Instructor’s Resource Materials (Download only) for Chemistry for Changing Times, 14/e John W. Hill, Terry W. McCreary © 2016 Pearson Education, Inc. John.

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Instructor’s Resource Materials (Download only) for Chemistry for Changing Times, 14/e John W. Hill, Terry W. McCreary © 2016 Pearson Education, Inc. John Singer, Jackson Community College Chemistry for Changing Times, Fourteenth Edition Lecture Outlines Chapter 2 Atoms

Instructor’s Resource Materials (Download only) for Chemistry for Changing Times, 14/e John W. Hill, Terry W. McCreary © 2016 Pearson Education, Inc. Learning Objectives Explain the ancient Greeks’ ideas about the characteristics of matter. (2.1) Describe the significance of the laws of conservation of mass and definite proportions. (2.2) Calculate the amounts of elements from the composition of a compound. (2.2) Explain why the idea that matter is made of atoms is a theory. (2.3)

Instructor’s Resource Materials (Download only) for Chemistry for Changing Times, 14/e John W. Hill, Terry W. McCreary © 2016 Pearson Education, Inc. Know how atomic theory explains the laws of multiple proportions and conservation of mass. (2.3) Describe what a mole is and how it is used. Convert between the masses and the moles of a substance. Describe how the elements are arranged in the periodic table and why the arrangement is important. (2.4) Learning Objectives

Instructor’s Resource Materials (Download only) for Chemistry for Changing Times, 14/e John W. Hill, Terry W. McCreary © 2016 Pearson Education, Inc. Distinguish atoms from molecules. (2.5) Identify elements that could be classified as hazardous or rare. Explain how green chemistry can change technologies that rely on hazardous or rare elements. Learning Objectives

Instructor’s Resource Materials (Download only) for Chemistry for Changing Times, 14/e John W. Hill, Terry W. McCreary © 2016 Pearson Education, Inc. Atoms: The Greek Idea ~384 B.C.E., Aristotle: All matter is composed of four elements and all matter is continuous, not atomistic.

Instructor’s Resource Materials (Download only) for Chemistry for Changing Times, 14/e John W. Hill, Terry W. McCreary © 2016 Pearson Education, Inc. Atoms: The Greek Idea ~ 450 B.C.E., Leucippus and Democritus Atomos: The point at which matter can no longer be subdivided.

Instructor’s Resource Materials (Download only) for Chemistry for Changing Times, 14/e John W. Hill, Terry W. McCreary © 2016 Pearson Education, Inc. Lavoisier: The Law of Conservation of Mass Early 1700s Lavoisier Law of conservation of mass: During a chemical change, matter is neither created nor destroyed.

Instructor’s Resource Materials (Download only) for Chemistry for Changing Times, 14/e John W. Hill, Terry W. McCreary © 2016 Pearson Education, Inc. Lavoisier: The Law of Conservation of Mass

Instructor’s Resource Materials (Download only) for Chemistry for Changing Times, 14/e John W. Hill, Terry W. McCreary © 2016 Pearson Education, Inc. Proust: The Law of Definite Proportions 1799, Proust Law of definite proportions: A compound always contains the same elements in certain definite proportions.

Instructor’s Resource Materials (Download only) for Chemistry for Changing Times, 14/e John W. Hill, Terry W. McCreary © 2016 Pearson Education, Inc. Proust: The Law of Definite Proportions Regardless of the source, copper carbonate always has the same composition.

Instructor’s Resource Materials (Download only) for Chemistry for Changing Times, 14/e John W. Hill, Terry W. McCreary © 2016 Pearson Education, Inc. Proust: The Law of Definite Proportions The Berzelius experiment illustrates the law of definite proportions.

Instructor’s Resource Materials (Download only) for Chemistry for Changing Times, 14/e John W. Hill, Terry W. McCreary © 2016 Pearson Education, Inc. John Dalton and the Atomic Theory of Matter 1803, John Dalton Law of multiple proportions: Elements may combine in more than one set of proportions, with each set corresponding to a different compound.

Instructor’s Resource Materials (Download only) for Chemistry for Changing Times, 14/e John W. Hill, Terry W. McCreary © 2016 Pearson Education, Inc. John Dalton and the Atomic Theory of Matter

Instructor’s Resource Materials (Download only) for Chemistry for Changing Times, 14/e John W. Hill, Terry W. McCreary © 2016 Pearson Education, Inc. John Dalton and the Atomic Theory of Matter All matter is composed of extremely small particles called atoms. All atoms of a given element are alike and differ from the atoms of any other element. Compounds are formed when atoms of different elements combine in fixed proportions. A chemical reaction involves the rearrangement of atoms.

Instructor’s Resource Materials (Download only) for Chemistry for Changing Times, 14/e John W. Hill, Terry W. McCreary © 2016 Pearson Education, Inc. Isotopes Much of John Dalton’s atomic theory has been modified. For example, John Dalton assumed that all atoms of an element are alike. He did not understand the existence of isotopes. Isotopes are atoms of the same element with different relative masses.

Instructor’s Resource Materials (Download only) for Chemistry for Changing Times, 14/e John W. Hill, Terry W. McCreary © 2016 Pearson Education, Inc. The Mole and Avogadro’s Number A mole is the number of atoms in grams of Carbon-12. That number is x atoms and is often referred to as Avogadro’s Number.

Instructor’s Resource Materials (Download only) for Chemistry for Changing Times, 14/e John W. Hill, Terry W. McCreary © 2016 Pearson Education, Inc. Molar Mass The mass, in grams, of one mole of a substance is known as the molar mass. This value is the sum of the atomic masses of the elements in a compound. For instance, the molar mass of water, H 2 O, is 18.0 grams or 18.0 g/mol.

Instructor’s Resource Materials (Download only) for Chemistry for Changing Times, 14/e John W. Hill, Terry W. McCreary © 2016 Pearson Education, Inc. The Mole and Avogadro’s Number

Instructor’s Resource Materials (Download only) for Chemistry for Changing Times, 14/e John W. Hill, Terry W. McCreary © 2016 Pearson Education, Inc. Out of Chaos: The Periodic Table 1869, Dmitri Mendeleev Mendeleev arranged the elements in order of increasing atomic mass. He left gaps for yet undiscovered elements. He also predicted the properties of those elements. When those elements were eventually discovered, many of his predictions were found to be accurate.

Instructor’s Resource Materials (Download only) for Chemistry for Changing Times, 14/e John W. Hill, Terry W. McCreary © 2016 Pearson Education, Inc. Out of Chaos: The Periodic Table

Instructor’s Resource Materials (Download only) for Chemistry for Changing Times, 14/e John W. Hill, Terry W. McCreary © 2016 Pearson Education, Inc. Out of Chaos: The Periodic Table

Instructor’s Resource Materials (Download only) for Chemistry for Changing Times, 14/e John W. Hill, Terry W. McCreary © 2016 Pearson Education, Inc. Atoms: Real and Relevant Atoms are a very real concept. It is even possible to observe computer-enhanced images of atoms.

Instructor’s Resource Materials (Download only) for Chemistry for Changing Times, 14/e John W. Hill, Terry W. McCreary © 2016 Pearson Education, Inc. Green Chemistry Green Chemistry means replacing rare or hazardous substances with more abundant or less hazardous substances.

Instructor’s Resource Materials (Download only) for Chemistry for Changing Times, 14/e John W. Hill, Terry W. McCreary © 2016 Pearson Education, Inc. Green Chemistry One example of green chemistry technology is the replacement of mercury fluorescent light bulbs with efficient mercury-free light bulbs.