Fundamentals of Chemistry – Notes Unit 6 – Matter & Energy

1. Fundamentals of Chemistry – Notes Unit 6 – Matter & Energy Matter:______________________________________________________________________ anything that has mass and takes up space The _____________________________________________ Law of Conservation of __________/________________ states that matter cannot be ________________ or Mass Matter created ________________ in an ordinary _________________ ________________. destroyed chemical reaction

2. different forms Matter can be changed into ____________ ___________. There are two types of _______________: _________________ and ________________ . __________________ changes involve a change in the _______________ _________________ of the substance. physical Physical changes chemical physical properties those characteristics of a substance that can be observed without the production of a new substance (such as color, taste, hardness, density, melting and boiling points and electrical conductivity) Properties are _________________________________________________________________ ____________________________________________________________________________. There are two types of ________________: __________________ and __________________ Cd bubbles_. properties extensive intensive

3. how much there is (volume, mass, weight, etc.) Extensive properties depend on __________________________________________________. Intensive properties depend on ___________________________________________________. _______________________ _____________________ describe how a substance _____________ or fails to __________________ with other substances to produce new ___________________. the type of matter - NOT how much there is (color, melting point, appearance etc.) properties Chemical reacts react substances A chemical change alters the chemical and physical properties of a substance and results in the formation of a new substance!

4. Properties _________________________ __________________________ ________________________ Chemical Physical ____________________________ _________________________ Intensive Extensive

5. Kinetic Energy:_______________________________________________________________________ ______________________________________________________________________________ Matter exists in ________________ states: ________________, _____________, ________________ and ___________________. The _____________ ____________ states that the _____________ ______________ in all forms of matter are in __________________ __________________. states of matter the energy an object has because of its motion four solid liquid plasma gas kinetic theory particles found constant motion

6. Phase of Matter Particles Movement Kinetic Energy arranged in an orderly pattern vibrational only low solid touching, but not tightly packed vibrational & translational moderate liquid far apart and rarely touch move freely high gas ionized gas – exists only at 40,000,000 K States of matter similar to gas high plasma

7. Matter can be classified as follows: Elements:_____________________________________________________________________ _____________________________________________________________________________ Compounds:__________________________________________________________________ _____________________________________________________________________________ a substance that cannot be changed into simpler substances under normal laboratory conditions (Ne, C, Mg, Na) a substance that can be separated into simpler substances by a chemical reaction (NaCl, H2O, MgSO4) Mixtures:_____________________________________________________________________ _____________________________________________________________________________ Homogeneous: Heterogeneous: a physical blend of two or more substances that are not chemically combined a mixture that is completely uniform in composition; it’s components are not easily distinguished a mixture that is not uniform in composition; its components are easily distinguished

8. homogeneous mixtures made up of very small particles such as individual atoms, ions or molecules Solutions:________________________________________ _________________________________________________ Four conditions for being a solution: 1.___________________________________________________________________________ 2.___________________________________________________________________________ _____________________________________________________________________________ 3.___________________________________________________________________________ 4.___________________________________________________________________________ _____________________________________________________________________________ The solution is well-stirred during it’s formation. The dissolved particles will not come out of the solution no matter how long the solution is allowed to stand The solution is clear and transparent. A solution is considered to be a SINGLE phase and can only be filtered using an extremely fine filter. Non newtonian fluids

9. solute solvent Solutions are composed of a __________________ and a __________________. The _________________ is the _________________ __________________ in a solution. The _________________ is the __________________ in which the _______________ is ____________________. For example: ______________ _______________ (salt water). The ______________ is the __________________ and the ____________________ is the _____________________.disassociation substance solute dissolved solvent substance solute dissolved saline solution solute salt solvent water

10. There are four types of solutions: 1. 2. 3. 4. (Listed first is the phase of the solute – the second is the solvent) Solid-liquid (such as kool-aid or salt water) Liquid-liquid (such as nail polish remover: acetone & water) Gas-liquid (carbonated sodas) Solid-solid (metal alloys, 10K gold)

11. The _________________ of ________________ is the _______________________ of _______________ that can ___________________ in a certain quantity of ___________________ at a specified ______________________. There are three factors that affect solubility: 1. 2. 3. How can the rate that a solute dissolves be increased? degree solubility maximum amount dissolve solute temperature solvent the nature of the solute and solvent temperature and pressure the amount of solute already dissolved decrease the particle size, stir the solution or increase the temperature reaction rate demo

12. Matter can be changed between phases by several methods: Melting/Freezing:______________________________________________________________ _____________________________________________________________________________ Evaporation/Condensation:_______________________________________________________ _____________________________________________________________________________ Sublimation:__________________________________________________________________ _____________________________________________________________________________ matter demochange of state solidliquid = melting; liquid  solid = freezing The melting point and freezing point of a substance occur at the same temperature. MILK VS BEER liquid  gas = evaporation (if at surface) boiling occurs below the surface gas  liquid = condensation Evaporation/Condensation points occur at the same temperature solid  gas (such as solid CO2 or solid air fresheners)

13. It is helpful to graph these phase changes using a heating/cooling curve: F Gas  120 D Evaporation  100 Condensation E 80 Temp. (0C) Liquid  60 BC: freezing/melting point 40 DE: evaporation/condensation point 20 B Melting  C 0 Freezing Solid A -20 10 15 0 5 Time (minutes) Heat energy added 

14. During a _____________ _______________, __________________ does NOT ____________! During a _____________ _______________, ________________ ________________ is added or removed. ______________ _____________ is changed during a ________________ _________________. change temperature phase change phase change heat energy Potential energy phase change NOTE: Kinetic energy is increased or decreased when heat energy is added and the substance is NOT undergoing a phase change. Iron energy

15. It is helpful to graph these phase changes using a heating/cooling curve: F Gas  120 D Evaporation  100 Condensation E 80 Temp. (0C) Liquid  60 BC: freezing/melting point 40 DE: evaporation/condensation point 20 (potential energy increased/decreased) B Melting  C AB, CD, EF: kinetic energy increased/decreased 0 Freezing Solid A -20 10 15 0 5 Time (minutes) phase diagrams Heat energy added 

16. ENERGY! Every _________________ in a substance is accompanied by a change in ________________. Reactions can be identified as _____________________ or ________________________. If heat energy is given off as a result of a chemical reaction, the reaction is _________________. If heat energy is _______________________, the reaction is ______________________. The minimum amount of energy needed for a reaction to begin is called ____________________ __________________. change energy exothermic endothermic exothermic absorbed endothermic activation energy Heat energy speed ______________ ______________ refers to the _______________ at which the ______________ of matter are ____________________. The more ____________ ___________ is added, the ______________ the particles move. The ______________ the ______________ _______________, the _________________ the particles move. particles moving heat energy faster lower heat energy slower NOTE:heat energy measures the total kinetic energy of particles; temperature is a measure of the average kinetic energy of particles (cup vs. tub of boiling water)

17. It is helpful to graph these phase changes using a heating/cooling curve: endothermic F Gas  120 D Evaporation  100 Condensation E exothermic 80 Temp. (0C) Liquid  60 BC: freezing/melting point 40 DE: evaporation/condensation point endothermic 20 (potential energy increased/decreased) B Melting  C AB, CD, EF: kinetic energy increased/decreased 0 Freezing Solid exothermic A -20 10 15 0 5 Time (minutes) Heat energy added 

18. There are three scales used for measuring heat energy: Celsius: Fahrenheit: Kelvin: To convert between Celsius and Kelvin: the freezing point of water is determined to be 00C and the boiling point of water is determined to be 1000C the freezing point of water is 320F and the boiling point is 2120F the theoretically lowest possible temperature is called ABSOLUTE ZERO and has never actually been reached. Absolute zero is estimated to be -2730C. Therefore, water freezes at 273 K and the boiling point of water is 373 K. • 1. K = 0C + 273 • 2. 0C = K – 273 Kelvin (fridge)