chapter 2 and 3 notes

Ch. 2 - Classification of Matter

I. Describing Matter (p.34 - 53)–Physical Property

–Physical Change

–Chemical Change

–Chemical Property

MATTER

What is Matter?

•Anything that has mass and volume

Characteristic properties

physical and chemical properties that help to define and identify a given substance. Density, freezing point and boiling point are characteristic physical properties. Reactivity is a characteristic 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, color, size, shape,

D. Chemical Property

A characteristic that indicates whether a substance can undergo a specific chemical change.

– EX: flammability, reactivity

A chemical property is the ABILITY of a substance to react with something else (air, water, acids, etc

Boiling pointBoiling pointMelting pointMelting pointColor (gray, red, etc.)Color (gray, red, etc.)CombustibilityCombustibilityConductivityConductivityCrystallinityCrystallinityDensityDensityDuctilityDuctilityFluorescenceFluorescenceMalleability (brittle, malleable)Malleability (brittle, malleable)Fracture / cleavageFracture / cleavageMassMassState (solid, liquid, gas, plasma)State (solid, liquid, gas, plasma)HardnessHardnessSolubility (soluble, insoluble)Solubility (soluble, insoluble)

Appearance / Homogeneity Appearance / Homogeneity (homogeneous, heterogeneous)(homogeneous, heterogeneous)

Reactivity (reactive with…, Reactivity (reactive with…, nonreactive with…, inert)nonreactive with…, inert)

Origin (naturally occurring, organic, Origin (naturally occurring, organic, inorganic, synthetic)inorganic, synthetic)

Luster (dull, shiny)Luster (dull, shiny)Texture (smooth, rough)Texture (smooth, rough)Shape (cubic, pyramidal, elliptical, Shape (cubic, pyramidal, elliptical,

spherical, etc.)spherical, etc.)StreakStreakOptical properties (transparent, Optical properties (transparent,

translucent, opaque)translucent, opaque)VolumeVolumeWeightWeightMagnetic (magnetic, nonmagnetic)Magnetic (magnetic, nonmagnetic)FlammabilityFlammability

Some properties…

=

if if

PROPERTIES OF MATTER

characteristics or qualities that describe matter or its behavior

can be classified as

PHYSICAL PROPERTIES

CHEMICAL PROPERTIES

they are characteristics that can be observed without

__________________________________________________________

they are characteristics that describe the substances ability to _______________ ______________________________________________________________

including including

(t) testable(o) observable

(m) measurable

=

if if

Main Idea

PROPERTIES OF MATTER

characteristics or qualities that describe matter or its behavior

can be classified as

PHYSICAL PROPERTIES

CHEMICAL PROPERTIES

they are characteristics that can be observed without changing the

identity of the substance.

they are characteristics that describe the substances ability to change into a new

substance with different properties / to

undergo a chemical change (reaction)

including

boiling point melting point color conductivitycrystallinity densityductility fluorescencemalleability fracture / cleavagehardness appearance / homogeneityorigin lustertexture shapestreak optical propertiesvolume weight

including

combustibilityreactivity

(t) testable(o) observable

(m) measurable

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

Chapter 3: States of MatterAKA: The Kinetic Model Theory (KMT)

4 States of Matter

Matter: is anything that has mass and volume

4 States of Matter: solid, liquid, gas, plasma

Solids Definite Shape and definite volume; particles

vibrate in place 2 types: crystalline and amorphous

1. Crystalline: particles are lined up neatly in repeating patterns of rows.

2. Amorphous: particles do not line up in repeated rows, has no true melting point

Examples of Solids: Crystalline: Amorphous:

Liquids

Definite volume Indefinite shape (takes shape of container) Particles are not arranged in repeating

patterns; particles slide past each other

Gas

Indefinite volume and indefinite shape Particle move rapidly to get away from each

other

Charles’s Law

Charles’s Law: as the temperature of a gas increases, the volume increases proportionally, provided that the pressure and amount of gas remain constant,

V1/T1 = V2/T2

temperature vo

lum

e

Boyle’s Law

This law is named for Charles Boyle, who studied the relationship between pressure, p, and volume, V, in the mid-1600s.

Boyle determined that for the same amount of a gas at constant temperature,

p * V = constant This defines an inverse relationship:

when one goes up, the other comes down.

pressure

volume

Boyle’s Law Boyle’s Law is one of the laws in physics that

concern the behaviour of gases When a gas is under pressure it takes up less

space: The higher the pressure, the smaller the

volume Boyles Law tells us about the relationship

between the volume of a gas and its pressure at a constant temperature

The law states that The law states that pressure is inversely pressure is inversely proportional to the volumeproportional to the volume

What’s up with Gas?

Temperature and volume are directly related-Charles Law

Volume and pressure are inversely related-Boyles Law

2. A sample of gas occupies 3.5 L at 300 K. What volume will it occupy at 200 K?V1 = 3.5 L, T1 = 300K, V2 = ?, T2 = 200KUsing Charles’ law: V1/T1 = V2/T2

3.5 L / 300 K = V2 / 200 KV2 = (3.5 L/300 K) x (200 K) = 2.3 L

For more lessons, visit www.chalkbored.com

K = C + 273

What volume changes occurs to a 400.0 mL gas sample as the temperature increases from 22.0 C to 30.0 C?

Plasma

Plasma

a. Hot, ionized gas particles.

b. Electrically charged.

c. Most common state in universe.

In summary,

Phase Properties

Phase

Particle Properties

Proximity Energy Motion Volume Shape

Solid

Liquid

Gas

close little vibrational definite definite

close moderate rotational definite indefinite

far apart a lot translational indefinite indefinite

ONE state of matter they didn’t teach you about in school…Until Now!

Bose-EinsteinCondensate

5th STATE OF MATTER

We all know about:

LIQUIDSSOLIDS GASES

Higher Temperature

Lower Temperature

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?

NO!If the gas is made up of particles which carry

an electric charge (“ionized particles”), but the entire gas as a whole has no electric charge, and if the density is not too high, then we can get

The 4th state of matter:

PLASMA

Some places where plasmas are found…

1. Flames

2. Lightning

3. Aurora (Northern Lights)

4. Neon lights

5. Stars

Stars make up 99% of the total matter in the Universe.

Therefore, 99% of everything that exists in the entire Universe is in the plasma state.

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

6

6. Clouds of gas and dust around stars

So now we know all about four states of matter:

LIQUIDSSOLIDS GASES

Higher Temperatur

e

Lower Temperature

PLASMAS

(only for low density ionized

gases)

But now what happens if you lower the temperature way, way, down to100 nano degrees above

“Absolute Zero” (-273°C)

Will everything just be a

frozen solid?

Not Necessarily!In 1924 (84 years ago), two scientists, Albert

Einstein and Satyendra Bose predicted a 5th state of matter which would occur at very, very low temperatures.

Einstein Bose

+

The 5th state of matter:

Bose-Einstein Bose-Einstein CondensateCondensate

Finally, in 1995 (only 16 years ago!), Wolfgang Ketterle and his team of graduate students discovered the 5th state of matter for the first time. Ketterle and his

students

In a Bose-Einstein condensate, atoms can no longer bounce around as individuals.

Instead they must all act in exactly the same way, and you can no longer tell them apart!

Here is a picture a computer took of

Bose-Einstein Condensation The big peak

happens when all the atoms act exactly the same way!(We can’t see

Bose-Einstein condensation with our eyes because the atoms are too small)

Some other computer images of Bose-Einstein Condensates…

To really understand Bose-Einstein condensate you need to knowQuantu

m Physics

In 2002, Ketterle and two other scientists received the highest award in science for

discovering Bose-Einstein condensate:

The Nobel Prize

The five states of matter:

LIQUIDSSOLIDS GASES

Higher Temperatur

e

Lower Temperatur

e

PLASMAS

(only for low density ionized gases)

BOSE-EINSTEIN

CONDENSATE

Ch. 8 - Solids, Liquids, & Gases

II. Changes in State (p.224-227)–Phase Changes

–Heating Curves

MATTER

A. Phase Changes

Melting– solid to liquid

Freezing– liquid to solid

melting point = freezing point

A. Phase Changes

Vaporization (boiling)– liquid to gas at the boiling point

Evaporation– liquid to gas below the boiling point

Condensation– gas to liquid

A. Phase Changes Sublimation

– solid to gas– EX: dry ice, freeze

drying, iodine

A. Phase Changes

B. Heating Curves

Kinetic Energy– motion of particles– related to temperature

Potential Energy– space between particles– related to phase changes

B. Heating Curves

Solid - KE

Melting - PE

Liquid - KE Boiling - PE

Gas - KE

B. Heating Curves

Heat of Fusion– energy required to change from solid to liquid– some attractive forces are broken

B. Heating Curves

Heat of Vaporization– energy required to change from liquid to gas– all attractive forces are broken– EX: steam burns, sweating, and… the drinking

bird

HEATING CURVE

Phase Change Graph

Start from: Change to: Name

solid liquid melting

liquid solid freezing

liquid gas boiling

gas liquid condensation

solidgas

(skipping liquid phase)sublimation

Ch. 16 - Chemical Reactions

IV. Energy & Chemical Reactions

Energy Changes Exothermic Reactions Endothermic Reactions

A. Energy Changes During a chemical reaction…

– energy is used to break bonds– energy is released when new bonds are formed

breakingbonds

makingbonds

C. Endothermic Reaction reaction that absorbs energy

energy req’d to break old bonds outweighs energy released by making new bonds

Feels cooler

Ex. Melting of ice absorbs energy, cold pack first aid kits

process used to obtain aluminum from aluminum ore

2Al2O3 + energy 4Al + 3O2

B. Exothermic Reaction reaction that releases energy

energy released by making new bonds outweighs energy req’d to break old bonds

Feels hot

Ex. Combustions, Digestion of food

H2(l) + O2(l) H2O(g) + energy

reaction that powers the space shuttle lift-off

Blue-Exothermic Green-Endothermic