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MODELS OF THE ATOM A HISTORICAL PERSPECTIVE WHAT IS MATTER? Anything that has mass and takes up space If you did not know this definition, how would you describe matter? EARLY GREEK THEORIES 460 Democritus B.C. - Democritus thought matter could not be divided indefinitely. • This led to the idea of atoms in a void. • The term “atomos” means uncuttable or indivisible • He speculated that all matter was composed of atoms fire earth Aristotle air water 350 B.C - Aristotle modified an earlier theory that matter was made of four “elements”: earth, fire, water, air. Aristotle was wrong. However, his theory persisted for 2000 years. JOHN DALTON 1800 -Dalton proposed a modern atomic model based on experimentation not on pure reason. • • • • All matter is made of atoms. Atoms of an element are identical. Each element has different atoms. Atoms of different elements combine in constant ratios to form compounds. • Atoms are rearranged in reactions. • His ideas account for the law of conservation of mass (atoms are neither created nor destroyed) and the law of constant composition (elements combine in fixed ratios). DALTON’S BILLIARD BALL MODEL Every atom was a spherical hard sphere Each element was different and therefore had a different symbol J. J. THOMSON First to provide existence of electrons Used cathode ray tubes (remember Grade 9 science???) cathode ray tube Reasoned that electrons could be produced from electrodes of various metals; therefore all atoms contained electrons since atoms are electrically neutral they must also contain a positive charge PLUM PUDDING (CHOCOLATE CHIP COOKIE) MODEL OF THE ATOM Thomson postulated that an atom consists of a cloud of positive charge with negative charged electrons embedded randomly inside of it Chocolate chips are electrons embedded in a positive sphere ERNEST RUTHERFORD RUTHERFORD MOVIE Rutherford shot alpha () particles at gold foil. Zinc sulfide screen Thin gold foil Lead block Radioactive substance path of invisible -particles Most particles passed through. So, atoms are mostly empty space Some positive -particles deflected or bounced back! Thus, a “nucleus” is positive & holds most of an atom’s mass. Rutherford’s reaction to the experiment was like shooting a 15 inch shell at a piece of paper and having it bounce back at you. PLANETARY OR NUCLEAR MODEL Because of the observations through the gold foil experiment, Rutherford proposed a model where electrons “orbited” the nucleus. Rutherford named the positive charges in the nucleus as protons JAMES CHADWICK Worked with Rutherford to determine the masses of nuclei of different elements In experiments found that masses of nuclei were different than the sum of the masses of protons Concluded that nucleus also contains neutral charged particles called neutrons ATOMS UP UNTIL THIS POINT IN OUR LIVES Atoms consist of a 1. Nucleus – protons (+) (identifies atom) and neutrons (0) 2. Orbiting electrons (-) (determines chemical properties of atom) Size of nucleus is small compared to atom (page 137) Some atoms are different. They have different number of neutrons but same number of protons and electrons - isotopes ISOTOPE NOTATION isotope notation indicates the chemical symbol of the element symbol used and the isotope of the element Z - represents atomic number A - represents mass number (total number of protons and neutrons X - represents the chemical symbol Occur naturally in nature ISOTOPES Can also be written as element name and mass number Why don’t we indicate the atomic number? Ex. carbon-12 and carbon-14 Some isotopes are unstable and spontaneously decay releasing radioactive material such as alpha and beta particles etc. Homework page 142 #1-4,7 ARE THERE THINGS SMALLER THAN SUBATOMIC PARTICLES OF PROTONS, NEUTRONS AND ELECTRONS? tour of super collider PROBLEM WITH NUCLEAR MODEL Contradicted laws of physics where electron in motion must continuously release energy, thereby creating smaller orbits and eventually crashing into nucleus ELECTROMAGNETIC SPECTRUM Visible light is part of a broader spectrum called the electromagnetic spectrum. Type of radiation is dependant on the wavelength. The shorter the wavelength, the higher the frequency, resulting in more energy. All radiation travels at the speed of light =3.00x108 m/s in a vacuum BOHR’S MODEL • Electrons orbit the nucleus in “shells” • Electrons can be bumped up to a higher shell if hit by an electron or a photon of light. There are 2 types of spectra: continuous spectra & line spectra. It’s when electrons fall back down that they release a photon (unit of light energy). These jumps down from “shell” to “shell” account for the line spectra seen in gas discharge tubes (through spectroscopes). ATOMS ABSORB AND RELEASE ENERGY Atoms can absorb specific amounts of energy and release the same amount of energy Forms an emission spectrum, not a continuous spectrum ATOMIC SPECTRA Atomic spectra of elements Will find emission spectra in IR region, UV regions etc. depending on the amount of energy released BOHR’S RULES Bohr incorporated Rutherford’s planetary model but made some restrictions based on the spectra he observed 1) atoms have specific energy levels called stationary states (fixed circular orbit) 2) while in a specific energy state, the electrons do not emit energy 3) electrons can change orbits by emitting or absorbing specific quantities of energy PROBLEMS WITH BOHR’S MODEL Model only successfully explained oneelectron systems such as hydrogen, He+, Li2+,etc. Unable to explain emission spectra of atoms with two or more electrons LOOK AT ATOMS WITH MORE THAN ONE ELECTRON Atomic spectra of elements Sublevels within an energy level Large gaps and small gaps