Chapter One

1. Fundamentals of General, Organic, and Biological Chemistry • 6th Edition Chapter One Matter and Life

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 Chapter One

3. Goals • 1. What is matter?Be able to discuss the properties of matter and describe the three states of matter. • 2. How is matter classified?Be able to distinguish between mixtures and pure substances, and between elements and compounds. • 3. What kinds of properties does matter have?Be able to distinguish between chemical and physical properties. • 4. How are chemical elements represented?Be able to name and give the symbols of common elements. Chapter One

4. Why Study Chemistry? • In every aspect of our modern life • Long life batteries • Materials & miniaturization • Cell phones/pagers • Laptops • Synthetic fibers • Dyes • CDs/DVDs—silicon wafers • Medications • DNA sequencing • Touches all areas of science

5. Chemistry and the Sciences Chemistry • Study of matter & its transformations • Seeks answers to fundamental questions about: • What makes up materials that compose our world • How composition affects properties of substances • How substances change when they interact with each other = Chemical Reactions

6. Chemistry and the Sciences Chemistry • Seeks to understand: • Underlying structures of matter • Forces that determine properties that we observe • Apply this knowledge to: • Create new materials not found in nature • Understand fundamental biological processes

7. Matter & Its Classifications Matter • Anything that has mass & occupies space Mass • How much matter given object has • Measure of object’s momentum, or resistance to change in motion Weight • Force with which object is attracted by gravity Ex.Mass vs. Weight Astronaut on moon & on earth • Weight on moon = 1/6 weight on earth • Same mass regardless of location

8. 1.1 Chemistry: The Central Science • Chemistry is often referred to as “The Central Science” Chapter One

9. 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 and chemical properties. • Transformations: A change in the properties of matter with time. There are physical changes and chemical changes. Chapter One

10. 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, how matter behaves, are chemical properties. Observing a chemical property alters the substance. Chapter One

11. 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. Chapter One

12. 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. Chapter One

13. Learning Check: • For each of the following, determine if it represents a Chemical or Physical Change: X X X X

14. 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. Chapter One

15. 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. Chapter One

16. The three states - the solid state, the liquid state, and the gaseous state - of water are shown below. Chapter One

17. 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. Chapter One

18. Element: Pure substance that can not 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. Chapter One

19. Classification of Matter

20. The Classification of Matter by Components • Matter can also be classified according to its composition: elements, compounds, and mixtures.

21. Homogeneous Mixtures • Same properties throughout sample • Solution • Thoroughly stirred homogeneous mixture Ex. • Liquid solution • Sugar in water • Gas solution • Air • Contains nitrogen, oxygen, carbon dioxide & other gases • Solid solution • US 5¢ coin – Metal Alloy • Contains copper & nickel metals

22. Heterogeneous Mixtures • 2 or more regions of different properties • Solution with multiple phases • Separate layers Ex. • Salad dressing • Oil & vinegar • Ice & water • Same composition • 2 different physical states

23. Learning Check: Classification X X X X X X

24. 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. Chapter One

25. 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 form”. Chapter One

26. 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. Chapter One

27. 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 lower case. 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. Chapter One

28. 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. Chapter One

29. Chemical Symbols for Elements Chemical Symbol • One or two letter symbol for each element name • First letter capitalized, second letter lower case Ex. C = carbon S = sulfur Ca = calcium Ar = argon Br = bromine H = hydrogen Cl = chlorine O = oxygen • Used to represent elements in chemical formulas Ex. Water = H2O Carbon dioxide = CO2 • Most based on English name • Some based on Latin or German names

30. Chemical Symbols

31. 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. Chapter One

32. 1.6 Elements and the Periodic Table • Periodic Table: 114 elements in tabular format. Chapter One

33. 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. Chapter One

34. A metal (red), a nonmetal (blue), and a metalloid (green) appear in distinct places on the periodic table Chapter One

35. 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 Chapter One

36. 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. Chapter One

37. Nonmetals: Appear on the right side of the Periodic Table. 17elements are nonmetals. • Elevenare 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. Chapter One

38. 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. Chapter One

39. 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. Chapter One

40. 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. Chapter One

41. 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. Chapter One

42. 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. Chapter One

43. Analysis WORKED EXAMPLE 1.1Classifying Matter Classify each of the following as a mixture or a pure substance: (a) Vanilla ice cream (b) Sugar Refer to the definitions of pure substances and mixtures. Is the substance composed of more than one kind of matter? Solution (a) Vanilla ice cream is composed of more than one substance—cream, sugar, and vanilla flavoring. This is a mixture. (b) Sugar is composed of only one kind of matter—pure sugar. This is a pure substance.

44. Example 1.2Physical and Chemical Changes and Properties Determine whether each change is physical or chemical. What kind of property (chemical or physical) is demonstrated in each case? a. the evaporation of rubbing alcohol b. the burning of lamp oil c. the bleaching of hair with hydrogen peroxide d. the forming of frost on a cold night Solution a. When rubbing alcohol evaporates, it changes from liquid to gas, but it remains alcohol—this is a physical change. The volatility (the ability to evaporate easily) of alcohol is a therefore a physical property. b. Lamp oil burns because it reacts with oxygen in air to form carbon dioxide and water—this is a chemical change. The flammability of lamp oil is therefore a chemical property. c. Applying hydrogen peroxide to hair changes pigment molecules in hair that give it color—this is a chemical change. The susceptibility of hair to bleaching is therefore a chemical property. d. Frost forms on a cold night because water vapor in air changes its state to form solid ice—this is a physical change. The temperature at which water freezes is therefore a physical property. .