The Structure of the Atom Section 3.2
Introduction Atom: the smallest particle of an element that retains the chemical properties of that element Nucleus: very small region located at the center; composed of proton(s) and usually one or more neutrons Proton: a positively charged particle in the nucleus
More Neutron: a neutral particle found in the nucleus Electron: a negatively charged particle found in a region surrounding the nucleus Subatomic particles: protons, neutrons, and electrons
Discovery of the Electron A glass tube was prepared with a gas in it with metal disks at each end The cathode ray tube was connected to a vacuum pump because the charges will only flow through gases at low pressure An electric current was passed through various gases
More When the current was passed through the gas, the surface of the tube opposite the cathode (negative charge) glowed Also, the ray of light traveled from the cathode to the anode The rays were deflected away from a negatively charged object
More In 1897, J.J. Thomson used the cathode ray tube to deduce the presence of a negatively charged particle: the electron
Charge and Mass of the Electron Thomson’s experiment revealed that the electron has a very large charge-to-mass ratio In 1909, Robert Millikan measured the charge of the electron More accurate experiments were conducted later to determine the mass
Mass of the Electron Mass of the electron is 9.109 x 10-31kg The oil drop apparatus Robert Millikan
Thomson’s Model of the Atom Thomson’s model is called the plum pudding model His model is not valid He believed that the negative electrons were spread evenly throughout the positive charge of the rest of the atom
J. J. Thomson and his Model
Ernest Rutherford’s Gold Foil Experiment Alpha particles are helium nuclei - The alpha particles were fired at a thin sheet of gold foil Go
Rutherford’s Findings Most of the particles passed right through A few particles were deflected Some were greatly deflected “Like howitzer shells bouncing off of tissue paper
Conclusions of the Experiment The nucleus is small The nucleus is dense The nucleus is positively charged The atom is mostly empty space
Rutherford’s Model All the positive charge, and almost all the mass is concentrated in a small area in the center. He called this a nucleus The nucleus is composed of protons and neutrons (they make the nucleus!) The electrons are distributed around the nucleus, and occupy most of the volume His model was called a “nuclear model”
Other Discoveries Eugene Goldstein in 1886 observed what is now called the “proton” - particles with a positive charge, and a relative mass of 1 (or 1836 times that of an electron) 1932 – James Chadwick confirmed the existence of the “neutron” – a particle with no charge, but a mass nearly equal to a proton
Subatomic Particles Particle Relative Charge Relative mass Location Actual mass in kg Electron (e-) -1 __1__ 1836 electron cloud 9.109 x 10-31 Neutron (n0) 1 nucleus 1.675 x 10-27 Proton (p+) +1 1.673 x 10-27
Other Interesting Stuff Atoms are electrically neutral because they contain an equal number of protons and electrons The number of protons determines the atom’s identity There are other subatomic particles, but they have little effect on the chemical properties of matter
Forces in the Nucleus Protons, with their positive charge, would be expected to repel each other in the nucleus When they are extremely close to each other, there is a strong attraction A similar attraction exists when neutrons are present
More Nuclear forces: the interaction that binds protons and neutrons, protons and protons, and neutrons and neutrons together in a nucleus Nuclei are very dense
Sizes of Atoms Electrons occupy the outer region known as the electron cloud Radius of an atom is the distance from the center of the nucleus to the outer portion of the electron cloud Atomic radii are extremely small so they are usually measured in picometers 1 x 1012 pm = 1 m