CHEM 1211 Lecture 5 Outline of Last Lecture I Nuclide Structure II Isotopes A Mass Spectrum B Natural Abundance III Atomic Weight A Example IV The Periodic Table A Main Group Metals V B Transition Metals C Metalloids D NonMetals Forms of Carbon Outline of Current Lecture I Problem II Metal Non Metal Properties A Natural States B Two Non Metal RXNS III Molecular Nomenclature A Greek Prefixes B Examples IV Ionic Compounds A Cation B Anion C Chemical Formula D Examples V The periodic table A Main Group Metals a Group 1A b Group 2A c Groups A B Transition Metals C Non Metals a Group 7A b Group 6A c Group 5A D Examples VI Chemistry and Numbers of Things A M Ms B Carbon Atoms VII The Mole mol Current Lecture I Problem The periodic chart states that the atomic weight of Boron is 10 811u Mass spectrometry gives the isotopic abundances of B 10 and B 11 as 19 91 and 80 09 respectively What are the masses for each isotope NOT ENOUGH INFO THE QUESTION WAS CHANGED Let x B 10 and y B 11 Weight of Boron 10 811u Mass of B 10 10 0129u Mass of B 11 11 0093u II X Y 1 10 0129x 11 0093y 10 811 Y 1 x 10 0129x 11 0093 1 x 10 811 X 0 8009 Y 0 1990 80 09 19 90 Natural Abundances Metal Non Metal Properties A Natural States Metal Na s Na s Cl2 g Ionic Compound NaCl s Non Cl2 g F x Q Q d2 affects melting point and solubility B Two Non Metal RXNS Non H2 H2O water covalent molecular compounds Non O Boiling can be hot and cold NON METALS Compound 1 Molecule Contains HCl 1 H 1 Cl H2O 2H 1O NH3 ammonia 1N 3H C3H3 C2H6 Ethane 2C 6H C3H8 Propane 3C 8H III Molecular Nomenclature A Greek Prefixes Mono 1 Di 2 Tri 3 Tetra 4 Penta 5 Hexa 6 Hepta 7 Octa 8 Nona 9 Deca 10 B Examples 1 CH4 methane and carbon carbon tetrahydride 2 CH3CH2OH ethanol 3 SO3 sulfur trioxide 4 P2O5 diphosphourous pentaoxide IV Ionic Compounds A Cation Positive charge Can be polyatomic NH4 Can be Metal Na Mg2 Negative charge Can be polyatomic CO32 PO43 Can be non metal F S2 B Anion Look on eLC at the list of ions you need to know C Chemical Formula cation then anion Formulas must be electronically neutral Mg2 Cl MgCl2 Magnesium is a metal and Chloride is a non metal D Examples 1 H If we took away one electron of protons 1 of protons 1 of electrons 1 of electrons 0 Total Charge 0 Total Charge 1 2 F If we added one electron of protons 9 of protons 9 of electrons 9 of electrons 10 Total Charge Total Charge 1 Fluorine F2 g Fluorine atom F Fluoride FV The periodic table A Main Group Metals a Group 1A ions 1 b Group 2A ions 2 c Groups A ions 3 B Transition Metals Iron II Fe2 Cu I Cu Iron III Fe3 Cu II Cu2 C Non Metals anions with negative change a Group 7A ions 1b Group 6A ions 2c Group 5A ions 3D Examples 1 Group IIA VIIA Ca2 I CaI2 Calcium iodide 2 Group IIA VIA Ca2 O2 CaO Calciumoxide VI Chemistry and Numbers of Things A M Ms Mass of 10 8 540g Mass of 1 0 8540g Bag Mass 1 587 6g HOW MANY M Ms ARE THERE 1587 6 854 1 859 M7Ms B Carbon Atoms C 12 Atom Mass 2 0 x 10 23g VII 12g of C in C 12 12g 1Catom 2 0 x 10 2gC 6 0 x 1023 atoms The Mole mol 6 02214179 x 1023 mol Na 6 02214179 x 1023 mol 1
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