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Unit 2 Chemistry and Matter.

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Presentation on theme: "Unit 2 Chemistry and Matter."— Presentation transcript:

1 Unit 2 Chemistry and Matter

2 Chemistry The study of matter and energy and the changes that they go through. Matter is anything that has mass and takes up space

3 Mass vs. Weight Mass – the measurement of the amount of matter
Mass vs Position Weight vs Position

4 Law of Conservation of Mass
Matter can not created nor destroyed only converted from one form to another.

5 OOBLECK Challenge!!! Write down in your lab notebook and predict if this material is a SOLID, LIQUID, or GAS? Write an observation or proof why you chose solid, liquid, or gas. (Defend your choice) Videos:

6 States of Matter Volume, Shape, Compression, Effects of Heating?
Solid – (add a particle picture) Definite Volume Definite shape Not compressible Expands Liquid – (add a particle picture) No Definite shape

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9 Gases – (add a particle picture)
No Definite Volume No Definite shape Compressible Vapor – A substance that is liquid at room temperature. (Examples: Water, Mercury)

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11 Fig. 1-7, p. 10

12 Plasma – High temperature physical state of matter in which atoms lose their electrons
Fluorescent Light Bulbs The Sun and other Stars

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15 Phase Change Diagram

16 Properties of Matter Physical Properties – characteristics you can describe any substance of matter Color Temperature Melting Point Boiling Point Density Malleability/Ductile

17 Properties cont… Chemical Properties – ability of a substance to combine with or change into one or more NEW substances. Iron rusting Copper turning green when exposed to air (rusting) Sodium reacting in the presence of water Gasoline burning Sulfur burning bright blue when in the presence of oxygen

18 Explore: Graphing Liquids Activity

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20 Intensive vs. Extensive Properties
Intensive property: properties that DO NOT depend on the amount of matter present Extensive property: properties that DO depend on the amount of matter present Melting/Freezing Point Mass Boiling Point Weight Luster - shiny Volume Malleability – flatten into thin sheets Length Ductility - drawn into thin wires Density

21 Viscosity: is a fluids resistance to flow
Buoyancy: Upward force that keeps things afloat

22 Changes in Matter Physical Change – Changing the state or shape that matter is in, without changing the matter itself. Examples Boiling water/Freezing water Cutting a Piece of paper Cracking open an egg Melting gold

23 Changes cont… Chemical Change – process by which one or two substances combine to form a NEW substance Examples: Burning wood to form Carbon, Carbon Dioxide, and water. Combining gaseous Hydrogen and Oxygen to form water. Reacting Iron and Oxygen to form Rust.

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25 Mixture Combination of two or more substances in which each substance retains its individual properties Combined with out exact ratios Salt in water Sand in Water Granite/Marble Dirt Salad Dressing

26 Types of Mixtures Homogenous – mixture is uniform in composition. (Homo – Same, Gene – Form) Salt dissolved in water. Coffee with sugar. Heterogeneous – mixture has a different composition throughout (Hetero – Different, Gene – Form) Ice in water Dirt (Rocks, Sand, Dirt, Roots, Worms, Bugs)

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35 Exercise 11, p. 41

36 Substances Pure substance: matter that is uniform and unchanging in its composition (exact ratios every time) Table Salt is always NaCl Water is always H2O

37 Pure Substances Element – A pure substance that can not be broken into smaller substances Examples: Copper, Oxygen, Gold. Compound – The combination of two or more different elements that are combined in the same ratios every time

38 Evidence of a Chemical Change
***We will investigate this in a Lab*** Change in ______________ Production of a _____________ Formation of a ______________ Detection of a _____________

39 Separating Mixtures Distillation – Separates materials based upon different boiling points.

40 Filtration – Where a barrier is used to separate solid material from liquid material

41 Chromatography – Separates the components of a mixture by traveling across a surface at different rates

42 Crystallization – produces a pure solid particles from a dissolved solid


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