CHEM 1211 Lecture 5Outline of Last Lecture I. Nuclide StructureII. IsotopesA. Mass SpectrumB. Natural % AbundanceIII. Atomic WeightA. ExampleIV. The Periodic TableA. Main Group MetalsB. Transition MetalsC. MetalloidsD. NonMetalsV. Forms of CarbonOutline of Current Lecture I. ProblemII. Metal/Non-Metal PropertiesA. Natural StatesB. Two Non-Metal RXNSIII. Molecular NomenclatureA. Greek PrefixesB. ExamplesIV. Ionic CompoundsA. CationB. AnionC. Chemical FormulaD. ExamplesV. The periodic tableA. Main Group Metalsa. Group 1Ab. Group 2Ac. Groups #AB. Transition MetalsC. Non-Metalsa. Group 7Ab. Group 6Ac. Group 5AD. ExamplesVI. Chemistry and Numbers of ThingsA. M&MsB. Carbon AtomsVII. The Mole (mol)Current LectureI. 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 = 10.811uMass of B-10= 10.0129uMass of B-11= 11.0093uX + Y = 110.0129x + 11.0093y = 10.811Y = 1-x10.0129x + 11.0093(1-x) = 10.811X = 0.8009 Y=0.1990 80.09% 19.90%  Natural AbundancesII. Metal/Non-Metal PropertiesA. Natural StatesMetal – Na(s) + Na(s) + Cl2(g)  Ionic Compound: NaCl(s)Non – Cl2(g) – F(x) = Q+Q- / d2: affects melting point and solubilityB. Two Non-Metal RXNSNon- H2 = H2O = water = covalent, molecular compoundsNon- O**Boiling can be hot and cold**NON-METALS!!Compound 1 Molecule ContainsHCl 1 H & 1 ClH2O 2 H & 1 ONH3: ammonia 1 N & 3 HC3H3 : C2H6 : Ethane 2 C & 6 HC3H8 : Propane 3 C & 8 HIII. Molecular NomenclatureA. Greek PrefixesMono – 1Di – 2Tri – 3Tetra – 4Penta – 5Hexa – 6Hepta – 7Octa – 8Nona – 9Deca - 10B. Examples1. CH4 = methane and carbon : carbon tetrahydride2. CH3CH2OH = ethanol3. SO3 = sulfur trioxide4. P2O5 = diphosphourous pentaoxide IV. Ionic CompoundsA. Cation: - Positive charge- Can be polyatomic: NH4+- Can be Metal: Na+, Mg2+B. Anion: - Negative charge- Can be polyatomic: CO32-, PO43-- Can be non-metal: F-, S2-***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-metalD. Examples1. 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 = F-V. The periodic tableA. Main Group Metalsa. Group 1A: ions 1+b. Group 2A: ions 2+c. Groups #A: ions 3+B. Transition MetalsIron (II) = Fe2+Cu(I) = Cu+Iron (III) = Fe3+Cu(II) = Cu2+C. Non-Metals: anions with negative changea. Group 7A: ions 1-b. Group 6A: ions 2-c. Group 5A: ions 3-D. Examples1. Group IIA & VIIACa2+ & I- = CaI2 = Calcium iodide2. Group IIA & VIACa2+ & O2- = CaO = CalciumoxideVI. Chemistry and Numbers of ThingsA. M&Ms- Mass of 10 = 8.540g- Mass of 1 = 0.8540g- Bag Mass = 1,587.6gHOW MANY M&Ms ARE THERE?1587.6 / .854 = 1,859 M7MsB. Carbon AtomsC-12 Atom Mass = 2.0 x 10-23g12g of C in C-12 : 12g (1Catom / 2.0 x 10-2gC) = 6.0 x 1023 atomsVII. The Mole (mol): 6.02214179 x 1023 molNa = 6.02214179 x 1023