I. States of Matter (p.12) Kinetic Molecular Theory States of Matter Ch. 1 - Matter I. States of Matter (p.12) Kinetic Molecular Theory States of Matter

A. Kinetic Molecular Theory KMT 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 variable shape 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, fluorescent light bulbs, CRTs

Ch. 1 - Matter II. Classification of Matter (p.15-17, 397-398) Matter Flowchart Pure Substances Mixtures C. Johannesson

Warm-Up What is the difference between a homogeneous and heterogeneous mixture? (how can you tell the difference?) C. Johannesson

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 C. Johannesson

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

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

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. Johannesson

B. Pure Substances Law of Definite Composition A given compound always contains the same, fixed ratio of elements. Law of Multiple Proportions Elements can combine in different ratios to form different compounds. C. Johannesson

Two different compounds, each has a definite composition. B. Pure Substances For example… Two different compounds, each has a definite composition. C. Johannesson

C. Mixtures Variable combination of 2 or more pure substances. Heterogeneous Homogeneous C. Johannesson

C. Mixtures Solution homogeneous very small particles no Tyndall effect Tyndall Effect particles don’t settle EX: rubbing alcohol C. Johannesson

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

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

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

Ch. 1 - Matter III. Properties & Changes in Matter (p.11-14) Extensive vs. Intensive Physical vs. Chemical C. Johannesson

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

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

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 C. Johannesson

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

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 C. Johannesson

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 C. Johannesson

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

Ch. 9 - Classification of Matter I. Describing Matter (p.254-261) Physical Property Physical Change Chemical Change Chemical Property

A. Physical Property A characteristic of a substance that can be observed without changing its identity. can be used to separate mixtures EX: magnetism, density

B. Physical Change A change in the form of a substance without changing its identity. properties remain the same reversible can be used to separate mixtures EX: dissolving, grinding

C. Chemical Change A change in the identity of a substance. properties change irreversible Signs: color change, formation of a gas/solid, release of light/heat EX: burning, rusting

D. Chemical Property A characteristic that indicates whether a substance can undergo a specific chemical change. EX: flammability, reactivity