Chapter 3Matter: Properties and Changes

Section 1Properties of Matter

Section 3.1 -Substances

Substances– Matter is anything that has mass and takes up

space.– Substances are matter with uniform and

unchanging composition. Pure Substances

– Salt– Water

Section 3.1 – States of Matter

States of Matter– States of matter

All matter that exists naturally on Earth can be classified as one of these physical forms.

The three common states are solid, liquid and gas. Scientists also acknowledge other states, such as

plasma, which is found in stars and lightning bolts.

Section 3.1 Solids

States of Matter– Solids

A solid is a form of matter that has its own definite shape and volume.

Particles are packed tightly together in a solid. Solids are not defined by rigidity or hardness. Tend to expand when heated.

Section 3.1 - Liquid

States of Matter– Liquid

Liquid is a form of matter that flows, has constant volume, and takes the shape of its container.

Particles are packed less tightly together, and are able to move past each other.

Tend to expand when heated.

Section 3.1 – Gas

States of Matter– Gases

Gas is a form of matter that not only flows to conform to the shape of its container but also fills the entire volumes of its container.

Vapor is the term of that refers to the gaseous state of a substance that is a solid or a liquid at room temperature.

– Steam is a vapor, because water exists as a liquid at room temp.

Section 3.1 Physical Property

Physical Properties of Matter– A physical property is a characteristic that can be

observed or measured without changing the sample’s composition.

Common Physical Properties– Density, color, odor, hardness, melting point, boiling point

There are two types of physical properties– Extensive properties– Intensive properties

Section 3.1 Physical Properties

Physical Properties of Matter Extensive Properties

– These are properties that are DEPENDENT on the amount of substance present.

Examples: mass, length, and volume Intensive Properties

– These are the properties that are Independent of the amount of substance present.

Examples: density.– Substances can be identified by intensive properties.

Section 3.1 Chemical Properties

Chemical Properties of Matter– A chemical property is the ability of a substance

to combine with or change into one or more other substances.

Example: Iron forming rust

Section 3.1 Observing

Observing Properties of Matter– Every substance has its own unique set of

physical and chemical properties.

Section 3.2Changes in Matter

Section 3.2 Physical Changes

Physical Changes– A physical change is a change that alters a

substance without changing its composition. In essence, the substance retains its intensive

properties, but the extensive can change. Example: cutting a piece of paper

Section 3.2 Phase Change

Physical Change– Phase change

A phase change is the transition of a substance from one state of matter to another.

– The Water Cycle Water freezes into ice Ice melts into water Water boils into steam Steam condenses into liquid

Section 3.2 Chemical Change

Chemical Change– A chemical change is commonly referred to as a

chemical reaction. A process in which one more more substances change

into new substances. These new substances have different compositions and

properties from its component substances.

– Terms: decompose, explode, rust, oxidize, corrode, tarnish, ferment, burn, rot

Section 3.2 Evidence

Chemical Changes– Evidence of a chemical reaction

Chemical properties have changed Heat is absorbed or released Change in color Change in odor

Products

Conservation of MassLaw of Conservation of Mass

– The law states that mass is neither created nor destroyed during a chemical reaction—it is conserved.

– Within a chemical reaction, the mass of the products is the same as the mass of the reactants.

Reactants

Look at it this way. . .

Just like

ProductsReactants

INGREDIENTS•2 ¾ cups all-purpose flour •1 teaspoon baking soda •½ teaspoon baking powder •1 cup butter, softened •1 ½ cups white sugar •1 egg •1 teaspoon vanilla extract

Section 3.3

Mixtures of Matter

Section 3.3 Mixtures

Mixtures– Mixture – a combination of two or more pure

substances, in which each pure substance retains its individual chemical properties.

Examples– Mercury-silver filling– Italian dressing

Section 3.3 Types o’ Mixtures

Mixtures– Types of mixtures

Heterogeneous mixtures – a mixture that does not blend smoothly throughout and in which the individual substances remain distinct. Will have two or more phases.

– Italian Dressing

Section 3.3 Types o’ Mixtures

Mixtures– Types of mixtures

Homogeneous mixtures – a mixture that has constant composition throughout; it always has a single phase.

– Also referred to as solutions. Solutions can be liquid, solids, and gases Solid-solid solution known as steel is an alloy. An alloy is

a homogeneous mixture of metals, or a mixture of a metal and non-metal where the metal is the major component.

Steel is carbon and iron. – Lemonade

Section 3.3 Separating Mixtures

Separating Mixtures– Most matter exists naturally in the form of a mixture.– Since mixtures are physically combined, we can

separate them by physical means.– Five types we will talk about:

Filtration Distillation Crystallization Sublimation Chromatography

Section 3.3 Filtration

Separating Mixtures– Filtration

Filtration is a technique that uses a porous barrier to separate a solid from a liquid.

Section 3.3 Distillation

Separating Mixtures– Distillation

Distillation is a separation technique that is based on differences in the boiling points of the substances involved.

– The boiling points must NOT be too close together.

Section 3.3 Crystallization

Crystallization– The separation technique that results in the

formation of pure solid particles of a substance from a solution containing the dissolved substance.

– Produces highly pure solids.

Section 3.3 Sublimation

Sublimation– The process during which a solid changes to a

vapor without melting. – It skips the liquid phase.– Can be used to separate two solids, when one

solid sublimates and the other does not.

Section 3.3 Chromatography

Chromatography– Is a technique that separates the components of a

mixture (called the mobile phase) based on the ability of each component to travel or be drawn across the surface of another material (called the stationary phase).

– Can be based on different factors.

Section 3.4

Elements and Compounds

Section 3.4 Elements

Elements– An element is a pure substance that cannot be

separated into simpler substances. Each element has a unique chemical name. Each element has a unique chemical symbol.

– The symbol consists of one or two letters, in which the first letter is capitalized.

Section 3.4 Elements

Elements– The Periodic Table – organizes the elements into

a grid of horizontal rows called periods and vertical columns called families or groups.

Elements in the same group have similar chemical and physical properties.

The table is called periodic, because the pattern of similar properties repeats from period to period.

Stay tuned for more to come, in Chapter 6!

Section 3.4

Compounds– Compound is made up of two or more different

elements that are combined chemically.– Most matter in the universe exists in compounds.

These are more stable than the individual elements.

– Today, there are approximately 10 million known compounds.

Section 3.4 Properties of cmpds.

Properties of Compounds– Different from those of the component elements– Compound – Water

Components – Hydrogen and Oxygen– Colorless and odorless gases– React with many different elements

Section 3.4 ~ Separating Cmpds.

Separating Compounds into Components– Compounds can be broken down into simpler

substances, by chemical means.– Separating compounds into its elements often

requires external energy.

Section 3.4 Law of Def. Prop.

Law of Definite Proportions– Law of Definite Proportions states that a

compound is always composed of the same elements in the same proportion by mass, no matter how large or small the sample.

– Percent by mass is the ratio of the mass of each element to the total mass of the compound expressed as a percentage.

Section 3.4 Law of mult. Prop.

Law of Multiple Proportions– Law of Multiple Proportions states that when

different compounds are formed by a combination of the same elements, different masses of one element combine with the same relative mass of the other element in a ratio of small whole numbers.

Section 3.4 Mult. Prop.

What are the differences between the words apple and pale?

Two examples in the chemistry world:– Water and hydrogen peroxide– Copper chloride and copper (II) chloride

End of Chapter 3

Section 3.4 Element Scavenger Hunt

Clear your desks, except for a piece of paper, a pen, and your textbook.

Section 3.4 Scavenger hunt

1. Al

2. P

3. Y

4. Hf

5. Be

6. Ni

7. Hg

8. Br

9. I

10. Mo

1. Tungsten

2. Potassium

3. Gold

4. Tin

5. Carbon

6. Chlorine

7. Dysprosium

8. Technetium

9. Rubidium

10. Xenon

Section 3.4 Scavenger Hunt. Pt.2

1. Ag

2. Zr

3. Nd

4. Cf

5. Tl

6. Sb

7. Os

8. La

9. Se

10. As

1. Rutherfordium

2. Holmium

3. Cadmium

4. Bohrium

5. Cesium

6. Americium

7. Krypton

8. Strontium

9. Vanadium

10. Palladium