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\nAndrew Rafalsky\/Shutterstock.com<\/a><\/span>
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Julie Pollock<\/a>, University of Richmond<\/a><\/em><\/span><\/p>\n When you see the periodic table, what comes to mind? The pieces on a scrabble board? Maybe you think about your high school chemistry class. Maybe you think of the colorful table plastered on the wall of a lecture hall in college. Maybe you remember your favorite teacher setting something on fire in the front of the classroom. I am an assistant professor of chemistry at University of Richmond<\/a> and when I hear the phrase \u201cthe periodic table,\u201d I think about life. <\/p>\n I think about how the molecules and chemicals that surround us and dictate our everyday activities are made up of the elements on that table \u2013 they sustain our life, they bring beauty to the world and they are vital in medicine.<\/p>\n Each column of the periodic table is called a group. Every member of the group has a similar arrangement of electrons which can result in similar chemical properties. The group 15 elements \u2013 nitrogen, phosphorus, arsenic, antimony, bismuth and moscovium \u2013 are interesting to me because of their pivotal role in life, as well as in my research lab<\/a>. One element we study is phosphorus because of its integral role in the fate of cells. <\/p>\n But before we get into those details, let\u2019s take a brief look at each of the group 15 elements. They are a unique set in their history, uses and properties. <\/p>\n Nitrogen (N) in its atmospheric form (N\u2082) makes up approximately 78% of the air we breathe. When bacteria living within plant roots convert it into a usable form through a process called nitrogen fixation, this elemental form of nitrogen gets incorporated into many compounds that are necessary for life \u2013 proteins and DNA, for example<\/a>. At the bottom of the column is Moscovium (Mc), which is interesting because it doesn\u2019t really exist in nature. It\u2019s a radioactive element that can only be generated in a laboratory and survives for less than a second<\/a>.<\/p>\n Arsenic (As) may be familiar to you because of its association with poisonings. In 1494, Pico della Mirandola, an Italian humanist philosopher during the Renaissance, was poisoned by arsenic, although the details surrounding his early death are still debated<\/a>. For a long time it was believed that Napoleon Bonaparte died of arsenic exposure in 1821, but after extensive comparisons of preserved hair samples<\/a> from different stages of his life, researchers concluded the increased levels of arsenic were most likely due to preservation techniques of the time. More recently, the World Health Organization estimated arsenic-contaminated drinking water in Bangladesh resulted in over 9,000 deaths in 2001<\/a>. How arsenic poisons and kills isn\u2019t completely understood, but there is no doubt that the element causes destruction of vital organs in the human body.<\/p>\n When the element antimony (Sb) is combined with three oxygen atoms to form antimony trioxide, it is used extensively as a flame retardant for furniture, carpets, drapes, rubber, plastics and adhesives. Quantities of this molecule in these household products tend to be very small, and these levels of antimony are regarded as safe<\/a>. <\/p>\n Bismuth (Bi) is a metal found in the same row of the periodic table as a number of toxic metals; however, compounds containing bismuth are harmless. Bismuth compounds can be found in cosmetics due to their distinctive and desirable silvery shimmer. Even if you haven\u2019t used bismuth-containing personal care products, you have probably encountered it in the well-known antacid Peptobismol\u00ae, which is used to treat upset stomachs<\/a>, or on the Fourth of July when you are watching fireworks. It is a bismuth compound that causes the crackling sounds of the dragon egg fireworks<\/a>.<\/p>\n Last, but not least, of the group 15 elements is phosphorus (P). It was discovered in 1669 by the alchemist Hennig Brandt and named from the Greek word \u201cphosphoros,\u201d meaning bringer of light<\/a>. That\u2019s because when the elemental form interacts with atmospheric oxygen it produces a brilliant light. Chemists figured out how to harness the power of this reaction for the development of matches. The red tip on a match still contains a form of phosphorus today.<\/p>\n In addition to sparks generated by the element, phosphorus is found in a compound known as a phosphate: phosphorus linked to four oxygen atoms. In cells, when a phosphate molecule is attached to a protein, it can turn on, or activate, the protein so that it can perform its function in the cell \u2013 like stimulating growth. <\/p>\n When the phosphate is no longer attached to the protein, the cells stop growing. You can think of it almost like the matches described above \u2013 when the phosphate is there, the match can ignite and business can proceed. When the phosphate is removed, the match is just a stick and no light is provided; not as much work can happen in the dark. <\/p>\n In cancerous cells, the phosphate status is out of control<\/a>. Imagine a lot of lit matches and a very bright room that can result in a flurry of activity. This activity can have severe consequences for cells. For example, unregulated growth and migration can lead to cancer. <\/p>\n In my laboratory<\/a> at the University of Richmond, we are interested in understanding these phosphates and one protein in particular that interacts with them. This protein, called MEMO1, is found in high quantities in breast cancer patients and helps the phosphates to always stay attached to proteins. We are trying to understand how MEMO1 interacts with these phosphates<\/a> and are developing strategies to disrupt those interactions. <\/p>\n We hope that our work reveals a way to help remove the phosphates to stop the unchecked growth of cells \u2013 in other words, to blow out the matches.<\/p>\n So next time you hear the words \u201cperiodic table,\u201d please think of life. Think of the molecules that you encounter every moment of every day, think of the medicine that keeps you healthy and think of those of us who are working to understand how to keep you that way. Julie Pollock<\/a>, Assistant Professor of Chemistry, University of Richmond<\/a><\/em><\/span><\/p>\n This article is republished from The Conversation<\/a> under a Creative Commons license. Read the original article<\/a>.<\/p>\n [\/et_pb_text][\/et_pb_column][\/et_pb_row][\/et_pb_section]<\/p>\n","protected":false},"excerpt":{"rendered":"![\"\"](\"https:\/\/images.theconversation.com\/files\/252876\/original\/file-20190108-32136-l3sinu.jpg?ixlib=rb-1.1.0&q=45&auto=format&w=754&fit=clip\")
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\nJulie Pollock<\/span>, CC BY-SA<\/a><\/span>
\n<\/figcaption><\/figure>\nGroup 15 \u2013 giving life and causing death<\/h2>\n
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\nAP Photo\/ A.M. Ahad<\/a><\/span>
\n<\/figcaption><\/figure>\nPhosphates \u2013 regulating cancer cell fate<\/h2>\n
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