By Aimee Chavez

Matter Heterogeneous mixture Homogenous Mixture solutionPure substance compoundElement Uniform Distribution? YES NO Fixed Composition ? Yes No Can it be broken down into simpler substances?

 Has a fixed, uniform composition and properties Can be an element or a compound.

 Elements: A substance that cannot be broken down into simple substances. An atom is the smallest particle of an element. An element has a fixed composition because it contains only one type of atom.  Atoms: basic building block of matter. Unique physical and chemical properties determined by the number or protons. Atoms:  Examples are nitrogen and oxygen the two main gases you breathe.

 Made from two or more simpler substances.  Can be broken down to simpler substances by chemical reactions (burning, reacting with chemicals, reacting with light)  Properties differ from those substances that make them. Example O and H are gases at room temperature, but water is a liquid.  Contains 2 or more elements joined in a fixed proportion /ratio.  H ₂ O water  CO ₂ carbon dioxide  Na Cl sodium chloride

 Retain some of the properties of their individual substances.  Properties of a mixture can vary because the composition of a mixture is not fixed. The type of pepper and quantity used determines hotness.  May or may not be evenly distributed : homogenous and heterogeneous

 The substances are so evenly distributed that it is difficult to distinguish one substance in the mixture from another.  Based on the size of its largest particles, a mixture can be classified as a solution, a suspension, or a colloid.

 Means different and kind  Particles are noticeably different from one another.

 A heterogeneous mixture that separates into layers over time. (pepper and water)  Particles are not evenly mixed and can be easily separated by settling or filtration  Can’t scatter light.  Muddy water

 Contains particles that are intermediate in size between the small particles in solution and the larger particles in a suspension  Doesn’t separate into layers and can’t use filter paper to separate particles  Can scatter light  Examples: milk, fog (water droplets in air),gelatin, mayonnaise, shaving cream, whipped cream

 When substances dissolve and forms a homogenous mixture, the mixture that forms is called a solution. (salt + water)  The particles are too small to settle out of the solution, be trapped by a filter, or scatter light.  Can separate by boiling and evaporating

 Solvent: Largest amount, dissolves other substance  Solute: Smaller amount, is dissolved  Water is a “universal solvent” and is part of many solutions. In many living organisms nutrients are dissolved in water. It is an important part of blood, saliva, tears. For trees water is a part of sap which carries sugar to the cells.

SoluteSolventSolution O Oxygen (g)Nitrogen (g)Air (g) carbon dioxide (g)Water (l)Soda (l) sodium chloride (s)Water (l)Sea Water (l) Zinc (s)Copper (s)Brass (s) Iron (s) Carbon (s)Steel (s) Acetic Acid (l)water (l)Vinegar (l) Silver (s) Mercury (l)Dental Fillings (s)

 Solubility: a measure of how well a solute can dissolve in a solvent at a given temperature. Can be used as a property  Saturated: no more sugar dissolves into tea, as much solute as possible is dissolved in a given temperature  Unsaturated: doesn’t hold as much of a solute as is possible at a given temperature

 1. Temperature: Most substances in crease when temperature is increased except gases  2. Pressure: Gases become more soluble with increased pressure  3. Like dissolves like: polar and non polar don’t mix

 Concentration : the amount of solute dissolved in a solvent.  Dilute: Little solute  Concentrated : more solute

 1. solutes can decrease the F.P. of solvent  2. solutes can increase the B.P. of solvent  Car antifreeze: acts to decrease the F.P to – 13 C and Increase B.P. to 176 C  Adding salt to water increases the boiling point.  Adding salt to ice decreases the freezing point

 Crystallization : Solute comes back out of solution to form a solid by cooling or evaporating.  Some are chemical reactions and form a precipitate. In a shower or sink minerals interact with the water and soap leaving soap scum.  In caves water can interact with limestone to form stalactites and stalagmites.

 Sour taste  Common examples: lemons, limes, citrus, vinegar, tea, tomatoes, green leafy vegetables ( folic acid), fertilizer ( nitric acid and phosphoric acid), car battery ( sulfuric acid), lactic acid from exercise  Reacts with metals (Mg, Zn, and Fe) and is corrosive and carbonates (forms a gas) limestone  Turns Blue litmus paper Red

 Mouth PH is 7 contains amylase which breaks down carbohydrates to simple sugars  Stomach contains HCL which has a PH of 2 the enzyme pepsin breaks down proteins to amino acids and works best with acids  Small Intestine contains Bicarbonate ion which is basic and has a PH of 8, other enzymes break down Carbohydrates, fates, and proteins which works best in a basic environment.

 Bitter taste  Slippery  Common examples: drain cleaners, glass cleaners, ammonia, MOM, calcium carbonate, baking soda, soap, shampoo, detergent  Turns red litmus paper Blue

 Tells if the substance is an acid or base  0-14  Low PH = High Hydrogen ions Acidic  High PH = Low Hydrogen ions Basic  Limes = 1.8 Bananas = 4.5  Milk = 6.3 Eggs = 7.1

 It is normal to have some acid in rain and a PH about 5.5. Some places the acid rain can have a PH as low as 3.0. The acid is from Nitrogen oxide and Sulfur Oxide. This acidic rain can damage statues, buildings, forests and kill fish

 Neutralization can occur with the correct concentration of acid and base. It forms salts and water.