Unit 4- chapters 10-13

Properties of Matter and Relationships to Energy

Essential Learnings

Using the kinetic‐molecular model of matter, explains and predicts phase changes of matter relative to changes in thermal energy

Explains that all elements have physical and chemical properties, which are determined by

their atomic structure and are reflected in the element’s location in the Periodic Table

Explains that all substances have chemical and physical properties (density, pH, melting

point, conductivity, magnetism, reactivity) that can be measured and used to compare and

classify substances

Essential Questions

What is heat energy, and how does the transfer of heat energy affect the physical characteristics of matter?

How do the properties of matter relate to its structure and how can they be measured and used to identify, classify and describe substances or objects?

How does scientific understanding support the statement that “there is nothing new under the sun”? How have science and technology affected the quality of life?

Vocabulary

Matter Atoms Elements Brownian Motion Compound Molecules Pure substance Mixture (homogeneous and heterogeneous) Temperature (Celsius and Fahrenheit) v. Heat Thermometer Absolute Zero Kelvin Scale Intermolecular Forces Melting and Boiling Points Sublimation, Evaporation, and Condensation Plasmas Specific Heat Physical v. Chemical Properties of Matter

MatterIs anything that has mass and takes up space.

Examples: ice, water and clouds.

Matter is made up tiny particles in constant motion

-Known as Brownian Motion

Brownian Motion Model

Brownian Motion of Water

Notice the “Jerky” motion…Dr. Brown theorized that all particles move in this manner

What makes up matter?

Nucleus Protons (+ charge) Neutrons (no

charge) Electrons (-

charge) Electron orbitals

Atomic Structure Video

The Elements Song-TMBG

Physical Properties of Matter

Anything you can observe about matter by using one or more of your senses is a

Physical Property.

Measuring Matter

•Is the amount of matter in something. Units= grams

Mass

•Is the amount of space matter takes up. Units= cm3 or mL

Volume

• Is the mass of matter compared to its volume. Units= g/mL

• Density= Mass/Volume

Density

What are States of Matter?

Solids:Is matter with a volume and shape

that stays (remains) the same.

Liquids: Is matter that has a volume

that stays the same but a shape that can change.

A liquid takes the shape of whatever container holds it.

Gases:

A gas has no definite shape or volume.

A gas takes up all the space in a container.

Plasma

Atoms start to break apart at temps above 10,000 degrees Celsius.

Matter becomes ionized as electrons are broken away from atoms.

Plasma can thus conduct electricity!

Changes of State Video

Video 1

Video 2

Change of State (Phase) Graph

Which freezes faster- hot or cold water? (See clicker Question)

Changes of State

Evaporation Condensation

The change of liquid to a gas.

The change of a gas to a liquid.

SublimationMatter goes directly from a solid to a gas

Example: Dry Ice

How do atoms and molecules interact?

CHEMICAL BONDSINTERMOLECULAR FORCES

How does temperature affect matter?

TEMPERATURE MEASURE OF THE AVERAGE KINETIC ENERGY

How is temperature measured?CELSIUS V. FAHRENHEIT

T Fahrenheit = (9/5 TCelsius)

+ 32

T Celsius = 5/9 (T Fahrenheit – 32)

KELVIN= CELSIUS + 273 ˚

Absolute Zero

5TH STATE OF MATTER!

The limit to how cold matter can get

Molecules have the lowest energy they can have

Occurs at negative 273˚C (or -459˚F)

CARL WIEMAN AND ERIC CORNELL- 2001 NOBEL PRIZE!

http://www.colorado.edu/news/nobel/wiemancornell/background.html

http://www.colorado.edu/news/nobel/wiemancornell/

Video: Bose Einstein Condensate

Applications: States of Matter

STARS AND LIGHTENING

TELEVISIONS

Plasma and Liquid Crystal

How does the matter change?Physical ChangesChanges in matter that don’t form new kinds of matter are

physical changes. These changes include: color, texture, density, brittleness and state of matter.

Physical Changes

Example# 1:

Cutting makes a piece of paper smaller, but the paper is still paper.

Cutting:

Example #2

Knitting

Physical Changes

Knitting a wool cap. The thick wool is cut from sheep in spring.

The wool is combed into soft strands, which are pulled into threads and twisted to make yarn.A knitter then knits the wool yarn into a cap.

In the cap, the wool looks different from the way it looked on the sheep, but it is still wool.

Physical Changes

Example # 3: MixtureA mixture is a substance that is made up of two or more kinds of matter.

You put different types of matter together, but no new types of matter are formed.

Solution

Your mixture of salt and water was a solution.

Is a mixture in which different kinds of matter mix evenly.

Since the sand didn’t dissolve in the water, that mixture

wasn’t a solution.A solution of

detergent and water gets

dishes clean.

Separation of Matter

PURE SUBSTANCE- CANNOT BE SEPARATED BY PHYSICAL MEANS

Atoms- Matter is composed of tiny atoms; smallest part of an element that still retains the chemical identity of the element

Elements-cannot be broken down into a simpler substance (single kind of atom)

Compounds- contains 2 or more elements chemically joined and has same composition throughout (one type of molecule)

Molecules- a group of 2 or more atoms joined together by a chemical bond (combination of different compounds and/or elements)

MIXTURES- CAN BE SEPARATED BY PHYSICAL MEANS

Homogeneous- mixture that is the same throughout (examples- soda, brass, olive oil, air)

Heterogeneous- mixture that is not the same throughout (example- chicken soup, blood, cookie batter, granite)

Chemical ChangesChanges that form different kinds of matter are chemical changes. These include: cooking, burning, rotting, and burning. Not easily reversible!

Cooking Burning

RottingRusting

Properties of Matter- Solids

Crystalline- orderly, repeating arrangement of atoms or molecules

Amorphous- a random arrangement of atoms or molecules

Properties of Matter- solids Mechanical Properties include:

Tensile Strength- measure of stress from pulling or tension a material can withstand.

Hardness- measure of a solid’s resistance to scratching. Elasticity- ability to be stretched or compressed Brittleness- tendency to crack or break Ductility- ability to bend without breaking Malleability- ability of a solid to be pounded into thin

sheets. Thermal expansion- tendency of atoms or molecules

in a substance (solid, liquid or gas) to take up more space as the temp increases▪ Related to cell phone, satellite and other technology testing!

Properties of Matter- Fluids

Any matter that flows when a force is applied; can be a liquid like water or a gas like air

Less dense than a solid (except in ice/water) Pressure- amount of force extended per unit

area; caused by collisions between molecules Demo- diet coke v. coke; can crush; diet coke and

mentos Bernoulli’s Principle- the three variable of height,

speed and pressure are related by the law of energy conservation ; If one increases, then at least one of the other 2 must decrease

Bernoulli’s Principle

Bernoulli’s Principle Videos

DemonstrationsDr. Carlson’s Science Theater

Archimedes Principal

In the 3rd Century a Greek mathematician, Archimedes, realized that bouyant force is equal to the weight of the fluid displaced by an object.

Example: Suppose a rock with a volume of 1,000 cm3 displaces 1,000 cm3 of water which has a mass of 1 kg. The bouyant force= weight of 1 kg of water or 9.8 Newtons.

Archimedes Principle Video

Challenge- Make a bouyant boat that can hold the most pennies without sinking

Hint: See pages 290-291

Specific Heat

A property that tells how much heat is needed to raise the temperature of one kilogram by one degree celsius

Water = 1 kg/ raised 1˚Celsius or 4,184 Joules

Steel = 1 kg raised 1˚C or 470 Joules Units of specific heat = Joules/kg ˚C E (heat energy J)=m(mass in kg)x Cp (spec.

heat) x ΔT (temp) See p. 254-256

Specific Heat Lab

Follow the instructions provided to figure out the specific heats of the unknown materials