chapter 3: matter—properties and changes chemistry matter and change
TRANSCRIPT
Chapter 3: Matter—Properties and Changes
Chapter 3: Matter—Properties and Changes
CHEMISTRY Matter and Change
Section 3.1 Properties of Matter
Section 3.2 Changes in Matter
Section 3.3 Mixtures of Matter
Section 3.4 Elements and Compounds
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CHAPTER
3 Table Of Contents
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• Identify the characteristics of a substance.
density: a ratio that compares the mass of an object to its volume
• Distinguish between physical and chemical properties.
• Differentiate among the physical states of matter.
SECTION3.1
Properties of Matter
states of matter
solid
liquid
gas
vapor
Most common substances exist as solids, liquids, and gases, which have diverse physical and chemical properties.
physical property
extensive property
intensive property
chemical property
SECTION3.1
Properties of Matter
• Matter is anything that has mass and takes up space.
• Matter is everything around us.
• Matter with a uniform and unchanging composition is a substance.
SECTION3.1
Properties of Matter
Substances
• The physical forms of matter, either solid, liquid, or gas, are called the states of matter.
• Solids are a form of matter that have their own definite shape and volume.
• Liquids are a form of matter that have a definite volume but take the shape of the container.
SECTION3.1
Properties of Matter
States of Matter
• Gases have no definite shape or volume. They expand to fill their container.
• Vapor refers to the *
SECTION3.1
Properties of Matter
States of Matter (cont.)
• A physical property is a *
SECTION3.1
Properties of Matter
Physical Properties of Matter
• Extensive properties, such as mass, length, and volume, are *
• Intensive properties, such as density, are dependent * .
SECTION3.1
Properties of Matter
Physical Properties of Matter (cont.)
• * is called a chemical property.
– Iron forming rust
– Copper turning green in the air
SECTION3.1
Properties of Matter
Chemical Properties of Matter
• A substance can change form–an important concept in chemistry.
• Both physical and chemical properties can change with specific environmental conditions, such as temperature and pressure.
SECTION3.1
Properties of Matter
Observing Properties of Matter
• Define physical change and list several common physical changes.
observation: orderly, direct information gathering about a phenomenon
• Define chemical change and list several indications that a chemical change has taken place.
• Apply the law of conservation of mass to chemical reactions.
SECTION3.2
Changes in Matter
Matter can undergo physical and chemical changes.
physical change
phase change
chemical change
law of conservation of mass
SECTION3.2
Changes in Matter
• * is known as a physical change.
• A phase change is a transition of matter from one state to another.
• Boiling, freezing, melting, and condensing all describe phase changes in chemistry.
SECTION3.2
Changes in Matter
Physical Changes
• * is called a chemical change.
• Decomposing, rusting, exploding, burning, or oxidizing are all terms that describe chemical changes.
SECTION3.2
Changes in Matter
Chemical Changes
• The law of conservation of mass states that *.
• The mass of the reactants equals the mass of the products.
massreactants = massproducts
SECTION3.2
Changes in Matter
Conservation of Mass
• Contrast mixtures and substances.
substance: a form of matter that has a uniform and unchanging composition; also known as a pure substance
• Classify mixtures as homogeneous or heterogeneous.
• List and describe several techniques used to separate mixtures.
SECTION3.3
Mixtures of Matter
Most everyday matter occurs as mixtures—combinations of two or more substances.
mixture
heterogeneous mixture
homogeneous mixture
solution
filtration
distillation
crystallization
sublimation
chromatography
SECTION3.3
Mixtures of Matter
• A mixture is a *.
• A homogenous mixture is a mixture where the *.
SECTION3.3
Mixtures of Matter
Mixtures
• Homogeneous mixtures are also called solutions.
• A heterogeneous mixture is a mixture where the individual substances remain distinct.
SECTION3.3
Mixtures of Matter
Mixtures (cont.)
SECTION3.3
Mixtures of Matter
Mixtures (cont.)
• Filtration is a technique that *
• Distillation is a separation technique *
• Crystallization is a separation technique for *
SECTION3.3
Mixtures of Matter
Separating Mixtures
• Sublimation is the process of a solid changing directly to a gas, which can be used to separate mixtures of solids when one sublimates and the other does not.
• Chromatography is a *
SECTION3.3
Mixtures of Matter
Separating Mixtures (cont.)
• Distinguish between elements and compounds.
proportion: the relation of one part to another or to the whole with respect to quantity
• Describe the organization of elements in the periodic table.
• Explain how all compounds obey the laws of definite and multiple proportions.
SECTION3.4
Elements and Compounds
A compound is a combination of two or more elements.
element
periodic table
compound
law of definite proportions
percent by mass
law of multiple proportions
SECTION3.4
Elements and Compounds
• An element is a *
• 92 elements occur naturally on Earth.
• Each element has a unique name and a one, two, or three-letter symbol.
• The periodic table organizes the *
SECTION3.4
Elements and Compounds
Elements
• The periodic table organizes *
• 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.
SECTION3.4
Elements and Compounds
Elements (cont.)
• A compound is a *.
• Most of the matter in the universe exists as compounds.
• Table salt, NaCl, and water, H2O, are compounds.
• Unlike elements, compounds can be broken into smaller components by chemical means.
SECTION3.4
Elements and Compounds
Compounds (cont.)
• Separating a compounds into its elements often requires external energy, such as heat or electricity.
• This figure shows electrolysis of water to form hydrogen and oxygen gas.
SECTION3.4
Elements and Compounds
Compounds (cont.)
• The properties of a compound are different from its component elements.
SECTION3.4
Elements and Compounds
Compounds (cont.)
• The 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.
–Ex. Water is always composed of 2 Hydrogen to 1 Oxygen
SECTION3.4
Elements and Compounds
Law of Definite Proportions
• The relative amounts are expressed as percent by mass, the *.
SECTION3.4
Elements and Compounds
Law of Definite Proportions (cont.)
• This table demonstrates that the percentages of elements in sucrose remain the same despite differences in sample amount.
SECTION3.4
Elements and Compounds
Law of Definite Proportions (cont.)
• The 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 whole number ratios.
– Ex. Peroxide, H2O2, and water, H2O.
–Different compounds formed from the same elements.
–Hydrogen mass the same in both compounds but oxygen mass is a 2:1 ratio in peroxide to water.
SECTION3.4
Elements and Compounds
Law of Multiple Proportions
SECTION3.4
Elements and Compounds
Law of Multiple Proportions (cont.)
Key Concepts
• The three common states of matter are solid, liquid, and gas.
• Physical properties can be observed without altering a substance’s composition.
• Chemical properties describe a substance’s ability to combine with or change into one or more new substances.
• External conditions can affect both physical and chemical properties.
SECTION3.1
Properties of Matter
Study Guide
• A physical change alters the physical properties of a substance without changing its composition.
• A chemical change, also known as a chemical reaction, involves a change in a substance’s composition.
• In a chemical reaction, reactants form products.
• The law of conservation of mass states that mass is neither created nor destroyed during a chemical reaction; it is conserved.
massreactants = massproducts
Study Guide
SECTION3.2
Changes in Matter
Key Concepts
• A mixture is a physical blend of two or more pure substances in any proportion.
• Solutions are homogeneous mixtures.
• Mixtures can be separated by physical means. Common separation techniques include filtration, distillation, crystallization, sublimation, and chromatography.
Study Guide
SECTION3.3
Mixtures of Matter
Key Concepts
• Elements cannot be broken down into simpler substances by physical or chemical means.
• Elements are organized in the periodic table of the elements.
• Compounds are chemical combinations of two or more elements and their properties differ from the properties of their component elements.
Study Guide
SECTION3.4
Elements and Compounds
Key Concepts
• The law of definite proportions states that a compound is always composed of the same elements in the same proportions.
• The law of multiple proportions states that if elements form more than one compound, those compounds will have compositions that are whole-number multiples of each other.
SECTION3.4
Elements and Compounds
Study Guide
Key Concepts