Transcript Chapter 3.1 Properties and States of Matter Chapter 3 Section 1 Properties of Matter Objectives • Describe the two properties of all matter. • Describe the.

Chapter 3.1
Properties and States of Matter
Chapter 3
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
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.
Chapter 3
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.
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
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
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
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
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.
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.
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.
Chapter 3
Section 1 Properties of Matter
Identifying Matter with Physical Properties,
continued
• Mass and Weight
•The force of gravity on an object is called
weight.
• Weight is sometimes confused with mass.
• Weight varies depending on where you are in the
universe.
•Weight on moon is 1/6th of weight on earth
•Mass on moon is the same as on earth
Chapter 3
Section 1 Properties of Matter
Comparing Mass and Weight
Chapter 3
Section 1 Properties of Matter
Identifying Matter with Physical Properties,
continued
• Volume
•The amount of space matter occupies is called
volume.
• Density
•The mass of an object per unit of volume is
called its density.
•Density is found by dividing mass by volume.
Chapter 3
Section 1 Properties of Matter
Identifying Matter with Physical Properties,
continued
• Other Important Physical Properties can help
identify and classify matter.
•Malleability substances are soft, such as
aluminum – how well it can be shaped.
•Conductivity - how well a substance conducts
electricity.
•boiling point.
Chapter 3
Section 1 Properties of Matter
Identifying Matter with Chemical Properties
• Chemical Properties describe matter based on its
ability to participate in chemical reactions and form
new substances.
• Reactivity is the ability of substances to combine
and form one or more new substances.
Chapter 3
Section 1 Properties of Matter
Categories of Matter and Their Properties
• Classification
•based on the chemical and physical properties
of matter.
• Properties of Pure Substances
•All pure substances have the same composition,
and exactly the same physical and chemical
properties.
Chapter 3
Section 1 Properties of Matter
Categories of Matter and Their Properties,
continued
• Pure substances are either elements or
compounds.
• Elements are composed of the same atoms.
• Compounds are composed of the same molecules.
Chapter 3
Section 1 Properties of Matter
Categories of Matter and Their Properties,
continued
• Properties of Mixtures The physical and chemical
properties of a mixture can vary.
• A mixture is a blend of pure substances which
retain their identity and properties.
• All matter can be classified according to the
categories shown on the next slide.
Chapter 3
Section 1 Properties of Matter
Chapter 3
Section 2 Physical and Chemical
Changes
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
Section 2 Physical and Chemical
Changes
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
1.
2.
3.
4.
5.
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 reweigh:_______
6. Amount of Baking soda = (#5 - #4) = __________
7. Total Mass of reactants: (#6 + #3) = __________
8. SLOWLY add the baking soda to the vinegar. If it
overflows, you have to start over.
9. Weigh the resulting mixture and cup: _______
10. Total Mass of Products (#9 - #1)= ___________
11. Was Conservation of Mass upheld? Does #10 =
#7? Explain why or why not.
Chapter 3
Section 2 Physical and Chemical
Changes
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.
Chapter 3
Section 2 Physical and Chemical
Changes
Chapter 3
Section 2 Physical and Chemical
Changes
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
Chapter 3
Section 2 Physical and Chemical
Changes
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.
Chapter 3
Section 2 Physical and Chemical
Changes
Chemical Change in Our World, continued
• Chemical Changes in Nature
•Photosynthesis
•Digestion.
• Physical Changes in Industry
•Making metal
•Refining oil for gasoline.
Chapter 3
Section 2 Physical and Chemical
Changes
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 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.
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.
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
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.
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.
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.
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.
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
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.
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
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
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
End of Chapter 3 Show
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