Matter. Matter is anything that takes up space and has mass.

Transcription

1 Matter Matter is anything that takes up space and has mass.

2 States of Matter Matter exists in three states: O Solid O Examples: rock, wood, chalk O Liquid O Examples: water, milk O Gas O Examples: oxygen, carbon dioxide

3 OSolids Properties of Matter O Have definite shape and volume O Particles are tightly packed O Particles can only vibrate O Incompressible

4 OLiquids Properties of Matter O Has a constant volume, shape can change O Takes the shape of the container O Particles move against each other (flow) O Very slightly compressible

5 Properties of Matter OGases (in gas form at room temp) O Completely fill the container O Particles are in constant, random motion O Particles are very far apart O Highly compressible

6 Particle Representation of Matter Which one has the most energy? The least energy?

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8 Phase Changes of Matter

9 Properties of Matter O Intensive properties are independent of amount of substance present. ex: color, smell, hardness, MP, BP, density, texture O Extensive properties depend on amount of substance. ex: mass, length, volume

10 Properties of Matter O Physical properties can be observed or measured without changing the chemical composition of substance. ex: odor, density, hardness, MP, BP, physical state, magnetism, compressibility

11 Properties of Matter O Chemical properties tell the ability of the substance to undergo reaction or not undergo reaction Ex: sodium will react with water

12 Changes of Matter O Physical changes occurs without changing chemical composition of substance Ex: melting, boiling, freezing, condensing, subliming, depositing, cutting, compressing

13 Changes of Matter O Chemical changes cause a substance(s) to form. Also called chemical reaction. Ex: rusting, corroding, fermenting, decomposing, reacting, photosynthesis, combustion (burning)

14 Types of Matter O Pure substance has uniform consistency throughout. ex. elements & compounds O Elements can t be separated into simpler substances by chemical or physical means. Contains 1 type of atom. O Compounds can be broken down by chemical means. Has 2 or more different types of atoms.

15 Types of Matter O Mixtures contain 2 or more different pure substances. O Homogeneous mixtures have constant composition throughout. 1 phase. Also called solutions. ex: butter, smooth peanut butter O Heterogeneous mixtures do not have constant composition throughout. More than 1 phase. ex: chunky peanut butter

16 Matter Flowchart

17 Definitions O Reactants are the substances present at the beginning of a chemical reaction. O Products are the substances present at the end of a chemical reaction. Ex: Sodium and chlorine react to form sodium chloride. Sodium, chlorine are reactants. Sodium chloride is product.

18 Evidence of Chemical Change O Color change O Formation of odor (smell) O Bubbles (formation of gas) O Solid (precipitate) formation O Temperature change (gets hot or cold)

19 Definitions O Endothermic reaction. The reaction gets cold; heat flows into the reaction. O Exothermic reaction. The reaction gets hot; heat flows out of the reaction. (fire)

20 The Law of Conservation of Mass or Matter O During a chemical reaction, matter is neither created nor destroyed. Mass of reactants = Mass of products Ex: When 48.6 g magnesium reacts with 32.0 g oxygen, how much magnesium oxide forms?

21 The Law of Definite Proportions O A compound is always composed of the same elements in the same proportion by mass. O % by mass = mass of element X 100 mass of compound

22 The Law of Definite Proportions O Example: A compound contains g carbon and g oxygen. What are the % by mass of each element?

23 Percent Error O Sometimes in chemistry we don t get the maximum or expected result. This can be due to many factors. Percent error indicates the accuracy of a measurement or calculation.

24 % Error = Percent Error experimental value actual value actual value x 100 your value from a literature source or given

25 Percent Error Example: An object has an actual mass of 35.0 g. Toni massed the object at 34.0 g. Calculate her percent error.

26 The Law of Multiple Proportions O When elements combine, they do so in a ratio of small whole numbers. O For example, carbon & oxygen react to form CO and CO 2, but not CO 1.3.

27 Separating Mixtures O Mixtures contain pure substances that can be separated based on their physical properties (solubility, BP, MP)

28 Filtration O Heterogeneous mixtures of solids & liquids can be separated by filtration.

29 Distillation O Homogeneous liquid mixtures can be separated by distillation which separates based on boiling point.

30 Crystallization O Separates solids from supersaturated solution.

31 Sublimation O Can be used to separate two solids from a mixture in which one substance sublimes.

32 Chromatography O Is used to separate compounds that have been dissolved in liquid or gas. Paper chromatography is shown below.