Katy Johanesen Ph.D. Candidate, USC Department of Earth Sciences Introduction • I am a geologist • I study the chemical reactions and physical changes in rocks and what they can tell us about the past, about plate tectonics, and about processes like earthquakes and volcanoes. • Chemistry is vital to my research! Questions? Email johanese@usc.edu Today’s lecture has two parts Atoms Molecules and Compounds The Atom • Name comes from the greek word atoma, or "indivisible particles“ – Democritus • This idea fell out of favor, Aristotle’s four elements became popular: – earth, wind, fire , and water • Robert Boyle later disproved this in the 1600’s http://atomictimeline.net/index.php for a full timeline of atom discoveries The atom is made up of even smaller particles Protons – positive charge Neutrons – no charge Electrons – negative charge Cathode ray tube experiment - discovery of the electron: electrons in the form of electricity flow from one end of the tube to the other. Watch what happens when a magnet comes near the tube. Which side of the magnet do you think they used? Source: http://chem.illinois.edu/CLCwebsite/demos.html Emission Spectroscopy • Each element emits different wavelengths of light (energy) when • Niels Bohr explained this with a new model of the atom! Bohr model of the Atom • Electrons are organized into energy levels or shells, also called orbitals Outermost shell = valence electrons • Energy is absorbed when an e- moves out a level, and emitted when it moves in. SchrÓ§dinger Model of the Atom • Electrons have properties of both particles and waves • Orbitals represent probability of where the electron will be (two e- in each orbital) The Elements • Each element has a unique atomic number • Atomic number = number of protons • Each atom has an equal number of electrons • Atoms with the same # protons but different # neutrons are called Isotopes • Periodic Table of the Elements: www.ptable.com Bonding • Atoms can combine to form compounds or molecules • Ionic – give and take electrons (NaCl) • Covalent – sharing (C) • Metallic – positive ions in a sea of valence electrons (Au, Cu) • Hydrogen bonds (weak) • Van der Waals bonds… we won’t talk about these. Ionic Bonds • Atoms donate or accept valence electrons and become ions, or charged particles • Na loses one e- and forms Na1+ • Cl gains one e- and forms Cl1• The charged ions attract each other and form NaCl • Most common for alkali and alkali earth metals (+), halogens (-), and some transition and post-transition metals like Fe and Al. Na (Sodium) and Cl (Chlorine) Na (Sodium) and Cl (Chlorine) + - NaCl (table salt) crystals Source: http://www.sciencephoto.com Covalent Bonds • Atoms share valence electrons in a hybrid orbital between them – Two atoms of O each need two valence electrons to complete their outer shell, so they bond together to form O2 • Most common for nonmetals like C, O, N, P, S, and H. Halogens also form covalent bonds with each other. O (Oxygen): atomic number 8 O2 Note: only two electrons from each atom are shared, not all the e- in the outer shell Carbon forms covalent bonds H DNA N S C caffeine C amino acidphenylalanine N O graphene Source: http://news.discovery.com Metallic bonds • Positive ions surrounded by unrestricted electrons – These can flow through the medium, which explains why metals are good conductors of electricity – Can bond atoms of a single element or form alloys of two or more metals. • Common metallic bonding elements are: Au, Ag, Ni, Cu, Zn, Pt. Xe atom on Ni crystal face • STM – Scanning Tunneling Microscope is used to image the atomic structure of solids – Xenon = blue circle – Nickel = red dots • Note vacancies in the structure (black holes) http://www.almaden.ibm.com/vis/stm/gallery.html Let’s try it • It’s time for some bonding! – You are an element. Take a card from the center of your table. – To what group of elements do you belong? Are you likely to bond in ionic, covalent, or metallic bonds? – You may have more than one option, or you may not bond at all. – Now find someone to bond with. Think about what your charges are if you become an ion.