MAIN IDEAS:

Section 8-1(matter and temperature)

-There are four states of matter: solid, liquid, gas and plasma.

-According to the kinetic theory, all matter is made of constantly moving particles.

-Most matter expands when heated and contracts when cooled.

Section 8-2(Fresh Water-Will there be Enough?)

-Fresh water on Earth is scarce, and this water is often wasted or polluted.

-There are many ways in which people can save water, and laws can be passed to regulate pollution

Section 8-3(Changes in State)

-Changes of state can be interpreted in terms of the kinetic theory of matter.

-The energy of the heat of fusion can vaporization overcomes attractive forces between particles of matter.

Section 8-4(Behavior of Gases)

-Gas pressure is caused by moving particles colliding with the inside walls of its container

-Boyle's law states that the volume of a gas decreases when the pressure increases, at constant temperature.

-Charles's law states that the volume of a gas increases when the temperature increases, at constant pressure.

Section 8-5(Uses of Fluids)

-Archimedes' principle states that the buoyant force on an object in a fluid

Is equal to the weight of the fluid displaced.

-Pascal's principle states that pressure applied to a fluid is transmitted

Unchanged throughout the fluid.

-Bernoulli's principle states that the pressure exerted by a fluid decreases as its velocity increases.

KEY SCIENCE WORDS:

Archimedes' principle Kinetic Theory of matter Bernoulli's principle Pascal

Boyle's law Pascal's Principle

Buoyant force Plasma

Charles's law Polluted Water Condensation Pressure

Crystal States of Matter

Evaporation Thermal Expansion

Heat of Fusion Thermal Pollution

Heat of Vaporization Venturi Effect

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Chapter 9 Review!!!

MAIN IDEAS:

Section 9-1(Composition of Matter)

-Elements and compounds are substances; a mixture is composed of two or more substances

-A Solution is a homogeneous mixture. Colloids and suspensions are two kinds of heterogeneous mixtures.

Section 9-2(The Colloid Connection)

-Lime and alum form an aluminum hydroxide colloid that is used to help remove finely suspended particles from water supplies.

-Exhaust from some industries may be a soot-containing colloid, which can be coagulated by using electricity in the smokestacks.

Section 9-3 (Describing Matter)

-Physical properties are characteristics of materials that you can observe without changing the identities of the substances themselves.

-In physical changes, the identities of substances in materials do not change. In chemical changes, substances in materials change to different substances.

-Physical properties indicate chemical changes substances can undergo.

-The law of conservation of mass states that during any chemical change, matter is neither created nor destroyed.

KEY SCIENCE WORDS:

Chemical change Law of Conservation of Mass

Chemical property Physical Change

Coagulation Physical Property

Colloid Solution

Compound Substance

Element Suspension

Heterogeneous mixture Tyndall Effect

Homogeneous mixture

Chapter 10 Review!!!

MAIN IDEAS:

Section 10-1(Structure of the Atom)

-A chemical symbol is a shorthand way of writing the name of an element.

-An atom consists of a nucleus made of protons and neutrons surrounded by an electron cloud.

-The electrons in an atom are arranged in several energy levels, each of which is able to hold a certain number of electrons.

Section 10-2 (Small particles of Matter)

-Quarks are particles of matter that make up protons and beutrons.

-Protons can be broken into quarks by having them collide while traveling near the speed of light.

Section 10-3(Masses of atoms)

-The number of neutrons in an atom can be computed by subtracting the atomic number from the mass number.

-The isotopes of an element are atoms of that same element that have different numbers of neutrons.

-The average atomic mass of an element is the average mass of the mixture of its isotopes.

Section 10-4 (The Periodic Table)

-The periodic table of elements is an arrangement of elements according to repeated changes in properties.

-In the periodic table, the 111 elements are arranged in 18 vertical columns, or groups, and seven horizontal rows, or periods.

-Metals are found at the left of the periodic table, nonmetals at the right, and metalloids along the line that separates the metals from the nonmetals.

KEY SCIENCE WORDS:

Atomic number Metal

Average atomic mass Metalloid

Chemical symbol Neutron

Dot diagram Nonmetal

Electron Nucleus

Electron cloud Period

Group Periodic Table

Isotope Proton

Mass number Quark

Chapter 11 Review!!!

MAIN IDEAS:

Section 11-1(Why Atoms combine)

-The properties of compounds are generally different from those of the elements they contain.

-A chemical formula for a compound indicates the composition of a unit of the compound.

-Chemical bonding occurs because atoms of most elements become more stable by gaining, losing, or sharing electrons.

Section 11-2 (Kinds of Chemical Bonds)

-Ionic bonds between atoms are formed by the attraction between ions. The sharing of electrons forms covalent bonds.

-Ionic bonding produces charged particles called ions. Covalent bonding produces units called molecules.

-The unequal sharing of electrons produces compounds that contain polar bonds and the equal sharing of electrons produces nonpolar compounds.

Section 11-3(Chemical risks in the Home)

-Compounds that are toxic, corrosive, or flammable are hazardous.

-People can protect their health and the environment from hazardous compounds in the home.

Section 11-4 (Formulas and Names of Compounds)

-An oxidation number indicates how many electrons an atom has gained, lost, or shared when bonding with other atoms.

-In the formula on an ionic compound, the element or ion with the positive oxidation number is written first, followed by the one with the negative oxidation number.

-The name of a binary compound is derived from the names of the two elements that compose the compound.

-A hydrate is a compound that has water chemically attached to its ions and written into its formula.

KEY SCIENCE WORDS:

Binary compound Hydrate

Chemical bond Ion

Chemical formula Ionic Bond

Chemically stable Nonpolar molecule

Corrosive Oxidation number

Covalent bond Polar molecule

Polyatomic Ion

Toxic

Chapter 12 Review!!!

MAIN IDEAS:

Section 12-1(Metals)

-A typical metal is a hard, shiny solid that due to metallic bonding-is malleable, ductile, and a good conductor.

-Groups 1 and 2 are the alkali and alkaline earth metals, which have some similar and some contrasting properties.

-The iron triad; the coinage metals; and the zinc, cadmium, and mercury group are among the transition elements, which make up groups 3-12 on the periodic table.

Section 12-2 (New elements, new properties)

-The lanthanides and actinides have atomic numbers 58-71 and 90-103 respectively, whereas transuranium elements have atomic numbers greater than 92.

-The making of synthetic elements with no immediate practical use is controversial.

Section 12-3 (Nonmetals)

-As a typical nonmetal, hydrogen is a gas that forms compounds by sharing electrons with other nonmetals and also with metals.

-All the halogens, group 17, have seven electrons and form both covalent and ionic compounds, but each halogen has some properties unlike the others.

-The noble gases, Group 18, are the elements whose properties and uses are related to their chemical stability.

Section 12-4(Mixed Groups)

-Groups 13-16 of the periodic table include metals, nonmetals, and metalloids.

-Allotropes are forms of the same element having different molecular structures.

-The properties of three forms of carbon-graphite, diamond, and buckminster fullerene-depend upon the differences in their crystal structures,

KEY SCIENCE WORDS:

Allotrope Radioactive element

Diatomic molecule Semiconductor

Ductile Sublimation

Malleable Transition Element

Metallic bonding Transuranium Element

Chapter 13 Review!!!

MAIN IDEAS:

Section 13-1(Simple organic compounds)

-Carbon is an element with a structure that enables it to form a large number of compounds, known as organic compounds.

-Saturated hydrocarbons contain only single bonds between carbon atoms, and unsaturated hydrocarbons contain double of triple bonds.

-Isomers of organic compounds have identical formulas but different molecular shapes.

Section 13-2 (Other organic compounds)

-Aromatic compounds, many of which have odors, contain the benzene ring structure.

-A substituted hydrocarbon contains one or more atoms of other elements that have replaced hydrogen atoms.

Section 13-3 (Growing Energy on the Farm)

-Biomass is the source of biogas and gasohol, two fuels that can be used to increase our energy supply.

-Ethanol and gasohol are useful as substitutes for gasoline, but their production may damage the environment.

Section 13-4 (Biological Compounds)

-Many important biological compounds are polymers-huge organic molecules made of many smaller units, or monomers.

-Proteins, nucleic acids, carbohydrates, and lipids are major groups of biological compounds.

KEY SCIENCE WORDS:

Alcohol Lipid

Aromatic compound Nucleic Acid

Biogas Organic Compound

Biomass Polymer

Carbohydrate Protein

Energy farming Saturated hydrocarbon

Gasohol Substituted Hydrocarbon

Hydrocarbon Unsaturated Hydrocarbon

Isomers

Chapter 15 Review!!!

MAIN IDEAS:

Section 15-1(How Solutions Form)

-Solutions are classified intro three types according to their final state: gaseous, liquid, and solid.

-Dissolving occurs when constantly moving solvent molecules attract particles of solute and surround them with solvent.

-Stirring, surface area, temperature, and pressure affect the rate of dissolving.

Section 15-2 (Regulating Organic Solvents)

-Many materials used for building or furnishing homes contain potentially harmful chemicals.

-OSHA and CPSC protect people by controlling use of these materials.

Section 15-3 (Solubility and Concentration)

-Solubility of substances varies among different solutes and for the same solute at different temperatures.

-Two precise ways to express solution concentrations are- percentage by volume and percentage by mass.

-A solution may be saturated, unsaturated, or supersaturated.

Section 15-4 (Particles in Solution)

-Usually, among polar and nonpolar solvents and solute, like dissolves like.

-Ionic Compounds dissociate when dissolved in water, and some polar compounds ionize when dissolved in water.

-Adding a solute to a solvent lowers its freezing point and raises its boiling point.

KEY SCIENCE WORDS:

Dissociation Solubility

Electrolyte Solvent

Ionization Supersaturated Solution

Nonelectrolyte Unsaturated Solution

Organic solvent

Saturate solution

Chapter 16 Review!!!

MAIN IDEAS:

Section 16-1(Chemical Changes in Matter)

-In a chemical reaction, the reactants are changed into the products, which are different substances.

-According to the law of conservation of mass, the mass of the reactants in a chemical reaction equals the mass of the products.

-A chemical equation is a shorthand way of describing chemical reaction using symbols, coefficients, and formulas.

Section 16-2(Chemical Reactions-Up in the Air)

-The ozone layer helps protect Earth by absorbing ultraviolet radiation from the sun.

-In the upper atmosphere, CFC's release atoms of chlorine that destroy ozone molecules.

-Replacing CFC's and regulating their use may slow down the loss of ozone.

Section 16-3(Chemical Equations)

-A balanced chemical equation has the same number of atoms of each element on both sides of the equation.

-The final step in the process of balancing a chemical equation is the choice of the correct coefficients.

Section 16-4 (Types of Chemical Reactions)

-Many specific chemical reactions can be classified as one of four reaction types-synthesis, decomposition, single-displacement, and double-displacement.

Section 16-5 (Energy and Chemical Reactions)

-In an exothermic reaction, energy is released; in an endothermic reaction, energy is absorbed.

KEY SCIENCE WORDS:

Balanced chemical equation Exothermic Reaction

Catalyst Inhibitor

Chemical reaction Precipitate

CFC's Product

Coefficient Reactant

Decomposition reaction Single-displacement reaction

Double-displacement reaction Synthesis Reaction

Endothermic reaction