemical composition Patterns Structure and Function C.1.3 Recognize observable macroscopic indicators of chemical changes. Use the indicators of energy released/absorbed during a reaction(heat, light, sound), gas production, precipitate formation, or color change to justify whether a chemical reaction occurred or if there was just a physical change. macroscopic indicators – observations made by the naked eye chemical changes – the making and/or breaking of chemical bonds resulting in the formation of new chemical substances Energy and matter
C.1.4 Describe physical and chemical changes at the particle level. Students examine and build models of what samples look like at the microscopic level. Manipulate atoms/particles to see that chemical changes rearrange particles and break/form new bonds. Physical changes – any change that does not change the chemical identity of a substance Chemical changes – the making and/or breaking of chemical bonds resulting in the formation of new chemical substances Particle – smallest individual units of a sample (formula units, molecules, atoms) Structure and function Energy and Matter C.1.5 Describe the characteristics of solids, liquids, and gases and changes in state at the macroscopic and microscopic levels. Students look at defining characteristic of each state of matter. Students make/examine models of particles at the microscopic/macroscopic levels and how these particles behave in each of the states of matter. Solid – state of matter characterized by structural rigidity and resistance to changes of shape or volume Liquid – state of matter characterized by nearly constant volume independent of pressure and conforms to the shape of its container. Gas – of matter that expands freely to fill any space available Change in state – transition from one state of matter to another state of matter Macroscopic – visible to the naked eye/large scale Microscopic – visible only with a microscope or various scale/particle level Cause and Effect Scale, proportion, and quantity Energy and Matter C.1.6 Demonstrate an understanding of the law of conservation of mass through the use of particle diagrams and mathematical models. Modeling a chemical reaction through diagrams, manipulatives so that as a chemical reaction occurs, the that make the reactants equal that in the final products, just rearranged and bonds formed/broke Law of conservation of mass – matter can be changed from one form into another, but the total amount of mass remains the same Particle diagrams – visual depiction in which atoms and molecules are drawn as dots/circles Mathematical models – description of a system using equations Patterns Proportion, and Quantity
C.2.5 Compare and contrast nuclear reactions with chemical reactions Emphasis is on simple qualitative models, such as pictures or diagrams, and on the scale of energy released in nuclear processes relative to other kinds of transformations. Nuclear reactions – change in the energy or structure of an atomic nucleus (fission, fusion, or radioactive decay) Chemical reactions – process of rearrangement of the molecular or ionic structure of a substance (making or breaking chemical bonds), as opposed to change in physical form or a nuclear reaction Energy and Matter Stability and change C.2.6 Describe nuclear changes in matter, including fission, fusion, transmutations, and decays. Emphasis is on simple qualitative models, such as pictures or diagrams, and on the scale of energy released in nuclear processes relative to other kinds of transformations. Nuclear changes – change in the number of protons or neutrons in the nucleus of an atom Matter – thing that has mass and takes up space Fission – splitting of a nucleus of an atom into two nuclei of lighter atoms and the release of energy Fusion – nuclei of light atoms join to form nuclei of heavier atoms Transmutation – the conversion of one element or nucleide into another either naturally or artificially Decay – nucleus of an unstable atom loses energy by emitting radiation Energy and matter Stability and change Structure and function C.2.7 Perform half-life calculations when the appropriate information about the isotope. Perform sample calculations and half-life to find time that has passed, original mass, final mass, and calculate half-life based on experimental data. Half-life – the time it for half of a radioactive sample to decay to a more stable isotope Isotope – any of two or more species of atoms of a chemical element with the same atomic number and nearly identical chemical behavior but with differing atomic mass or mass number and different physical properties Patterns proportion, and quantity Standard 3: Bonding and Molecular Structure Indiana Academic Standard Clarifying Statement Highlighted Vocabulary from the Standard Defined Crosscutting Concept
C.3.1 Investigate the observable characteristics of elements, ionic, and covalent compounds. Examine conductivity, solubility, melting boiling point, etc. using lab data and observations Elements – smallest unit of matter that maintains its unique properties compounds – chemical compound comprised of ions held together by electrostatic forces Covalent compounds – two or more nonmetal bonded by sharing valence electrons Patterns Structure and function C.3.2 Compare and contrast how ionic and covalent compounds form. Ionic compounds – chemical compound comprised of ions held together by electrostatic forces Covalent compounds – two or more nonmetal bonded by sharing valence electrons Structure and function Systems and system models C.3.3 Draw structural formulas for simple molecules and determine their molecular shape. Introduction to drawing structural formulas and simple molecular shapes emphasizing three dimensional molecules (water is bent because of lone pairs of electrons) Structural formulas – a formula that shows the arrangement of atoms in the molecule of a compound Molecules – group of atoms held together by chemical bonds Molecular shape – three dimensional arrangement of the atoms bonded in a molecule System and system models C.3.4 Write chemical formulas for ionic compounds and covalent compounds given their names and vice versa. Writing formulas and naming compounds for simple binary and binary covalent compounds Chemical formula – set of chemical symbols showing the elements present in a compound and their relative proportions Patterns System and system models
Indiana Academic Standard Clarifying Statement Highlighted Vocabulary Words from the Standard Defined Crosscutting Concept C.6.1 Explain that atoms and molecules are in constant motion and that this motion increases as thermal energy increases. Motion –moving or changing place or position Thermal energy – internal energy of an object due to kinetic energy of its atoms and/or molecules Scale, proportion, and quantity Cause and effect C.6.2 Distinguish between the concepts of temperature and heat flow in macroscopic and microscopic terms. Temperature – measure of thermal energy Heat flow – process whereby heat moves from one body or substance to another by radiation, conduction, convection, or a combination of these methods Macroscopic – visible to the naked eye/large scale Microscopic – visible only with a microscope or various technology/small scale/particle level Scale, proportion, and quantity Energy and matter C.6.3 Classify chemical reactions and phase changes as exothermic or endothermic based on enthalpy values. Use a graphical representation to illustrate the energy changes involved Emphasis is on the idea that a chemical reaction is a system that affects the energy change. Examples of models could include molecular-level drawings and diagrams of reactions, graphs showing the relative energies of reactants and products, and representations showing energy is conserved Phase changes – transition between solid, liquid, and gaseous phases Exothermic – accompanied by the release of heat Endothermic – accompanied by or requiring the absorption of heat Enthalpy – measure of energy in a thermodynamic system Energy and matter C.6.4 Perform calculations involving heat flow, temperature changes, and phase changes by using known values of specific heat, phase change constants, or both. Specific heat – thermal energy required to raise the temperature of one gram of a given substance by one degree Celsius Phase change constants – rate of energy required to change a mass of sample from one state to another(heat of fusion, heat of vaporization) Scale, proportion, and quantity Energy and matter Standard 7: Solutions