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1 CHEMISTRY & YOU Chapter 4 Atomic Structure 4.1 Defining the Atom 4.2 Structure of the Nuclear Atom How did scientists determine the structures that are inside an atom? X-rays are used to see structures that cannot be seen through your skin. 4.3 Distinguishing Among Atoms 1 Copyright Pearson Education, Inc., or its affiliates. All Rights Reserved. 2 Copyright Pearson Education, Inc., or its affiliates. All Rights Reserved. Subatomic Particles How were the three subatomic particles discovered? Disproving Dalton s Atomic Theory Atoms are now known to be divisible. Subatomic particles Protons, neutrons, electrons, etc. However, this was not always the case. 3 Copyright Pearson Education, Inc., or its affiliates. All Rights Reserved. 4 Copyright Pearson Education, Inc., or its affiliates. All Rights Reserved English physicist J. J. Thomson are negatively charged subatomic particles. Experiments involved passing electric current through gas samples Sealed gases in glass tubes with 2 electrodes. Electrodes connected to electricity. 5 dwb.unl.edu/.../demos/jpeg/cath7.jpg Copyright Pearson Education, Inc., or its affiliates. All Rights Reserved. 6 Copyright Pearson Education, Inc., or its affiliates. All Rights Reserved. 1
2 The result was a glowing beam, or cathode ray, that traveled from the cathode to the anode. 7 Copyright Pearson Education, Inc., or its affiliates. All Rights Reserved. 8 Copyright Pearson Education, Inc., or its affiliates. All Rights Reserved. Cathode ray deflected by external, electrically charged metal plates. Positively charged plate attracts the cathode ray Negatively charged plate repels it. 9 Copyright Pearson Education, Inc., or its affiliates. All Rights Reserved. A cathode ray can also be deflected by a magnet. 10 Copyright Pearson Education, Inc., or its affiliates. All Rights Reserved. From his experiments, Thomson hypothesized that a cathode ray is composed of tiny negatively charged particle Later named electrons To test his hypothesis, Thompson set up an experiment to measure the charge:mass ratio of the particles (electrons). Found charge:mass ratio to be constant. The ratio did not change if: Hypothesis: cathode ray is composed of tiny negatively charged particle the kind of gas in the cathode-ray tube was changed the type of metal used for the electrodes was changed 11 Copyright Pearson Education, Inc., or its affiliates. All Rights Reserved. 12 Copyright Pearson Education, Inc., or its affiliates. All Rights Reserved. 2
3 Concluded that e- are a component of the atoms of all elements U.S. physicist Robert A. Millikan Discovered the quantity of an electron s charge. Oil drop experiment www-news.uchicago.edu 13 Copyright Pearson Education, Inc., or its affiliates. All Rights Reserved. 14 Copyright Pearson Education, Inc., or its affiliates. All Rights Reserved. Suspended negatively charged oil droplets between charged plates. Changed voltage on the plates to see how this affected the droplets rate of fall. www-news.uchicago.edu Millikan found the charge of an electron (1.60 x coulomb (C)) Using this charge and Thomson s charge:mass ratio, Millikan calculated an electron s mass. electron = one unit of negative charge Mass = 1/1840 the mass of a hydrogen atom. 15 Copyright Pearson Education, Inc., or its affiliates. All Rights Reserved. 16 Copyright Pearson Education, Inc., or its affiliates. All Rights Reserved. Four ideas about matter and electric charges. 1. Atoms have no net electric charge; they are electrically neutral. 2. Electric charges are carried by particles of matter. 3. Electric charges always exist in whole-number multiples (there are no fractions of charges). 4. If the number of + particles (protons) = number of particles (electrons), the particle (atom) is electrically neutral. If matter is electrically neutral, but we know that negative particles (electrons) exist, then.. There must be something else there to balance it out that is opposite in charge 17 Copyright Pearson Education, Inc., or its affiliates. All Rights Reserved. 18 Copyright Pearson Education, Inc., or its affiliates. All Rights Reserved. 3
4 1886 Eugen Goldstein Found rays reverse cathode rays. Concluded they were composed of + particles (protons) Other scientists contributed to the discovery of protons 1932 (much later) English physicist James Chadwick Protons did not account for the whole mass of an atom Hypothesized that there must be some other particle confirmed the existence of the neutron w/his mentor (Rutherford) physics/laureates/1935/chadwick-bio.html Neutrons: subatomic particles with no charge; but with a mass nearly equal to that of a proton Copyright Pearson Education, Inc., or its affiliates. All Rights Reserved. 20 Copyright Pearson Education, Inc., or its affiliates. All Rights Reserved. Interpret Data Properties of Subatomic Particles Particle Symbol Relative charge Relative mass (amu) (mass of proton = 1) Actual mass (g) Electron e 1 1/ x Proton p x Neutron n x Theoretical physicists believe that these subatomic particles are composed of yet smaller subnuclear particles called quarks. The Atomic Nucleus Although scientists now knew protons, neutrons, and electrons existed, they still did not know how they were arranged in the atom. 21 Copyright Pearson Education, Inc., or its affiliates. All Rights Reserved. 22 Copyright Pearson Education, Inc., or its affiliates. All Rights Reserved. Plum Pudding Model (Thomson) stuck into a lump of positive charge. Ernest Rutherford, New Zealand Student of Thomson Advisor to Chadwick, Bohr, Moseley Colleagues with Geiger Nobel Prize for Chemistry quantised_world/structure-1.html 23 Copyright Pearson Education, Inc., or its affiliates. All Rights Reserved. 24 Copyright Pearson Education, Inc., or its affiliates. All Rights Reserved. 4
5 1911 tested the existing plum-pudding model of atomic structure. α- particles Gold-foil experiment: Shot alpha particles (helium nucleii) at gold foil 25 Copyright Pearson Education, Inc., or its affiliates. All Rights Reserved. 26 Copyright Pearson Education, Inc., or its affiliates. All Rights Reserved. If the plum pudding model (theory) were correct, what would the results have been? Actual Results: most alpha particles went straight through, or were slightly deflected. The plum pudding model couldn t be true. 27 Copyright Pearson Education, Inc., or its affiliates. All Rights Reserved. 28 Copyright Pearson Education, Inc., or its affiliates. All Rights Reserved. Rutherford disproved Thomson s Plum Pudding Theory, Suggested the Nuclear Model of the Atom The atom is mostly empty space with a small, dense, positively charged solid center. The electrons must be distributed around the nucleus and occupy almost all the volume of the atom. 29 Copyright Pearson Education, Inc., or its affiliates. All Rights Reserved. 30 Copyright Pearson Education, Inc., or its affiliates. All Rights Reserved. 5
6 Rutherford s model turned out to be incomplete. It had to be revised in order to explain the chemical properties of elements observed in coming years. 31 Copyright Pearson Education, Inc., or its affiliates. All Rights Reserved. 32 Copyright Pearson Education, Inc., or its affiliates. All Rights Reserved. 6
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Chemistry Made by Saleem Abu-Tayeh Chapter 4 - Many philosophers concluded that matter was composed of things such as earth, water, air, and fire. It was also commonly accepted that matter could be endlessly