Unit 4- chapters 10-13

Properties of Matter and Relationships to Energy Unit 4- chapters 10-13

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

Matter Is 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

Anything you can observeaboutmatter by using one or more of your senses is a Physical Property. Physical Properties of Matter

Measuring Matter

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.

Sublimation Matter goes directly from a solid to a gas Example: Dry Ice

How do atoms and molecules interact? Chemical Bonds Intermolecular Forces

How does temperature affect matter? Temperature Measure of the average kinetic energy

How is temperature measured? Celsius v. Fahrenheit Kelvin= Celsius + 273 ˚ • T Fahrenheit = (9/5 TCelsius)+ 32 • T Celsius = 5/9 (T Fahrenheit – 32)

Absolute Zero 5th state of matter! Carl Wieman and Eric Cornell- 2001 Nobel Prize! http://www.colorado.edu/news/nobel/wiemancornell/background.html http://www.colorado.edu/news/nobel/wiemancornell/ • The limit to how cold matter can get • Molecules have the lowest energy they can have • Occurs at negative 273˚C (or -459˚F) Video: Bose Einstein Condensate

Applications: States of Matter Stars and Lightening Televisions Plasma and Liquid Crystal

How does the matter change? Changes 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

Physical Changes Example# 1: Cutting: Cutting makes a piece of paper smaller, but the paper is still paper.

Example #2 Physical Changes Knitting 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: Mixture A 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 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. Your mixture of salt and water was a solution. A solution of detergent and water gets dishes clean.

Separation of Matter Pure Substance- cannot be separated by physical means 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) • 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)

Chemical Changes Changes that form different kinds of matter are chemical changes. These include: cooking, burning, rotting, and burning. Not easily reversible! Burning Cooking Rotting Rusting

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 Dr. Carlson’s Science Theater Demonstrations

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

Unit 4- chapters 10-13