The figures all look near identical and perhaps do not carry that much information. I would suggest cutting them down
Reviewer: Bao Chau Nguyen
1) Synopsis: This module is about the difference in atomic radii of different atoms. Because the electrons do not stay in one spot around the atom, it is hard to determine the exact atomic radius. This gives rise to the several types of atomic radii, including covalent radius, ionic radius, and metallic radius, each with a different method of measurement. The trend in atomic radii increases as we go down a group and as we go from right to left on the same period due to the decrease in nuclear effective charge. We also know that as an atom loses an electron and become a cation, its atomic radius is smaller than the original atom, while gaining an electron will make its atomic radius bigger than the original atom.
covalent radius (google) - no plagiarism detected since there is really one way of defining it ionic radius (google) - no plagiarism detected since there is one way of defining it metallic radius (google) - no plagiarism detected since there is one way of defining it
3) Review Details: Compared to other modules, this module is fairly short in length, but it is understandable since there is only so much basic groundwork that can be taught about atomic radii. It would be more effective if you were to include an explanation about the nuclear effective charge and its impact in the trend of the atomic radii on the periodic table (like how nuclear effective charge increases as we go from left to right on one period because there is an extra proton added each time, and the added strength of an extra electron in the outer shell does not overcome the increase in nuclear effective charge, making the atomic radii decrease so). This module should also include a comparison in atomic radii of an anion and a cat ion that have the same electron configuration, showing how the cation would have a smaller radius than the anion, even though they have the same electron configuration.
Reviewer Name: Kimberly Song
Synopsis: The atomic radius is defined as the chances of an electron existing around the nucleus at a certain distance. The distance is different with covalent, ionic, and metallic bonds. You can determine the atomic radius by looking at adjacent atoms and their nuclei and looking at the distance between them and dividing by half. The distance between nuclei’s of atoms that have ionic, covalent, and metallic bonds. The covalent radius is 160pm, the ionic radius is 100 pm, the metallic radius is 180 pm. By examining the periodic table you notice that the atomic radius increases as it goes down the table and decrease as it goes across the table. This is because the atoms increase in size as it builds up electron shells. Transition metals however are an exception as they have electrons added in their inner shells, while the outer electrons remain the same. In addition cations have smaller radius than the atom that they originated from, while an anion has a bigger radius.
Keywords: Google (Atomic Radius), Yahoo (metallic radius), Bing (covalent radius)
Review Details: This module had a substantial amount of data, maybe a little less than other modules. There is a lack of text and information for certain areas, but there was a substantial amount of diagrams that were well done. To lengthen the overall module maybe it could include an explanation on the SI units of atomic dimensions. In addition maybe there could also be something about the concept of screening and penetration as well. The exceptions should be a bit clearer, but besides this the module is overall very good. In particular the Youtube video was clarifying and informative as well. The information was correct, and the introduction left a bigger picture for readers on how everything was connected. There were a few spelling mistakes in the introduction and underneath the atomic radius section.
Mistake: Fixed spelling error for the word “measured” in the introduction.