MATTER Does it Really MATTER? YES

The Four States of Matter Solid Liquid Gas Plasma Based upon particle arrangement Based upon energy of particles Based upon distance between particles

States of Matter

States of Matter A. The Kinetic Theory 1. All matter is composed of small particles (atoms, molecules, or ions). 2. They are in constant, random motion. 3. They constantly collide with each other and with the walls of their container.

STATES OF MATTER SOLIDS Particles of solids are tightly packed, vibrating about a fixed position. Solids have a definite shape and a definite volume.

STATES OF MATTER LIQUID Particles of liquids are tightly packed, but are far enough apart to slide over one another. Liquids have an indefinite shape and a definite volume.

STATES OF MATTER GAS Particles of gases are very far apart and move freely. Gases have an indefinite shape and an indefinite volume.

B. Phase Properties Particle Properties Phase Proximity Energy Motion Volume Shape Solid close little vibrational definite definite Liquid close moderate rotational definite indefinite Gas far apart a lot translational indefinite indefinite

Description of Phase Change PHASE CHANGES Description of Phase Change Term for Phase Change Heat Movement During Phase Change Solid to liquid Melting Heat goes into the solid as it melts. Liquid to solid Freezing Heat leaves the liquid as it freezes.

Description of Phase Change PHASE CHANGES Description of Phase Change Term for Phase Change Heat Movement During Phase Change Liquid to gas Vaporization, which includes boiling and evaporation Heat goes into the liquid as it vaporizes. Gas to liquid Condensation Heat leaves the gas as it condenses. Solid to gas Sublimation Heat goes into the solid as it sublimates.

"Bunsen! my flame! I melt whenever I see you" said the ice. Chemistry Joke A small piece of ice which lived in a test tube fell in love with a Bunsen burner. "Bunsen! my flame! I melt whenever I see you" said the ice. The Bunsen burner replied : "It's just a phase you're going through".

Thermal E x p a n s i o n 1. Particles in any state expand when heated (generally). 2. Examples of solids: a. Expansion joints b. Power lines c. Thermostats 3. Different materials expand at different rates.

4. Mercury and alcohol are liquids that expand in thermometers 5. Air expands when heated (becoming less dense) 6. Water reaches maximum density at about 4 C. Ice particles are farther apart than liquid water (so it floats).

Will everything just be a gas? But what happens if you raise the temperature to super-high levels… between 1000°C and 1,000,000,000°C ? Will everything just be a gas?

a. Hot, ionized gas particles. Plasma a. Hot, ionized gas particles. b. Electrically charged. c. Most common state in universe.

Some places where plasmas are found… 1. Flames

2. Lightning

3. Aurora (Northern Lights)

The Sun is an example of a star in its plasma state

Plasma

STATES OF MATTER LIQUID PLASMA SOLID GAS Tightly packed, in a regular pattern Vibrate, but do not move from place to place Close together with no regular arrangement. Vibrate, move about, and slide past each other Well separated with no regular arrangement. Vibrate and move freely at high speeds Has no definite volume or shape and is composed of electrical charged particles

Physical Properties What are some physical properties? color melting and boiling point odor

Physical Changes Some physical changes would be boiling of a liquid can be observed without changing the identity of the substance Some physical changes would be boiling of a liquid melting of a solid dissolving a solid in a liquid

Chemical Properties and Chemical Change Burning hydrogen (H2) in oxygen (O2) gives H2O. Chemical change or chemical reaction — transformation of one or more atoms or molecules into one or more different molecules.

Sure Signs of a Chemical Change Heat Light Gas Produced (not from boiling!) Precipitate – a solid formed by mixing two liquids together

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

Can it be physically separated? 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

What Are Substances ?? Substances can be identified as either an element, compound, or a mixture.

A substance is matter of a particular kind. A substance cannot be further broken down or purified by physical means. A substance is matter of a particular kind. Each substance has its own characteristic properties that are different from the set of properties of any other substance. Definition of a substance.

Pure substances Elements Compounds Can be decomposed into simpler substances by chemical changes, always in a definite ratio A compound is a substance that contains two or more elements chemically combined in a fixed proportion Elements The simplest form of matter that has a unique set of properties. Cannot be decomposed into simpler substances by chemical changes The two categories of pure chemical substances.

Elements, Molecules and Compounds Some elements, such as the noble gases, exist as individual atoms. Often, elements consist of two or more atoms joined together. We call these molecules. If more than one type of atom is in a molecule, we call it a compound.

Definitions A solution is a homogeneous mixture A solute is dissolved in a solvent. A saturated solution is one where the concentration is at a maximum - no more solute is able to dissolve. A saturated solution represents an equilibrium: the rate of dissolving is equal to the rate of crystallization. The salt continues to dissolve, but crystallizes at the same rate so that there “appears” to be nothing happening.

solute - is the substance being dissolved Solvent - is the liquid in which the solute is dissolved an aqueous solution has water as solvent

Variable combination of 2 or more pure substances. Types of Mixtures Variable combination of 2 or more pure substances. Heterogeneous – visibly separate phases Homogeneous – Same throughout

Mixtures Atom, molecule or compound? atom molecule compound This is a mixture of elements made up of atoms, elements made up of molecules, and compounds. In a mixture, the particles are not joined together. Atom, molecule or compound? atom molecule compound

HOMOGENEOUS MIXTURES Homogenous mixtures look the same throughout but can be separated by physical means (dissolution, centrifuge, gravimetric filtering, etc.). Examples: milk, yogurt

INDICATORS OF A HOMOGENEOUS MIXTURE Have the same composition throughout Components are indistinguishable May or may not scatter light Examples: milk, yogurt, etc. Brainstorm more examples of homogenous mixtures.

HETEROGENEOUS MIXTURES Heterogeneous mixtures are composed of large pieces that are easily separated by physical means (ie. density, polarity, metallic properties).

INDICATORS OF A HETEROGENEOUS MIXTURE Do not have same composition throughout Components are distinguishable Examples: fruit salad, vegetable soup, etc. Brainstorm more examples of heterogenous mixtures.

WHAT ARE COLLOIDS? Colloids are solutions. They can be described as a substance trapped inside another substance. They can be identified by their characteristic scattering of light. For example: air trapped inside the fat molecules in whipped cream. Brainstorm more ideas of colloids: fog, egg merangue, jello, smoke, etc.

TYNDALL EFFECT

Intensive and Extensive Properties Physical and chemical properties may be intensive or extensive.

What are intensive properties? Intensive properties such as density, color, and boiling point do not depend on the size of the sample of matter and can be used to identify substances.

What are extensive properties? Extensive properties such as mass and volume do depend on the quantity of the sample.