Chapter 2: The Atomic Nature of Matter Olmsted and Williams, 3 rd Edition
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1 Chapter 2: The Atomic Nature of Matter Olmsted and Williams, 3 rd Edition HW: 5, 7, 10, 13, 15, 17, 19, 22, 23, 27, 30, 31, 35, 36, 41, 42, 59, 63, 69, 70 Atomic Theory and How It Came About Aristotle believed that substances appeared uniform in composition BC In contrast Leucippus and Democritus believed that every substance is made up of tiny blocks that have distinct properties of their own BC Since there was no experimental evidence of tiny blocks (atoms), Aristotle s view was accepted for the next 2000 years It was not until John Dalton ( ) that the modern atomic theory was developed and accepted He realized that fixed proportions result if matter is made up of indivisible atoms.
2 Modern View of Atomic Theory 1. All matter is composed of tiny particles called atoms. 2. All atoms of a given element have identical chemical properties that are characteristic of that element. 3. Atoms form chemical compounds by combining the whole number ratios. 4. Atoms can change how they are combined, but they are neither created or destroyed in chemical reactions. Conservation of Atoms and Mass Molecular picture of the reaction of methane (CH 4 ) with oxygen (O 2 ) to produce carbon dioxide (CO 2 ) and water (H 2 O). Atoms of each element are conserved. What happened to the matter (wood)?
3 Atoms Combine to Make Molecules A molecular view of several oxygen molecules reacting with hydrogen molecules to form water. Note that atoms are conserved. Fig 2-7 Pg 44 Atomic pictures of a monatomic solid(left), liquid(center), and gas(right), showing how atoms move about in each phase. Dynamic Molecular Equilibrium
4 Forces Fig 2-11 Pg 46 Charged objects are attracted to one another if the charges have opposite signs. However, charged objects of the same sign, either both positive or both negative, repel one another. Gravitational Electrical Magnetic Do Atoms Have an Inner Structure? How would you determine that? Schematic drawing of a gas discharge tube in operation. When a very high voltage is applied to the two perforated plates, an electrical discharge occurs between them. The positively charged particles that form in the gas then move in opposite directions. What does a proton say to an electron? How do electrons behave around one another?
5 Fig 2-14 Pg 48 Schematic drawing of a cathode ray tube. An electrical discharge generates electrons. These negative electrons form a beam. A pair of charged plates deflects the beam (bent line), but if a magnetic force is also imposed, it is possible to counterbalance the effect of the electric force (straight line). From the cathode ray tube, Thomson was able to calculate the ratio of the electron s charge to its mass Charge Mass Fig 2-15 Pg 48 Schematic view of Millikan s Oil drop experiment. An atomizer generated a fine mist of oil droplets(yellow circles). Xrays gave some droplets extra charge (orange circles). In the presence of sufficient electrical force, these negatively charged droplets could be suspended in space.
6 Fig 2-16 Pg 49 Schematic view of Rutherford s scattering experiment. When a beam of positively charged helium particles was shot at a thin gold foil, most of them passed through without much effect.some, however, were reflected backward. Fig 2-17 Pg 50 Schematic drawing of an atom, showing a central, positive nucleus surrounded by a cloud of electrons. This model of the atom is consistent with the results of Rutherford s scattering experiments. Atomic Building Blocks Name Symbol Charge Mass (kg) Electron e x x Proton p x x Neutron n x 10-27
7 Every element has a unique nuclear charge and a specific and unchanging number of protons The number of protons in a nucleus is the atomic number Symbolized by the letter Z. What is the atomic number of zinc? Mass Number What two things in the atom actually have mass? Protons and neutrons These two make up the mass number symbolized by the letter A. Mass Number Atomic Number A Z X Elemental Symbol
8 Isotopes Atoms with the same number of protons but with different numbers of neutrons Pg 52 The titanium in TiO 2, the white solid used to make white paint opaque, has the same isotopic composition as the titanium metal in artificial knee joints. Courtesy of Sachtleben Chemie GmbH (Paint) Courtesy M. Freeman/PhotoLink/Phoyo Disc (Knee Joint) 46 Ti = 8.2% 47 Ti = 7.4% 48 Ti = 73.8% 49 Ti = 5.4% 50 Ti = 5.2% Fig 2-18 Pg 53 The natural abundances of the isotopes of four elements (Cl,Cr,Ge, and Sn) illustrate the diversity of isotopic distributions. The mass number and percent abundance of each isotope are indicated.
9 Atomic Weight The atomic weight of an element is weighted average of the masses of the isotopes which should be approximately the same as its mass number Ions Atoms are neutral - meaning that the number of protons is equal to the number of electrons If an atom loses or gains electron(s), the atom is no longer neutral. It now has a charge on it This is an ion!! Question: Are the protons and electrons equal now? Periodic Table
10 What are monatomic ions? Single atoms that have lost or gained electrons
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