Matter

Matter is anything that has mass and volume.

OK… so what isn’t matter?

Anything that does not have mass or

volume… in other words, ENERGY

What is Matter?

The scientific definition of energy is: the capacity of a physical system to

perform work.

In everyday terms, we could call it: the ability to do work or cause

change (make something happen).

OK-- So what is Energy?

Everything in the universe falls into one of these two categories:

MATTER or ENERGY

Examples:

people, dirt, water, air, the sun, worms, bacteria, plants

All these things have mass and volume.

Examples:

gravity, magnetism, light, sound, motion,

electricity, heat

None of these things have mass or volume.

… the amount of matter in an object.

Mass is measured with a triple-beam balance, or scale.

The units of mass are grams.

What is mass?

… the amount of space an object takes up.

Volume is measured in 3 ways:1) If the object is a liquid,

use a graduated cylinder. Units are

milliliters.

2) If the object is a rectangular solid, measure the length, height and width, and multiply them.V = L x H x W. Units are cubic centimeters (cm3)

What is volume?

3) If the object is an irregularly-shaped solid, use the displacement method. Partially fill a graduated cylinder. Measure the amount of water in it. Add the object. Measure the amount of water in the cylinder now. Calculate the difference between the two measurements. This is the object’s volume.

Units are milliliters.

Water Displacement method

is the mass per unit volume of a substance (how tightly packed the particles are).

Density = Mass ÷ Volume, or D = M V

Units are grams/cm3, or g/mL

Density cannot be measured. To find it, you must measure the mass and volume of an object, then calculate its density.

Density

1. All matter is composed of small particles (atoms, molecules, or ions).

2. These particles are in constant, random motion.

3. The particles constantly collide with each other and with the walls of their container. These collisions transfer energy.

The Kinetic Theory of MatterThe Kinetic Theory of Matter

SOLID

LIQUID

GAS

particles are packed close together

• particle motion is slow

• particle energy level is low

• definite shape and volume

• particles are loosely connected

• particle motion is medium

• particle energy level is medium

• definite volume, indefinite shape

• particles are far apart

• particle motion is fast

• particle energy level is high

• indefinite shape and volume

States of Matter

• A plasma is an ionized gas (gas that has been energized to the point that some of the electrons break free from, but travel with, their nucleus).

• A plasma is a very good conductor of electricity and is affected by magnetic fields. • Plasma, like gases, have an indefinite shape and an indefinite volume.

weblink

The fourth state of matter: PLASMA

SOLID

LIQUID

add heat

GAS

add heat

Melting

Vapor-ization

GAS

Condensa-tion

take away heat

LIQUID

SOLID

take away heat

Freezing

Sublimation: process in which a solid changes directly to a gas, skipping the liquid phase.

Phase Changes

Solid Liquid Gas

is the process in which a solid changes directly to a gas, skipping the liquid phase.

is the process in which a solid turns to a liquid.

Both processes require heat in order for the change to occur.

Melting

Sublimation

Melting & Sublimation

Dry Ice video clipshttp://www.youtube.com/watch?v=KGGbCuf2-2I (flow patterns)http://www.youtube.com/watch?v=12f1as8wIHw (4 short clips)http://www.youtube.com/watch?v=JbO2MbMgLJw(mug with bubble on top)http://www.youtube.com/watch?v=oJWNvxRnxw0&feature=related(dry ice + soap, dry ice bottle bomb, dry ice cannon)

Dry Ice is not frozen water, but frozen carbon dioxide. It is created by pressuring and refrigerating carbon dioxide gas until it becomes solid in a form similar to snowflakes. The solid CO2 is then compressed into a block.

Dry ice’s temperature is -109.3°F.

Dry Ice

… is the process in which a a liquidliquid turns to turns to a a gasgas..

There are two types of vaporization:

Boiling

occurs throughout the liquidthroughout the liquid liquid gains energy from a directly-applied heat sourcedirectly-applied heat source

Evaporation

occurs only at the surfaceat the surface liquid gains energy from gains energy from the surrounding the surrounding environmentenvironment

Vaporization

A

A

B

B

C C

D

D

E

E

Changes of State, or Phase Changes

I. Physical Properties…characteristics of a substance that can be observed without changing it into another substance.

Properties of Matter

• How It Looks Looks (Shiny, Dull, Color, etc.)

• How It FeelsFeels (Hard, Soft, Rough, Smooth, etc.)

• How It SmellsSmells (Sweet, Sharp, Rotten, No Smell, etc.)

• How It SoundsSounds (Loud, Soft, Crackly, Melodious, etc.)

• What It DoesDoes (Bounce, Stretch, Tear, Break, Reflect, Magnetic, etc.)

I. Physical Properties…characteristics of a pure substance that can be observed without changing it into another substance.

Examples: color, texture, density, odor, luster, state, flexibility, solubility, boiling point, melting point, ability to conduct heat or electricity, hardness

II. Chemical Properties…characteristics of a pure substance that describe its ability to change into different substances

Examples: flammability, reactivity

Properties of MatterProperties of Matter

I. Physical Changes

… is a change in how something looks, but not in what it is. After a physical change, a substance is still the same substance, it just looks different.

A. Changes of State

Examples: solid liquid (ice water)

B. Change in Shape or Form

1. dissolving in water

2. bending

3. crushing

4. breaking

5. chopping

6. others as well

melting, freezing, vaporization, condensation, & sublimation are all physical changes.

Changes in MatterChanges in Matter

II. … when a substance turns into something else.

A chemical change produces new substances whose properties are different from those of the original substance.

A. Combustion (Burning) FAST

fuel + oxygen heat + light + CO2 + water vapor

Chemical Changes

C. Tarnishing SLOWmetal + sulfur tarnish

Ex: silver + sulfur tarnish

D. Electrolysis FAST

using electricity to break down a substance

Ex: water hydrogen + oxygen

B. Oxidation (Rusting) SLOW

substance + oxygen new substance

Example: iron + oxygenoxygen rustrust

original Statue of Liberty

Statue of Liberty todayWhat happened?

Oxidation!The Statue’s coppercopper reacted

with oxygenoxygen in the air to form verdigris (cupric oxide or

copper carbonate), which gives it its green color)

Statue of Liberty

1. Bubbles (gasgas is released)

2. Color change (Example: glow stick)

3. Temperature changea.a. exoexothermicthermic reaction– heat is released– solution gets

hotter. Example: pocket warmerpocket warmerb. endoendothermicthermic reaction– heat is absorbed– solution gets colder. Example: chemical ice packchemical ice pack

5. A solid precipitatesprecipitates (forms) out of 2 liquids

4. A new odor is produced

6. A release of energy in the form of heat, light, heat, light, or sound sound

Evidence of a Chemical Change

energy: the ability to do work or cause change.Every chemical or physical change includes a change in energy.

temperature: measure of the average kinetic energy of all the particles of matter in an object.

thermal energy: total energy of all particles of matter in an object.

endothermic change: energy is taken in (absorbed). Solution gets colder. Example: chemical ice pack

exothermic change: energy is released. Solution gets hotter. Example: pocket warmer

kinetic energy: the energy of motion.

Matter and Thermal Energy

Exothermic & Endothermic Reactions in Solution

reaction

reaction

Exothermic reactionExothermic reaction, heat , heat given off & temperature of given off & temperature of water rises (gets water rises (gets hotterhotter))

Endothermic reactionEndothermic reaction, , heat taken in & heat taken in &

temperature of water temperature of water drops (gets drops (gets coldercolder))

Matter is not created or destroyed in any chemical or physical change.

Example: When methane combines with oxygen during burning, the mass of the methane and oxygen equals the mass of the water and carbon dioxide that are produced.

CH4 + 2 O2 CO2 + 2 H2O

methane + oxygen carbon dioxide + water

1 Carbon atom4 Hydrogen atoms4 Oxygen atoms

1 Carbon atom4 Hydrogen atoms4 Oxygen atoms

Law of Conservation of Mass

Open SystemOpen System: area where matter can get in or out

Examples: Pollard, a house, a beaker, a person

Closed SystemClosed System: area where matter can’t get in or out

Examples: bottle with a balloon on it

More Vocab

QuickTime™ and aTIFF (Uncompressed) decompressor

are needed to see this picture.

QuickTime™ and aTIFF (Uncompressed) decompressor

are needed to see this picture.

QuickTime™ and aTIFF (Uncompressed) decompressor

are needed to see this picture.

Charles’ LawCharles’ Law: For a fixed amount of gas at a constant pressure, as the temperature increases, the volume increases.

Boyle’s LawBoyle’s Law: For a fixed amount of gas at a constant temperature, as the pressure increases, the volume decreases.

T V Remember: CC is for CharlesCharles & for CelsiusCelsius (temperature)

V o l u m e temperature

P V Remember: PPeanut BButter (PPressure, BBoyle’s)

V o l u m e

pressure

The Gas Laws