It is one of two elements with Z < 83 that have no stable isotopes the other element is promethium (Z = 61). All the isotopes of technetium are radioactive. Twenty-two isotopes of technetium with masses ranging from 90 to 111 are reported. Technetium has been found in the spectrum of S-, M-, and N-type stars, and its presence in stellar matter is leading to new theories of the production of heavy elements in the stars. If it does exist, the concentration must be very small. Finally in 1962, technetium-99 was isolated and identified in African pitchblende (a uranium rich ore) in extremely minute quantities as a spontaneous fission product of uranium-238 by B.T. Since its discovery, searches for the element in terrestrial material have been made. Technetium was the first element to be produced artificially. Lawrence that was bombarded by deuterons in the Berkeley cyclotron. It was also found in a sample of molybdenum sent by E. The element was actually discovered by Perrier and Segre in Italy in 1937. Element 43 was predicted on the basis of the periodic table, and was erroneously reported as having been discovered in 1925, at which time it was named masurium. Connect topics discussed in lecture and lab observations.Back to Elements List Technetium Atomic Number:ħ, 6, 5, 4, 3, 2, 1, −1, −3 (a strongly acidic oxide)įrom the Greek word technetos, artificial.Use basic lab equipment including: balance, hot plate and thermometer.Use volumetric glassware, including a buret.The formal lab report must include good data analysis. Students will write 1 formal lab report using proper scientific analytical writing.Utilize spreadsheets to graph (plot) and analyze data and do basic error analysis.Students will perform a minimum of 2 wet labs using a lab notebook.The notebook needs to include an introduction, procedure, data table and conclusion. Utilize notebook skills (especially data acquisition, data handling and data analysis).Make measurements using the correct number of significant figures.Properly handle and dispose of chemicals.Wear Splash resistant goggles, proper clothing and closed toed shoes. Perform a minimum of 8 "wet" supervised hands-on labs per semester.Explain the difference between real and ideal gases. Use the Gas laws to do gas law calculations. Distinguish between endothermic and exothermic processes and do energy calculations that accompany reactions. Use Hess's law and enthalpies of formation to calculate heats of reactions.Perform calorimetry calculations. Describe and employ basic Thermochemistry.Apply hybrid orbital theory to predict hybridization and explain pi and sigma bonding.Draw Lewis structures for covalent compounds and use VSEPR concepts to predict: a) bond angles b) geometry c) polarity.Apply formal charge to understand resonance and determine the best Lewis structure.Differentiate between ionic, polar covalent and covalent bonds.Recognize the periodic properties of electronegativity, electron affinity, ionization energy, and ionic or covalent radius from the position of the element in the Periodic Table.Explain quantum numbers and apply quantum numbers to depict electron configurations of neutral atoms and ions Show how light and spectroscopy led to the understanding of the wave-particle duality. Explain the electronic structure of the atom.Demonstrate an understanding of stoichiometry by calculating theoretical yield, actual yield, percent yield and limiting reagent. Determine empirical and molecular formulas.Write net ionic equations and predict products for precipitation and acid/base reactions. Describe and predict properties of electrolytes. Predict the solubility of ionic compounds.Apply the rules for nomenclature to write formulas as well as name: ionic compounds, binary molecules and acids. Use the periodic chart to predict the ionic charge of the main group elements. Explain molar mass and the mole concept: convert between mass, moles, number of molecules, number of atoms, and molarity.Describe Isotopes and calculate average atomic mass. Explain the organization of the Periodic Table and predict periodic properties of the elements. Apply significant figures in calculations and measurements.Describe the phases and classifications of matter. Employ the scientific method, explain measurements and uncertainty, and use dimensional analysis and problem solving in conversion questions.Prerequisites: MTE 1-9 and ENG 111 Eligible Course Objectives The general purpose of this course is to prepare the student for advanced study in science through development of: skills in problem solving and in critical thinking, an understanding of the methods of scientific inquiry, and an understanding of the general concepts and principles of chemistry. The course outline below was developed as part of a statewide standardization process.
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