Unit 2: Study of Matter

1. Unit 2: Study of Matter You may already know why ice floats. Ironically, if the ice was “dry,” it would sink. What explains that?

2. Unit 2 Objectives • Definitions: matter, element, compound, mixture, (chemical) symbol, heterogeneous, homogeneous, metal, nonmetal, metalloid, physical change, chemical change, nuclear change, Laws of conservation, exothermic, endothermic, Kinetic Molecular Theory, real gas, ‘ideal’ gas, change of state, phase diagram, triple point, critical point. • Differentiate between elements, compounds, and mixtures. • Arrange a matter hierarchy. • Identify chemical symbols for elements. • Separate mixtures physically. • Differentiate between hetero- and homogeneous mixtures. • Sepearate metallic, nonmetallic, and metalloid elements. • Determine the physical and chemical properties of a substance. • Distinguish chemical and physical properties from chemical and physical changes. • Perform calculations using the Law of Definite Composition.

3. Unit 2 Objectives Pt.2 • The Kinetic Molecular Theory (KMT) is based on the idea that particles in matter are always in motion. • The KMT can be applied to describe properties of solids, liquids, and gases. • Boiling, metling, freezing are among the physical processes that can alter a substances state. • How to interpret a phase diagram. • Identify the triple point and critical point. • (EFS D4) To use systems thinking and systems tools to identify patterns, impacts, and relationships between a product’s life cycle and the health of the system as a whole. Embed their understanding of the Materials cycle principle in their work. • (EFS D5) Articulate how human choices regarding consumption, production, distribution, and disposal of material goods affect our ability to thrive over time.

4. Essential Questions • How do the types of substances – elements and compounds – differ? • How do the states of matter differ according to the Kinetic Molecular Theory? • GUIDING QUESTIONS: • What are the characteristics of elements and compounds? • Why can’t a compound be separated by physical means? • What are the different categories of elements? • How do the properties of the general types of elements compare? • What are the characteristics of mixtures? • What physical means are used to separate mixtures? • What are the distinctions between matter and energy? • Why are chemical and physical properties important? • What is the importance of the Laws of Conservation of Matter and Energy and Definite Composition? • How are physical, chemical, and nuclear changes distinguished? • What is the Kinetic Molecular Theory of Matter? • How can the theory be used to describe matter? • How does a ‘real’ gas differ from an ‘ideal’ gas? • What is a change of state? • What occurs when a substance undergoes a change of state? • What is a phase diagram and how is it interpreted?

5. Your Take • Lasers (P1) • Does “empty” space have matter? • Antimatter • Lava Lamps • What is fire? (P4) • Black holes and matter • How much matter (atoms) is in our bodies? • What atoms are allowed to touch each other? • How do you split an atom? • Different colored lightbulbs (P6) • Where did the name “matter” come from? • Do we actually “touch” anything? • Invisible Ink (P7) • Glow in the dark stuff • Dark matter

6. Castagno Chemistry Challenge II • Rules: • 1) Do NOT help anyone else. • 2) You have a maximum of 10 minutes to complete the challenge. • 3) Credit only goes to COMPLETELY correct answers • 1st – 2pts, 2nd – 1pt, 3rd – 0pts, 4th – 0pts • Questions?

7. The Challenge • Organize the matter hierarchy.

8. What Is Matter? • As defined in Unit 1, matter is “anything that has mass and occupies space (volume)” • There are 3 visible in this picture, sort of.

9. Classification of Matter Can it be separated? Yes No Mixtures Pure substances Is the composition uniform? Can it be decomposed by ordinary chemical means? Yes No Yes No Homogeneous Mixtures Heterogeneous mixtures Compounds Elements Forward

10. Mixtures • A mixture is a combination of two or more substances. • Substances can be elements or compounds. • Mixture can be easy to identify or not.

11. Solid - Solid • Jewelry alloys • Rocks

12. Solid - Liquid • Iced Tea • Chocolate Milk • Aka Powdered-drink mixes

13. Liquid-Liquid • Liquid mixture • Vinegar and other household liquids

14. Liquid - Solid • Mercury in Silver dental amalgam (filling)

15. Liquid - Gas • Fog

16. Gas – Liquid • Carbonated- beverages

17. Gas – Gas • Atmosphere

18. Mixtures II – Separation Anxiety • Mixtures can be separated physically • Filters – based on particle size • Distillation – based on boiling point • Centrifuge – based on density Back

19. Homogeneous Mixtures • Uniformity throughout the entire mixture. Back

20. Heterogeneous Mixtures • Easy to identify different materials within the sample. • Different colors stand out • Different densities settle into layers Back

21. Pure Substances • FIXED composition • Each sample (like salt) has the same • Composition (make-up) • Characteristics (color, density, etc.) Back

22. Compounds • Composed of chemically bonded atoms of different elements • Individual Molecules (water) • Ionic crystals (salt) Back

23. Elements (I) • A pure substance composed of atoms that cannot be broken down into simpler, stable substances.

24. Elements (II) – Symbols • Every element is abbreviated with a symbol • Saves space on a periodic table • Makes writing formulas much easier • Some are common or make sense • C – carbon • Al – aluminum • But some seem very out of place…

25. Elements (III) – Symbols (II) • Challenge #2 – Thou fhouldethputeththynenotebookf away. • Medieval Matching Game

26. Elements (IV) - Identification • Challenge #3 – Notebooks away! • The rare back-to-back challenge! • Can you identify the elements as metallic, nonmetallic, metalloid, or the single, very special, undecided one?

27. Elements Examples • 1) Worlds largest gold bar, 250kg • Estimated worth (9/30/13): $10,663,679 ($42.53/g) • 2) The Hope Diamond (carbon) • Estimated worth: $350,000,000 ($38,461,538/g) • 3) Chunks of Boron • Estimated worth: $11.14/g (pure)

28. Elements (V) - Metals • As challenge #3 revealed, the majority of elements are metallic. • Typical properties associated with them • Conductors of heat and electricity • Malleable (sheets, foils) • Ductile (wires)

29. Elements (VI) – Nonmetals • The second largest category of elements are nonmetallic • “Opposite” properties of the metals • Poor conductors of heat and electricity • Brittle • Typically break instead of flatten into sheets or wires • Of course, most nonmetals are gases so how can you flatten a gas anyway?

30. Elements (VIII) – Metalloids • Just a few elements, located on the “staircase,” have intermediate properties. • Less malleable than metals • Less brittle than nonmetals • Semiconductors • Not as conductive as a metal, more conductive than a nonmetal

31. Elements (IX) – Specialty • Hydrogen! • Typically non-metallic with all associated properties • However, it is believed to behave as a metal inside the gas giants Jupiter and Saturn. • This metallic form helps explain the massive magnetic fields those planets have. Back

32. Check Yourself • Challenge #4 - Notebooks away! • Class Quiz

33. The Grand Unified States of Matter • The extremely rare double back-to-back Challenge #5 – Notebooks out! • Describe as much as possible of the 4 examples of matter located on the desks in the classroom.

34. States of Matter • So we know there are 4 states of matter but do any others exist? • Fundamental (4) • Solid, liquid, gas, plasma • Non-classical (8*) • Glass, plastic crystal, liquid crystal, magnetically ordered (ferro-, antiferro, ferri- magnet), Copolymers, Quantum spin liquids • Low-Temperature States (7*) • Superfluid, Bose-Einstein Condensate, Fermionic condensate, Rydberg molecule, Quantum Hall State, Strange matter (quark), Photonic matter (formed September 2013) • High Energy States (3*) • Quark-gluon plasma, color-glass condensate, gravitational singularity (VERY high energy) • Other proposed states (6*) • Degenerate matter, supersolid, string-net liquid, superglass, dark matter, equilibrium gel • Total: 4 + 8 + 7 + 3 + 6 = 28 (source: wikipedia…)

35. Kinetic Molecular Theory • Every state of matter, from the “normal” to the strange, have one thing in common: • Manner of definition • Each state of manner is defined by the movement of the particles within.

36. Kinetic Molecular Theory II • The KMT is what describes the movement • It can be applied specifically to each state of matter

37. Gas • The Kinetic Molecular Theory has 5 distinct points for gases • 1) Individual particles are far apart relative to their size • 2) Collisions between particles and containers are elastic (no energy loss) • 3) Particles are in constant motion • 4) No forces of attraction between particles • 5) Temperature of the gas depends on the average kinetic energy of the particles

38. Gas II • Steam and smoke are good examples. • The KMT describes • 1) Indefinite shape (only containers define the shape) • 2) Indefinite volume (any amount “fills” a container)

39. Gas III • 3) Low density & • 4) High compressibility • Gas particles are very far apart • 5) Fluidity • Gas particles always moving

40. Gas IV • 6) Expansion (Gas tanks) • Volume can grow • 7) Diffusion (Scented candle) • Spreading through an area • 8) Effusion (flat tire) • Escape tiny opening

41. Solid • What explains solids always keeping their shape? • 1) Specific, repeating pattern of atom arrangement • 2) Particles vibrate in position

42. Solid II • Lack of movement explains • 1) Definite volume • 2) Definite shape • 3) Incompressibility • Close arrangement results in • 4) Typically high density (solid v liquid v gas of the same substance)

43. Liquid • Unlike solids, liquids particles are not in fixed positions • They do remain fairly close together • This allows a liquid to take any shape

44. Liquid II • Shifting positions explains • Fluidity, Indefinite shape • Closeness of particles means • Definite volume • Still fairly dense (usually less so than the solid, water is an exception) • Relatively incompressible

45. Plasma • Typical properties of a gas except most/all particles are ionized (charged) • Extremely common, albeit temporarily seen on Earth

46. St. Elmo’s Fire* • A weather phenomenon typically produced during thunderstorms. • There needs to be a sustained imbalance Of electric energy often found in places we would consider a ‘lightning rod.’ • When a limit is, reached, the energy is discharged into the glow of ‘fire.’

47. STOP! In the name of conservation! • Challenge #6 – Notebooks closed! • There are two major “laws” (among many) that we encounter in this class. • What are they?

48. Conservation of Matter • In chemical reactions, matter cannot be created nor destroyed. • 20g of reactants will form a minimum and maximum of 20g product.

49. Conservation of Energy • The amount of energy present in a system will remain constant. • The energy present could cause a change, such as melting of an ice cube, but overall energy is conserved.

50. Ch-ch-changes! • Challenge #7 – Notebooks away! • There are 6 changes of state between solid, liquid, and gas. • Name the transition AND the associated change (ie: L -> G)