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Nature

Nature. Nature - Largely made of 2 things…. Energy - the ability to produce heat or do work Matter – Anything that has mass and occupies space. Observe Nature = Law.

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Nature

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  1. Nature Nature - Largely made of 2 things…. Energy - the ability to produce heat or do work Matter – Anything that has mass and occupies space.

  2. Observe Nature = Law Laws of Conservation of Energy – Energy is never created or destroyed, but can be transformed to other forms, or transferred to other objects Law of Conservation of Matter – matter is never created or destroyed, but can be rearranged into different forms, or converted to Energy Contradiction? - when matter is converted to energy it seemingly “disappears” Dynamite explosion vs. Nuclear Explosion Nuclear Fusion and the Sun ** E=mc2

  3. Phases of Matter Plasma - particles are moving so rapidly they “blur” and break into charged (ionized) particles (pieces break off) Gas- particles are not connected to each other and in constant rapid random motion (like several rubber balls bouncing around) Liquid - particles loosely connected but are free to flow past each other or separate Solid- particles are locked to each other in a rigid “crystal lattice” with a regular pattern. They vibrate in space. Einstein Bose Condensate - theoretical phase of matter where all particle motion has stopped. Particles aren’t even vibrating. Forms a new “probability cloud” state of matter. Does not exist in nature. Considered to be “absolute zero”. Coldest possible temperature. Zero heat. Measure to be -456 F, -273 C or 0 Kelvin.

  4. Elements & Compounds Pure SubstanceMatter that has a fixed composition and distinct properties. All substances are made up of either elements or compounds or a combination of the two. Elements All atoms are the same, i.e. Oxygen (O2), Gold (Au), Silicon (Si) and Diamond (C). Made of a single type of atom. You should memorize the elemental symbols and names 1-20 Compounds Contains more than one type of atom that are chemically attached (bonded), but all molecules are the same, i.e. Water (H2O), Ethanol (C2H6O), Quartz (SiO2), Sodium Chloride (NaCl). All compounds follow the law of constant composition. Water is the same formula (H2O) everywhere Nothing else can be water

  5. Periodic Table

  6. Ne N2 SO3 Mixture

  7. Unique Properties and Characteristics Atom – The smallest stable building block of matter. Made up of protons, neutrons & electrons. (H, O, Na, Cl) Molecule – Groups of atoms held together with a specific connectivity and shape.(0, O2, O3, NaCl)

  8. Unique Properties and Characteristics Combination-some compounds are combinations of the two, and therefore can exhibit properties of both substances Composition tells us the types of atoms that are present in a compound and the ratio of these atoms (for example H2O, H2O2). Structure tells us which atoms are chemically attached (bonded) to each other, how far apart they are, and the shape of the molecule. (C6H12O6)

  9. Mixtures Mixture Have variable composition and can be separated into component parts by physical methods. Mixtures contain more than one kind of particle, and their properties depend on the relative amount of each component present in the mixture.

  10. Mixtures Two or more elements or compounds that are physically mixed, but not chemically attached (bonded). A combination of the two. Some mixtures you can see there are 2 or more substances Cereal and Milk, gravel, Soapy water Some mixtures you cannot see there are 2 or more substances Steel, Kool-Aid, Salt Water, Air

  11. Homogeneous & Heterogeneous Mixtures Homogeneous Mixture Composition and properties are uniform. Sometimes called a solution. You can’t see 2 substances Air – principle components include O2, N2 & CO2 Kool-Aid – principle components are sugar and water Steel – solid solution of Fe and C Ruby – solid solution of Al2O3 and Cr2O3 Heterogeneous MixtureComposition and properties are non-uniform. You can see two or more substances Chocolate Chip Cookie – Chocolate, Dough, etc. Concrete – Cement, Rocks, etc. Vomit – Depends upon previous intake of food and drink

  12. Complete Description of Matter Individually, neither Classifications or Phases of Matter offer a complete picture of a substance. Solid - what do aluminum, steel and ice have in common? Homogeneous Mixture - what do Kool-Aid and air have in common? You use a combination of the two systems to better describe a substance Aluminum = solid element Ice = solid compound Steel = solid homogenous mixture Kool-Aid = liquid homogenous mixture Air = Gaseous homogenous mixture

  13. Chemical and Physical Properties • Physical PropertiesThe identifying characteristics of matter. Some properties can be readily measured with our senses, such as odor and color, instruments are needed to measure other properties, such as electrical resistivity, compressibility, hardness, melting point, etc. The original substances are unchanged. • Mixtures are a physically combined substance, so can be physically separated. • Processes to separate a heterogeneous mixtures • Filtration (dirty water, sizes of rock) • Processes to separate a homogeneous mixtures • Distillation (salt and water) • Crystallization (hard tack candy) • Chromatography (our lab)

  14. Chemical and Physical Properties • Chemical PropertiesDescribe the reactivity of a substance toward other substances. Due to a rearrangement of bonds. A new substance is formed. Examples include: • Ethanol burns in air (reacts with oxygen in the air) • Sodium reacts vigorously with water • Corrosion of metal parts (rust) • Trinitrotoluene (TNT) is explosive • Chemical Processes to change identity of substance • Electrolysis (our lab) • Rusting • Burning

  15. Ethanol Stoichiometry = C2H6O Melting Point = -115 ºC Boiling Point = 78 ºC Density = 0.79 g/cm3 Chemical Prop. = Intoxicating Dimethyl Ether Stoichiometry = C2H6O Melting Point = -140 ºC Boiling Point = -24 ºC Density = Gas Chemical Prop. = Intermediate Ethylene Glycol Stoichiometry = C2H6O2 Melting Point = -16 ºC Boiling Point = 197 ºC Density = 1.11 g/cm3 Chemical Prop. = Toxic

  16. Evidence of a Chemical Change • Chemical Changethe particles in a compound break apart from their current chemical attachments (bonds) and rearrange to form new attachments. Either to new and different elements or in new amounts of attachments. • Bubbles - (baking soda in vinegar, or bubbles in electrolysis) • Change in temperature - (heat given off in a burning reaction) • Formation of a precipitate - (our lab example) • Sometimes changes in appearance - color, sound, texture, rot

  17. Chemical Reactivity 2H2(g) + O2(g)  2H2O(g)

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