UNIT 1 Matter What is matter anyway Matter

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UNIT 1– Matter

UNIT 1– Matter

What is matter anyway? Matter is ANYTHING that has MASS & takes up SPACE

What is matter anyway? Matter is ANYTHING that has MASS & takes up SPACE (has VOLUME)

Kinetic Molecular Theory This is NOT in your notes…write it in!!! ö KMT=Kinetic Molecular

Kinetic Molecular Theory This is NOT in your notes…write it in!!! ö KMT=Kinetic Molecular Theory w Particles of matter are always in motion. w The kinetic energy (speed) of these particles increases as temperature increases.

Four States of Matter ö Solids w very low KE (kinetic energy) particles vibrate

Four States of Matter ö Solids w very low KE (kinetic energy) particles vibrate but can’t move around w fixed shape w fixed volume

Four States of Matter ö Liquids w low KE - particles can move over

Four States of Matter ö Liquids w low KE - particles can move over & around each other but are still close together w variable shape w fixed volume

Four States of Matter ö Gases w high KE - particles have enough energy

Four States of Matter ö Gases w high KE - particles have enough energy to separate and move throughout container; so much so that gases are mostly empty space! w variable shape w variable volume

Four States of Matter ö Plasma w Highest KE - particles collide with enough

Four States of Matter ö Plasma w Highest KE - particles collide with enough energy to break into charged particles (+/-) w gas-like, variable shape & volume w stars, fluorescent light bulbs

Fluids ö What is a fluid? w a substance that can FLOW & has

Fluids ö What is a fluid? w a substance that can FLOW & has particles that are able to move around each other. ö What 2 phases of matter are considered FLUIDS? w Liquids & Gases

Properties of Fluids ö What is viscosity? w The ability of a liquid to

Properties of Fluids ö What is viscosity? w The ability of a liquid to flow or the resistance to flow. (Honey is MORE viscous than water) ö What is buoyancy? w The upward force a fluid exerts on an object.

Properties of Fluids ö What 3 properties allow an object to be “buoyant”? w

Properties of Fluids ö What 3 properties allow an object to be “buoyant”? w The buoyant force exerted upward on the object is greater than the force downward of the object’s weight. w The density of the object is less than the density of the fluid. w The weight of the water displaced by the object is greater than the weight of the object

States of Matter…Test YOUR knowledge! Type of Matter Solid Liquid Gas Plasma Kinetic energy

States of Matter…Test YOUR knowledge! Type of Matter Solid Liquid Gas Plasma Kinetic energy Shape Volume

States of Matter…Test YOUR knowledge! Type of Matter Kinetic energy Shape Volume Solid Very

States of Matter…Test YOUR knowledge! Type of Matter Kinetic energy Shape Volume Solid Very low Definite/fixed Liquid Low Indefinite/ not fixed/ variable Definite/fixed Gas High Indefinite/ Not fixed/ variable Plasma Very high Indefinite/ Not fixed/ variable

Matter Flowchart MATTER yes MIXTURE yes Is the composition uniform? Homogeneous Mixture (solution) PURE

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

Matter Flowchart ö Test yourself… w graphite element w pepper hetero. mixture w sugar

Matter Flowchart ö Test yourself… w graphite element w pepper hetero. mixture w sugar (sucrose) compound w paint hetero. mixture w soda solution

Pure Substances: only TWO types…element OR compound! ö Element w composed of identical atoms

Pure Substances: only TWO types…element OR compound! ö Element w composed of identical atoms w Found on the PERIODIC TABLE w EX: copper wire, aluminum foil

Pure Substances: only TWO types…element OR compound! ö Compound w composed of 2 or

Pure Substances: only TWO types…element OR compound! ö Compound w composed of 2 or more elements in a fixed ratio w It has a chemical formula!!! w properties differ from those of individual elements w EX: table salt (Na. Cl)

Pure Substances ö Law of Definite Composition w A given compound always contains the

Pure Substances ö Law of Definite Composition w A given compound always contains the same, fixed ratio of elements. w In other words, water is always H 2 O with a 2: 1 ratio of H to O and hydrogen peroxide is always H 2 O 2 with a 2: 2 ratio of H to O. C. Johannesson

Pure Substances ö Law of Multiple Proportions w Elements can combine in different ratios

Pure Substances ö Law of Multiple Proportions w Elements can combine in different ratios to form different compounds. w Same as before, ratios matter. You can have the same elements, such as H & O combined in DIFFERENT ratios. H 2 O (water) and H 2 O 2 (peroxide) are two very different compounds!!!

A. Matter Flowchart--REVIEW MATTER yes MIXTURE yes Is the composition uniform? Homogeneous Mixture (solution)

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

Mixtures ö Variable combination of 2 or more pure substances. NOT chemically combined! Heterogeneous

Mixtures ö Variable combination of 2 or more pure substances. NOT chemically combined! Heterogeneous Homogeneous

Mixtures ö Homogeneous Mixtures are called Solutions w Appear the same throughout w very

Mixtures ö Homogeneous Mixtures are called Solutions w Appear the same throughout w very small particles w no Tyndall effect (light doesn’t scatter) w particles don’t settle; they are dissolved w EX: rubbing alcohol

Mixtures ö Heterogeneous Mixtures: Two Types ö Colloid w medium-sized particles w Tyndall effect

Mixtures ö Heterogeneous Mixtures: Two Types ö Colloid w medium-sized particles w Tyndall effect (will scatter light) w particles don’t settle (they’re too small) w EX: milk

Mixtures ö Suspension w large particles w Tyndall effect w particles settle (because they

Mixtures ö Suspension w large particles w Tyndall effect w particles settle (because they are so large) w EX: fresh-squeezed lemonade; pond water

C. Mixtures ö You try… w mayonnaise colloid w muddy water suspension w fog

C. Mixtures ö You try… w mayonnaise colloid w muddy water suspension w fog colloid w saltwater solution w Italian salad dressing suspension

Properties of & Changes in Matter… Intensive vs. Extensive Physical vs. Chemical

Properties of & Changes in Matter… Intensive vs. Extensive Physical vs. Chemical

Extensive vs. Intensive ö Extensive Property w depends on the amount of matter present

Extensive vs. Intensive ö Extensive Property w depends on the amount of matter present w Can be “extended” or changed ö Intensive Property w depends on the identity of substance, not the amount

A. Extensive vs. Intensive ö Examples: w boiling point intensive w volume extensive w

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

Physical vs. Chemical Property ö Physical Property w can be observed without changing the

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

Physical vs. Chemical PROPERTY ö You try it… w melting point physical w flammable

Physical vs. Chemical PROPERTY ö You try it… w melting point physical w flammable chemical w density physical w magnetic physical w tarnishes in air chemical

Physical Changes ö Changes the composition of a substance without changing its identity. ex:

Physical Changes ö Changes the composition of a substance without changing its identity. ex: cutting, separating, dissolving

Changes of state (phase changes) are physical changes that involve changes of energy.

Changes of state (phase changes) are physical changes that involve changes of energy.

Phase Changes (physical change) sublimation melting SOLID vaporization LIQUID freezing condensation deposition GAS

Phase Changes (physical change) sublimation melting SOLID vaporization LIQUID freezing condensation deposition GAS

Chemical Changes (Reactions) ö Changes the identity of the substance. Products have different properties

Chemical Changes (Reactions) ö Changes the identity of the substance. Products have different properties from the original ö ex: burning, tarnishing, cooking

Indicators of Chemical Change ö New Substance Formed ö Change of color or odor

Indicators of Chemical Change ö New Substance Formed ö Change of color or odor ö Release or formation of gas ö Formation of precipitate (solid) ö Changes in heat or light (change in energy)

ö Exothermic: Release energy as heat ö Exergonic: Release energy ö Exo- means RELEASE

ö Exothermic: Release energy as heat ö Exergonic: Release energy ö Exo- means RELEASE ö Endothermic: Absorb energy as heat ö Endergonic: Absorb energy ö Endo- mean ABSORB

Physical vs. Chemical CHANGE ö You try it… w rusting iron chemical w dissolving

Physical vs. Chemical CHANGE ö You try it… w rusting iron chemical w dissolving in water physical w burning a log chemical w melting ice physical w grinding spices physical