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Scientific Process/Matter

Scientific Process/Matter. Unit 1. Chemistry –. the study of the composition of matter and the changes it undergoes. There are 5 main branches of chemistry:. Organic -. The study of compounds that contain carbon. Inorganic -. The study of compounds which, in general, do not.

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Scientific Process/Matter

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  1. Scientific Process/Matter Unit 1

  2. Chemistry – the study of the composition of matter and the changes it undergoes There are 5 main branches of chemistry: Organic - The study of compounds that contain carbon Inorganic - The study of compounds which, in general, do not Biochemistry - The study of chemical processes which take place in organisms Analytical - The study of the composition of matter Physical - The study of reaction rates and mechanisms, as well as the energy transfer which occurs during a reaction

  3. Pure vs. Applied • Pure Chemistry – the pursuit of chemical knowledge for its own sake • The chemist doesn’t expect that there will be any immediate practical use for the knowledge. • Ex. – Studying the composition of desks. • Applied Chemistry – research that is directed toward a practical goal or application. • The chemist is applying what they have researched to solve a problem, produce a product, etc. • Ex. – Testing the effectiveness of certain drugs on the H1N1 virus.

  4. Chemical Technology • Technology is the means by which a society provides its members with those things needed and desired. • Allows humans to do some things more quickly or with less effort. • It allows people to do things that would otherwise be impossible.

  5. Chemical Elements • The simplest form in which a substance exists. Cannot be broken down by a chemical reaction. • 91 occur naturally, the rest are man made. • Colors on the periodic table are determined by state at room temperature. • Each is represented by a one or two-letter symbol. First letter is capitalized, second is lower case.

  6. Some Elements are named after a property • Au: Latin aurum – shining dawn • Br: Greek bromos – stench • H: hydros genes – water born (water former)

  7. Some are named after the location of discovery • Indium (In) • Francium (Fr) • Germanium (Ge) • Californium (Cf) • Helium (He)

  8. Others are also named for a celestial body • Tellurium (Te) • Mercury (Hg) • Uranium (U)

  9. Still others were named after famous scientists. • Nobelium (No) • Curium (Cm) • Einsteinium (Es)

  10. Names for the elements have their origins in several languages: Latin, Greek, OldeEnglish, even Arabic Most of the symbols we use come from the English or Latin names. Some examples of symbols derived from the Latin include: Au - gold Ag - silver Cu - copper Pb - lead

  11. There is one symbol, however, that does not come from English or Latin. W - tungsten The W is from wolfram, the German word for tungsten. The metal is found in the mineral known as wolframite.

  12. The Scientific Method • A process of studying natural phenomena that involves making observations, forming laws and theories, and testing theories by experimentation • Effective problem solving involves developing and implementing a plan. • Science is a dynamic and self-correcting and it involves a certain process, or method.

  13. Science as a Process Observation direct indirect Hypothesis (Testable explanation for a set of observations) Experiment (Controlled as much as possible – variables: independent - manipulated, dependent – responding) (Example – reaction time (dependent) vs. temperature (independent))

  14. Science as a Process No Yes verification Theory New hypothesis (Well-tested explanation for a broad set of observations) Law (Summarizes the results of many observations) Relate While science involves a process, it is also very often influenced by serendipity.

  15. The Difference Between a Theory and a Law • Laws predict what will happen • Theories explainwhy something happens • Which will also allow you to predict what will happen!

  16. Matter • Something that has mass and takes up space (volume) • 4 different states of matter: • Solid – definite shape and volume • Liquid – definite volume, indefinite shape • Gas – indefinite shape and volume • Gas & vapor are NOT the same thing • Vapor describes the gaseous state of a substance that is usually a liquid or solid at room temp • Plasma – very hot, electrons stripped away • The 5th state of matter - ????

  17. Classifying Matter Matter Pure Substance Mixture Element Compound Heterogeneous Homogeneous (solution) Phase –term used to describe any part of a sample with a uniform composition and properties.

  18. Properties of Matter • Properties used to describe matter can be classified as extensive or intensive. • Intensive Properties – depends on the type of matter present, not the amount • density, malleability, conductivity, ductility, luster, mp, bp, color, temp • Extensive Properties – depends on the amount of matter in a sample • mass, length, volume, shape, size • Most properties are INTENSIVE

  19. What to Study?

  20. Physical Properties/Changes • Physical Property – quality or condition of a substance that can be observed or measured without changing the composition of that substance • odor, color, density, solubility, mp, bp • metals – conductivity, malleability, ductility, luster

  21. Physical Change • Physical Change – some properties of the substance change, but the composition does not change • boil, freeze, melt, condense, break, split, cut, grind

  22. Chemical Properties/Changes • Chemical Property – the ability of a substance to undergo a change in composition • rust, burn, rot, decompose, ferment, explode, corrode • Chemical Change – the composition of matter always changes • Deciding between a physical & chemical change, ask yourself if you can get back what you started with. • Answer YES – physical change • Answer NO – chemical change

  23. Chemical Reactions • One or more substances turn into one or more new substances. • Mass is always conserved – Law of Conservation of Mass • Reactant – substance present at the beginning • Product – substance present at the end • Evidence of a chemical change: • Evolution of a gas • Formation of a precipitate (ppt) • Color change • Evolution of heat/transfer of energy • Odor produced

  24. Practice • Identify the following as element, heterogenous mixture, or homogeneous mixture: • Rubbing alcohol • Ice water • Penny • Paint • Paper • Ink • Brass • Al foil • Salsa

  25. Practice • Decide if the following are a chemical or physical change: • Color fades • Digest lunch • Cutting paper • Plant grows • Cloud formation • Turn on flashlight • Ice melts • Wound heals • Fry an egg

  26. Practice • Classify as intensive or extensive property: • Conductivity • Volume • Density • Color • Temperature • Heat content

  27. Phys/Chem Properties Lab REMINDERS!!! Get PART A (observations/properties) done as soon as possible. Don’t put magnet directly on chemical! Once done with Part A, go immediately to steps 7 & 8. Remember whatever water you add you have to evaporate off, so don’t go overboard. Give Fe and S mixture from step 6 to me after you complete your observations. We will do step 11 as a class demo, DO NOT burn the sugar in a test tube. 6 M HCl is located in the beaker on the demo table. BE CAREFUL with this acid, it is strong!!! Disposal  anything in water – down the sink anything else – in the trash

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