1. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu 8/14/15 Notes Chapter 1-1 Section 1 What Is Chemistry? Chapter 1

2. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Working with the Properties and Changes of Matter Chemistry is the study of chemicals and the changes chemicals can undergo. A chemical is any substance that has a definite composition. A chemical reaction is the process by which one or more substances change to produce one or more new substances. Chemical reactions are necessary for living things to grow and for dead things to decay. Section 1 What Is Chemistry? Chapter 1

3. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Visual Concepts Chemical Chapter 1

4. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Physical States of Matter The states of matter are the physical forms of matter. There are different states of matter: solid, liquid, gas, and plasma. Macroscopic refers to what you can see with the unaided eye. Microscopic refers to what you would see if you could see individual atoms. Section 1 What Is Chemistry? Chapter 1

5. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Physical States of Matter, continued Properties of the Physical States Solids have a fixed volume and shape that result from the way their particles are arranged. Liquids have a fixed volume but not a fixed shape. Gases have neither fixed volume nor shape. Plasma is a gas whose particles have broken apart and are charged. (space) Section 1 What Is Chemistry? Chapter 1

6. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Visual Concepts Solid, Liquid and Gas Chapter 1

7. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Water in Three States Section 1 What Is Chemistry? Chapter 1

8. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Changes of Matter All matter is made of particles. This matter can change. Physical changes are changes in which the identity of a substance doesn’t change. The arrangement, location, and speed of the particles may change. Changes of state are physical changes. Chemical changes occur when the identities of substances change and new substances form. Section 1 What Is Chemistry? Chapter 1

9. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Changes of Matter, continued Chemical Changes mercury(II) oxide  mercury + oxygen Reactants are the substances that are on the left- hand side of the arrow. (what we start with) They are used up in the reaction. Products are the substances that are on the right- hand side of the arrow. (what we end up with) They are made in the reaction. Section 1 What Is Chemistry? Chapter 1

10. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Changes of Matter, continued Evidence of a Chemical Change Evidence that a chemical change may be happening generally falls into one of the following categories. the evolution of a gas: gas is produced (normally with bubbles and/or odor the formation of a precipitate: solid forms from two liquids the release or absorption of energy: such as a change in temperature or the giving off of light energy a color change in the reaction system Section 1 What Is Chemistry? Chapter 1

11. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Evidence of a Chemical Change Section 1 What Is Chemistry? Chapter 1

12. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Visual Concepts Chemical Reaction Chapter 1

13. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Matter Has Mass and Volume Matter is anything that has mass and volume. Section 2 Describing Matter Chapter 1

14. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Is photosynthesis, in which light energy is captured by plants to make sugar from carbon dioxide and water, a physical change or a chemical change? Explain your answer. Standardized Test Preparation Quick Write 8/14/15 Chapter 1

15. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu 1. A chemical is any substance that has [definite, indefinite] composition. 2. The type and arrangement of [particles, crystals] in a sample of matter determine the properties of the matter. 3. The characteristics of a solid include [fixed, variable] volume and shape. Particles that make up solids are held [loosely, tightly] in a [flexible, rigid] structure, so the particles can [vibrate only slightly, flow past each other]. 4. Liquids have a [fixed, variable] volume but a [fixed, variable] shape. This situation occurs because particles in a liquid are held [tightly, loosely] and [can, cannot] slip past each other. 5. Gases have [fixed, variable] volume and [fixed, variable] shape. Gas particles may move apart to fill any container they occupy. Standardized Test Preparation Classwork 8/14/15-Part A Chapter 1

16. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu 8/17/15 Notes Chapter 1 Section 2 Section 1 What Is Chemistry? Chapter 1

17. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Matter Has Mass and Volume Matter is anything that has mass and volume. Volume is the space an object occupies. Mass is the quantity of matter in an object. Devices used for measuring mass in a laboratory are called balances. Weight is the force produced by gravity acting on a mass. Section 2 Describing Matter Chapter 1

18. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Visual Concepts Comparing Mass and Weight Chapter 1

19. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Units of Measurement When working with numbers, be careful to distinguish between a quantity and its unit. Quantity describes something that has magnitude, size, or amount. Unit is a quantity adopted as a standard of measurement. Section 2 Describing Matter Chapter 1

20. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Units of Measurement, continued Scientist Express Measurements in SI Units Scientists worldwide use a set of units called the Système Internationale d’Unités or SI. Section 2 Describing Matter Chapter 1

21. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Units of Measurement, continued Scientist Express Measurements in SI Units, continued Base units can be too large or too small for some measurements, so the base units may be modified by attaching prefixes. Section 2 Describing Matter Chapter 1

22. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Section 2 Describing Matter Unit of Measurement, continued Converting One Unit to Another A conversion factor is a simple ratio that relates two units that express a measurement of the same quantity. example: You can construct conversion factors between kilograms and grams as follows: Chapter 1

23. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Section 2 Describing Matter Converting Units Sample Problem A Convert 0.851 L to milliliters. Chapter 1

24. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Sample Problem A Solution The equality that links the two units is 1000 mL = 1 L. (The prefix milli- represents 1/1000 of a base unit.) The conversion factor needed must cancel liters and leave milliliters. Thus, liters must be on the bottom of the fraction and milliliters must be on the top. Section 2 Describing Matter Chapter 1

25. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Derived Units, continued Volume is another commonly used derived unit. Volume can be found by multiplying length, width, and height. The unit of volume is the cubic meter (m 3 ). This unit is too large and inconvenient in most labs. Chemists usually use the liter (L). 1L = 1000 mL = 1000 cm 3 Section 2 Describing Matter Chapter 1

26. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Properties of Matter, continued Density is the Ratio of Mass to Volume The density of an object is the mass of the object divided by volume of the object. Densities are expressed in derived units such as g/cm 3 or g/mL. Density is calculated as follows: Section 2 Describing Matter Chapter 1

27. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Properties of Matter, continued Density of an Object The density of a substance is the same no mater what the size of the sample is. Section 2 Describing Matter Chapter 1

28. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Properties of Matter, continued Density of an Object A sample of bismuth has a mass of 342 g and a volume of 1.64 cm 3. What is the density of bismuth? Section 2 Describing Matter Chapter 1

29. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Properties of Matter, continued Density Can Be Used to Identify Substances Because the density of a substance is the same for all samples, you can use this property to help identify substances. Section 2 Describing Matter Chapter 1

30. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Properties of Matter, continued Chemical Properties A chemical property a property of matter that describes a substance’s ability to participate in chemical reactions. A chemical property of many substances is that they react with oxygen. example: rusting Some substances break down into new substances when heated. Section 2 Describing Matter Chapter 1

31. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Visual Concepts Comparing Physical and Chemical Properties Chapter 1

32. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu 8/18/15 Notes Chapter 1 Section 3 Section 1 What Is Chemistry? Chapter 1

33. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Classifying Matter An atom is the smallest unit of an element that maintains the properties of that element. Matter exists in many different forms but there are only 110 types of atoms. Atoms are joined together to make up all the different kinds of matter. Section 3 How Is Matter Classified? Chapter 1

34. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Pure Substances A pure substance is a sample of matter, either a single element or a single compound, that has definite chemical and physical properties. Elements are pure substances that only contain one kind of matter. They cannot be separated or broken down into simpler substances by chemical means. Each element has its own unique set of physical and chemical properties. Section 3 How Is Matter Classified? Chapter 1

35. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Pure Substances Section 3 How Is Matter Classified? Chapter 1

36. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Elements are Pure Substances Each elements is represented by a distinct chemical symbol. Section 3 How Is Matter Classified? Chapter 1

37. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Pure Substances, continued Elements as Single Elements or Molecules A molecule is the smallest unit of a substance that keeps all of the physical and chemical properties of that substance. A molecule usually consists of two or more atoms combined in a definite ratio. Diatomic elements exist as two atoms of the same element joined together. Section 3 How Is Matter Classified? Chapter 1

38. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Pure Substances, continued Compounds are Pure Substances Pure substances that are not elements are compounds. Compounds are composed of more than one kind of atom. example: carbon dioxide (CO 2 ) There may be easier ways of preparing them, but compounds can be made from their elements. Compounds can be broken down into their elements, though often with great difficulty. Section 3 How Is Matter Classified? Chapter 1

39. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Pure Substances, continued Compounds are Represented by Formulas Because every molecule of a compound is made up of the same kinds of atoms arranged the same way, a compound has characteristic properties and composition. Compounds can be represented by an abbreviation or formula. A formula has subscripts which represent the ratio of different atoms in the compound. example: H 2 O has 2 hydrogen atoms and one oxygen atom Section 3 How Is Matter Classified? Chapter 1

40. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Pure Substances, continued Compounds are Represented by Formulas, continued Molecular formulas give information only about what makes up a compound. example: the molecular formula for aspirin is C 9 H 8 O 4 A structural formula shows how the atoms are connected This two-dimensional model does not show the molecule’s true shape. Section 3 How Is Matter Classified? Chapter 1

41. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Pure Substances, continued Compounds are Represented by Formulas, continued A ball-and-stick model shows the distances between atoms and the angles between them in three dimensions. A space-filling model attempts to represent the actual sizes of the atoms and not just their relative positions. A hand-held model can provide more information than models shown on the flat surface of the page. Section 3 How Is Matter Classified? Chapter 1

42. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Pure Substances, continued Compounds are Represented by Formulas, continued These models convey different information about acetylsalicylic acid (aspirin). Section 3 How Is Matter Classified? Chapter 1

43. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Mixtures A mixture is a combination of two or more substances that are not chemically combined. Air is a mixture of mostly nitrogen and oxygen. All the different gases in air are physically mixed. The proportions of the gases can vary. Water is not a mixture. The H and O atoms are chemically bonded The ratio of H to O atoms is always 2 to 1. Section 3 How Is Matter Classified? Chapter 1

44. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Mixtures, continued Mixtures Can Vary in Composition and Properties The proportion of the materials in a mixture can change. The properties of the mixture may vary. An alloy is a solid mixture. example: An alloy of gold and other metal atoms is stronger than pure gold. 18-karat gold contains 18 grams of gold per 24 grams of alloy. 14-karat gold contains 14 grams of gold per 24 grams of alloy. Section 3 How Is Matter Classified? Chapter 1

45. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Particle Models for Gold and Gold Alloy Chapter 1

46. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Mixtures, continued Homogenous Mixtures A homogenous mixture describes something that has uniform structure or composition throughout. examples: gasoline, syrup, and air Because any two samples of a homogenous mixture will have the same proportions of ingredients, homogenous mixtures have the same properties throughout. Section 3 How Is Matter Classified? Chapter 1

47. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Mixtures, continued Heterogeneous Mixtures A heterogeneous mixture describes something that is composed of dissimilar components. example: A mixture of sand and water is a heterogenous mixture. Any two samples of a heterogeneous mixture will have the different proportions of ingredients. Heterogeneous mixtures have different properties throughout. Section 3 How Is Matter Classified? Chapter 1

48. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Examples of Mixtures Mixtures are either homogenous or heterogeneous. Section 3 How Is Matter Classified? Chapter 1

49. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Types of Mixtures Chapter 1 Section 3 How Is Matter Classified?

50. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Mixtures, continued Distinguishing Mixtures from Compounds The properties of a mixture reflect the properties of the substances it contains. The properties of a compound often are very different from the properties of the elements that make it up. A mixture’s components can be present in varying proportions. A compound has a definite composition in terms of the masses of its elements. Section 3 How Is Matter Classified? Chapter 1

51. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Classifying Matter Chapter 1 Section 3 How Is Matter Classified?

52. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu T/F 8. The terms odorless and colorless are quantitative terms. T/ F 9. To say that the mass of a gold nugget is 5.0 grams is to use a quantitative term. T/F 10. The kelvin is used to express length in SI. T/F 11. The pound is used to express forces such as weight in SI. T/F 12. The liter is used to express volume in SI. Calculate- 13. How many millimeters are there in 2.0 meters? Standardized Test Preparation Classwork 8/18/15 Part A Chapter 1

53. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Pg. 28 #3-9, 13-14 Standardized Test Preparation Classwork 8/18/15 Part B Chapter 1