![]() This is a platinum ion,Ī positive platinum ion. Four more of the positive thing than you have of the negative things. So you're going to haveĪ positive four charge. That we have four more protons than electrons. So by definition platinum hasħ8 protons, so we know that. Neutrons does it contain and what is its charge? Alright, so let's thinkĪbout this a little bit. And 195 looks prettyĬlose to that atomic mass we have there. An atom of platinum hasĪ mass number of 195. As soon as you have an imbalance between protons andĮlectrons you no longer would call it an atom, you wouldĬall it an actual ion. So you can write it like this, one minus. But this one has one extra electron, so it has one extra negative charge. The other way around? What if you were to have five protons, five protons and six electrons? What would this be? Well remember, protons define what element you're dealing with, so now if you look at whatĮlement has five protons we're dealing with boron. This you would now call an ion because it has that net charge. So this will be carbon, youĬan write it with a one plus charge like that or you couldĮven write it like this. So we're still dealing with carbon, but now we have one more positive charge than we have a negative charge. ![]() What define what element we're dealing with. So for example, if you had six protons and five electrons what would that be? Well, we still have six protons. Is if you don't have an equal amount of protons and electrons. Now you could have a carbon ion, although they aren't that typical. You have the six positive charges and the six negative charges. It is going to have six electrons and that's what makes it neutral. And if it is neutral carbon it is going to have the That one atom of carbon? Well, by definition an atom For example, if I haveĬarbon, carbon is an element. So before we talk about ions we're just going to talkĪbout the idea of an element. Talk about in this video is the notion of an ion. Seaborg G (1964) Plutonium: the ornery element.- So my apologies. Railsback LB (2003) An earth scientist’s periodic table of the elements and their ions. Oddo G (1914) Die molekularstruktur der radioaktiven atome. Newlands JAR (1865) On the law of octaves. Annalen der Chemie und Pharmacie Supplement 8:133–229. Zhurnal Russkoe Fiziko-Khimicheskoe Obshchestvo 3:25. Mendeleev D (1871) Die periodische gesetzmässigkeit der chemischen elemente. Mendeleev D (1869) Ueber die beziehungen der eigenschaften zu den atomgewichten der elemente. McDonough WF, Sun S-S (1995) The composition of the Earth. Lodders K (2010) Solar system abundances of the elements. Kean S (2010) The disappearing spoon and other true tales of madness, love, and the history of the world from the periodic table of the elements. Janet C (1929) The helicoidal classification of the elements. Harkins WD (1917) The evolution of the elements and the stability of complex atoms. Green J (1959) Geochemical table of the elements for 1959. Gray HB, Simon JD, Trogler WC (1995) Braving the elements. The seventh Hugo Müller Lecture, delivered before the chemical society. Goldschmidt VM (1937) The principles of distribution of chemical elements in minerals and rocks. Goldschmidt VM (1926) Geochemische verteilungsgesetze der elemente. Die lanthaniden kontraktion und ihre konsequenzen. Isomorphie und polymorphie der sesquioxyde. Goldschmidt VM (1925) Geochemische verteilungsgesetze der element, Part V. Comptes Rendus 54:757–761Įmsley J (2011) Nature’s building blocks: everything you need to know about the elements. De Chancourtois A-EB (1862) Mémoire sur un classement naturel des corps simples ou radicaux appelé vis tellurique.
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