S8P1. Students will examine the scientific view of the nature of matter.

1. Page 42 S8P1. Students will examine the scientific view of the nature of matter. Distinguish between atoms and molecules

2. Page 43 Matter 10/12/12 S8P1a. What is matter and how can it be classified? Matter is anything that has mass and takes up space. Examples: book, toy, car, paper Non-examples: heat, light Matter is made of tiny indivisible particles called atoms. Atoms are the basic building blocks of all matter. For many years, people have wondered what matter is made of including Democritus, Lavoisier, Dalton, Thompson, Rutherford and Bohr.

3. Page 45 Democritus thought the universe was made of empty space and tiny bits of stuff that were so small they could no longer be divided into smaller pieces. He called these pieces atoms. Lavoisier came up with the law of conservation of matter, which states that matter is not created or destroyed – it only changes forms. wood + oxygen = ash + gases + water vapor Dalton developed the atomic theory of matter. He felt that matter was too small to be seen by the human eye and that each type of matter was made of only one kind of atom.

4. Page 47 Thompson discovered that atoms were a ball of positive charge embedded with negatively charged particles, called electrons. Rutherford called the positively charged, center part of the atom the nucleus. He named the positively charged particles in the nucleus, protons. He concluded that the atom must be mostly empty space in which electrons travel in random paths around the nucleus. Chadwick, a student of Rutherford’s discovered uncharged particles in the nucleus, called neutrons.

5. Page 49 Bohr found that electrons are arranged in energy levels in an atom. The lowest energy level is closest to the nucleus. It can only have two electrons. Higher energy levels are farther from the nucleus. According to Modern Atomic Theory, electrons move in a cloud around the nucleus. Atoms are very small. It would take a million of them combined to be the size of a pencil tip. As tiny as atoms are, they consist of even smaller particles – protons, neutrons and electrons.

6. On page 46,neatly illustrate, color and label Rutherford’s Model of the Atom with Chadwick’s contribution of the neutron. When labeling, label and define the nucleus, electrons, protons, neutrons. On the top half of page 48, neatly illustrate, color and label Bohr’s Model of the Atom On the bottom half of page 48, neatly illustrate, color and label the current model of the atom.

7. Page 51 The nucleus is the small dense, positively charged center of an atom. It contains the most of the atom’s mass. The nucleus contains protons and neutrons. Protons are positively charged particles located inside the nucleus. Neutrons are neutrally charged particles located inside the nucleus. Electrons are negatively charged particles found in electron clouds outside the nucleus.

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9. Page 51 & 53 There are two kinds of pure substances: elements and compounds. An element is matter made up of only one kind of atom. There are over 100 known elements. About 90 of them are found naturally on Earth and the other 20+ are synthetic (man-made). All known elements are arranged in a chart called the periodic table of elements. Each element on the chart has a chemical symbol with one to three letters. The periodic table is arranged in rows called periods and columns called groups or families. There are 7 periods and 18 groups.

10. Page 53 Elements in the same group share similar properties. Each element has an atomic number and an atomic mass. The atomic mass is the average of all of the isotopes of an element. The atomic number isALWAYS the number of protons. It is also the number of electrons in a neutral atom. To determine the number of neutrons, you must subtract the atomic number from the atomic mass. For example, Copper has an atomic number of 29 and an atomic mass of 63. It has 29 protons , 29 electrons and 34 neutrons.

11. On page 52 Look at the periodic table and identify the group name of the following elements: Lithium Xenon Gold Beryllium

12. Page 55 Sometimes the atomic mass of elements can change. For example Hydrogen sometimes has an atomic number of 1, 2 or 3. This is because the number of neutrons may vary. Isotopes are atoms of the same element that have a different number of neutrons. When referring to an isotope, you state the element name followed by its atomic mass. For example: Hydrogen-1 or Hydrogen-2 or Hydrogen-3

13. Page 59 Matter 10/31/12 S8P1a., S8P1f., S8P1d How can matter be classified? All forms of matter can be classified into two groups: pure substances and mixtures. A pure substance is one having a homogeneous composition. There are two types of pure substances: elements and compounds. An element is matter that is made of only one kind of atom. A compound is matter that is formed when two or more elements join (bond) chemically. They cannot be broken apart.

14. On page 58 Identify whether each of the following are elements or compounds in the table below. H H20 Ca Na NaCl CO2 Co Fe2S OH CH4NaOH CO SiO2

15. Page 61 A molecule is the smallest unit of a compound that has all the properties of the compound. The makeup of a molecule is shown in a chemical formula. A chemical formula uses chemical symbols and subscripts to identify the number and types of atoms of each element that make up a compound. A subscript is a small number written to the right and slightly below a chemical symbol to tell the number of atoms of that element is in the substance. The chemical formula for water is H20. This means one molecule of water has 2 Hydrogen atoms and 1 Oxygen atom.

16. On page 60 Determine the number of atoms of each element present in each of the following compounds. CO CO2 H2O2 NaCl NaOH C12H22O11 FeS2 Fe2O3 C2O Na2O CH4

17. Page 63 Elements can combine in different ways to form either compounds or mixtures. A mixture forms when two or more substances combine without joining chemically. They are not bonded together. Because they are not bonded chemically, the parts of a mixture retain their own individual identities and properties and can be separated. A mixture that is unevenly mixed is called a heterogeneous mixture. Ex. Trailmix. A mixture that is mixed evenly is called a homogeneous mixture. Ex. Kool-Aid Summary: EQ- How can matter be classified?

18. On page 62 Identify whether each of the following are heterogeneous or homogeneous mixtures in the table below. Vegetable soup Chex Mix coffee cake batter chocolate chip cookie milk salt water pizza spaghetti & meatballs cereal in milk taco salad

19. Page 65 11/2/12 States of Matter S8P1a., S8P1f., S8P1d Water can be found in solid, liquid and gas forms, how does that happen? A state of matter is the physical form in which matter exists. There are four states (phases) of matter : solid, liquid, gas and plasma. Matter often changes state when heat is added or taken away. A solid is a substance with a definite shape and a definite volume. The particles in a solid are packed closely together and maintain a rigid form without a container. They vibrate slowly against one another.

20. Page 67 A liquid is a substance with a definite volume, but not a definite shape. The particles in a liquid move faster and freely past one another, but are still close to one another. Liquids take the shape of the container they are in. A gas is a substance that does not have a definite shape or a definite volume. Gas particles move very fast and bounce off of one another. Gases fill the container they are in.

21. Page 69 The transformation of matter from one state to another is called a phase transition. Phase transitions occur at precise points when the energy of motion in the atom is too much or too little for the atom to remain at that state. Summary: EQ-Water can be found in solid, liquid and gas forms. How does that happen?

22. On page 64 Identify whether each of the following are solids, liquids or gases in the table below. Milk toy car helium hydrogen water ice steam sugar salt pepsi oxygen

23. On page 66 The freezing point and melting point are the same temperature.

24. On page 68 The following processes are phase transitions. Make the table below and identify what they are.

25. Page 71 11/27/12 S8CS1, S8CS2, S8CS5, S8CS9 and S8P3 Scientific Method How does the design and construction of a bridge affect its durability and ability to withstand weight?

26. On page 70 Popsicle Bridge Lab Write-Up Question: Hypothesis: Procedure: Materials: Observations: Analysis: Results: Conclusion:

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28. Page 75 12/3/12 S8P1d. Properties of Matter What are the various properties of matter and how can I distinguish between physical and chemical properties of matter? A property is a characteristic of matter. A physical property is a characteristic that can be observed or measured without changing the identity of a substance. Examples: density (mass/volume), electrical conductivity, hardness, pH, state of matter and luster A chemical property is a characteristic that describes how a substance will interact with other substances during a chemical reaction. Examples: reactivity, the ability to burn and rust Summary: What are the various properties of matter and how can I distinguish between physical and chemical properties of matter?

29. page 74 Create a two-column table and classify each of the terms below as either a physical property or a chemical property. reacts with base to form water Boiling point density Taste reacts with an acid color flammability melting point luster reacts to oxygen solubility hardness odor reacts with water to form gas

30. Page 77 12/3/12 S8P1.d & S8P1.e Changes in Matter What types of changes can matter undergo? What happens to matter when it undergoes changes? Matter can change. The types of changes matter undergoes are classified into two groups: physical changes and chemical changes. A physical change alters the physical properties of a substance without changing the identity of the substance. Physical changes cause a change in properties such as volume, mass, or state of matter. Many physical changes can be reversed. Examples: melting, evaporating, freezing, cutting A chemical change occurs when a substance is changed into a new substance with different properties. During a chemical change, the identity of a substance is changed. Examples: burning, rusting, baking, combusting

31. Page 79 A chemical reaction is the process by which new substances are formed during a chemical change. Some signs that indicate a chemical reaction has occurred include the forming of gases, a change in color, the release of heat, or the emission of light. Another sign of a chemical reaction is the formation of a precipitate. A precipitate is a solid that forms from a chemical reaction that takes place in a solution. It is very difficult or impossible to reverse the effects of a chemical change. Summary: EQ - What types of changes can matter undergo? What happens to matter when it undergoes changes?

32. page 76 Create a two-column table and classify each of the descriptions below as either a physical change or a chemical change. Iron rusts sodium hydroxide dissolves in water milk goes sour a match ignites and burns an ice cube melts to form a puddle of water icicles form at the edge of a roof chocolate bar melts in the sun water is heated and changed into steam vinegar and baking soda react acid on limestone produces carbon dioxide gas wood and leaves rot a tea kettle begins to whistle

33. page 78 PHYSICAL OR CHEMICAL CHANGE? NO CHEMICAL CHANGE YES PHYSICAL CHANGE QUESTION: AFTER THE CHANGE IS IT THE SAME SUBSTANCE? EVIDENCE OF A CHEMICAL CHANGE BUBBLING TURNS CLOUDY TEMPERATURE CHANGES EXOTHERMIC – ENERGY IS EXITING - GETS HOTTER ENDOTHERMIC – ENERGY IS ENTERING – GETS COOLER COLOR CHANGE CHANGE IN SMELL OR TASTE

34. Page 81 12/4/12 Conservation of Matter S8P1g. During a change in matter, how does the amount of matter compare before and after it changes? The law of conservation of matter states that, during a chemical reaction, matter cannot be created or destroyed. Even though the matter may change from one form to another, the same number of atoms exist before and after the changes take place. Reactant – the substances there before a reaction occurs. Product – the substances there after the reaction takes place. MASS OF REACTANT = MASS OF PRODUCT

35. UNDERSTANDING CHEMICAL REACTIONS & THE LAW OF CONSERVATION OF MATTER Page 83 If 25g of Potassium is reacted with 5g of Oxygen, how much Potassium Oxide is produced? 4K + O2 2K20 25g + 5g 30g Reactants Products 2H2 + O2 2H20 A coefficient shows the number of molecules. 2H2 means 2 hydrogen molecules for a total of 4 hydrogen atoms. A subscript shows how many atoms are in a formula. In O2, the 2 means 2 atoms of oxygen.

36. page 80 – Write the questions and answer each. How many different elements are present? N2 CaF2 CO2 NaSO3 CaCO3 SiO2 How many molecules are present? 2H2O 5Be2Br 8CO2 3NaCl O2MgS How many total atoms are present? 2H2O 2Be2Br 7CO2 6NaCl 4O2 2MgS Using this reaction, answer the following questions. Li2O + MgCl2 2LiCl + MgO Name the first reactant. Circle the second reactant. Underline the first product. Name the second product. How many Mg atoms are on the reactant side? the product side? How many Chlorine atoms are on the reactant side? the product side?

37. page 82 – Write each chemical reaction (and question) and determine the missing value? 2Mg + O2 2Mg0 23g + ?g 38g 2KCl + Li2O  K2O + 2LiCl 21g + 4g ?g + 12g If 23g of Magnesium is reacted with Oxygen to produce 38 g of Magnesium Oxide, how much Oxygen was used in the reaction? Using the numbers provided, determine how much K2O is produced in the reaction.