CHEM 101 1nd Edition Lecture 6 Outline of Last Lecture I. MoleII. Periodic Table of the ElementsOutline of Current Lecture I. Periodic TableII. Elemental GroupsIII. Neils BohrIV. IonsCurrent LectureI. Periodic Tablea. 1A - Alkali Metalsb. 2A - Alkaline Earth Metalsc. 6A - Chalcogensd. 7A - Halogense. 8A - Noble Gasesf. 1B-8B - Transition Metalsg. Main Group Metal = Nontransition Metalh. Element Abundancei. The elements that show up in the crust aren't in the same abundance as in organismsII. Elemental Groupsa. Hydrogeni. Non-metal in Group 1Aii. Can be used for fuelb. Group 1A: Alkali Metalsi. Li, Na, K, Rb, Csii. Very reactive with wateriii. Oxidize very quicklyc. Group 2A: Alkaline Earth Metalsi. Be, Mg, Ca, Sr. Ba, Raii. Silvery white metalsiii. Mg1. Burns very brightly used in agricultureThese notes represent a detailed interpretation of the professor’s lecture. GradeBuddy is best used as a supplement to your own notes, not as a substitute.iv. Ca1. Makes up teeth, and other natural thingsd. Group 3Ai. B, Al, Ga, In, Tlii. Boron is metalloid, everything else is a metal1. Consequently has different reactionse. Group 4Ai. C, Si, Ge, Sn, Pbii. Most varied groupiii. Nonmetals like Carbon have allotropes1. Allotropes are the different forms an element can exist in.2. Graphite, Diamond, Buckyballs, Amorphous Carbon (soot)iv. Carbon is one of the most important elements1. Carbon cyclef. Group 5Ai. N, P, As, Sb, Biii. N and P are essential for lifeiii. Nitrogen has a cycle just like carbong. Group 6A - Chalcogensi. O, A, Se, Te, Poii. Oxygen supports combustion1. This is how we get a lot of our energyiii. Oxygen supports life1. Cellular respirationh. Group 7A - Halogensi. F, Cl, Br, I, Atii. All are non metalsi. Group 8a: Noble Gasesi. He, Ne, Ar, Kr, Xe, Rnj. Transition Metals - 1B-8Bi. A hint of diversity ii. Can be very colorfulIII. Neils Bohra. Won the Noble Prize, and won a house next to brewery from thatb. Greatest contribution to science was in building a simple model of the atomc. Did a broad Spectrum White Light prismi. Excited atoms emit light of only certain wave lengths1. The wavelengths emitted depend on the elementd. Atomic Spectrai. Bohr proposed a model for the electronic structure of atoms and with it an explanation for the emission spectra of excited atomsii. However this contradicts laws of classical physics1. Any orbit should be possible and so should any energy2. A charged particle moving in an electric field should emit energy, and destroy the atome. Model of the Atomi. Electrons in an atom can only occupy certain orbits (corresponding to certain energies)ii. Electrons in permitted orbits had specific "allowed" energies; those energies will not be radiated from the atomiii. Energy is only absorbed or emitted in such a way as to move an electron from one "allowed" enter state to another; the energy is defined by E= hvf. Energy Adsorptioni. Absorption of energy can excite election from ground state to excited stateii. Energy is emitted when the election returns from the excited state to the ground stateIV. Ionsa. When neutral atoms lose or gain electron, the become ionsb. Cationsi. Positive and are usually formed by metalsc. Anionsi. Negative and are usually formed by nonmetalsd. Polyatomic ions also
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