{"id":70,"date":"2021-09-16T19:28:26","date_gmt":"2021-09-16T19:28:26","guid":{"rendered":"https:\/\/pressbooks.ccconline.org\/accphysicalgeography\/chapter\/2-2-bonding-and-lattices-physical-geology-2nd-edition\/"},"modified":"2022-02-02T16:45:53","modified_gmt":"2022-02-02T16:45:53","slug":"2-2-bonding-and-lattices-physical-geology-2nd-edition","status":"publish","type":"chapter","link":"https:\/\/pressbooks.ccconline.org\/accphysicalgeology\/chapter\/2-2-bonding-and-lattices-physical-geology-2nd-edition\/","title":{"raw":"2.2 Bonding and Lattices \u2014 Physical Geology \u2013 2nd Edition","rendered":"2.2 Bonding and Lattices \u2014 Physical Geology \u2013 2nd Edition"},"content":{"raw":"

2.2 Bonding and Lattices<\/h1>\r\nAs we\u2019ve just seen, an atom seeks to have a full outer shell (i.e., eight electrons for most elements, or two electrons for hydrogen and helium) to be atomically stable. This is accomplished by transferring or sharing electrons with other atoms.<\/a>\r\n
\"An<\/a>
Figure 2.2.1 A very simplified electron configuration of sodium and chlorine atoms (top). Sodium gives up an electron to become a cation (bottom left) and chlorine accepts an electron to become an anion (bottom right).\u00a0[Image Description]<\/a><\/figcaption><\/figure>\r\nSodium has 11 electrons: two in the first shell, eight in the second, and one in the third (Figure 2.2.1). Sodium readily gives up that single third-shell electron, and when it loses this one negative charge, it becomes positively charged (because it now has 11 protons and only 10 electrons). By giving up its lone third-shell electron, sodium ends up with a full outer shell. Chlorine, on the other hand, has 17 electrons: two in the first shell, eight in the second, and seven in the third. Chlorine readily accepts an eighth electron to fill its third shell, and therefore becomes negatively charged because it has 17 protons and 18 electrons. In changing their number of electrons, these atoms become\u00a0