Harnett County High Schools s1

HARNETT COUNTY HIGH SCHOOLS

Course: Physical Science Title of Unit: 2.1 & 2.2 Chemistry Timeframe: 40 days Content Area Standard(s): http://www.dpi.state.nc.us/docs/acre/standards/support-tools/unpacking/science/physical.pdf

PSc.2.1 Understand types, properties, and structure of matter. PSc.2.1.1 Classify matter as: homogeneous or heterogeneous; pure substance or mixture; element or compound; metals; nonmetals, or metalloids; solution, colloid, or suspension. PSc.2.1.2 Explain the phases of matter and the physical changes that matter undergoes. PSc.2.1.3 Compare physical and chemical properties of various types of matter. PSc.2.1.4 Interpret the data presented in the Bohr model diagrams and dot diagrams for atoms and ions of elements 1 - 18

PSc.2.2 Understand chemical bonding and chemical interactions. PSc.2.2.1 Infer valence electrons, oxidation number, and reactivity of an element based on its location in the Periodic Table. PSc.2.2.2 Infer the type of chemical bond that occurs, whether covalent, ionic, or metallic, in a given substance. PSc.2.2.3 Predict chemical formulas and names for simple compounds based on knowledge of bond formation and naming conventions. PSc.2.2.4 Exemplify the law of conservation of mass by balancing chemical equations. PSc.2.2.5 Classify types of reactions such as synthesis, decomposition, single replacement, or double replacement. PSc.2.2.6 Summarize the characteristics and interactions of acids and bases.

Unpacked What does this standard mean a child will know, understand and be able to do? PSc.2.1.1

• Classify a sample of matter as homogeneous or heterogeneous based on uniformity of the material.

• Classify a sample of matter as a pure substance or mixture based on the number of elements or compounds in the sample.

• Classify an element as a metal, nonmetal, or metalloid based on its location on the periodic table.

• Classify a substance as an element or compound using its chemical formula.

• Classify samples and sets of matter as a solution, colloid or suspension based on the application of characteristic properties: particle size, “settling out” of one or more components, and interaction with light (Tyndall Effect).

PSc.2.1.2 • Develop a conceptual cause-and-effect model for the phase change process that shows the relationship among particle attraction, particle motion, and gain or loss of heat – when a solid melts it has absorbed heat that increased the potential energy of its particles (space between particles) thus reducing the attraction between particles so that they can flow in a liquid phase. (Consider conditions of normal atmospheric pressure as well as the qualitative effects of changes in pressure involving gases.)

• The focus should be on the following phase changes: solid to liquid (melting), liquid to gas (vaporization), gas to liquid (condensation), and liquid to solid (freezing).

• Compare the process of evaporation to vaporization – materials that evaporate verses those which do not; attraction between surface particles and colliding air molecules.

• Recognize that the formation of solutions is a physical change forming a homogenous mixture. (Review from 8th grade.)

• Develop a conceptual model for the solution process with a cause and effect relationship involving forces of attraction between solute and solvent particles. A material is insoluble due to a lack of attraction between particles.

• Interpret solubility curves to determine the amount of solute that can dissolve in a given amount of solvent (typically water) at a given temperature.

• Qualitatively explain concentration of solutions as saturated, unsaturated or supersaturated; dilute or concentrated. PSc.  Calculate the density of different substances using the relationship. D= m/v

• Compare physical properties of a mixture that could be used to separate its components such as solubility, density, boiling point, magnetic property, etc.

• Compare various physical and chemical properties of metals, nonmetals and metalloids such as state of matter at a given temperature, density, melting point, boiling point, luster, conductivity, ductility, malleability, color, reactivity, etc.

• Compare physical and chemical properties of various everyday materials such as salt, sugar, baking soda, corn starch, rubbing alcohol, water, etc.

PSc.2.1.4

• Describe the charge, relative mass, and the location of protons, electrons, and neutrons within an atom.

• Calculate the number of protons, neutrons, electrons, and mass number in neutral atoms and ions.

• Explain how the different mass numbers of isotopes contributes to the average atomic mass for a given element (conceptual, no calculations).

• Use isotopic notation to write symbols for various isotopes (ex. Carbon-12, C-12, 12C, etc.)

• Explain Bohr’s model of the atom.

• Draw Bohr models from hydrogen to argon including common isotopes and ions.

• Construct dot diagrams, a shorthand notation for Bohr models, using the element symbol and dots to represent electrons in the outermost energy level.

* Note: While there is value in students understanding the historical development of atomic theory, the focus is on understanding the relationship between structure and properties of matter. The Quantum Mechanical Model of the atom provides a more in-depth understanding of atomic structure; it can be included as an enrichment PSc.2.2.1

• Predict the number of valence electrons of representative elements (A Groups or 1, 2, 13-18) based on its location in the periodic table.

• Predict an element’s oxidation number based on its position in the periodic table and valence electrons. (Representative groups including multiple oxidation states for tin and lead.)

• Predict reactivity of metals and nonmetals from general periodic trends.

PSc.2.2.2

• Describe how ionic, covalent, and metallic bonds form and provide examples of substances that exhibit each type of bonding.

• Predict the type of bond between two elements in a compound based on their positions in the periodic table.

PSc.2.2.3

• Name and write formulas for simple binary compounds containing a metal and nonmetal l using representative elements (A Groups or 1, 2, 13-18) and compounds involving common polyatomic ions: ammonium (NH4⁺), acetate (C2H3O2⁻), nitrate (NO3⁻), hydroxide (OH⁻), carbonate (CO32⁻), sulfate (SO42⁻), phosphate (PO43⁻).

• Name and write formulas for binary compounds of two nonmetals using Greek prefixes (mono-, di-, tri-, tetra-, etc.).

PSc.2.2.4

• Use coefficients to balance simple chemical equations involving elements and/or binary compounds.

• Conclude that chemical equations must be balanced because of the law of conservation of matter.

PSc.2.2.5

• Classify chemical reactions as one of four types: single replacement, double replacement, decomposition and synthesis. (Neutralization reaction is a type of double replacement reaction.)

• Summarize reactions involving combustion of hydrocarbons as not fitting into one of these four types. Hydrocarbon + oxygen carbon dioxide + water. PSc.2.2.6

• Recognize common inorganic acids including hydrochloric (muriatic) acid, sulfuric acid, acetic acid, nitric acid and citric acid.

• Recognize common bases including sodium bicarbonate, and hydroxides of sodium, potassium, calcium, magnesium, barium and ammonium.

• Define acids and bases according to the Arrhenius theory.

• Develop an understanding of the pH scale and the classification of substances therein.

• Generalize common characteristics of acids and bases– pH range, reactivity with metals and carbonates (acids) or fats/oils (bases), conductivity.

• Relate general household uses of acids and bases with their characteristic properties.

• Explain what happens in a neutralization reaction, identifying each component substance.

Reading Standard(s):

3. Follow precisely a 4. Determine the meaning 7. Translate quantitative or complex multistep of symbols, key terms, and technical information procedure when carrying other domain-specific expressed in words in a out experiments, taking words and phrases as they text into visual form (e.g., measurements, or are used in a specific a table or chart) and performing technical tasks, scientific or technical translate information attending to special cases context relevant to grades expressed visually or or exceptions defined in 9–10 texts and topics. mathematically (e.g., in an the text. equation) into words. Writing Standard(s):

2. Write and analogy to manage the produce, publish, and informative/explanatory complexity of the topic; update individual or shared texts, including the convey a knowledgeable writing products in narration of historical stance in a style that response to ongoing events, scientific responds to the discipline feedback, including new procedures/ experiments, and context as well as to arguments or information. or technical processes… d. the expertise of likely Use precise language, readers. 9. Draw evidence from domain-specific informational texts to vocabulary and techniques 6. Use technology, support analysis, such as metaphor, simile, including the Internet, to reflection, and research.

Math Practice(s):

1. Make sense of problems and 4. Model with mathematics. persevere in solving them. 5. Use appropriate tools 2. Reason abstractly and strategically. quantitatively. 6. Attend to precision. 3. Construct viable arguments and critique the reasoning of others. 7. Look for and make use of structure.

Technology Standard(s):

1. Use technology and other resources 2. Design project-based products that for assigned tasks (involves address global problems. accessing & organizing information.) Learning Experiences:

Eureka videos (YouTube) (RBT A2) Episodes 16 - 25

Google Mr. Guch chemistry worksheets (RBT C3)

Differentiate between an element and compound - students create their own compound (RBT A2)

Using note cards to identify cations and anions to make viable ionic compounds (RBT A2)

Naming ionic compounds after activity above (RBT C2)

Identify sub atomic particles - protons, neutrons, electrons (RBT A1)

Designing Bohr models for the 1st 20 elements followed by organizing each element according to valence electrons (groups) and energy levels (periods) (RBT B6) Note: explain helium’s position in group 18.

Demo’s of chemical reactions (Ex. Combustion of hydrogen in a balloon, single replacement of

Ag in AgNO3 by Cu under a microscope) (RBT B2)

Safe hands-on activities involving chemical reactions (Ex. Test for oxygen, single and double replacement reactions, safe combustion reactions) (RBT C4)

Analysis of chemical reactions in terms on bonding (metallic, ionic and covalent) and classification (single or double replacement, synthesis, decomposition, exothermic or endothermic) (RBT D4)

Dalton’s playhouse (internet activity) for simulations of chemical reactions using Dalton’ Students will determine the Law of Conservation of Matter (RBT C5)

Project Goals and Description of Unit: The chemistry unit will provide students with an overall understanding the composition of particles.

Students will be able to identify elements and compounds, distinguish a heterogeneous and homogenous mixture.

Students will be able to classify, analyze and balance chemical equations/reactions.

Student will be able to analyze and interpret the periodic trends. Student will be able to draw Lewis dot structures, analyze and create Bohr models.

Students will be able to understand the atomic structure.

Student will be able to apply laboratory safety practices to real life experiments. Essential Questions:

1. How is matter identified based on its particles?

2. How do various condition affect how particles interact with each other?

3. How do you think scientist have developed the concept of particles over time? Vocabulary:

Bose-Einstein Solid Liquid Gas plasma matter Condensate homogeneous Solution Heterogeneous mixture element compound

Law of Chemical Physical Colloid Tyndall suspension alloy conservation of Properties properties effect mass allotropes Pure substance density Boiling point Freezing point Melting point crystallization Condensation evaporation Sublimation Deposition Saturated supersaturated unsaturated solubility concentration atom elements

Thomson Plum pudding Rutherford Gold foil Chadwick Bohr model experiment

Bohr model Electron cloud Proton Neutron Electron Atomic number model

Atomic mass isotopes Bohr model periodic table alkali metals alkaline earth metals

halogens noble gases transition metals inner transition valence oxidation metals electrons numbers

Lewis dot Octet rule ion anion cation ionic bond diagram covalent bond metallic bond chemical polyatomic ion chemical balanced formula reaction equation reactant product coefficient subscript synthesis decomposition single double acid base neutralization combustion replacement replacement

Ph scale Instructional Resources (print materials, technology):

http://www.vocabahead.com

http://harnettcountyschools.wikispaces.com

Facilitator’s Role:

Ensure all students are conscious of laboratory safety rules.

Demonstrate various experiments

Model chemical reactions

Provide descriptive feedback

Assessment: Formative Assessments:

 Ticket out the door  Bell ringers  White boarding

 Online assessments  Clock buddies  Parking Lot to allow students to ask  Think-Pair-Share  Pop quizzes questions  Peer Assessment  Popcorn questioning  Writing summary of  KWL learned concepts

Summative Assessments:

 projects

 quizzes  unit tests,  midterm exam,

 lab report  comprehensive final SAS (Access via the Harnett County Schools homepage) Goal 2 PSc.2.1 Understand types, properties, and structure of matter. PSc.2.1.1 Classify matter as: homogeneous or heterogeneous; pure substance or mixture; element or compound; metals; nonmetals, or metalloids; solution, colloid, or suspension.

SAS: Investigate and analyze the properties and composition of solutions:

Solutions, Suspensions & Colloids, Inquiry 68 Solubility curves. Solubility Curves, Web Lesson 467 VLab: Solution Properties, Interactive Tool 1199 Concentration. Lab: Determining Salinity, Web Lesson 999 Solubility Curves, Web Lesson 467 Understanding pH, Web Lesson 475 Lab: Indicators, Web Lesson 992 VLab: Measures of Concentration, Interactive Tool 866 Lab: Using Colligative Properties to Identify Pure Substances & Mixtures, Web Lesson 259 Colligative Properties: Freezing & Boiling Points, Inquiry 60 VLab: Solution Properties, Interactive Tool 1199 Polarity. VLab: Solution Properties, Interactive Tool 1199

PSc.2.1.2 Explain the phases of matter and the physical changes that matter undergoes. Lab: Heating Curve for Water QL #973 Phase Diagram QL# 258 Structure & Properties of Water QL #42

PSc.2.1.3 Compare physical and chemical properties of various types of matter. SAS: Identify substances through the investigation of physical properties: Density. Lab: Using Specific Gravity to Identify Unknowns, Web Lesson 1005 Archimedes' Principle, Web Lesson 481 VLab: Density, Interactive Tool 11 Air Density, Web Lesson 273 Melting point. Properties of Elements, Web Lesson 453 Melting Points & Boiling Points, Web Lesson 977 Phase Diagrams, Web Lesson 258 Lab: Heating Curve for Water, Web Lesson 973 Properties of Solids, Web Lesson 466 Boiling point. Properties of Elements, Web Lesson 453 Melting Points & Boiling Points, Web Lesson 977 Phase Diagrams, Web Lesson 258 Colligative Properties: Freezing & Boiling Points, Inquiry 60 Lab: Heating Curve for Water, Web Lesson 973 Properties of Solids, Web Lesson 466

* Note: While there is value in students understanding the historical development of atomic theory, the focus is on understanding the relationship between structure and properties of matter. The Quantum Mechanical Model of the atom provides a more in-depth understanding of atomic structure; it can be included as enrichment. Develop an understanding of how scientific processes have led to the current atomic theory. Dalton’s atomic theory. The Evolution of Atomic Theory, Web Lesson 988 J.J. Thomson’s model of the atom. The Evolution of Atomic Theory, Web Lesson 988 Rutherford’s gold foil experiment. The Evolution of Atomic Theory, Web Lesson 988 Bohr’s planetary model. The Evolution of Atomic Theory, Web Lesson 988 VLab: Atomic Structure, Interactive Tool 1197 Lab: Line Spectra, Web Lesson 276 Electron cloud model. The Evolution of Atomic Theory, Web Lesson 988 VLab: Electron Transitions, Interactive Tool 7

PSc.2.1.4 Interpret the data presented in the Bohr model diagrams and dot diagrams for atoms and ions of elements 1 – 18

SAS: Examine the nature of atomic structure: Protons. VLab: Atomic Structure, Interactive Tool 1197 Neutrons. VLab: Atomic Structure, Interactive Tool 1197 Electrons. Using the Periodic Table to Determine Oxidation States , Inquiry 57 VLab: Atomic Structure, Interactive Tool 1197 Lab: Line Spectra, Web Lesson 276 Elements: Chemical & Physical Properties, Web Lesson 262 VLab: Electron Transitions, Interactive Tool 7 Molecular Structures, Web Lesson 256 Lewis Electron Dot Structures, Inquiry 39 Atomic mass. Formula & Molecular Masses, Inquiry 63 VLab: Atomic Structure, Interactive Tool 1197 Atomic number. VLab: Atomic Structure, Interactive Tool 1197 Elements: Chemical & Physical Properties, Web Lesson 262 Isotopes. VLab: Atomic Structure, Interactive Tool 1197

PSc.2.2 Understand chemical bonding and chemical interactions.

PSc.2.2.1 Infer valence electrons, oxidation number, and reactivity of an element based on its location in the Periodic Table. Analyze the periodic trends in the physical and chemical properties of elements. Groups (families). Periodic Properties, Web Lesson 470 Using the Periodic Table to Determine Oxidation States , Inquiry 57 Properties of Elements, Web Lesson 453 Chemical Nomenclature, Inquiry 46 Elements: Chemical & Physical Properties, Web Lesson 262 Lewis Electron Dot Structures, Inquiry 39 Periods. Periodic Properties, Web Lesson 470 Using the Periodic Table to Determine Oxidation States , Inquiry 57 Properties of Elements, Web Lesson 453 Elements: Chemical & Physical Properties, Web Lesson 262

PSc.2.2.2 Infer the type of chemical bond that occurs, whether covalent, ionic, or metallic, in a given substance. Ionic & Covalent Bonds QL #464

PSc.2.2.3 Predict chemical formulas and names for simple compounds based on knowledge of bond formation and naming conventions.

SAS: Investigate and analyze the formation and nomenclature of simple inorganic compounds Chemical Nomenclature, Inquiry 46 Ionic bonds (including oxidation numbers). Using the Periodic Table to Determine Oxidation States , Inquiry 57 Chemical Nomenclature, Inquiry 46 Ionic & Covalent Bonds, Web Lesson 464 Lewis Electron Dot Structures, Inquiry 39 Covalent bonds. Chemical Nomenclature, Inquiry 46 Lewis Electron Dot Structures, Inquiry 39 Metallic bonds. Properties of Solids, Web Lesson 466

PSc.2.2.4 Exemplify the law of conservation of mass by balancing chemical equations. Lab: Conserving Mass QL #238 Balancing Chemical Equations QL #989

PSc.2.2.5 Classify types of reactions such as synthesis, decomposition, single replacement, or double replacement. SAS: Identify the reactants and products of chemical reactions and balance simple equations of various types: Single replacement. VLab: Chemical Equations, Interactive Tool 1194 Writing & Classifying Chemical Equations, Web Lesson 970 The Chemical Basis of Industry, Web Lesson 465 Lab: Chemical Reactions: Classes and Characteristics, Web Lesson 257 Double replacement. VLab: Precipitation Reactions, Interactive Tool 867 Lab: Conserving Mass , Web Lesson 238 VLab: Chemical Equations, Interactive Tool 1194 Writing & Classifying Chemical Equations, Web Lesson 970 The Chemical Basis of Industry, Web Lesson 465 Lab: Chemical Reactions: Classes and Characteristics, Web Lesson 257 Decomposition. Decomposition Reactions, Inquiry 58 VLab: Chemical Equations, Interactive Tool 1194 Writing & Classifying Chemical Equations, Web Lesson 970 The Chemical Basis of Industry, Web Lesson 465 Lab: Chemical Reactions: Classes and Characteristics, Web Lesson 257 Synthesis. VLab: Chemical Equations, Interactive Tool 1194 Writing & Classifying Chemical Equations, Web Lesson 970 The Chemical Basis of Industry, Web Lesson 465 Lab: Chemical Reactions: Classes and Characteristics, Web Lesson 257 PSc.2.2.6 Summarize the characteristics and interactions of acids and bases.

SAS: Investigate and analyze the properties and composition of solutions: Solutions, Suspensions & Colloids, Inquiry 68 Solubility curves. Solubility Curves, Web Lesson 467 VLab: Solution Properties, Interactive Tool 1199 Concentration. Lab: Determining Salinity, Web Lesson 999 Solubility Curves, Web Lesson 467 Understanding pH, Web Lesson 475 Lab: Indicators, Web Lesson 992 VLab: Measures of Concentration, Interactive Tool 866 Lab: Using Colligative Properties to Identify Pure Substances & Mixtures, Web Lesson 259 Colligative Properties: Freezing & Boiling Points, Inquiry 60 VLab: Solution Properties, Interactive Tool 1199 Polarity. VLab: Solution Properties, Interactive Tool 1199 pH scale. Understanding pH, Web Lesson 475 Lab: Indicators, Web Lesson 992 Acids & Bases: Physical & Chemical Properties, Web Lesson 267 VLab: Acid-Base Chemistry (Titrations), Interactive Tool 9

PSc.2.3 Understand the role of the nucleus in radiation and radioactivity. PSc.2.3.1 Compare nuclear reactions including alpha decay, beta decay, and gamma decay; nuclear fusion and nuclear fission.

SAS: Understand the role of the nucleus in radiation and radioactivity.

Nuclear Reactions QL#77 Radioactivity QL#1008 Nuclear Power: The Pros & Cons, Web Lesson 268

Notes and Additional Information:

To add and/or check for new materials check the following: http://harnettcountyhighschools.wikispaces.com/Science