I. States of Matter Kinetic Energy States of Matter Ch. 1 - Matter I. States of Matter Kinetic Energy States of Matter

A. Kinetic Energy Particles of matter are always in motion. The kinetic energy (speed) of these particles increases as temperature increases.

B. Four States of Matter Solids very low KE - particles vibrate but can’t move around fixed shape fixed volume

B. Four States of Matter Liquids low KE - particles can move around but are still close together Take the shape of the container fixed volume

B. Four States of Matter Gases high KE - particles can separate and move throughout container variable shape variable volume

B. Four States of Matter Plasma very high KE - particles collide with enough energy to break into charged particles (+/-) gas-like, variable shape & volume stars

Another look at all the states of matter

II. Matter Flowchart Pure Substances Mixtures Ch. 1 - Matter II. Matter Flowchart Pure Substances Mixtures

Can it be physically separated? A. Matter Flowchart MATTER yes no Can it be physically separated? MIXTURE PURE SUBSTANCE Is the composition uniform? no yes Can it be chemically decomposed? no yes Homogeneous Mixture (solution) Heterogeneous Mixture Compound Element Colloids Suspensions

A. Matter Flowchart Examples: graphite pepper sugar (sucrose) paint soda element hetero. mixture compound homo. mixture solution

B. Pure Substances Element composed of identical atoms EX: copper wire, aluminum foil

B. Pure Substances Compound composed of 2 or more elements in a fixed ratio properties differ from those of individual elements EX: table salt (NaCl)

C. Mixtures Combination of 2 or more pure substances. Heterogeneous Homogeneous

C. Mixtures Solution homogeneous very small particles particles don’t settle EX: rubbing alcohol

C. Mixtures Colloid heterogeneous medium-sized particles particles don’t settle EX: milk

C. Mixtures Suspension heterogeneous large particles particles settle EX: fresh-squeezed lemonade

C. Mixtures Examples: mayonnaise muddy water fog saltwater Italian salad dressing colloid suspension solution

Ch. 1 - Matter III. Properties & Changes in Matter Extensive vs. Intensive Physical vs. Chemical

A. Extensive vs. Intensive Extensive Property depends on the amount of matter present Intensive Property depends on the identity of substance, not the amount

A. Extensive vs. Intensive Examples: boiling point volume mass density conductivity intensive extensive

B. Physical vs. Chemical Physical Property can be observed without changing the identity of the substance Chemical Property describes the ability of a substance to undergo changes in identity

B. Physical vs. Chemical Examples: melting point flammable density magnetic tarnishes in air physical chemical

B. Physical vs. Chemical Physical Change changes the form of a substance without changing its identity properties remain the same Chemical Change changes the identity of a substance products have different properties

B. Physical vs. Chemical Signs of a Chemical Change change in color or odor formation of a gas formation of a precipitate (solid) change in light or heat

B. Physical vs. Chemical Examples: rusting iron dissolving in water burning a log melting ice grinding spices chemical physical

How would you separate the following mixture? IRON FILINGS, SALT, CHALK POWDER AND WATER Dissolve as much of the mixture as possible Add water and stir Filter the mixture so that the soluble salt will be obtained in the filtrate and the insoluble chalk powder will be the residue on the filter paper Place the dry mixture into a beaker Dry out the filter paper to keep the dry chalk powder  Use a magnet to attract and extract the iron filings from the dry mixture  Pour the filtrate into an evaporating basin to evaporate the water and leave behind the salt