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Periodic Table, Atomic Structure, and Trends
Periodic Table, Atomic Structure, and Trends
Learning Objectives
Learning Objectives
Upon completion of this experiment, students will have experienced:
(CLO1). Explain basic chemical concepts related to chemical changes, energy, and properties of matter.
(CLO2). Apply the methods of scientific inquiry
(CLO3). Analyze evidence to decide if generalizations or conclusions based on the obtained data are warranted
(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.
(MLO2-8) Graph and Predict properties of effective nuclear charge, ionic or covalent radius, ionization energy, electron affinity and electronegativity using the periodic table.
Experiment 3 and 4 combined covers the key ideas of the electronic structure of the atom, how it relates to the periodic table and the physical properties that are linked the both the electronic structure and the position of the element on the periodic table.
The assignments that must be completed are the following:
The assignments that must be completed are the following:
Laboratory Report of the experiment using the resources listed below
Discussion
Discussion
Rutherford, Bohr, Schrodinger, Planck, Heisenburg and many other 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:
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 Problems
Pre laboratory Problems
There is no pre laboratory writing assignment for this experiment.
The Pre laboratory problems are questions about the laboratory assignment, background, definitions, 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
Part A: Periodic Table
Part A: Periodic Table
Use the following resources to observe 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
We will look at samples of elements, describing and researching their physical properties. The Visual Periodic table of picture and videos of the elements can be used to "see" images of the elements.
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.
You can view my presentation of The Periodic Table
Part B: Flame Tests
Part B: Flame Tests
Use the following videos to describe the light emission in the flame tests of the following ionic compounds: 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 B and C.
Part C: Emission Spectra of Elements
Part C: Emission Spectra of Elements
Observe the emission spectra of several elements.
Use the following resources to describe or draw the line spectra for the four elements.
Visible spectra of the elements:
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 D: Electron Configuration and the Periodic Table
Part D: Electron Configuration and the Periodic Table
Use the resources below to understand quantum number and how they relate to the orbitals and then how to use the orbitals to complete the electronic configuration or orbital diagram for the elements on 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
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. 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
Part E: Periodic Trends of physical properties
Part E: Periodic Trends of physical properties
The following web addresses should allow you to obtain the required data for this activity:
use this site to find the first and all other ionization potential. Click on an element and then find the drop down menu of other properties. Click on electron shell data, the ionization potentials are listed about midway down the page. If you continue to move down this page, you can also find the effective nuclear charge values for table 4-2.
This site can also be used to find the number of isotopes of each element. Click on the element, then in the drop down menu, click on Isotopes and NMR.
http://environmentalchemistry.com/yogi/periodic
Use this site to find the electronegativity, atomic size and density of the each element. The list of properties is toward the bottom of the page.
The Visual Periodic table of picture and videos of the elements
Interactive Periodic Table by the American Chemical Society
other web addresses may be provided by your instructor.
The Periodic Table: Atomic Radius, Ionization Energy, and Electronegativity
The Periodic Table: Atomic Radius, Ionization Energy, and Electronegativity
Professor Dave Explains - Why is the periodic table arranged the way it is? There are specific reasons, you know. Because of the way we organize the elements, there are special patterns that emerge. And you know how Professor Dave feels about patterns. He likes them.
Extended Periodic Table
http://jeries.rihani.com/index3.html
http://en.wikipedia.org/wiki/Extended_periodic_table
Click on Elements for an extended list of Periodic Tables
Part F: Relative reactivity of the Alkali metals.
Part F: Relative reactivity of the Alkali metals.
Observe the reactions of of each of the alkali metals by viewing the videos at The Video Periodic Table. You can compare these to the reactivity of the IIA group with the videos by NCSSM online in YouTube.
Reaction of Lithium with Water
North Carolina School of Science and Mathematics
Part of NCSSM CORE collection: This video shows the physical properties of Li metal and its reaction with water. http://www.dlt.ncssm.edu Please attribute this work as being created by the North Carolina School of Science and Mathematics. This work is licensed under Creative Commons CC-BY http://creativecommons.org/licenses/b...
Lithium - Periodic Table of Videos
Lithium - Periodic Table of Videos
Our new and improved Lithium video - from Neil's fumehood to the Bikini Atoll. Videos on all 118 elements in order... http://bit.ly/118elements This video features Professor Sir Martyn Poliakoff and Neil Barnes.
https://youtu.be/7IT2I3LtlNE
Sodium - Periodic Table of Videos
Sodium - Periodic Table of Videos
Our new and improved Lithium video - from Neil's fumehood to the Bikini Atoll. Videos on all 118 elements in order... http://bit.ly/118elements This video features Professor Sir Martyn Poliakoff and Neil Barnes.
Reaction of Sodium with water
North Carolina School of Science and Mathematics
Part of NCSSM CORE collection: This video shows the physical properties of Na metal and its reaction with water. http://www.dlt.ncssm.edu Please attribute this work as being created by the North Carolina School of Science and Mathematics. This work is licensed under Creative Commons CC-BY http://creativecommons.org/licenses/b...
Reaction of Magnesium and Water
Reaction of Magnesium and Water
North Carolina School of Science and Mathematics
Part of NCSSM CORE collection: This video shows the physical properties of Mg metal and its reaction with water. http://www.dlt.ncssm.edu
Reaction of Potassium and Water
Reaction of Potassium and Water
North Carolina School of Science and Mathematics
Part of NCSSM CORE collection: This video shows the physical properties of K metal and its reaction with water.
Reaction of Calcium and Water
Reaction of Calcium and Water
North Carolina School of Science and Mathematics
Part of NCSSM CORE collection: This video shows the physical properties of Ca metal and its reaction with water. http://www.dlt.ncssm.edu
Part G: Physical Properties of a Family
Part G: Physical Properties of a Family
The bulk density of either group 5 or group 6 in the transition metals will be determined and compared to the atomic density and the known density. Trends in density, melting point, boiling point and atomic size will be observed. The class data for Part C contains the data required to complete the first part of this calculation.
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