Unit+1+-+Intoduction+to+Chemistry

The study of matter and the changes it undergoes. Anything that was mass and occupies space (volume). ex. glass,wood,table,chair ex. milk, water ex. methane, carbon monoxide ex: elements and compounds - made of atoms -113 known elements and 91 occur naturally -Water is a compound composed of hydrogen and oxygen ex. rocks, milk
 * ** Chemistry: **
 * ** Matter: **
 * ** 3 Phases of matter: **
 * Solid- fixed shape and volume
 * Liquid- fixed volume, takes the shape of the container
 * Gas-no fixed volume, takes volume and shape of container
 * A**. Matter can be classified into two categories: Pure substances and Compounds
 * 1) Pure substances: Fixed composition and unique set of properties
 * Elements: type of matter that cannot be broken down into two or more pure substances.
 * Compounds: pure substances that contains more than one element and can be broken down
 * B**. **Mixtures** : composed of two or more substances; 2 types
 * 1) Homogeneous: uniform mixtures are ones in which the composition is the same throughout (solution) ex. sea salt
 * 2) Heterogeneous: nonuniform mixtures which the composition varies throughout

media type="youtube" key="9EDl2FhVZis" height="349" width="425"

[] from mindbites Solvent: Most present substance in which the solution in places Solute: Dissolved in the solvent
 * C.** Solution: Another name for a homogeneous mixture (solvent plus solute)


 * D.** Grams=Mass Temperature=Celsius or Kelvin Length=Meters Volume- Liters or mL


 * [[image:http://www.essex1.com/people/speer/speer.gif]] || =The Metric Prefixes= ||

http://www.essex1.com/people/speer/large.html
 * ~ Prefix: ||~ Symbol: ||~ Magnitude: ||~ Meaning (multiply by): ||
 * Hepa- || H || 1021 || 1 000 000 000 000 000 000 000 ||
 * Exa- || E || 1018 || 1 000 000 000 000 000 000 ||
 * Peta- || P || 1015 || 1 000 000 000 000 000 ||
 * Tera- || T || 1012 || 1 000 000 000 000 ||
 * Giga- || G || 109 || 1 000 000 000 ||
 * Mega- || M || 106 || 1 000 000 ||
 * Kilo- || K || 103 || 1000 ||
 * hecto- || h || 102 || 100 ||
 * deka- || da || 10 || 10 ||
 * deci- || d || 10-1 || 0.1 ||
 * centi- || c || 10-2 || 0.01 ||
 * milli- || m || 10-3 || 0.001 ||
 * micro- || µ (mu) || 10-6 || 0.000 001 ||
 * nano- || n || 10-9 || 0.000 000 001 ||
 * pico- || p || 10-12 || 0.000 000 000 001 ||
 * femto- || f || 10-15 || 0.000 000 000 000 001 ||
 * atto- || a || 10-18 || 0.000 000 000 000 000 001 ||
 * ento- || e || 10-21 || 0.000 000 000 000 000 000 001 ||
 * ento- || e || 10-21 || 0.000 000 000 000 000 000 001 ||

1. All numbers 1 to 9 are significant 2. Any zero between significant figures is significant ex: 109 3. Any trailing zeros are significant ONLY if the number has a decimal ex: 100. NOT 100 4. Place holding zeros are NEVER significant when they begin a number ex: 0.0097 (2 sig figs) 5. Any zero that follows a decimal IS significant ex: .50000 (5 sig figs)
 * E.** __ Five Rules of Sig Figs :__

__Multiplying and Dividing Sig Figs:__ ex: 300x12= 3600 BUT because 1 sig fig it equals 4 x 10^3 __Adding and Subtracting Sig Figs:__ ex: 3.06+1.2= 3.3
 * The number of sig figs is equal to the smallest number of sig figs in the equation
 * The number of decimal places is equal to the smallest number of decimal places in the equation

ex: 129.3 ms ->_s (answer 1.293)
 * F.** Conversion Factors
 * See table 1.3 in reference table

grams/liter g/mL g/cc g/cm3
 * G.** Density= mass/volume Solubility= grams solute/ 100g solvent
 * Density: intensive property
 * Solubility: the process by which a solute is dissolved in a solvent to make a solution.(physical change)
 * 1) Saturated: the point when no more solution can be dissolved
 * 2) Unsaturated: when the solvent can dissolve more solute
 * 3) Supersaturated:when the solvent contains to much solute and the solute settles out

ex. color,denesity,conductivity ex.mass,volume,molarity ex. sand to glass ex. melting point, cutting wood ° F=1.8( ° C)+32 K= ° C+273 ° C= ° F-32/ 1.8
 * H.** Properties of a Substance:
 * Intensive : properties are independent of amound
 * Extensive: properties are dependent upon the amount
 * Chemical properties : when a chemical reaction takes place and the composition of the matter changes to a new substance.
 * Physical properties : when there is a change in the apperance of matter without changing the chemical identity.
 * I.** Temperature conversations