Lecture 0201 The Atomic Nature of Matter © 2009, Prentice-Hall, Inc.

Atomic Theory of Matter The theory that atoms are the fundamental building blocks of matter reemerged in the early 19th century, championed by John Dalton. Figure 2.1 John Dalton (1766-1844)

Dalton's Postulates Each element is composed of extremely small particles called atoms. Figure 2.1 John Dalton (1766-1844) © 2009, Prentice-Hall, Inc.

Dalton's Postulates All atoms of a given element are identical to one another in mass and other properties, but the atoms of one element are different from the atoms of all other elements. Figure 2.1 John Dalton (1766-1844) © 2009, Prentice-Hall, Inc.

Dalton's Postulates Atoms of an element are not changed into atoms of a different element by chemical reactions; atoms are neither created nor destroyed in chemical reactions. Figure 2.1 John Dalton (1766-1844) © 2009, Prentice-Hall, Inc.

Dalton’s Postulates Compounds are formed when atoms of more than one element combine; a given compound always has the same relative number and kind of atoms. © 2009, Prentice-Hall, Inc.

Dalton’s Law of Multiple Proportions If two elements A and B combine to form more than one compound, the masses of B that can combine with a given mass of A are in the ratio of small whole numbers. Examples: Carbon Monoxide and Carbon Dioxide; Water and Hydrogen Peroxide. © 2009, Prentice-Hall, Inc.

Law of Constant Composition Joseph Proust (1754–1826) This is also known as the law of definite proportions. It states that the elemental composition of a pure substance never varies. © 2009, Prentice-Hall, Inc.

Law of Conservation of Mass The total mass of substances present at the end of a chemical process is the same as the mass of substances present before the process took place. © 2009, Prentice-Hall, Inc.

The Electron Figure 2.4 Streams of negatively charged particles were found to emanate from cathode tubes. J. J. Thompson is credited with their discovery (1897). © 2009, Prentice-Hall, Inc.

The Electron Figure 2.4 Thompson measured the charge/mass ratio of the electron to be 1.76  108 coulombs/g. © 2009, Prentice-Hall, Inc.

Millikan Oil Drop Experiment Once the charge/mass ratio of the electron was known, determination of either the charge or the mass of an electron would yield the other. Figure 2.5 © 2009, Prentice-Hall, Inc.

Millikan Oil Drop Experiment Robert Millikan (University of Chicago) determined the charge on the electron in 1909. Figure 2.5 © 2009, Prentice-Hall, Inc.

Milikan Oil Drop Experiment Trial 1: rdrop = 1.64 x 10 -4 cm E = 1.92 x 105 N/coul where N = unit of force F = ma

Milikan Oil Drop Experiment E = 1.92 x 107 g/coul Vdrop = 4/3 r 3 = 1.85 x 10 -11 cm3 E = (.851 g/cm3) x (1.85 x 10 -11 cm3) x (1coul/1.92x107g) = 8.0 x 10 -19 coul

Trial E 1 8.0 x 10-19 C 2 3.1 x 10-19 C 3 6.5 x 10-19 C 4 9.5 x 10-19 C

Trial E 1 5(1.6 x 10-19 C) 2 2(1.6 x 10-19 C) 3 4(1.6 x 10-19 C) 4 6(1.6 x 10-19 C)

Radioactivity Radioactivity is the spontaneous emission of radiation by an atom. It was first observed by Henri Becquerel. Marie and Pierre Curie also studied it. © 2009, Prentice-Hall, Inc.

Radioactivity Three types of radiation were discovered by Ernest Rutherford:  particles  particles  rays Figure 2.8 © 2009, Prentice-Hall, Inc.

The Atom, circa 1900 The prevailing theory was that of the “plum pudding” model, put forward by Thompson. It featured a positive sphere of matter with negative electrons imbedded in it. Figure 2.9 © 2009, Prentice-Hall, Inc.

Discovery of the Nucleus Ernest Rutherford shot  particles at a thin sheet of gold foil and observed the pattern of scatter of the particles. Figure 2.10 © 2009, Prentice-Hall, Inc.

The Nuclear Atom Since some particles were deflected at large angles, Thompson’s model could not be correct. Figure 2.11 © 2009, Prentice-Hall, Inc.

The Nuclear Atom Rutherford postulated a very small, dense nucleus with the electrons around the outside of the atom. Most of the volume of the atom is empty space. Figure 2.12 © 2009, Prentice-Hall, Inc.

Other Subatomic Particles Protons were discovered by Rutherford in 1919. Neutrons were discovered by James Chadwick in 1932. © 2009, Prentice-Hall, Inc.

Subatomic Particles Protons and electrons are the only particles that have a charge. Protons and neutrons have essentially the same mass. The mass of an electron is so small we ignore it. Table 2.1 © 2009, Prentice-Hall, Inc.