The study of matter and the changes it undergoes Chemistry The study of matter and the changes it undergoes

UNIT 1: Properties Of Matter Objectives: Learn the states of matter and be able to describe them Be able to classify matter Investigate and describe the properties of matter.

Chemistry is... The study of matter C. Johannesson

Matter VS. Non-Matter Matter Non-Matter paper sound Heat electricity water electricity Apples Matter paper Heat sound

Matter VS. Non-Matter Matter Non-Matter apples heat water electricity sound electricity heat Matter paper water apples

Matter VS. Non-Matter Describe the characteristics of the items you classified as matter what do they have in common? How are they different than the items you classified as non-matter?

Takes up space (volume) Chemistry Matter Takes up space (volume) Made up of atoms Or molecules Has Mass C. Johannesson

Use the Kinetic Molecular Theory to describe Four States of Matter Energy Phase Transition Use the Kinetic Molecular Theory to describe Particle Motion C. Johannesson

Kinetic Molecular Theory All matter is made up of particles Particles of matter are always in motion. The kinetic energy (speed) of these particles increases as temperature increases. C. Johannesson

Four States of Matter Solid Liquid Gas Plasma

Solids Very low KE Fixed shape Fixed volume Vibrate but do not move around particles are tightly packed, usually in a regular pattern. Fixed shape Fixed volume

Liquids low KE Variable shape Fixed volume. Particles vibrate & slide past each other but are still close together ability to flow and be poured and to spread when a liquid is spilled. Variable shape Fixed volume.

Gases High KE Variable shape Variable volume Particles vibrate, rotate, and move throughout the container Variable shape Variable volume

Plasma Very High KE Gas-like Variable shape Variable volume Particles vibrate, rotate, and move around Particles collide with enough energy to break into charged particles Gas-like Variable shape Variable volume Stars, fluorescent light bulbs, cathode ray tubes

Phase Transition The change of a substance from one state of matter to another by the addition or removal of heat energy.

In Relation to the Kinetic Molecular Theory

At the phase transition point (for instance, boiling point) the two phases of a substance, liquid and vapor, have identical energies and are equally likely to exist.

Energy Changes in Matter when any change occurs, energy is always involved energy can be in different forms (light, heat, etc.) energy is never destroyed or created (law of conservation of energy)

Energy Changes in Matter Exothermic change- change that gives off energy (feels warm on outside) Endothermic Change- change that uses up energy (feels cold on outside)

Classification of Matter Objectives: Differentiate between pure substances elements compounds mixtures Heterogeneous homogeneous mixtures.

Pure Substances Mixtures Classification Of Matter Elements Compounds Page 15-17 in Modern Cheistry Pure Substances Elements Compounds Mixtures Heterogeneous Homogeneous

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

Use your matter flowchart to classify these examples element hetero. mixture compound solution Examples: graphite pepper sugar(sucrose) paint soda

Pure Substances Element composed of one type of atom EX: copper wire, aluminum foil C. Johannesson

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

Law of Definite Composition 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.

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

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

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

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

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

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

Mixtures are separated by differences in their physical property Separating Mixtures Mixtures are separated by differences in their physical property Technique Separates by Filtration Phase of matter Decanting Density Distillation Boiling point Magnetism Metals / non-metals

Properties of Matter Objectives: identify and explain physical properties density, melting point, boiling point, conductivity, and malleability chemical properties ability to form new substance Distinguish between chemical and physical changes.

Properties of Matter Physical Intensive Extensive Chemical

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

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

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

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

Physical vs. Chemical Physical Change Chemical 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

Physical Changes in Matter change in a substance that doesn’t change the identity of the substance Ex. grinding, cutting, melting, boiling Can be reversible, or irreversible Includes all changes of state (physical changes of a substance from one state to another)

Chemical Changes in Matter a change in which a substance is converted into a different substance same as chemical reaction doesn’t change the amount of matter present reactants- substances that react products- substances that form Arrow points from the reactants to the new products

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

Conservation of Mass During any chemical reaction, the mass of the products is always equal to the mass of the reactants. All the mass can be accounted for: Burning of wood results in products that appear to have less mass as ashes; where is the rest? Law of conservation of mass

In the pictures how do you know right away that a chemical change took place? reactants = product 43.43 g Original mass = 43.43 g Final mass

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

The changes it undergoes Chemistry Chemistry The study of matter Its composition Its structure Its properties The changes it undergoes C. Johannesson