Properties and States of Matter

Chapter 3 Objectives Describe the two properties of all matter. Section 1 Properties of Matter Objectives Describe the two properties of all matter. Describe the difference between a pure substance and a mixture. Define physical properties. Define chemical properties. Explain how matter is organized.

Chapter 3 What is Matter? Matter has mass and takes up space. Section 1 Properties of Matter What is Matter? Matter has mass and takes up space. Everything you can see in the universe is matter. Atoms are the Building Blocks of Matter All matter is made from particles called atoms. Atom is the smallest unit of matter that has unique properties.

Flow Chart Of Matter MATTER MIXTURE PURE SUBSTANCE HOMOGENEOUS physical change PURE SUBSTANCE HOMOGENEOUS HETEROGENEOUS solutions chemical change ELEMENT COMPOUND

Chapter 3 Pure Substances Section 1 Properties of Matter Pure Substances A pure substance consists of one type of atom or one type of molecule. A pure substance may be an element or a compound. A molecule is not necessarily a compound.

Pure Substances, continued Chapter 3 Section 1 Properties of Matter Pure Substances, continued Elements: A Single Type of Atom Elements cannot be broken down chemically or physically. An element is a single kind of atom. There are more than 100 different elements. Three Major Categories of Elements Metals Metalloids Non-metals

Chapter 3 Section 1 Properties of Matter

Pure Substances, continued Chapter 3 Section 1 Properties of Matter Pure Substances, continued Molecules & Compounds A Molecule is two or more atoms joined by chemical bonds A molecule has a fixed composition all of its molecules have the same atoms in the same proportion. A compound is a molecule of two or more different atoms joined by chemical bonds.

Chapter 3 Section 1 Properties of Matter

Chapter 3 Mixtures A mixture contains two or more pure substances. Section 1 Properties of Matter Mixtures A mixture contains two or more pure substances. A homogeneous mixture is uniform throughout, such as apple juice. A heterogeneous mixture is not uniformly mixed, such as salad dressing. A mixture can be separated with physical methods

Chapter 3 Mixtures, continued Section 1 Properties of Matter Mixtures, continued A Solution is a mixture that appears to be a single substance. The particles are too small to be affected by gravity and do not separate. Salt water Many solutions are liquids, but may also be a gas or solid. air

Chapter 3 Mixtures, continued Suspensions Section 1 Properties of Matter Mixtures, continued Suspensions A mixture where the particles eventually settle out. May be gas or liquid. Colloids A mixture that has particles larger than a solution Particles do not settle out. May be solid, liquid, or gas.

Identifying Matter with Physical Properties Chapter 3 Section 1 Properties of Matter Identifying Matter with Physical Properties A physical property is a characteristic of a substance that can be observed or measured. Examples are mass, density, color, hardness, melting point, boiling point.

Identifying Matter with Physical Properties, continued Chapter 3 Section 1 Properties of Matter Identifying Matter with Physical Properties, continued Mass and Weight The amount of matter in an object is called mass. Mass is constant at any place in the universe, because the amount of matter does not change.

Physical States of Matter Solid Liquid Gas Plasma

Solid Particles are tightly compact Particles vibrate without the ability to move freely Definite shape and volume Solid Animation

Liquid Particles are tightly compact, but able to move around close to each other No definite shape, but definite volume Liquid Animation

Gas Particles can easily spread out or move close together Particle move freely and with a lot of energy No definite shape or volume Gas Simulation

Plasma Why do you think this is the most common form/state of matter in the universe? Exist at extremely high temperatures (several million degrees Celsius) Particles are broken apart Particles move freely and with extremely high energy This form is not too common on earth, however it is the most common form of matter in the universe No definite shape or volume? Examples: Florescent and neon lights, lightning, aurora borealis

Energy and the States of Matter The physical states of matter result from the amount of energy the particles composing the matter have. Basically, more energy means more movement for the particles and less energy means less movement. Energy/Temperature and Matter If you were to compare an ice cube and the steam created from boiling water, which would you think has more energy?

Properties of Matter Chemical Property Any property of matter that describes a substance based on its ability to change into a new substance Examples flammability reactivity with vinegar reactivity with oxygen Iron + Oxygen  Iron oxide (rust) 2Fe + 3O2  Fe2O3

Chemical or Physical Property? Paper is white Boiling point of H2O is 100oC Zinc reacts with hydrochloric acid and creates hydrogen gas Nitrogen does not burn Sulfur smells like rotten eggs Physical Property Physical Property Chemical Property Chemical Property Physical Property

Comparing Physical and Chemical Properties Substance/Matter Physical Property Chemical Property Helium Less dense than air Nonflammable Wood Grainy texture Flammable Baking soda White powder Reacts with vinegar to produce bubbles Powdered sugar Does not react with vinegar Rubbing alcohol Clear liquid Red food coloring Red color Reacts with bleach and loses color Iron Malleable Reacts with oxygen

Changes in Matter Physical Change a change in shape, size, color, or state a change without a change in chemical composition a change that is reversible The Mixtures Lab Examples tearing paper cutting your hair change in state

Changes in States (Physical Changes) Plasma Plasma Plasma Disposition Vaporization (Evaporation/Boiling) Gas Gas Gas Gas Liquid Liquid Liquid Liquid Condensation Melting Solid Freezing Sublimation All changes in state require a change in energy All changes in state require a change in energy

States of Matter Simulation This is what happens when energy is added and taken away

combining sulfuric acid and sugar Changes in Matter Chemical Change a change in which a substance becomes another substance having different properties a change that is not reversible using ordinary physical means Changes that usually cause heat, sound, light, odor, fizzing/foaming, color changes You usually need more than one of the above characteristics to be considered a chemical change! Examples combining sulfuric acid and sugar burning a piece of wood soured milk

Chemical or Physical Change? Bending a Paper Clip Baking a cake The sublimation of carbon dioxide Crushing an aluminum can Vinegar and baking soda combining to create salt and water Physical Change Chemical Change Physical Change Physical Change Chemical Change

Chapter 3 Section 1 Properties of Matter

Chapter 3 Section 2 Objectives Define the law of conservation of mass. Section 2 Physical and Chemical Changes Chapter 3 Section 2 Objectives Define the law of conservation of mass. Describe the difference between physical and chemical changes. Explain why some changes are reversible and some are not.

Chapter 3 Conservation of Mass Section 2 Physical and Chemical Changes Chapter 3 Conservation of Mass Mass is not created or destroyed in ordinary chemical or physical changes. In ordinary physical or chemical changes, the amount of matter, which is called mass, does not change.

Conservation of Mass Lab Weigh a clean, dry cup: _________ Add a small amount of vinegar and re-weigh: ____ Amount of Vinegar = (#2 - #1) = ______________ Weigh a 2nd clean, dry cup:_________ Add a small amount of baking soda and re-weigh:_______ Amount of Baking soda = (#5 - #4) = __________ Total Mass of reactants: (#6 + #3) = __________ SLOWLY add the baking soda to the vinegar. If it overflows, you have to start over. Weigh the resulting mixture and cup: _______ Total Mass of Products (#9 - #1)= ___________ Was Conservation of Mass upheld? Does #10 = #7? Explain why or why not.

Physical Changes in Our World Section 2 Physical and Chemical Changes Chapter 3 Physical Changes in Our World A physical change is any change in which the properties of a substance, but not the identity of the substance, change. The next slide shows the physical changes that occur when sulfur and salt are separated.

Section 2 Physical and Chemical Changes Chapter 3

Physical Changes in Our World, continued Section 2 Physical and Chemical Changes Chapter 3 Physical Changes in Our World, continued Physical Changes in Nature Movement of soil and rock Ponds freezing Water freezing or melting Physical Changes in Industry Making sugar Building furniture

Chemical Change in Our World Section 2 Physical and Chemical Changes Chapter 3 Chemical Change in Our World A chemical change occurs when new substances are formed Different identity Different physical properties. A Chemical Change producing new substances are also called chemical reactions.

Chemical Change in Our World, continued Section 2 Physical and Chemical Changes Chapter 3 Chemical Change in Our World, continued Chemical Changes in Nature Photosynthesis Digestion. Physical Changes in Industry Making metal Refining oil for gasoline.

Are Physical and Chemical Changes Reversible? Section 2 Physical and Chemical Changes Chapter 3 Are Physical and Chemical Changes Reversible? Most physical changes are reversible Physical changes only affect the matter’s form. Most chemical changes are not reversible.

Chapter 3 Section 3 Objectives Section 3 States of Matter Section 3 Objectives Explain why particles in matter are always in motion. Compare the properties of solids, liquids, and gases. Explain the behavior of gases. Describe plasma.

Particles of Matter in Motion Chapter 3 Section 3 States of Matter Particles of Matter in Motion There are movements in matter that are too small to see or feel. Particles in matter are always in motion because particles have energy.

Particles of Matter in Motion, continued Chapter 3 Section 3 States of Matter Particles of Matter in Motion, continued States of Matter Determined by Particle Energy The more energy a particle has, the faster it moves. Particle energy and movement determines the physical forms of matter, or the states of matter. Four states of matter are solid, liquid, gas, and plasma. They are physically different because their particles have different amounts of energy.

Chapter 3 Section 3 States of Matter

Physical Differences Between States of Matter Chapter 3 Section 3 States of Matter Physical Differences Between States of Matter Solids Have Rigid Structure Particles are fixed into place water molecules in ice. Does not change shape or size. Temperature measures the energy of the particles. The temperature at which a solid change to liquid is called its melting point.

Physical Differences Between States of Matter, continued Chapter 3 Section 3 States of Matter Physical Differences Between States of Matter, continued Liquids A liquid assumes the shape of its container. Molecules are in contact with each other, but are not held rigidly in place. A liquid has a definite volume but no definite shape.

Physical Differences Between States of Matter, continued Chapter 3 Section 3 States of Matter Physical Differences Between States of Matter, continued Gas The particles of matter have enough energy to escape their attraction to each other. Due to their high energy and rapid motion, particles of a gas fill whatever volume is available. A gas has no definite shape and no definite volume.

Physical Differences Between States of Matter, continued Chapter 3 Section 3 States of Matter Physical Differences Between States of Matter, continued Changing from One State to Another Changes occur when energy is added to or removed from a substance. The change from a liquid to a gas is called evaporation or boiling. Energy is added to the liquid to cause its molecules to escape the attraction to one another.

Physical Differences Between States of Matter, continued Chapter 3 Section 3 States of Matter Physical Differences Between States of Matter, continued When a gas is cooled, attractions between the particles becomes stronger and the gas condenses into a liquid. When a liquid changes to a solid, it freezes. The liquid cools enough for attractions between the particles to lock the particles into fixed positions.

Chapter 3 Section 3 States of Matter Solid, Liquid and Gas

Chapter 3 Behavior of Gases Section 3 States of Matter Behavior of Gases The volume of a gas is the amount of space taken up by the gas particles in a container. Temperature Heat causes a gas to expand because the molecules have more energy. Cold causes the gas to contract because the molecules move slower.

Behavior of Gases, continued Chapter 3 Section 3 States of Matter Behavior of Gases, continued Volume The volume of a gas depends on the container that holds the gas. Pressure measures the amount of force exerted per unit area of a surface. When air particles collide within a container, they exert more pressure. In the next slide, the beach ball has less pressure because it has fewer gas particles.

Chapter 3 Section 3 States of Matter

Plasma: A Fourth State of Matter Chapter 3 Section 3 States of Matter Plasma: A Fourth State of Matter Plasma is a state of matter that starts as a gas and then becomes ionized. Its properties differ from those of a solid, liquid, or gas. Plasma is created when energy is added to a gas. Plasma is similar to a gas in that it has no fixed shape, but it is different in that it conducts electric current and is attracted to magnetic fields.

Chapter 3 Concept Mapping Properties and States of Matter Concept Mapping Use the terms below to complete the concept map on the next slide. changes of state melting evaporating solid liquid condensing chemical formulas

Chapter 3 Properties and States of Matter

Chapter 3 Properties and States of Matter

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