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Matter chapter 3 Slide 2 Matter massspace anything that has mass & occupies space mass: gramskilograms mass: measured in grams or kilograms volumeliterscm 3 space/volume: measured in liters or cm 3 Slide 3 Phases SOLIDS LIQUIDS GASES Slide 4 solid: solid: definite volume definite shape Slide 5 liquid 0 definite volume indefinite shape takes the shape of container Slide 6 gas indefinite volume indefinite shape takes the shape & volume of container Slide 7 States of Matter 1.How are the particles packed in each phase? 2.How do the particles move in each phase? 3.Why do liquids and gases flow? 4.Why are gases so easy to compress? Slide 8 4 th phase of matter plasmaplasma exists in stars, lightning bolts e lectrons are stripped from atoms Slide 9 Physical Properties describe appearance & form of matter descriptive words: color, texture, luster, odor solid, liquid, gasmeasurements: a number and a unit Slide 10 Intensive Properties physical constants independent independent of sample size amount doesnt matter density, freezing/melting points, and boiling point solubility in water (g/ml) Slide 11 Extensive Properties extensive properties:extensive properties: depend on sample size: amount) mattersquantity (amount) matters mmass & volume Slide 12 Chemical Properties describe how matter: behaves in presence of other matter changes into another kind of matter examples: flammability resistance to corrosion ability to neutralize acids or bases Slide 13 Properties of Copper physical prop: reddish brown shiny malleable ductile good conductor density = 8.92 g/cm 3 mp = 1085 C bp = 2570 C chemical prop: reacts to form green copper carbonate forms deep blue solution when in contact with NH 3 forms new substances with HNO 3 Slide 14 Physical Change identityform or appearance of matter may change but identity remains same phase changes dissolving crushing, grinding cutting tearing Slide 15 Dissolving dissolving is physical change: think of putting sugar in water still have sugar sugar molecules just spread out between water molecules C 6 H 12 O 6 (s) C 6 H 12 O 6 (aq) Slide 16 Phase Changes phase changes are physical changes no new substance is created (chemical formula stays the same) ex: ice melting: H 2 O(s) H 2 O(l) water boiling: H 2 O (l) H 2 O(g) Slide 17 Chemical Change chemical change - identity of matter is changed new substance with own unique properties is formed chemical formula changes Slide 18 Burning oxidation reactioncommon name for oxidation reaction indicates matter reacting with oxygen chemical change: original substance changed into new kind(s) of matter ex: CH 4 (g) + 2O 2 (g) CO 2 (g) + 2H 2 O(g) Slide 19 Evidence of Chemical Change 1.bubbling [formation of a gas] Slide 20 2. color change Slide 21 3. heat absorbed/released Slide 22 4. light produced Slide 23 5. formation of a solid 2 liquids mix and solid is formed - this is a precipitate (ppt) Slide 24 What kinds of matter are there? Slide 25 Matter SubstancesMixtures Elements Compounds Heterogeneous Mixtures Homogeneous Mixtures mixtures separated by physical methods compounds separated by chemical methods Slide 26 Element substance that: cannot be broken down (decomposed) into simpler substance only 1 kind of atom has definite properties formulas have 1 uppercase letter K Br Slide 27 Element Song Slide 28 Atom smallest particle of element that retains properties of element smallest particles of element that can undergo a chemical reaction represented by SINGLE symbol Cu Co Ag Au Slide 29 Compounds 2 or more DIFFERENT elements chemically combined in a definite ratio homogeneous in composition formulas have 2 or more symbols CO 2 MgO H 2 O Slide 30 Compounds different properties of compound are different from properties of elements formed from ex: sodium chloride (table salt) is created from sodium metal and chlorine gas 2Na(s) + Cl 2 (g) 2NaCl(s) Slide 31 Compounds can be separated into elements by chemical decomposition reaction ex: 2H 2 O(l) 2H 2 (g) + O 2 (g) Slide 32 Mixtures combo of 2 or more pure substances NOTphysically combined NOT chemically combined physically can be separated each substance retains its own identity and properties Slide 33 Mixtures variable composition no unique properties (think of sugar and salt mixed together) may be homogeneous or heterogeneous Slide 34 Types of Mixtures Slide 35 homogeneous: uniform composition throughout single phase ex: solutions (all 3 phases) Slide 36 heterogeneous: see a boundary or regions that look different ex: ice water, granite, suspensions, colloids Slide 37 Slide 38 Suspensions particles in suspensions are larger than those in solutions components of suspension can be evenly distributed by mechanical means (shaking the contents) but components will settle out Slide 39 Colloids homogeneous combination of molecules mixed through another substance that will not settle out or join with the other substance made up of very small, insoluble particles that remain in suspension in a surrounding solid, liquid, or gas medium of different matter can be solid, liquid, or gas Slide 40 Colloid subtypes Slide 41 Aerosols: solid or liquid particles in gas smoke: solid in a gas fog: liquid in a gas Slide 42 Foams: substance where air or gas bubbles are trapped inside a solid or liquid Styrofoam: air in solid whipped cream: air in liquid Slide 43 Sols: solid particles in a liquid ex: milk of magnesia (solid MgOH in water) Slide 44 Emulsions: liquid particles in liquid milk: fat in water mayonnaise: oil in water Slide 45 Gels: liquids in solid ex: jello: protein in water quicksand: sand in water Slide 46 Hints to distinguish homogeneous from heterogeneous mixtures: Slide 47 Homogeneous Mixtures solutions in gas & liquid phases transmit light particles not big enough to scatter light look translucent Slide 48 Heterogeneous Mixtures suspensions look cloudy particles big enough to scatter light settle on standing Slide 49 Separating Mixtures mixtures are PHYSICALLY combined separation based on physical properties Slide 50 Sorting: based on size & appearance of particles Slide 51 Filtration: solid in liquid liquid goes through filter paper but solid stays behind Slide 52 Distillation: liquids mixed together but have with different boiling points Slide 53 crystallization: solubility of solid in liquid Slide 54 Magnets: separate magnetic metals from non-magnetic substances Slide 55 chromatography: variable solubility of mixed liquids (travel ability) Slide 56 Conservation of Mass mass begin with = mass end up with # of atoms before = # of atoms after 10 Hs as reactants = 10 Hs as products Slide 57 Particle Diagrams atoms of a monatomic element (single same atoms) molecules of a diatomic element (double same atoms) Slide 58 Particle Diagrams molecules of a triatomic compound mixture: - monatomic element - diatomic element - triatomic compound