1. anything that occupies space and has mass. Macroscopic Microscopic Particulate

2. Color of a liquid Flammability ofalcohol Odorof a gas Density of gold Reactivity with HCl Melting point of sulfur Boiling point of water Volumeof a metal Hardness of diamond sphere 3. Can be determined without changing the nature of the substance (color, odor, physical state, density, hardness, melting point and boiling point) 4. Describes the ability of a substance to participate in chemical reactions (reactivity with oxygen, reactivity with acids, flammability) 5. Donot depend o the amount of the sample being examined Depend on the quantity of the sample 6. Odor Hardness Color Volume Weight Area Mass Thickness Density Freezing point 7. Has definite shape and definite volume Rigid Molecules are held tightly together Molecules can wiggle or vibrate only very slightly 8. Distinct volume independent of its container No specific shape Molecules slide over each other Pours easily 9. No fixed volume or shape Moleculesare very far apart and are moving at high speeds Moleculescolliding repeatedly with each other and with the walls of the container 10. Copper 11. Nitrogen 12. Highly ionized state positively charged ions Free negatively charged electrons 99%of the matter in the universe 13. BOSE-EINSTEIN CONDENSATE (BEC) Predicted in 1924 by Albert Einstein, whobuilt on the work of Styendra Bose Condensationoccurs when individual atoms meld into a superatom behaving as a single entity at just a few hundred billionths of a degree above absolute zero 14. Chemical Initial state Final state Physical or System ChemicalChange? 15. PHYSICAL Change Changesthat alter the physical form of matter without changing its chemical identity. ALL changes of state are physical changes 16. CHEMICAL Change Occurswhen the chemical identity of a substance is destroyed and a new substance is formed. Chemical reactions 17. Indicators of Chemical change/reaction Color changes Odor changes Production of gas Production of solid or precipitate 18. Physical and Chemical Changes and Properties Chemical PhysicalChanges Old substances New form of olddestroyedsubstanceNew substances No new substanceformed formedPropertiesProperties defined Description byby types ofsenseschemical changespossible Measurable properties 19. ENDOTHERMIC Process The system absorbs heatSURROUNDINGSHEAT SYSTEM Melting of ice 20. EXOTHERMIC Process The system evolves heatSYSTEMHEAT SURROUNDINGS 21. Combustion Freezingof water Melting of ice Boiling of water Condensing steam 22. Hasits own set of chemical and physicalproperties Cannot be separated into parts by physicalmeans Has a definite, fixed composition that doesnot vary from one sample to another 23. Consists of two or more chemicals Properties depend on the substances on it Compositions can vary 24. Definedby its atomic number Cannot be decomposed into simplersubstancesAtomic Number - the numberof protons in an unreactedatomMass Number - the number ofprotons and neutrons together 25. Hydrogen H63.0%Oxygen O25.5%Carbon C9.45%Nitrogen N1.35%CalciumCaPhosphorus PChlorine ClSulfur S0.7%Sodium NaPotassiumKMagnesiumMg 26. asubstance made of more than one typeof atom Composed of 2 or more elements Atoms combined in fixed proportions Can be decomposed into two or moreother substances by chemical change 27. Turnblue litmus to red React with many metals React with bases 28. An acid can be defined as a substancethat yields hydrogen ions (H+) whendissolved in water. HCl Pure substance, hydrogen chloride Dissolved in water (H+ Cl-), hydrochloric acid Anoxoacid is an acid that contains hydrogen, oxygen, and another element. 29. Cause color changes in plant dyes. React with certain metals to producehydrogen gas.2HCl (aq) + Mg (s)MgCl2 (aq) + H2 (g) Reactwith carbonates and bicarbonates to produce carbon dioxide gas2HCl (aq) + CaCO3 (s)CaCl2 (aq) + CO2 (g) + H2O (l) Aqueousacid solutions conduct electricity. 30. pH A Measure of Acidity 31. Turnred litmus to blue React with acids 32. A base can be defined as a substance that yields hydroxide ions (OH-) when dissolved in water. NaOH sodium hydroxide KOHpotassium hydroxide Ba(OH)2barium hydroxide 33. A salt, is defined as the product formedfrom the neutralization reaction of acidsand bases. Salts are ionic compoundscomposed of cations (positively chargedions) and anions (negative ions) so thatthe product is electrically neutral (without anet charge) 34. acid + basesalt + waterHCl (aq) + NaOH (aq) NaCl (aq) + H2OH+ + Cl- + Na+ + OH- Na+ + Cl- + H2O H+ + OH-H2O 4.3 35. Wala akong bosesKaya please, konting katahimikan at pag- itindi ang aking hiling Salamat,Maam Pie 36. 1. Identify the physical state of the following: a) Helium in a toy balloon b) vitamin tablets in a bottle c) mercury in a thermometer 37. 2. Identify the type of property in thefollowing statements:a. Yellow-green chlorine gas attacks silvery sodium metal to form white crystals of sodium chloride.b. A magnet separates the mixture of black iron shavings and white sand. 38. 3. State which type of change occurs in thefollowing statements:a. Passing an electric current through molten magnesium chloride yields molten magnesium and gaseous chlorine.b. The iron in discarded automobiles forms reddish brown, crumbly rust. 39. c. Chopping a logd. Burning a loge. Toasting a slice of bread 40. 4. What is the key difference between anelement and a compound?5. List two differences between a compoundand a mixture.6. Make a concept of the Classification ofMatter. 41. HETEROGENEOUS Varies in composition and or propertiesfrom one part of the mixture to anotherHOMOGENEOUS Has the same/uniform composition andproperties throughout 42. Kind of mixture Particle size Examples Characteristics 43. SUSPENSION >1000 nm Particles are more orless evenly dispersedthroughout a liquid orgas Different partsseparate over time 44. SOLUTION 0.2-2.0 nm A homogeneous mixture of two or moresubstances uniformly dispersed throughouta single phase 45. GasLiquidSolidGasOxygen and The odor of a other gases in Water vapor insolid -- nitrogen (air) air (humidity)molecules ofthat solid beingdissolved in theairLiquid Carbon dioxide Ethanol Sucrose (table in water (common sugar) in water; (carbonatedalcohol) in sodium chloride water) water; various(table salt) inhydrocarbons in watereach other(petroleum) *SolidHydrogen Water inSteel, Brass, dissolved to activated other metal palladiumcharcoalalloys 46. COLLOID 2.0-1000 nm Consists of tiny particles that aresuspended in a liquid, solid, or gas Stable heterogeneous mixtures Exhibits Tyndall effect 47. Decantation separates liquids from solids that have settled Evaporation Separates the solid (residue) from the liquid (filtrate) parts of the mixture 48. Distillation 49. Filtration 50. Centrifugation 51. Chromatography 52. Sugardissolved in water Mixture of ethyl alcohol and water Mixture of salt and sand Iron filings, mongo seeds and salt mixture