1. Chapter Two Matter and Change

2. Properties of Matter Matter is anything that has a mass and takes up space Mass is the amount of matter an object contains Mass is different from weight because weight depends upon gravity. For example, mass on moon is same as earth, but weight is 1/6 of that on earth.

3. States of Matter Expansion on heating VolumeShape greatindefinite Gas moderatedefiniteindefiniteLiquid very slightdefinite Solid Liquid Gas

4. Plasma as a 4th state of matter In physics and chemistry, plasma (also called an ionized gas) is an energetic gas-phase state of matter in which some or all of the electrons in the outer atomic orbitals have become separated from the atom or molecule. The result is a collection of ions and electrons which are no longer bound to each other. This state of matter was first identified by Sir William Crookes in 1879, and dubbed "plasma" by Irving Langmuir.physicschemistrystate of matterelectronsatomic orbitalsatommoleculeionselectronsSir William Crookes1879Irving Langmuir Example: Fire, lightning, sun

5. States of Matter Solid- Matter with definite shape and volume. Coal,ice,iron, liquid-A form that flows, has a fixed volume, and takes the shape of its container. Water,milk,blood, Gas-Takes the shape and volume of its container. Air, carbon dioxide

6. Physical and Chemical Properties A physical property is a quality or condition of a substance that can be observed without changing the substance’s composition. –Intensive: depends upon internal make-up. –Size is not a factor: Example: color –Extensive: depends upon the amount of the substance…external Example: length, mass

7. Chemical Property Chemical property: describes how a substance reacts. Example: rusting, burning

8. An egg is cracked but hasn’t changed it’s composition. Food coloring is mixed with water, it dissolved, this is an example of a physical change. Ice melts and turns solid to liquid. Water boils and turns liquid to gas. Physical Change- alters a given material without changing it’s composition.

9. Chemical Changes A new substance is created. Example: Paper burns into ash

10. Matter, Compounds, and Elements

11. Elements and Compounds Elements are the simplest forms of matter that can exist under normal lab conditions. Compounds are substances that can be separated into simpler substances only by chemical means.

12. Mixture- a physical blend of two or more substances. Heterogeneous- one that is not uniform in composition, different throughout Homogeneous- one that is completely uniform in composition, the same throughout. Heterogeneous Homogeneous

13. Classifying Mixtures A mixture is a physical blend of two or more substances. Heterogeneous-A mixture not uniform in composition Homogeneous-A mixture completely uniform in composition Solution-Any gases, liquids,or solids.

14. Separating mixtures Distillation is when a liquid is boiled to produce a vapor and then condensed to form a liquid. This separates the water from what is dissolved in it.

15. Symbols and Formulas Chemical symbol-A one or two letter symbol representing the element’s name. Sodium-Na Potassium-K Gold-Au Tin-Sn

16. Changing Reactants to Products Chemical reaction- One or more substances change into new substances. Reactants-The starting substances in a chemical reaction Products-Substances formed in a chemical reaction Chemical property- The ability of a substance to undergo a chemical reaction and to form new substances.

17. Conservation of Mass Law of conservation of mass-In a chemical reaction or physical change the mass of the reactants stays constant with the mass of the products.

18. Universe Classified Matter is the part of the universe that has mass and volume Energy is the part of the universe that has the ability to do work Chemistry is the study of matter –The properties of different types of matter –The way matter behaves when influenced by other matter and/or energy

19. Classification of Matter Three States(Phases) of Matter: Solid (s)Liquid (l) Gas (g)Three States(Phases) of Matter: Solid (s)Liquid (l) Gas (g)

20. States(Phases) of Matter

21. Gas (Vapor) Liquid Solid (Crystal) Vaporization (Evaporization) Fusion (Melting) Condensation Crystallization (freezing) Solid to Gas Sublimation EnergyEnergy Low High

22. Properties Characteristics of the substance under observation Properties can be either ¬directly observable or ­the manner something interacts with other substances in the universe

23. Properties of Matter Physical Properties: Characteristics of substances that change without the substance becoming a different substance. Examples: Melting Point, Boiling Point, Density, Structure, Odor, Volume, Phase of Matter, Color, volatility

24. Properties of Matter Chemical Properties: The ability of substances to change into a different substance. Examples: Reactivity, Flammability, polarity

25. Changes of Matter Physical Changes: A change in the arrangement of the molecules in matter. Does not result in new matter forming. Examples: Melting, Boiling, Freezing, Condensing, Grinding, Dissolving, Crumbling, Tearing, Mixing

26. Changes in Matter Chemical Changes: A change in which the atoms rearrange and form new substances. Examples: tarnishing, burning, rusting, fermenting, producing, decomposing, reacting, cooking, spoiling

27. Classify Each of the following as Physical or Chemical Properties ¬The boiling point of ethyl alcohol is 78°C. –Physical property – describes inherent characteristic of alcohol – boiling point ­Diamond is very hard. –Physical property – describes inherent characteristic of diamond – hardness ®Sugar ferments to form ethyl alcohol. –Chemical property – describes behavior of sugar – forming a new substance (ethyl alcohol)

28. Matter Elements Pure SubstancesMixtures CompoundsHomogeneous (Solutions) Heterogeneous Physically combined Chemically Combined

29. Classification of Matter Pure Substances: Matter that has the same composition throughout. Mixtures: Matter that has varying composition.

30. Pure Substances Element: A substance that cannot be decomposed into simpler substances by chemical means. Element: A substance that cannot be decomposed into simpler substances by chemical means. Compound: A substance with a constant composition that can be broken down into elements by chemical processes.

31. Types of Mixtures A homogeneous mixtureA homogeneous mixture Also known as a solution.Also known as a solution. The components are in the same phase, (s,l,g) throughoutThe components are in the same phase, (s,l,g) throughout Example: salt water, vinegar, coffee, air, alloys of metalsExample: salt water, vinegar, coffee, air, alloys of metals

32. Types of Mixtures A heterogeneous mixtureA heterogeneous mixture non-uniform, contains regions with different properties than other regions Examples: a bottle of ranch dressing, blood, soil, oil/vinegar Examples: a bottle of ranch dressing, blood, soil, oil/vinegar

33. Separation of Mixtures Can be isolated by separation methods that utilize varying physical properties.Can be isolated by separation methods that utilize varying physical properties. -  Chromatography -  Chromatography Uses differences in the ability of a compound to move through a substance.Uses differences in the ability of a compound to move through a substance. - Filtration - Filtration Uses differences in the size of substancesUses differences in the size of substances - Distillation - Distillation Uses differences in the temperature substances evaporate..Uses differences in the temperature substances evaporate..

34. Distillation Apparatus