1. Matter and Change Chapter 2

2. Definitions Matter –Anything that has ____ and takes up _____ Volume –Space the object ______ What would you use to determine the volume of… –Book? Air? Water? Mass –______ of matter contained in an object. What do we use in lab to determine mass?

3. Mass vs. Weight Are they the same?????? Big difference… –Weight depends on the location in the ______. It will change, mass does not change no matter the location. Weight is defined as –The force produced by ______ acting on mass

4. Solid Liquid Gas

5. Phase Changes Solid Liquid Gas

6. What makes up matter All matter is composed of about 118 different kinds of ________s. Atom –Smallest unit of an element that maintains the properties of that element.

7. Pure Substance single element or compound that has definite chemical & physical properties Element –Contains only ____ type of atom –Can not be broken down by chemical means or physical means Compound –Made up of atoms of two or more elements joined by a _____bond –Can be broken down by chemical means, cannot be broken down by physical means

8. Elements exist as: Single atoms –Example: He in balloon (monatomic gas) Molecules –____ or more atoms combine in a definite ratio. Examples Br 2, I 2, N 2, Cl 2, H 2, O 2, F 2 -all diatomic molecules

9. Allotrope One of a number of different molecular forms of an element. –Examples O 2 is oxygen O 3 is ozone Carbon you know as _________ and __________

10. Compounds Are represented by formulas. Molecular formulas –Tells only what makes up a compound Structural formulas –Shows how the atoms are connected

11. Mixture vs. Pure Substance A pure substance has only ____ kind of element or ____________. Where as a mixture has more than one kind of ______ or compound.

12. Mixtures vs. Compound Mixture ____ chemically joined Reflect the properties of the substances it contains Mixture’s components can vary in proportions Compound Chemically joined Has properties different from elements that make it up Has a ____________ composition

13. Types of Mixtures Homogeneous Mixtures Mixtures in which the composition is uniform throughout. (i.e. the phases cannot be distinguished.) Heterogeneous Mixtures Mixtures in which the composition is not uniform throughout. (i.e. the phases can be distinguished.) Called a _________________!!! Known as a _______________!!!

14. Separation of Matter Elements: Can only be broken down by _________________ reactions. Compounds: Can only be broken down by __________________ reactions. Mixtures (hetero) and Solutions (homogeneous): Can be broken down by ______________________ means.

15. Physical Means of Separation Filtration: Separates mixtures by particle size. Used to separate solids from liquids

16. Physical Means of Separation Distillation: Separates liquid mixtures by differences in boiling point. http://www.dit.ie/DIT/science/chemistry/rsccomp/competition00/distillation/labdistillation.JPG Txtbk p34

19. Physical Means of Separation Chromatography: A broad range of physical methods used to separate and or to analyze complex mixtures by their attraction to a liquid or solid. There are three types of chromatography we will be discussing: Paper Gas Column

20. Physical Means of Separation Paper chromatography: Substances are distributed between a stationary phase and a mobile phase. The stationary phase is usually a piece of high quality filter paper. The mobile phase is a solution that travels up the stationary phase. Components of the sample will separate readily according to how strongly they adsorb on the stationary phase versus how readily they dissolve in the mobile phase. http://liston.50megs.com/chromatography.jpg

21. Matter Flowchart MATTER Can it be separated by physical means? yesno Can it be separated by chemical means? noyes Is the composition uniform? noyes p38 textbook

22. Matter Flowchart MATTER Can it be separated by physical means? Homogeneous Mixture (solution) Heterogeneous MixtureCompounds Elements MIXTUREPURE SUBSTANCE yesno Can it be decomposed by chemical means? noyes Is the composition uniform? noyes p38 textbook

23. Matter Flowchart MATTER Homogeneous Mixture (solution) Heterogeneous Mixture CompoundsElements MIXTUREPURE SUBSTANCE Contains 2 or more types of matter Contains only one type of matter Another way to think about it Does not look the same throughout Has a uniform appearance Contains only one kind of atom Contains 2 or more different kinds of atoms

25. Words to know and use Mixture Pure substance Element/Atom Compound/Molecule Homogeneous (solution) Heterogeneous (mixture) Allotrope Alloy Filtration Distillation

26. What is wrong with the phrase… –“heterogeneous compound” –“pure mixture” –“pure tap water”

27. Properties of Matter (How we describe matter) Physical –Can be determined without ______ the nature of the substance. –Examples: Density, hardness, color Chemical –Describes a substance’s ______ to participate in a chemical reaction. –Ability to change –Examples: Reactivity, Stability, Flammability Reactivity with oxygen, decomposes with light

28. Types of Physical Properties Extensive- depends on the _____ of matter Ex: volume, mass, amount of energy Intensive- _____ _____ depend on the amount Ex: density, boiling point, ability to conduct

29. Properties Flowchart Properties Does the substance need to be changed to observe the property extensiveintensive yesno Does the property change when the amount changes? noyes PhysicalChemical

30. Changes of Matter Physical Change –Identity (or chemical makeup) of a substance does not change, however the ________, ______ and ______ of particles may change. –Examples: Crushing Ripping Bending Phase changes

31. Phase Changes Solid Liquid Gas

32. Changes of Matter Chemical Change –Identities of substances changes and ____ substances form. Examples: –______

33. 5 Indicators of a Chemical Change: Evolution of a gas Odor change Production of heat/light Color change Formation of a precipitate

35. Reactions A reaction has –Reactant (left side) What ________ in the reaction –Product (right side) What is ______ Example of a chemical: Burning Dollar CH 3 OH + O 2  CO 2 + H 2 O –Law of Conservation of Mass Mass is neither created nor destroyed in a chemical reaction –Almost true