1. Classification of Matter SWBAT classify matter based off its characteristics.

2. Matter Anything that has mass and takes up space.

3. States of Matter http://www.reptox.csst.qc.ca/Documents/SIMDUT/GuideAng/Images/P07EtatP hys.gif

4. Plasma A Fourth State Of Matter Plasmas are the most common state of matter in the universe. All stars are composed of plasma. The charged air produced by lightning is a plasma.

5. Plasma A Fourth State Of Matter Heating a gas gives electrons enough energy to dissociate from the nucleus, resulting in the presence of free electrons and ions. Because the electrons are no longer bound to the nuclei, they move freely through the plasma. This makes plasmas highly conductive – a unique property that makes them a different state of matter.

6. Pure Substance Consists of one chemically distinct material – could be an element or a compound Every sample of a particular substance has the same set of properties. It cannot be separated by physical means. Example: A bag of sugar is a pure substance. Every sample you take out of the bag consists of only sucrose (C 12 H 22 O 11 )

7. Elements Made up of one type of atom. Cannot be chemically broken down. Have a symbol on the periodic table.

8. Metals- React by losing electrons Nonmetals- React by gaining or sharing electrons

9. Compounds Two or more elements chemically combined. The elements do not retain their own properties when they form compounds. Examples: NaCl, H 2 O, CH 4

10. Types of compounds Ionic compounds Electrons are transferred Metals and nonmetals Covalent compounds Electrons are shared Nonmetals

11. Mixtures Two or more substances physically combined. Substances retain their own properties. Composition can vary from one mixture to another. Example: sweet tea

12. Homogeneous Mixture Has a uniform composition throughout the mixture Also called a “solution” A solution can be: – Liquid, like sweet tea – Gas, like air (O 2, CO 2, N 2 and other gases) – Solid, like stainless steel (iron, chromium, and nickel)

13. Solutions (Homogeneous mixtures) Solvent – Substance doing the dissolving. Usually present in larger quantities. Solute – particles dissolved in a solution http://www.spacesciencegroup.org/sootw/Default.asp?Theme=mixtures&pagename=unsaturated A solvent dissolves the solute. The solute becomes dispersed in the solvent. Solvents and solutes can be solid, liquid, or gas

14. Heterogeneous Mixture Not uniform. Areas of distinctly different composition. Examples: http://www.medlaunches.com/entry-images/1206/25/chocolate-chip-cookies-480.jpg

16. Questions to ask yourself! 1.Does it have areas of different composition? YES – it is a heterogeneous mixture 2.Does it have a symbol on the periodic table? YES – it is an element. 3.Does it have a chemical formula? YES – it is a compound. 4.Is it made of two or more substances? YES – it is a solution

17. Properties are used to describe and identify a substance. Two types: 1. Physical properties: Properties describing a substance that can be observed without changing the substance’s composition – melting point, freezing point, malleability 2. Chemical properties: Properties that describe how a substance undergoes a change – rusting, burning, decomposing

18. Physical properties Extensive: Depend on the amount of substance present. Examples: mass, volume Intensive: Characteristic of the substance itself. Do not depend on the amount. Examples: hardness, color, density

19. Physical vs Chemical Changes in Matter In a physical change, the original substance still exists. It has just changed form. Some properties change, but the composition of the substance is the same. Boiling, freezing, melting, and condensing are used to describe physical changes. These are reversible physical change. Grinding, breaking, crushing, and cutting also describe physical changes, but these are not reversible.

20. Physical vs Chemical Changes in Matter During a chemical change, the composition of matter changes. Bonds are broken and new bonds are formed. Chemical changes occur when a substance undergoes a chemical reaction. Example: rusting Fe + O 2 → Fe 2 O 3 What are the signs that a chemical change (reaction) has taken place?

21. Separation of Mixtures Differences in physical properties can be used to separate mixtures. Some mixtures can be separated based on chemical properties as well.

22. Filtration Method for separating a solid from a liquid. Uses holes in filter paper to separate parts of a mixture based on size of particles (think of using a strainer on beach sand, the larger sand crystals stay in the strainer)

23. Distillation: Method for separating or purifying liquids based on boiling point. Uses the different boiling points of substances in a mixture to separate them We distill alcohol because the alcohol has a lower boiling point than water – it boils off first and we can re-condense it in a purer form.

24. Chromatography Method for separating components of a mixture The components are separated based on their attraction between two phases: a stationary phase bed and a mobile phase which percolates through the stationary bed. The phases may be liquid, solid, or gas (there are many types of chromatography!)