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Happy Birthday Large Hadron Collider (2008)

Happy Birthday Large Hadron Collider (2008). Reading for Monday: Chapter 4 all Homework 3.1 – Due Monday 9/15/14 Chapter 3 #s 1, 3, 4, 5, 6-40 (even), 66, 68, 74, 78 Homework 3.2 – Due Wednesday 9/17/14 Chapter 3 #s 42-52 (even), 55, 56, 59, 60-64 (even), 80, 86, 88, 94, 96

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Happy Birthday Large Hadron Collider (2008)

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  1. Happy Birthday Large Hadron Collider (2008) • Reading for Monday: • Chapter 4 all • Homework 3.1 – Due Monday 9/15/14 • Chapter 3 #s 1, 3, 4, 5, 6-40 (even), 66, 68, 74, 78 • Homework 3.2 – Due Wednesday 9/17/14 • Chapter 3 #s 42-52 (even), 55, 56, 59, 60-64 (even), 80, 86, 88, 94, 96 • Misc. #1 – Due Wednesday 9/17/14 • Quiz MONDAY • Lab next week • Exp. #5

  2. Thermometers measure temperature!! The AVERAGE energy in a body of matter Temperature and Heat Heat is a measure of TOTAL energy in a body of matter Energy typically measured in: joule (J) or calorie (cal)

  3. Specific Heat The amount of energy (J or cal) that is required to raise 1 g of a substance by 1 degree Celsius. Specific heat for water = or Specific heat for silver = or

  4. Specific Heat A SMALLER specific heat means a LARGER temperature change given the same amount of energy. Temperature change when 51000 calories are added to 1000.0 grams of each: ~900 oC

  5. Specific Heat change in temp. (oC) heat (J or cal) DT = Tfinal - Tinitial mass (g) specific heat ( or )

  6. Specific Heat How many joules are needed to raise the temperature of 500.0 grams of water by 23.0 oC? joules raise 500.0 grams 23.0 oC

  7. Specific Heat How many joules are needed to raise the temperature of 500.0 grams of water by 23.0 oC?

  8. Specific Heat 3718 J is removed from a 51.73 gram piece of copper which was originally at 391.0 oC. What is the final temperature? (S.H. = 0.385 J/goC) 3718 J removed 51.73 gram 391.0 oC 0.385 J/goC

  9. Specific Heat When 16.23 calories were added to a piece of gold, its temperature rose from 23.0 oC to 89.7 oC. What was the mass of the gold? (S.H. = 0.1276 J/goC)

  10. Chemistry:The study of the properties and transformations of matter. Property: A characteristic that can be used to describe a substance. Substances have both physical and chemical properties. Transformations:A change in the properties of matter with time. There are physical changes and chemical changes. Matter: Anything that has mass and occupies space – things you can see, touch, taste, or smell.

  11. Gas Indefinite (variable) shape Indefinite (variable) volume Highly compressible HUGE amounts of space Highly disordered!! Lots of KINETIC energy Low relative density

  12. CONDENSATION!!!!!

  13. Liquid Indefinite (variable) shape Definite (fixed) volume NOT compressible Very little space between More ordered than gas Moderate KINETIC energy High relative density

  14. FREEZING!!!!!

  15. Solid Definite (fixed) shape Definite (fixed) volume NOT compressible Tightly packed Well ordered (organized) Little KINETIC energy High relative density

  16. Substances have both physical and chemical properties. Physical Properties:Density, color, and melting point are physical properties of matter. Observing a physical property can be done without altering the makeup of a substance.

  17. Physical Change: Does not alter the chemical makeup of a substance. • Chemical reactivity is unchanged. • Changes in state, changes in particle size, and the formation / separation of mixtures are all examples of physical change. • Melting of ice to form liquid water is a physical change. In this case only a change in form takes place. The chemical makeup of the substance remains H2O.

  18. Phase Transitions!! ADD ENERGY sublimation melting boiling solid liquid gas freezing condensation deposition REMOVE ENERGY

  19. Substances have both physical and chemical properties. Chemical Properties:Chemical composition, what matter is made of, and chemical reactivity, how matter behaves, are chemical properties. Observing a chemical property alters the substance.

  20. Chemical Change: • Alters the makeup of a substance. • Reactivity changes with the formation of new substances. • Heat, light, or electrical energy is often emitted or absorbed. • Potassium reacting with water is an example of a chemical change.

  21. Classification of Matter • Pure Substance: Matter that is constant in its chemical composition and properties. • Mixture: A blend of two or more pure substances in any ratio each retaining their identity. • Physical changes can separate mixtures into one or more pure substances.

  22. Element • A pure substance that cannot be broken down into a simpler substance by chemical means. pure substances compound compound element mixture ice cream  sugar  CO2  carbon physical changes chemical changes

  23. Each element has its own unique symbol. One or two letter symbols are used to represent elements. The first letter is always capitalized and the second letter is always a lower case. Examples: C, Cr, P, Pb Most are “easy” to remember. ‘H’ for hydrogen, ‘O’ for oxygen, ‘N’ for nitrogen Some are more difficult to learn. ‘Na’ for sodium (from its Latin name Natrium) ‘Pb’ for lead (from its Latin name Plumbum)

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