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The Periodic Table, Atomic and Electronic Structure
The Periodic Table, Atomic and Electronic Structure
Learning Objectives
Learning Objectives
Upon completion of this experiment, students will understand:
(CLO1). Explain basic chemical concepts related to chemical changes, energy, and properties of matter.
(MLO1-14) Identify the symbols and names of common elements on the periodic table.
(MLO1-15) Explain the organization of the Periodic Table of Elements in terms of families, periods, metals, semimetals and nonmetals
(MLO2-1) Utilize the electromagnetic spectrum to distinguish and convert between wavelength, frequency and energy different types of radiation.
(MLO2-2) Explain how light and spectroscopy lead to the understanding of the electronic structure of an atom.
(MLO2-3) Apply quantum number (principal, angular momentum, magnetic and electron spin) rules to determine allowable values for each type of quantum number and how the quantum numbers relate to atomic orbitals.
(MLO2-5) Explain how the Pauli exclusion principle and Hund's rule are used to determine electron configurations.
(MLO2-6) Utilize the periodic table to determine the electron configuration of a neutral atom or an ion
(MLO2-7) Predict the charge of an ion formed utilizing the number of valence electrons and its location on the periodic table.
This experiment does not have an on campus versus virtual laboratory assignment. Use the resources below to complete this laboratory assignment.
Experiment 3 introduces atomic structure, electronic structure and the periodic table.
The assignments that must be completed are the following:
The assignments that must be completed are the following:
Complete the Pre laboratory problems
Laboratory Report of the experiment using the resources listed below
Discussion
Discussion
The periodic table that students and professional chemists alike use today was first devised by a Russian chemist, Dmitri Mendeleev, in 1869. At the time, there were only 56 known elements with a new element being discovered at a rate of approximately one per year. There had been several attempts to devise a table of elements prior to Mendeleev’s work, but Mendeleev’s claim to fame was the fact that he had the foresight to leave gaps in his periodic table for elements that had not yet been discovered. ( A recent video,”Hunting the Elements,” (NOVA, PBS) hosted by David Pogue and found on You Tube, is an excellent introduction to the wonders of the periodic table.)
Simple atomic theory and experimentation showed that each atom is composed of three fundamental particles: positively charged protons, negatively charged electrons, and uncharged or neutral neutrons. From the Rutherford Gold Foil experiment, atomic theory expanded to show that the atom has a dense central nucleus which contains protons and neutrons with electrons moving around the nucleus at relatively large distances from the center of the atom.
Rutherford, Bohr, Schrodinger, Planck, Heisenburg and many other scientists contributed to our present understanding of the atom and its structure. Rutherford proposed the nucleus of the atom which contain most of the mass present in the atom, containing the protons and neutrons. Bohr began to describe how the electrons are present in the atom. His classic equation can be used to predict the energy and wavelength of light emitted from a hydrogen atom. Quantum Physics has a rich history but an evolving theory that is still attempting to find the answers about the structure of the atom. http://hyperphysics.phy-astr.gsu.edu/hbase/hframe.html The energy of the orbitals in Bohr's model of the atom can be determined using the equation:
This equation can be used to determine the energy, frequency and wavelength of light in an emission spectrum of hydrogen. Where h is Planck's constant, 6.63 x 10-34 J s; c is the speed of light, 3.00 x 108 m/s; and ∆E, Energy, is in Joules, J.
The last equation can be used to determine the wavelength of the light and then using the relationship, ∆E = hv = hc/ λ, the energy of the transition can be determine.
IntroAtomElectronic.mp4This video is my lecture building on the Rutherford model to the Bohr model with an understanding of the nature of "light".
BohrModel.mp4This video expands on the Bohr model and how light is used to understand the electronic structure of the atom - moving into the quantum model of the atom.
QuantumNumbers.mp4This video builds on the use of quantum numbers to define the electronic structure of the atom and the orbitals.
The quantum model of the atom led to more understanding about how the electrons move around the nucleus which cannot be solved by the above equation. Quantum number and Schrodinger's equation allow us the understand the orbitals that are a better representation of the electronic structure.
The electron configuration helps us to understand where the electrons are present in the orbitals and how these electrons can be used in understanding bonds, ions, and chemical reactions.
There are three rules or principles that govern how electrons fill the orbitals: Pauli Exclusion principle; Aufbau principle and Hund's Rule.
What are the Pauli Exclusion Principle, Aufbau Principle, and Hunds Rule?
What are the Pauli Exclusion Principle, Aufbau Principle, and Hunds Rule?
What are the Pauli Exclusion Principle, Aufbau Principle, and Hunds Rule? They are rules we use to fill electron orbital filling diagrams. Fill from the bottom up, Spread them out before you double up, and always have one up one down in each orbital.
Pre laboratory assignment
Pre laboratory assignment
The Pre laboratory problems are questions about the laboratory assignment, background, definitions or procedure and calculations. These problems should be completed BEFORE coming to the class where the assignment will be discussed.
Procedure and Report
Procedure and Report
Complete the individual parts of this laboratory using the resources given below and in the laboratory assignment.
Part A: The Periodic Table
Part A: The Periodic Table
In the Laboratory Report , you will either study samples of the elements or use various visual periodic tables to observe the physical properties (color, state of matter, and other appearance) of the elements.
Use the following periodic tables:
WebElements (This is probably the best periodic table online for finding the most up-to-date information about the elements on the periodic table.)
Theodore Gray's Visual Periodic Table shows pictures and videos of each element.
The Periodic Table was first organized by Mendeleev in 1860 using physical and chemical properties of the elements. Understanding the organization helps scientist understand the elements.
Metals are on the left side of the periodic table and non metals are on the right side.
The A and B groups on the table are still used but a second number system is also used (1 - 18) see http://periodic.lanl.gov/metal.shtml
A little history of the periodic table http://periodic.lanl.gov/mendeleev.shtml see the video on the bottom of the page - very large file.
A PBS trilogy, The Mystery of Matter, shows the development of the Periodic Table with the discover of the first elements to the atomic age and new elements being formed. These videos are no longer on PBS but can be accessed in YouTube. They are linked to Chapter 2 website
You can view my presentation of The Periodic Table
Part B: Colors
Part B: Colors
This procedure can be done using the following pictures of different solids and aqueous solutions of the ionic compounds.
After viewing these solutions of various salts, some colored and some colorless. Can you make a statement about where on the periodic table most of the colored elements are located?
The video explains the tasks needed to complete Part B. (This video is approx. 3 minutes long)
Cations of Elements
Cations of Elements
Lab3PartB.mp4
Lithium Chloride - LiCl
Sodium Chloride - NaCl
Potassium Chloride - KCl
Calcium Chloride - CaCl2
Barium Chloride - BaCl2
Strontium Chloride - SrCl2
Chromium (III) Chloride - CrCl3
Manganese (II) Chloride - MnCl2
Anhydrous Cobalt (II) Chloride - CoCl2
Copper (II) Chloride - CuCl2
Iron (III) Chloride - FeCl3
Nickel (II) Chloride - NiCl2
Anions of Elements
Anions of Elements
Sodium Bromide - NaBr
Sodium Iodide - NaI
Lead (II) Iodide - PbI2
Soda Ash Sodium Carbonate - Na2CO3
Sodium Dichromate - Na2Cr2O7
Sodium Phosphate - Na3PO4
sodium Permanganate - NaMnO4
Sodium Ferrocyanide - Na4Fe(CN)6
Part C: Flame Tests
Part C: Flame Tests
The emission spectra of the following salts will be observed: LiCl, NaCl, KCl, CaCl2, SrCl2, BaCl2, and CuCl2.
Flame Tests of Metal Ions, With Labels
Flame Tests of Metal Ions, With Labels
North Carolina School of Science and Mathematics
Part of NCSSM CORE collection: This video shows the flame tests for several metal ions. http://www.dlt.ncssm.edu
Lab3PartCandD.mp4This video shows the tasks that need to be completed for Parts C and D.
Part D: Emission Spectra of Elements
Part D: Emission Spectra of Elements
Use the following resources to describe or draw the line spectra for the four elements.
Visible spectra of the elements:
http://www.umop.net/spctelem.htm (click on the link for the interactive periodic table to view an individual electronic spectrum for an element)
Spectrum Demo: Continuous and Emission
Spectrum Demo: Continuous and Emission
Physics Demos - This is a demonstration of the continuous spectrum of white light and the emission spectra of mercury, nitrogen, neon, and hydrogen, imaged through a diffraction grating.
Bohr Model of the Hydrogen Atom
Bohr Model of the Hydrogen Atom
Professor Dave Explains - Why don't protons and electrons just slam into each other and explode? Why do different elements emit light of different colors? Niels Bohr knew why. And now you will too!
Part E: Electron Configuration and the Periodic Table
Part E: Electron Configuration and the Periodic Table
modified bohr model 2.mp4This video continues to explain how to use the periodic table to determine the electron configuration of an atom.
electronconfigexp3.mp4This video continues electron configuration and explains several of the questions in Part E.
Ions.mp4Electron configuration of ions
A Step-by-step tutorial: http://terpconnect.umd.edu/~wbreslyn/chemistry/electron-configurations/
Crash Chemistry Academy:
Hydrogen Orbital viewer: https://chemapps.stolaf.edu/jmol/unplugged/orbitals.htm You can use this simulation to view the electron density of the orbitals as shown in the image to the right of the 3p orbital.
http://billvining.com/mmlib_sims/#gen_1_4
You can use this simulation to show the electron configuration and Box Diagram of most of the elements on the Periodic Table.
A similar presentation of the electronic configuration is displayed for each element in WebElements
Writing Electron Configurations Using Only the Periodic Table
Writing Electron Configurations Using Only the Periodic Table
A step-by-step description of how to write the electron configuration for elements using just the Periodic Table.
In order to write the electron configurations using the Periodic Table we first need to know the number of electrons for the each atom. When we write the configuration we'll put these electrons in orbitals around the nucleus of the atom.
Electron configuration notation provides an easy way for scientists to write and communicate how electrons are arranged around the nucleus of an atom. This makes it easier to understand and predict how atoms will interact to form chemical bonds.
You can also use just the Periodic Table to help write the notation elements instead of the Periodic Table. See https://youtu.be/ououF9nHUhk.
Get more chemistry help at http://www.breslyn.org
Tyler DeWitt - Valence Electrons and the Periodic table.
Bozeman Science - Electron Configuration
This is the document that contains the learning objectives, discussion, procedure, pre writing assignment, pre laboratory problems, report and post laboratory problems and conclusion assignments.
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