1. Fundamentals of General, Organic, and Biological Chemistry
5th Edition
Chapter One
Matter and Life
James Mayhugh
Oklahoma City University
2007 Prentice Hall, Inc.

2. Outline 1.1 Chemistry: The Central Science 1.2 States of Matter
1.3 Classification of Matter
1.4 An Example of a Chemical Reaction
1.5 Chemical Elements and Symbols
1.6 Elements and the Periodic Table
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3. Figure: 01-01
Title:
Chemistry: The central science
Caption:
Some relationships between chemistry, the central science, and other scientific and health-related disciplines.
Notes:
Chemistry is the “central science” because of its close relationship to all other science disciplines. Our understanding of chemistry aids our understanding of all sorts of other scientific processes, in disciplines such as biology, geology, and environmental science.
Keywords:
chemistry, central science, science disciplines

4. Chemistry: The study of the properties and transformations of matter.
Matter: Anything that has mass and occupies space – things you can see, touch, taste, or smell.
Property: A characteristic that can be used to describe a substance. Substances have both physical properties and chemical properties.
Transformations: A change in the properties of matter with time. There are physical changes and chemical changes.
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5. Substances have both physical and chemical properties.
Physical Properties: Density, color, and melting point are physical properties of matter. Observing a physical property can be done without altering the makeup of a substance.
Chemical Properties: Chemical composition, what matter is made of, and chemical reactivity, how matter behaves, are chemical properties. Observing a chemical property alters the substance.
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6. Figure: 01-02
Title:
Familiar pure substances
Caption:
Samples of the pure substances water, sugar, and baking soda.
Notes:
Keywords:
pure substance

7. Figure: 01-01UN01T01
Title:
Some properties of water, sugar, and baking soda
Caption:
Physical and chemical properties of water, sugar, and baking soda.
Notes:
Keywords:
physical properties, chemical properties

8. Physical Change: Does not alter the chemical makeup of a substance.
Chemical reactivity is unchanged.
Changes in state, changes in particle size, and the formation / separation of mixtures are all examples of physical change.
Melting of ice to form liquid water is a physical change. In this case only a change in form takes place. The chemical makeup of the substance remains H2O.
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9. Chemical Change: Alters the makeup of a substance.
Reactivity changes with the formation of new substances.
Heat, light, or electrical energy is often emitted or absorbed.
Potassium reacting with water is an example of a chemical change.
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10. Intensive and Extensive Properties
Intensive Properties
Properties are the same regardless of size or amount of material.
Examples: density, color, melting point, conductivity
Extensive Properties Properties are dependent on size and amount of material. Examples: mass, length, volume, shape, texture
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11. 1.2 States of Matter
Common states of matter are: solid, liquid, and gas.
Solid: A substance that has a definite shape and volume. Solids are rigid and dense.
Liquid: A substance that has a definite volume but that changes shape to fill the container. Liquids are dense and fluid.
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12. Common states of matter are: solid, liquid, and gas.
Gas: A substance that has neither a definite volume nor a definite shape. Gases are low density fluids.
Substances can exist in each of these three states depending on the pressure and the temperature. The conversion of a substance from one state into another is known as change of state.
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13. The three states - the solid state, the liquid state, and the gaseous state - of water are shown below.
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14. 1.3 Classification of Matter
Pure Substance: Matter that is uniform in its chemical composition and properties. Sugar is a pure substance and water is a pure substance.
Mixture: A blend of two or more pure substances in any ratio, each retaining their identity. Dissolving sugar in water creates a mixture.
Physical changes can separate mixtures into one or more pure substances. Evaporation and condensation can separate water from sugar.
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15. Element: Pure substance that cannot be broken down chemically into simpler substances. Hydrogen and oxygen are examples of elements.
Chemical Compounds: Two or more elements combined chemically in specific ratios to form a pure substance. Water is a compound composed of two parts hydrogen and one part oxygen.
Chemical changes can separate chemical compounds into elements. Water can be broken down into hydrogen and oxygen by passing an electric current through it.
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16. The classification of matter is summarized below.
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17. Figure: 01-04UN02
Title:
A typical chemical reaction (nickel and hydrochloric acid)
Caption:
The flat dish contains pieces of nickel, an element that is a typical, lustrous metal. The bottle contains hydrochloric acid, a solution of the chemical compound hydrogen chloride in water. These reactants are about to be combined in the test tube.
Notes:
Not all chemicals will react with one another.
Keywords:
reactants, nickel, hydrochloric acid, reaction

18. 1.4 Example of a Chemical Reaction
Nickel, a solid metal, is mixed with a colorless solution of hydrochloric acid in a test tube.
The nickel is slowly eaten away, the colorless solution turns green, and a colorless gas bubbles out of the test tube.
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19. Nickel + Hydrochloric Acid
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20. Nickel + Hydrochloric Acid
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21. Figure: 01-04UN04
Title:
The product of the reaction of nickel and hydrochloric acid
Caption:
Hydrogen gas can be collected as it bubbles from the solution. Removal of water from the solution leaves behind the other product, a solid green chemical compound known as nickel (II) chloride.
Notes:
Water may be removed by evaporation or filtration.
Keywords:
nickel, nickel (II) chloride, hydrogen gas

22. Reactants: One or more starting materials
Reactants: One or more starting materials. Between reactants, the “+” can be read as “reacts with.”
Products: One or more substances formed as a result of a chemical reaction. Between products, the “+” can be read as “and.”
Between products and reactants, the “” can be read as “to yield” or “to form.”
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23. 1.5 Chemical Elements and Symbols
114 elements have been discovered.
90 occur naturally.
24 are produced artificially.
Some familiar elements are iron, tin, carbon, oxygen, hydrogen, sulfur, etc.
Some unfamiliar elements are niobium, rhodium, thulium, californium, etc.
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24. Figure: 01-05
Title:
The periodic table
Caption:
The periodic table is an organized listing of all elements.
Notes:
The periodic table is an organized listing of all the elements. Its organization is based on the structures of the atoms of each element as well as the properties of elemental substances. Elements classified as metals appear on the left and elements classified as nonmetals appear on the right side of the table.
Keywords:
periodic table, elements, metals, nonmetals

25. Each element has its own unique symbol
Each element has its own unique symbol. One or two letter symbols are used to represent elements. The first letter is always capitalized and the second letter is always a lowercase. Examples: C, Cr, P, Pb
Most symbols are derived from modern names and are easy to remember. Examples: “H” for hydrogen, “O” for oxygen, “N” for nitrogen, etc.
Be careful when writing symbols: “Co” is cobalt (an element), whereas “CO” is carbon monoxide (a compound).
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26. A few symbols for elements are derived from their Latin names and are more difficult to learn. Examples: “Na” for sodium comes from its Latin name Natrium, “Pb” for lead comes from its Latin name Plumbum.
All naturally occurring elements are not equally abundant. Oxygen and silicon together constitute 75% of the Earth’s crust.
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27. Chemical Formula: A notation for a chemical compound using symbols and subscripts to show how many atoms of each element are present. When no subscript is given for an element a subscript of “1” is understood.
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28. Figure: 01-05
Title:
The periodic table
Caption:
The periodic table is an organized listing of all elements.
Notes:
The periodic table is an organized listing of all the elements. Its organization is based on the structures of the atoms of each element as well as the properties of elemental substances. Elements classified as metals appear on the left and elements classified as nonmetals appear on the right side of the table.
Keywords:
periodic table, elements, metals, nonmetals

29. Metals: Found on the left side of the table.
Large amounts of information regarding the properties of elements are embedded in the periodic table. Elements are roughly divided into 3 groups:
Metals: Found on the left side of the table.
Nonmetals: Found on the right side of the table.
Metalloids: Found along a diagonal line between metals and nonmetals.
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30. A metal (red), a nonmetal (blue), and a metalloid (green) appear in distinct places on the periodic table
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31. Some common properties of metals are:
Metals: 90 of the 114 elements are metals. They appear on the left side of the periodic table.
Some common properties of metals are:
Solid at room temperature (except mercury which is a liquid)
Good conductor of heat and electricity
Lustrous on fresh surfaces
Malleable and ductile
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32. Metals: (a) Gold is very unreactive and is used primarily in jewelry and in electronic components.
(b) Zinc, an essential nutrient, is used in the manufacture of brass, roofing materials, and batteries.
(c) Copper is widely used in electrical wiring, in water pipes, and in coins.
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33. Eleven are gases at room temperature (H, N, O, F, Ne, etc.).
Nonmetals: Appear on the right side of the periodic table. 17 elements are nonmetals.
Eleven are gases at room temperature (H, N, O, F, Ne, etc.).
Five are solids (C, P, S, Se, I).
One is a liquid (Br).
Nonmetals are poor conductors of heat and electricity.
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34. Nonmetals: (a) Nitrogen constitutes almost 80% of air and is a colorless gas at room temperature.
(b) Sulfur, a yellow solid, is found in large underground deposits in Texas and Louisiana.
(c) Iodine crystals.
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35. Metalloids: Seven elements are metalloids
Metalloids: Seven elements are metalloids. Their properties are between those of metals and nonmetals. Metalloids are semiconductors and are important to the electronics industry. (a) Boron and (b) silicon are examples of metalloids.
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36. Chapter Summary Matter is anything with mass that occupies volume.
Matter can be classified as solid, liquid, or gas.
A solid has a definite volume and shape, a liquid has a definite volume but indefinite shape, and a gas has neither a definite volume nor shape.
A substance can be characterized as being either pure or a mixture.
A pure substance is uniform in its composition and properties, but a mixture can vary in both composition and properties.
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37. Chapter Summary Cont.
Pure substances are either elements or chemical compounds.
Elements are fundamental substances that cannot be chemically changed into anything simpler.
A chemical compound can be broken down by chemical change into simpler substances.
A property describes or identifies something.
A physical property can be seen or measured without changing the chemical identity of the substance.
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38. Chapter Summary Cont.
A chemical property can only be seen or measured when the substance undergoes a chemical change.
Elements are represented by symbols. Most symbols are the first one or two letters of the element name.
Some symbols are derived from Latin names.
All the known elements are organized into a tabular form called the periodic table.
Most elements are metals, 17 are nonmetals, and 7 are metalloids.
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