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Matter Make a “Matter” title page in toolkit: •Properties of Matter-Physical and Chemical •Phases of Matter •Atoms •Elements, Molecules, and Compounds •Periodic Table of Elements Priority Standards Learning Targets Proficiencies Matter Pre/Post Assessment Complete the pretest quietly on your own, trying your best! Sit quietly until everyone is finished. Correct pretest as a class using a different colored writing utensil. Matter Open thin, blue textbook titled “Matter” to Chapter 1. Read the introduction page silently to yourself. Next look at ALL pictures/diagrams in the chapter READING ALL captions. Title next page in toolkit “Basics of Matter” Basics of Matter (Toolkit Entry) Define each of the following words (4 flipper or this chart): Matter anything that has ______ and takes up space (_______) Law of Conservation _____ cannot be created nor destroyed of Matter Chemistry the study of _______ Phases a change in ____ or condition of _____ Make a “ Matter” keeper pocket for this unit, and glue in on the next page. Matter Open thin, blue textbook titled “Matter” to Chapter 2. Read the introduction page silently to yourself. Next look at ALL pictures/diagrams in the chapter READING ALL captions. Return to the Section 1 and quietly read the whole text to yourself. Title the next page in your toolkit “Laws of Gases” Matter Open thin, blue textbook titled “Matter” to Chapter 2. Read the introduction page silently to yourself. Next look at ALL pictures/diagrams in the chapter READING ALL captions. Return to the Section 2 and quietly read the whole text to yourself. Title the next page in your toolkit “Phase Changes Vocab” 3 Common States of Matter on Earth Gas •No definite _______ •No definite _______ •Molecules move _______ •Molecules are _______ ____ •Steam (draw picture) Liquid •No definite _______ •Has a definite _______ •Molecules move _______ •Molecules are a little _______ ____ •Water (draw picture) Solid •Definite _______ •Definite _______ •Molecules move _____ ________(vibrate) •Molecules are _____ ________ •Ice (draw picture) 4th Phase of Matter Plasma •No definite _______ •No definite _______ •Atoms move very _______ •Atoms are very _____ ________ •The most common form of matter in the universe •EXTREMELY HOT!!!! Laws of Gases Boyle’s Law Describe this law Draw a diagram. Charles’s Law Describe this law Draw a diagram. Phase Change Lab You will be working with your shoulder partner. Half of the team will complete the lab, while the other half complete notes in toolkit. Teams will switch roles half way through class. Phase Changes Vocab Term Freezing Freezing Point Melting What’s Happening Energy-Remove or Add (Solid/Liquid/Gas/Temperature) Temperature- Change or Not _______ changing to _____ Energy _________ the specific ____________ each type of matter changes from a _______ to a ______ Energy _________ BUT NO ______________ CHANGE _____ changing to _______ Energy _________ the specific __________ each Melting Point type of matter changes from ______ to _________ Boiling ________ changes to _____ throughout the liquid the specific ____________ Boiling Point each type of matter changes from ________ to ______ Energy _________ BUT NO ______________ CHANGE Energy _________ Energy _________ BUT NO ______________ CHANGE Phase Changes Vocab (Con’t) Term Evaporation Vaporization Condensation Sublimation Frost Formation What’s Happening? Energy ______ changes to ___ Energy _________ at the surface at any temperature ______ changes to ___ Energy _________ at boiling point ___ changes to a ____ Energy _________ ______ changes straight to a ____ Energy _________ ____ changes straight to ______ Energy _________ Phases of Matter Graphic Representation Plasma Gas Liquid Solid Particle Movement Particle Movement Particle Movement Phases or States of Matter Discuss what the molecules or atoms are doing in each of the 3 phases of matter. Phase Change Worksheet Complete the Phase Change Worksheet. It will be turned in for a grade at the beginning of the next class (Lunch Academy Assignment). Properties of Matter (2 Long Flippers) Properties are the characteristics to describe matter. 2 Types of Properties Physical Chemical Physical Properties Color, Texture, Mass, Volume, Weight, Temperature Density- d=m/v amount of ______ in a ______ Buoyancy- how well an object ________ Viscosity- how fast matter will _______ Solubility- how well matter _________ Elasticity- how well matter _________ Brittleness- how easily matter _________ Hardness- how well matter does not _________ Ductile- how well can it be made to a thin ______ Luster- ________ Malleability- how well can it be made to a thin ______ Chemical Properties Corrosive- matter that gradually wears away _________ Flammable- how well matter ________ Combustible- how easily matter ______ to burn Reaction rate- how fast matter _______ with other matter Ease or not of bonding- how easily matter ______ together Conductivity- how well matter lets _______ and/or _________ flow through it Physical Changes No new substance made- still same substances with same properties. Can be separated by physical means Sorted Filtered Magnetism Spinning Phase change Gravity (separates over time) Evidence of Chemical Change New substance made Color Change Heat given off or removed from environment Light given off Change in odor Gas given off Precipitate made (solid made) Physical or Chemical Change Lab Travel with your team to each station Read the directions at each station Record observations BEFORE completing the task Record observations AFTER completing the task Decide if the task resulted in a Physical change or a Chemical change. Return each station to it’s ordered state. Assessment Physical and Chemical Changes: Properties of Matter (worksheet) Classifying Matter Six Flipper or Chart Atom Basic unit of all matter. Molecules Elements Matter that can not be broken down into anything simpler, by simple means. A pure substance or the same through out. All are on the Periodic Table of Elements-all the types of atoms. Compounds Matter that is made of 2 or more elements that are chemically bound. Ex: NaCl A pure substance or the same through out. Ex: NaCl (Table Salt) Mixtures Matter made of 2 or more other types of matter that is NOT chemically bound. Can be separated by physical means. May or may not be the same through out -Homogeneous- same through out Ex: Salt water -Heterogeneous- different through out Ex: Milk Types of mixtures Suspensions-large particles and settles out (Italian Dressing) Colloid-Medium particle and settles out (Jello, paint, milk) Solution-minute particles don’t settle out (Salt water) Alloy-metals mixed together (Brass) Solutions Homogeneous mixture, usually in liquid form -Solvent- the substance that dissolves the solute Ex: Water -Solute- the substance that is dissolved Ex: Salt Review Sheets Heterogeneous vs. Homogeneous Mixtures Solutions, Compounds, Mixtures Review of Classifying Matter Matter Is it uniform throughout? No Yes Homogeneous mixture Can it be separated by physical means? No Yes Heterogeneous mixture Pure Substance Can it be decomposed into other substance by a chemical process? No Element Yes Compound Homogeneous Mixture (solution) Review Classification of Matter Activity Find the 3 title strips-Element, Compound, and Mixture Make 3 columns with the title strips. Deal out the strips of paper with examples to each team member evenly. WithOUT team input, each member places their examples under the appropriate title. Once all examples are out, then team mates can start to discuss and support their thoughts with evidence. Key will be revealed, make corrections and copy. Classifying Activity Key Compounds Elements Gold Copper Helium Sodium Barium Francium Lithium Sulfur Carbon Argon o o o o o o o o o o Water Ammonia Carbon dioxide Sugar Table salt Carbon monoxide Ozone Cholesterol Glucose Copper sulfate Mixtures o Milk o Coffee o Air o Ink o Blood o Sand o Soil o Aluminum foil o Chocolate Chip Ice Cream o Paint History of the Atomic Model History of the Atomic Model Timeline foldable: Fold the strip of paper in half, then “burrito” fold it into three equal sections. (total of 6 sections) Label the first section “The Atomic Model” Each of the remaining 5 sections should then include the information on each screen: Name Year Diagram of the model Major facts History of the Atomic Model All elements are made of atoms, which cannot be divided or destroyed. “Billiard Ball” theory – atoms are tiny particles Atoms of the same elements are alike, and different from John Dalton other element’s atoms. (1766-1844) (1856-1940) J.J. Thomson Atoms had even smaller, “subatomic” particles. Subatomic particles had a charge (+ or -). Plum Pudding = Atoms as a positively-charged “pudding” with electrons (-) scattered in it. Ernest Atoms have lots of empty Rutherford space! (1871-1937) 1st model to show a nucleus. Positively-charged particles are in the nucleus (center) of an atom. Negatively-charged particles are around the atom’s edge. Neils Bohr Added to Rutherford’s (1885-1962) model. “Planetary Orbit” model Electrons orbit around an atom’s nucleus, like the planets around the Sun. Wave Model Atoms have a nucleus with (Current) protons (+) and neutrons (neutral) The nucleus is surrounded by electrons (-). Electrons don’t follow a set orbit. We can only predict their locations. Subatomic Particles: Parts of atoms! 3 Sided Pyramid Foldable Fold a top corner down to the side to make a triangle Unfold and repeat opposite direction. Before unfolding fold bottom section for anchor. Unfold and cut 1 angle fold to the center. Mark 1 triangle with the word “glue” Write the title on the anchor and complete the notes for each side. Spread a small amount of glue on the triangle marked “glue” and tuck it inside the pyramid and stick together. Finally, glue the anchor down into your toolkit. Additional vocab Subatomic particles- particles that make up an atom Electron Proton Neutron *Protons + Neutrons = Atomic Mass Proton A positive (+) particle within the nucleus (center) of an atom. Electron A negative (-) particle that orbits the nucleus (outside of the nucleus) of an atom in what’s called an electron cloud. Neutron A neutral (no charge or +/-) particle in the nucleus (center) of an atom. Subatomic Particles A positive (+) particle within the nucleus (center) of an atom. Neutrons A neutral (no charge or +/-) particle in the nucleus (center) of an atom. Electrons A negative (-) particle that orbits the nucleus (outside of the nucleus) of an atom in what’s called an electron cloud. Protons Isotopes Isotope- atoms of the same element that have different numbers of neutrons in the nucleus. C12 and C14 Forces Within the Atom (Toolkit page title) Multiple shutter fold Hold your paper horizontally and burrito fold (2 folds/make 3 equal sections) Unfold the burrito and turn upside down, so the folds make 2 “mountains”. Fold the 2 end sections in half Fill in your notes using the 4 sides Glue down the back middle section. Electromagnetic Force Repels particles of the same force. Attracts particles of the opposite force. + N + - N Strong Force Attracts particles of the same charge when they are close together. This keeps protons together in the nucleus of the atom. + N + N Weak Force The force responsible for radioactive decay, where a neutron turns into one electron and one proton. N + - Gravity Force of attraction between all objects in nature The Periodic Table of Elements https://www.youtube.com/watch?v=zUDDiWtFtEM http://www.search.ask.com/search?o=100000031cr&gct=kwd&q=periodic+table+elemen ts+songs&tpr=10&ctype=videos Vertical columns: Groups or Families (# of valence electrons) Dimitri Mendeleev: Creator of the 6 Atomic Number:# of Protons or Electrons C Carbon 12.011 Element Symbol: 1st Capital 2nd Lower Case Element Name Atomic Mass: # Protons + # Neutrons Key Metals Metalloids Non-Metals Horizontal rows: Periods (# of shells of electrons) Classifying the Periodic Table Metals Metalloids Non-Metals Metals Cu Cr Metals Ag Au Metals Physical Properties •Luster or shine • Conduct heat and electricity • Ductile (can spread thin) • Malleable (can be shaped) Chemical Properties • Lose electrons • Corrode, or wear away Metals Na W http://www.youtube.com/watch?v=sXanNFGY1kA&feature=related Non-metals Ne He Non-metals Physical Properties No shine or luster, dull in appearance Chemical Properties Gain electrons when bonding Not good conductors Noble Gases are nonof heat or electricity. reactive Brittle and break easily Non-metals Nitrogen http://www.youtube.com/watch?v=MaxZwsqs tFs Hydrogen http://www.youtube.com/watch?v=DbmV5lM4 z74&feature=related Metalloids As Si Metalloids Physical Properties Chemical Properties •Solids that are shiny or dull •Ductile and malleable •Semiconductors •Properties of both metals and non-metals Reading the Periodic Table Reading the Periodic Table of Elements 6 C Atomic Number:# of Protons or electrons Element Symbol: 1st Capital 2nd+ Lower Case Carbon Element Name 12.011 Atomic Mass: # Protons + # Neutrons Putting it all together 6 C 12.011 Atomic Number: Atomic Mass: Element Symbol: Number of Protons: Number of Neutrons: Number of Electrons: Putting it all together 8 O 15.999 Atomic Number: Atomic Mass: Element Symbol: Number of Protons: Number of Neutrons: Number of Electrons: Putting it all together 26 Fe 55.847 Atomic Number: Atomic Mass: Element Symbol: Number of Protons: Number of Neutrons: Number of Electrons: Periodic Table Vocabulary Atomic Number Number of _________ in each atom of an element Number of _________= Number of _________ Atomic Mass The number of ________ and __________ _ together in the nucleus Atomic Symbol 1-3 __________ abbreviation for an element. The first letter is ___________ and the next letter(s) is __________ Chemical Bonding The combining of atoms to create a new substance. Electron Mapping Electrons orbit the nucleus of an atom in an electron cloud. The electron cloud is made of energy levels, depending on how many electrons. Each energy level can only hold a certain number of electrons, energy levels start around the nucleus. 1st Energy Level can only hold up to 2 electrons 2nd Energy Level can only hold up to 8 electrons 3rd through unlimited energy levels can only hold up to 18 electrons The outer most level of electrons that are used for bonding are called valence electrons. How to fill the energy levels Start with the 1st (inner) level and work your way outward. Let’s map N (Nitrogen), Ni (Nickel), and then Si (Silicon) 1st Energy Level: 2 electrons 2nd Energy Level: 8 electrons 4th and more Energy Levels: 18 electrons Valence electrons: ______ http://www.brooklyn.cuny.edu/bc/ahp/SDP S/SD.PS.electrons.html M&M Electrons N How to fill the energy levels Let’s do this on paper! Ex: Ti (Titanium) 1. Map Nitrogen 2. Map Nickel 1st Energy Level: 2 electrons 2nd Energy Level: 8 electrons 4th and more Energy Levels: 18 electrons Valence electrons: ______ Chemical Bonds Foldable: 3 sided pyramid Anchor title: 3 Types of Chemical Bonds Ionic (Giving/Taking) Bonds One atom loses an electron to make it positively charged. The other atom gains an electron to make it negatively charged. The positive and negative charges attract, forming an ionic bond. Covalent (Sharing) Bonds Two or more nonmetal atoms are in need of electrons to fill their outer energy levels. The atoms decide to share electrons. This “sharing of electrons” is the definition of a covalent bond Metallic (free-moving) Bonds The electrons become property of all the atoms. Electrons are not tied to their nucleus alone. Ions Electron Affinity- Tendency (or desire) to attract electrons Ion-An atom or atoms that have lost or gained electrons, thus having a charge. +cation -anion Ionization Energy- The energy it takes to form an ion. Chemical Bonding Vocabulary (6 Flipper) Chemical Bonding Combination of ______to form new __________ Valence Electrons Electrons in the ___________ energy level of an ________ Ionization Energy The energy it takes to ______ an ion. Electron Affinity Tendency (or desire) to _________ electrons Ion An atom or atoms that have _______ or _______ electrons, thus having a charge. +_____ -_____ Oxidation Number The number of __________ an atom gains, loses, or shares when it forms ______ bonds Chemical Formulas and Equations Chemical Formulas and Equations Chemical Formula- symbols and numbers to represent atoms and/or molecules. Ex: H2O Chemical Equation- represents chemical reactions. Ex: 2 H2 + O2 2 H2O Co-efficient 2 H2 + O2 2 H2O Subscripts Reactant: What goes in. 2 H2 + O2 2 H2O Hydrogen + Oxygen Water Product: What comes out Equation Examples Fruit Salad: Strawberries + Apples + Grapes Fruit Salad Tuxedo: Jacket + Shirt + Bowtie Tuxedo ABC’s where A and B bond together: A + B + C AB + C Salt: Sodium + Chlorine Salt Photosynthesis: 6CO2 + 6H2O + Energy C6H12O6 + 6O2 Cellular Respiration: C6H12O6 + 6O2 6CO2 + 6H2O + Energy Oxidation Numbers and Chemical Bonding Reminders about chemical bonds: Covalent bonds: Occur between non-metals, where atoms share electrons Ionic bonds: Occur between metals and non-metals, where one atom gives up electrons and another atom takes electrons How chemical bonding works Atoms either share or give/take electrons. Atoms work together to become stable and fill their energy shells. Example: Covalent bond – HCl Oxidation numbers: H= +1 Cl = -1 Cl H How chemical bonding works Example: Ionic bond – KCl Oxidation numbers: K= +1 + Cl = -1 - Oxidation Numbers Oxidation Number: The number of electron(s) an atom gains, loses or shares when it forms chemical bonds Examples: O -2 Oxygen’s oxidation number is -2 because it wants to take two electrons Chemical Reactions Chemical Reaction Vocab Chemical Reaction Process where substances undergo ______ and chemical _______ changes, resulting physical in a newsubstances ________ with new _________. properties Catalyst Substance that _______ speeds up chemical reactions ______ without being used up itself Exothermic Chemical reaction where heat energy is _________ released (Heat _____ exits the reaction so it feels _____). warm Endothermic Chemical reaction where heat energy is _________ _____ the absorbed (Heat enters reaction so it feels _____). cool Chemical Reaction Labs Hot or Not Ice Ice Baby Understanding a Catalyst Catalytic Oxidation Demonstrations Catalytic oxidation Demonstration: A penny is heated to glow red-hot and hung over acetone. https://www.youtube.com/watch?v=TWF0-jIdU-0 Observations: The penny glows until all of the acetone is consumed. Explanation: The copper penny catalyzes the oxidation of the acetone to its combustion products of CO2 and H2O. However, although the combustion products are being formed, keep in mind that combustion itself is not taking place. The copper is simply providing a catalytic surface for the acetone to react upon. The copper, being a catalyst, is not expended during the reaction. What Happened – Hot or not? Calcium Chloride + Sodium Bicarbonate = Sodium Chloride + Calcium Carbonate + Carbonic Acid Carbonic Acid breaks down to water and CO2 Phenol Red turns yellow in acids and red in bases What happened – Ice Ice Baby The reaction feels cold because the energy (heat) is absorbed by the reactant (sodium bicarbonate). Acids and Bases Acids vs. Bases Acids (Acidic) Bases (Alkaline) Form an _________ hydrogen ion (___) H+ in water - Ex. HCl and H3PO4 hydroxide ion Form a ___________ (___) OH- in water - Ex. NaOH and NH4OH sour in foods Taste _______ bitter -Taste _________ in foods slippery -Feels _________ donor Called a “proton _______” acceptor Called a “proton ________” The pH Scale pH Measures the acidity of a solution Neutral pH Scale Less than 7 = Acid Water = 7 = Neutral More than 7 = Base Acid or Base? HCl H3BO3 HC2H3O2 Ca(OH)2 NaOH NH4OH KOH H2SO4 H2CO3 HNO3 H 3 C 6H 5O 7 Mg(OH)2 H3PO4 Al(OH)3 What does salt and water have to do with acids and bases? Can you figure it out????? HCl + NaOH (H+) + (Cl-) + (Na+) + (OH-) HCl + NaOH H2O + NaCl Acid + Base Water + Salt Acid/Base Lab Acid/Base Lab Review 1. If a solution has a pH of 14, is it an acid or base? 2. If a solution has a pH of 3, is it an acid or base? 3. Is HCl an acid or a base? 4. Is NaOH an acid or base? 5. Why are acids called “proton donors”? Ticket to Lab You must have the Acid/Base Lab notes complete before you begin the lab! Materials List: 1 tube of pH stripes with key 1 apple slices 1 orange slices 1 small cup of baking soda solution 1 small cup of water 1 small cup of milk 1 small cup of dishwashing detergent 1 small cup of ammonia 1 small cup of salt solution 1 small cup of sugar solution 1 small cup of apple cider vinegar 1 small cup of vinegar 1 small cup laundry starch 12 small cups Testing pH Procedure 1. Write down the name of the solution you are testing in the first column. 2. Dip one end of your litmus paper into the solution. 3. Record observations and any changes in color of the litmus paper under “Observations”. 4. Write the pH that matches the color of the litmus paper. 5. Record if the solution is an acid or base. Solution Samples Apples Orange Baking Soda Tap Water Milk Dishwasher Detergent Ammonia Salt Water Sugar water Apple Cider Vinegar Vinegar Starch Clorox Bleach Saliva Acids and Bases Videohttp://app.discoveryeducation.com/player/view/assetGuid/410F287B-55FA4A7A-BE2A-14E9B813F994