1. Matter PSc.2.1: Understand types, properties, and structure of matter.

2. What is matter?  Anything that has mass and volume (takes up space)  Examples: wood, candy, water, ice  Forms of energy such as electricity, heat, and lightning are NOT matter according to the definition.

3. Classifying Matter MatterPure substanceElementcompoundMixtureheterogeneoushomogeneous

4. Pure Substance  Has a fixed chemical composition  Examples: water (H 2 O) Hydrogen (H 2 )  The composition of a pure substance is the same all of the time. Sugar is a pure substance because its chemical composition is the same no matter what manufacturer produces it.

5. Pure Substances Can Be Classified as either element or compound.  Element: composed of only 1 kind of atom. You will find elements listed on the Periodic Table of Elements;  Elements have a single symbol that is either one or two letters.  If the symbol is two letters, the first one is ALWAYS capitalized and the second is ALWAYS lower case.  Example: carbon (C), Helium (He)

6. Elements can be classified as metals, non-metals or metalloids (semi-metals)  The periodic table of elements organizes the elements into metals, non-metals and metalloids.

7. Metals Metalloids Non- metals

8. Compound  a substance formed from two or more different elements that have undergone a chemical reaction to combine them  Has a chemical formula that contains the symbols of each element in the compound  Example: oxygen (element) combines with hydrogen (element) to create a water molecule (H 2 O)

9. Mixtures  Have a composition that varies depending upon the amount of substances combined or mixed together  Example: sugar mixed with tea; ice cream sundae; soil

10. Mixtures can be classified according to how well the substances are mixed.  Heterogeneous mixture: substances do not mix well; you can see different layers or substances settle out to bottom  Homogeneous mixture: substances are well mixed and look like one substance; you don’t see layers or particles settling to the bottom

11. Homogeneous and heterogeneous mixtures can be classified as……  Solutions: homogeneous mixture where particles are evenly dispersed throughout  Suspension: heterogeneous mixture where particles are somewhat evenly dispersed  Colloid: heterogeneous mixture of tiny particles that are intermediate in size suspended in a liquid, solid or gas; will scatter light (tyndall effect)

12. Classify the following……  Orange juice with pulp  Lithium (Li)  Carbon monoxide (CO)  Koolaid  Chocolate chip cookies  Sugar water

13. Solutions (homogeneous)  Solutions are homogeneous mixtures of substances.  When a substance dissolves in another substance it is described as soluble because there is an attraction between the particles of the solute (substance being dissolved) and the solvent (the substance doing the dissolving.  Insoluble: the substance will not dissolve in the solvent because there is a lack of attraction between the particles.  Solutions can be described in the following manner:  Unsaturated: there is more solvent and less solute so there is “room” for more solute to dissolve  Saturated: the solvent has dissolved the maximum amount of solute: “no more room”  Supersaturated: there is more solute than the solvent can dissolve and the excess settles out  Temperature is very important in the process of dissolving. Usually at high temperatures, more solute can dissolve. The EXCEPTION is gases. More gas particles can dissolve if the temperature is low.

14. States (Phases) of Matter  Kinetic Molecular Theory  All matter is composed of tiny, constantly moving particles.  The kinetic energy of these particles increases with more motion.  As kinetic energy (and motion) of particles increases, the temperature of the matter increases.

15. Solids  Have a definite shape  Have a definite volume  Have low Kinetic energy because the particles are packed so close together that they vibrate but don’t move around  Crystalline solids: particles are arranged in a repeating geometric pattern  Diamonds, sugar, salt  Amorphous solids: particles do not have a defined pattern  Wax, glass

16. Liquids  Have a definite volume  Measure using a graduated cylinder  DO NOT have a definite shape  Take the shape of the container that its in  Have more Kinetic energy than liquids because particles are not as closely spaced; the particles can move past each other but are still close

17. Gases  DO NOT have a definite shape  DO NOT have a definite volume  Have very high Kinetic energy  Particles are tiny and spread very far apart and move very fast.

18. Changes in State or Phase  Require the addition (endothermic) or removal (exothermic) of heat or energy  Kinetic energy is due to motion of particles. Potential energy is related to the space between particles. ChangeNameProcessKinetic Energy Potential Energy Solid to liquidMeltingEndothermicincreasesdecreases Liquid to solid FreezingExothermicDecreasesincreases Liquid to gas (vapor) at the boiling point VaporizationEndothermicIncreasesDecreases Gas to liquidCondensationExothermicDecreasesIncreases Solid to gas (vapor) SublimationExothermicIncreasesDecreases Gas to solid depositionEndothermicDecreasesIncreases Evaporation is also a liquid to gas change but the substance does not have to be boiling. **melting point = freezing Point temperature

19. Phase Changes Solid Liquid Gas Melting Vaporization CondensationFreezing

20. Liquid Sublimation Melting Vaporization Deposition Condensation Solid Freezing Gas

21. Water and Ice Ice Water and Steam Steam -20 0 20 40 60 80 100 120 0 40120 220760800 Heating Curve for Water Temperature is constant during a phase change! boiling melting

22. Vaporization versus Evaporation  Vaporization:  Substance must be heated to its boiling point  Takes place throughout the entire liquid  The attractive forces between molecules is very low.  Fast and vigorous process  Evaporation:  Substance does not have to be at its boiling temperature  Takes place at all temperatures  Slow process  Takes place only at the surface of the liquid  Depends on external factors such as surface area, wind, humidity, and temperature  https://www.youtube.com/watch?v=7zo10Yxicn1 https://www.youtube.com/watch?v=7zo10Yxicn1

23. Properties of matter  Physical property: a characteristic that can be observed about a sample of matter without changing the identity of the matter  Magnetism, density, color, shape, weight, volume, mass, phase or state  Physical properties can be used to separate mixtures of substances  Sand and water mixture can be separated by filtering through filter paper or strainer. The sand will be trapped by the filter paper and the water will flow through.  A mixture of sand and iron can be separated using a magnet because iron is magnetic and will be attracted to the magnet. Sand is not.  A mixture of salt and water can be separated by boiling the mixture. Water evaporates and the solid salt will be left behind.  A mixture of oil and water can be separated because oil and water have different densities and the oil will float on top of the water because it is less dense.

24.  Chemical property: characteristics of a substance that indicate how it will interact with other matter or undergo a specific chemical change  Flammability: will it ignite or burn  Reactivity: will it react with other substances  Lithium is highly reactive with water but not oil.  Helium is not flammable but oxygen is.

25. Physical Changes in Matter  Physical changes are changes in the form or phase of a substance but the identity is still the same  Properties remain the same  Physical changes are reversible; ice can be melted and liquid water results however the chemical makeup is still the same H2O  Physical properties can be used to separate mixture Examples: dissolving a substance in another one grinding something into smaller pieces cutting a piece of wood any phase or state change: melting, boiling, freezing, sublimation, condensation, deposition

26. Chemical changes in Matter  Chemical changes will change one substance into a completely different Ewith new chemical and physical properties  Cannot be reversed  Rusting, burning, tarnishing, decomposing, rotting, oxidizing  Can be recognized by the following signs:  Gas or bubbles are produced  Odor changes  Precipitate (a solid substance) forms usually when 2 liquids are combined  Energy change occurs (heat and/light produced, temperature changes (gets hotter or colder)  Color changes: something clear turns to another color; a color disappears; a color changes to a different color