S8P1. Students will examine the scientific view of the nature of matter. a.Distinguish between atoms...

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

S8P1a. Matter10/12/1 2 What is matter and how can it be classified? Page 43 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.

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.

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 Rutherfords discovered uncharged particles in the nucleus, called neutrons.

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.

On page 46,neatly illustrate, color and label Rutherfords Model of the Atom with Chadwicks 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 Bohrs Model of the Atom On the bottom half of page 48, neatly illustrate, color and label the current model of the atom.

The nucleus is the small dense, positively charged center of an atom. It contains the most of the atoms 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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& 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.

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 is ALWAYS 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.

On page 52 Look at the periodic table and identify the group name of the following elements: 1.Lithium 2.Xenon 3.Gold 4.Beryllium

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

S8P1a., S8P1f., S8P1d Matter10/31/1 2 How can matter be classified? Page 59 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.

On page 58 Identify whether each of the following are elements or compounds in the table below. H H 2 0 Ca Na NaCl CO 2 Co Fe 2 S OH CH 4 NaOH CO SiO 2 ElementCompounds

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 H 2 0. This means one molecule of water has 2 Hydrogen atoms and 1 Oxygen atom.

On page 60 Determine the number of atoms of each element present in each of the following compounds. 1.CO 2.CO 2 3.H 2 O 2 4.NaCl 5.NaOH 6.C 12 H 22 O 11 7.FeS 2 8.Fe 2 O 3 9.C 2 O 10.Na 2 O 11.CH 4

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?

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 Heterogeneous MixtureHomogeneous Mixture

S8P1a., S8P1f., S8P1d States of Matter 11/2/12 Water can be found in solid, liquid and gas forms, how does that happen? Page 65 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.

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.

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? Phase TransitionDescription Melting (add heat)Solid to Liquid Evaporation (heat added)Liquid to Gas Sublimation (heat added)Solid to Gas (skipping Liquid) Condensation (heat removed)Gas to Liquid Freezing (heat removed)Liquid to Solid Deposition (heat removed)Gas to Solid (skipping Liquid)

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 SolidLiquidGas

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

On page 68 The following processes are phase transitions. Make the table below and identify what they are. Phase Transition Water droplets coat your cold soda can on a hot day. A cloud releases rain. Solid dry ice steams in air. Glaciers floating in the ocean are shrinking. Morning dew disappears from the grass by midday. A cloud releases snow.

S8CS1, S8CS2, S8CS5, S8CS9 and S8P3 Scientific Method 11/27/12 How does the design and construction of a bridge affect its durability and ability to withstand weight? Page 71 Bridge #Design / DescriptionMaximum Weight Failure Description 1 2 3 4 5 6 7 8 9

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

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S8P1d. Properties of Matter 12/3/12 What are the various properties of matter and how can I distinguish between physical and chemical properties of matter? Page 75 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?

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 Physical PropertyChemical Property

S8P1.d & S8P1.e Changes in Matter 12/3/12 What types of changes can matter undergo? What happens to matter when it undergoes changes? Page 77 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

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?

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 Physical ChangeChemical Change

PHYSICAL OR CHEMICAL CHANGE? YES PHYSICAL CHANGE NO CHEMICAL 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

S8P1g. Conservation of Matter 12/4/12 During a change in matter, how does the amount of matter compare before and after it changes? Page 81 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

UNDERSTANDING CHEMICAL REACTIONS & THE LAW OF CONSERVATION OF MATTER 2H 2 + O 2 2H 2 0 Reactants Products 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. 4K + O 2 2K 2 0 25g + 5g 30g If 25g of Potassium is reacted with 5g of Oxygen, how much Potassium Oxide is produced? Page 83

Write the questions and answer each. How many different elements are present? N 2 CaF 2 CO 2 NaSO 3 CaCO 3 SiO 2 How many molecules are present? 2H 2 O 5Be 2 Br 8CO 2 3NaCl O 2 MgS How many total atoms are present? 2H 2 O 2Be 2 Br 7CO 2 6NaCl 4O 2 2MgS Using this reaction, answer the following questions. Li 2 O + MgCl 2 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?

Write each chemical reaction (and question) and determine the missing value? 2Mg + O 2 2Mg0 23g + ?g 38g 2KCl + Li 2 O K 2 O + 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 K 2 O is produced in the reaction.

S8P1. Students will examine the scientific view of the nature of matter. a.Distinguish between atoms...

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