1. Chapter One Matter and Life Fundamentals of General, Organic & Biological Chemistry 4 th Edition Mohammed Hashmat Ali Southeast Missouri State University  2003 Prentice Hall, Inc.

2. Hall © 2003 Prentice Hall © 2003 Chapter One 2 1.1 Chemistry: The Central Science Chemistry is often referred to as “The Central Science” because it is crucial to all other sciences.

3. Hall © 2003 Prentice Hall © 2003 Chapter One 3  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. Size, color, temperature are most familiar properties of matter. Less familiar properties include: Chemical composition: what matter is made of. Chemical Reactivity: how matters behave.

4. Hall © 2003 Prentice Hall © 2003 Chapter One 4  Physical Change: Does not alter the chemical makeup of a substance. Change is reversible. Melting of solid ice is a physical change. In this case only change in form takes place and the change is reversible.  Chemical Change: Alters chemical makeup of a substance. Change is irreversible. Rusting of iron is a chemical change. Here, iron combines with oxygen and produces a new substance rust.

5. Hall © 2003 Prentice Hall © 2003 Chapter One 5 1.2 States of Matter Matter exist in three forms: solid, liquid, and gas. Solid: A substance that has a definite shape and volume. Liquid: A substance that has a definite volume but that changes shape to fill the container. Gas: A substance that has neither a definite volume nor a definite shape. Many substances, such as water, can exist in all three states depending on the temperature. The conversion of a substance from one state into another is known as change of state.

6. Hall © 2003 Prentice Hall © 2003 Chapter One 6 The three states - the solid state, the liquid state, and the gaseous state - of water are shown in Figure 1.3 below.

7. Hall © 2003 Prentice Hall © 2003 Chapter One 7 1.3 Classification of Matter  Pure Substance: Uniform in its chemical composition and properties. Sugar and water are pure substances.  Mixture: Composition and properties may vary. Different amounts of sugar dissolved in water will determine sweetness of water. Sugar water is an example of a mixture.

8. Hall © 2003 Prentice Hall © 2003 Chapter One 8  Chemical Compounds: Substance that can be broken down into simpler substances. Water is a chemical compound since it can be broken down into hydrogen and oxygen by passing electric current through it.  Element: Substance that can not be broken down chemically into simpler substances. Hydrogen, oxygen, nitrogen are example of elements.

9. Hall © 2003 Prentice Hall © 2003 Chapter One 9 The classification of matter is summarized in Fig 1.4 below.

10. Hall © 2003 Prentice Hall © 2003 Chapter One 10 1.4 An Example of a Chemical Reaction When the element 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.

11. Hall © 2003 Prentice Hall © 2003 Chapter One 11 1.5 Chemical Elements and Symbols 113 Elements are known until today. Only 90 of these elements occur naturally, remaining are produced artificially by chemists and physicist.  Some familiar elements are iron, tin, carbon, oxygen, hydrogen, sulfur, etc.  Some unfamiliar elements are niobium, rhodium, thulium, californium etc.

12. Hall © 2003 Prentice Hall © 2003 Chapter One 12 Each element has its own unique symbol. –One or two letter symbols are used to represent elements. –First letter is always capitalized and the second letter is always a lower case. –Some symbols came from elements modern name such as ‘H’ for hydrogen, ‘O’ for oxygen, ‘N’ for nitrogen, etc.

13. Hall © 2003 Prentice Hall © 2003 Chapter One 13  A few symbols for elements are derived from their Latin names. For example, ‘Na’ for sodium came from its Latin name Natrium.  All naturally occurring elements are not equally abundant. Oxygen and silicon together constitute 75% of the earth’s crust.  Chemical Formula: A notation for chemical compound using element symbols and subscripts to show how many atoms of each element are present.

14. Hall © 2003 Prentice Hall © 2003 Chapter One 14 The formula for water is H 2 O. H 2 O indicates that two hydrogen and one oxygen combined together to produce water. When no subscript is given for an element a subscript of ‘1’ is understood.

15. Hall © 2003 Prentice Hall © 2003 Chapter One 15 1.6 Elements and the Periodic Table Periodic Table, shown below, is a representation of 113 elements in a tabular format.

16. Hall © 2003 Prentice Hall © 2003 Chapter One 16 Large amounts of information regarding the properties of elements is embedded in periodic table. Elements are roughly divided into 3 groups  Metals  Nonmetals  Metalloids

17. Hall © 2003 Prentice Hall © 2003 Chapter One 17 Metals, nonmetals, and metalloids appear in distinct places on the periodic table

18. Hall © 2003 Prentice Hall © 2003 Chapter One 18 Metals: 89 of the 113 elements are metals. They appears 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  Good conductor of electricity  Malleable.

19. Hall © 2003 Prentice Hall © 2003 Chapter One 19 Nonmetals: Appears on the right side of the Periodic Table. 17 elements are nonmetals. Nonmetals are poor conductor of heat and electricity. Out of these 17 nonmetal elements – Eleven are gases at room temperature (H, N, O, etc.) – Five are solids (sulfur) – One is a liquid (bromine).

20. Hall © 2003 Prentice Hall © 2003 Chapter One 20 Metalloids: Appears between metals on the left side and nonmetals on the right side on the periodic table. Their properties are between metals and nonmetals. Boron, silicon, arsenic are examples of some of the metalloids.

21. Hall © 2003 Prentice Hall © 2003 Chapter One 21 Chapter Summary  Chemistry is the study of matter.  Matter is anything that has mass and occupies space.  Physical change does not alter the chemical makeup of a substance. Change is reversible.  Chemical change alters chemical makeup of a substance. Change is irreversible.  Pure substances have uniform chemical composition and properties.

22. Hall © 2003 Prentice Hall © 2003 Chapter One 22 Chapter Summary Contd.  Composition and properties of a mixture may vary.  Substance that can be broken down into simpler substances is a chemical compound.  Substance that can not be broken down chemically into simpler substances is known as an element.  Elements are represented by one or two letter symbols. First letter is always capitalized and the second letter is always a lower case.

23. Hall © 2003 Prentice Hall © 2003 Chapter One 23 Chapter Summary Contd.  Chemical Formula is a notation for chemical compound to show how many atoms of each element are present.  Periodic Table is a representation of 113 elements in a tabular format.  Elements are roughly divided into 3 groups – Metals – Nonmetals – Metalloids

24. Hall © 2003 Prentice Hall © 2003 Chapter One 24 End of Chapter 1