Ms. Wiseman's Chemistry 1: Unit 2: Properties of Matter


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	Unit 2: Atomic Structure Guiding Questions: How do we know atoms exist? How do we know that electrons, protons, and neutrons exist? What is radiation and what does it come from? Is radiation safe? Where does matter come from? How are elements formed? Are all atoms of an element the same? What you should learn: Unit outline Because all scientific ideas depend on experimental and observational confirmation, all scientific knowledge is subject to change as new evidence becomes available. Scientific explanations must meet certain criteria: they must be consistent with experimental and observational evidence about nature and must make accurate predictions when appropriate about systems being studied. Atoms are made up of 3 subatomic particles and a lot of empty space; two particles make up the mass of the atom and are located in the nucleus and one, the electron, is located in the area outside of the nucleus. The ability to create a model and then make predictions that prove to be correct, based upon that model, is what science is all about. When elements are listed in order according to the number of protons, repeating patterns of physical and chemical properties result and can be used to make predictions Radiation is a natural, daily occurrence and can have both beneficial and negative impacts. Because atoms cannot, practically, be measured individually and because atoms of the same element can have different masses which occur in various proportions, the use of the weighted average Nuclear energy comes from the conversion of mass into energy as a result of unstable nuclei. This requires an adjustment to the conservation of energy and the conservation of mass to be the conservation of mass and energy. The color of light indicates the relative amount of energy of the light. Spectroscopic information can be used to identify elements because the amount of energy that can be absorbed or emitted is dependent on how much energy it takes to change the motion or position of a particle within an atom which is controlled by the atomic structure of the substance More Specifically...: Nature of Science and Evolution of Atomic Model Describe the contributions of Democritus and early Greek Philosophers, Dalton, Thompson, Millikan, and Rutherford on the structure of the atom. a. particles - Democritus b. first atomic theory of matter - John Dalton c. discovery of the electron - J. J. Thompson d. discovery of the nucleus - Ernest Rutherford e. discovery of charge of electron - Robert Millikan f. discovery of the neutron - James Chadwick Describe the contributions of Mendeleev and Mosley on the periodic table a. periodic table by atomic mass and property - Dimitri Mendeleev b. periodic table by atomic number - Henry Moseley Describe the experimental evidence that used to construct the principles of modern atomic theory. a. Laws of Conservation of Mass, Definite Composition, and Multiple Proportions b. Cathode ray experiment d. Gold Foil Experiment Define inference and give an example of how it was used in the development of the atomic model. Discuss the importance of a scientific model's ability to make accurate predictions. Matter Classification and the Periodic Table Use Law of Definite Composition to determine if two compounds are the same State and solve problems involving the law of conservation of mass Distinguish between chemical and physical properties Classify matter as mixture or pure substance, element or compound Associate rows in the periodic table with periods and columns with families or groups. Identify the seven diatomic gases Give locations and list characteristic properties of metals, non-metals, metalloids, and noble gases. Label the following areas on a periodic chart a. Alkali metals b. Alkaline Earth Metals c. Transition Metals d. Metalloids e. Halogens f. Noble gases g. Lanthanides h. Actinides Atomic Mass and Isotopes List the two particles that make up most of the mass of the atom Define atomic mass unit and explain how masses of atoms were first determined. Define isotope and explain why atomic masses are not whole numbers Write isotopes using isotope notation Use isotope notation to give the numbers of protons, neutrons and electrons Calculate atomic mass from isotope abundances. Explain the relationship between unstable nuclei and radioactive decay State that mass can be converted into energy and is the source of energy released in nuclear reactions. Distinguish between irradiation and contamination Distinguish between radiation and radioactivity Electrons Draw Bohr diagrams and indicate what happens to the electrons when light is absorbed and emitted. Relate emitted light to an element's characteristic spectra Lecture Notes: History of Atom, Reading Periodic Chart, Bohr Models Atomic Mass and Isotopes Notes Unstable Nuclei Notes Radiation Notes Half-Life Notes Nuclear Energy Radiation Packet Diatomic Gases Periodic Table Properties Regions of the Periodic Table Assignments: Independent Study Not all of it "How do we know?" Presentation Atomic History Text Frame Atomic # and Atomic Mass Global Warming Calculation of Atomic Mass Nuclear Pre-Assessment Isotopes and Average Atomic Mass Isotopic Abundances (Terrestrial) Radiation Dose Calculator Periodic Table Coloring Periodic Table Colors Atomic Structure Timeline Section 5.1 Notes Element Spectra Bohr Models Light Cartoons Black Light Glow-in-the-Dark Microwaves Night Vision Energy of Light Problems w/Answers Labs: Rutherford Lab Half-life lab Twizzler Half-Life Lab Fruit Loop Isotope Lab (Atomic Mass Calculation Simulation) Use flame tests to identify elements Element Spectra Lab Mendeleev Lab Cards Resources:
	Atomic Structure Quizzes Quiz Yourself: Number of Protons, Electrons, Neutrons Dalton's Atomic Theory Quiz Finding # of electron/proton/neutron problems History Atomic Structure Atomic Structure Timeline Rutherford experiment Atomic Structure Analogies Other Visual Elements How TV Screens Work (the old CRT kind) Radiation Therapy: Using Radioactivity to kill Cancer Cells Wikipedia: Ionizing Radiation Atomic Mass and Moles Quizzes and Practice WS Average Atomic Mass Problems Radioactive Decay Problems Mole Practice w/ Answers Mole Conversions Quiz Other Isotopic Abundances Periodic Trends The Periodic Table of Comic Books Periodic Table Regions Visual Elements Quizzes Periodic Trends Quiz Prentice Hall Self-test More Ion Quizzes Interesting Stuff: Why do we care about the size of an atom? (Atomic radius)? Because, radius tells us what kind of crystal structure a compound will have. The crystal structure determines the physical properties. How the Millitary used to dispose of sodium metal Cesium and Rubidium in water (on YouTube)
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