CHEM 1211Exam # 1 Study Guide Lectures: 1 - 6Lecture 1 (January 9)Atoms- Compounds and MoleculesReminder: E = mc2E = Energy, M = Mass, C = LightC = (m/s), m = kg, e = joules Joules = kg (m/s)2 = kg x m2/s2**NEED TO KNOW ELEMENTS 1-54 ON PERIODIC TABLE. HOW TO SPELL ELEMENT CORRECTLY & THE SYMBOL.EXAMPLES OF ATOMS (ELEMENTS): Notice the Color of the Elements!!= Hydrogen Atom x 2 = 2H= Carbon Atom (Bigger than hydrogen atom) x 3 = 3C= Oxygen x 2 = 2O = Nitrogen x 2 = 2NA. Alloy: Mixture of two or more moleculeso Alloys are solutionso Example: H-N-H H3NH3 = 3N & 9HN:H = 1:3 ALWAYS!!B. States of Matter: o Kinetic Molecular Theory: Theory that makes up mattera. Solids: Regular array of particles closely packed- You are going to see motion because it has kinetic energy (JIGGLES) b. Liquids: Randomly arranged, free moving particles spaced close together - Liquids are fluids.c. Gas: Randomly moving particles which are spaced far apart.- Collisions are elastic because the energy is conservedLecture 2 (January 14)Mixtures, Properties, and MeasurementsI. Chemical and Physical PropertiesA. Chemical1. Rusting/oxidation2. Chemical reactionsB. Physical1. Changes in state2. Density, color, solubilityC. Extensive properties: depend on quantityD. Intensive properties: do not depend on quantityII. Common Conversion Factors a. Length1. 1m = 39.37 inches2. 2.54 cm = 1 inch **EXACT!!b. Volume1. 1 Liter = 1.06qt2. 1qt = 0.946 LitersIII. Rules for Sig. Figs.A. Rule #1: All non-zero digits are significanta. 123 mm = 3 sig. figs.B. Rule #2A: Leading zeros are never significanta. 0.000357 =3 sig. figs.C. Rule #2B: Trailing zeros are significant ONLY if decimal point is presenta. 1300 = ambiguous or 2 sig. figs.D. Rule #2C: Imbedded zeros are ALWAYS significanta. 1300.033 = 7 sig. figsE. Rule #3: Exact numbers have infinite numbers of sig. figs.a. 15 eggs = infiniteF. Rule #4: use scientific notation to remove doubta. 2.40 x 103 (mantissa) = 3 sig. figsb. 5.003 x 106 = 4 sig. figs.Lecture 3 (January 16)Percentage, Density, Specific Gravity, & Subatomic ParticlesExact Figures:10mm = 1cm 2.54cm = 1 inch 1 yard = 3 feet 1 Gallon = 4 qts 1qt = 2 pints o V= l x w x hCube = l=w=hVcube = a3A = ∛ VCubeA. Percentage: Amount of Substance x 10x x=2 pphTotal amount of sample x=3 ppt x=4 ppmPPH* percent in part per hundredB. Density = Mass / VolumeC. Specific Gravityo Unitlesso Example:1. 31.0 g piece of chromium dropped in 5.00 mL of water. What is SG ofchromium if water level rises to 9.32 mL?V= 9.32 mL – 5.00 mLV= 4.32 mLD= 31.0g / 4.32 mL = 7.18 g/mLSG = 7.18/1.00 = 7.18D. Subatomic particlesa. Protons + Located in the Nucleus- Mass = 1.672623 x 10-24 g- Mass = 1.007 u = atomic mass unit = amu- Defines an element: Atomic # = number of protons = Zb. Neutrons: No charge, Located in the Nucleus- Mass = 1.009 uc. Electrons: - Located in the space around the nucleus- Relative mass = 0.0005 u**# of protons = # of electronsLecture 4 (January 21)Isotopes, Atomic Weight, & the Periodic TableI. Nuclide StructureA: Mass NumberZ: # of Protons** All Atomic masses are based on Carbon-12 (12C) = 12amuMass of Carbon: 1.99265 x 10-23g 1.99265 x 10-26kgII. Isotopes: Same element, different massX= ClSame Element… Different number of neutrons / different massesA. Mass Spectrum- Isotopes: Chemically of same reactivityB. Natural % Abundance3:1 Ratio: Cl-35: 100%Cl-37:32%Atomic Weight: AW= (%Ne-20)(19.9924u) + (%Ne-21)(20.9938u) + (%Ne-22)(21.9914u)III. The Periodic TableAZX14Si28.0855126C35173717xxCl-35: (100% / 132%) x 100% = 75.7% = 75%Cl-37: (32% / 132%) x 100% = 24.2% = 25% 14: Atomic NumberSi: Symbol of Element28.0855: Mass Number1.99265 x 10 -23 g = 1.66 x 10-24g 12amuLecture 5 (January 23)Nomenclature, Ionic Compounds, & Groups of the Periodic TableMetal/Non-Metal PropertiesA. Natural StatesMetal – Na(s) + Na(s) + Cl2(g)  Ionic Compound: NaCl(s)Non – Cl2(g) – Molecular Nomenclatureo Greek PrefixesMono – 1Di – 2Tri – 3 Tetra – 4Penta – 5Hexa – 6A. Examples1. CH4 = methane and carbon : carbon tetrahydride2. CH3CH2OH = ethanol3. SO3 = sulfur trioxide4. P2O5 = diphosphourous pentaoxideHepta – 7Octa – 8Nona – 9Deca - 10Ionic CompoundsA. Cation: Positive Charge… Can be metal & polyatomicB. Anion: Negative Charge… Can be non-metal & polyatomicC. Chemical Formula (cation, then anion)***See list of Ions you should know at bottom of page.***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 atomsThe Mole (mol): 6.02214179 x 1023 mol: Na = 6.02214179 x 1023 mol-1Lecture 6 (January 28) Moles, Formula Weight, Percent & Elemental Compositiono MolesV = l x w x h or a x h12.00 g of C-12 contains 6.022 x 1023 atoms of C-12 Atomic Mass of any element (g) = 1 mol of atoms of element = 6.022 x 1023How do we calculate formula weight of a compound?The molecular weight of C4H10H = 10.10 amu = 10 x 1.01C = 48.04 amu = 4 x 12.011 mol of C4H10 = 54.14g***EXAMPLE: Calcium Carbonate = chalk***Ca2+ + CO32- = 2.958g 29.58 – 2.740 = 0.218g CaCO3 usedAfter writing on the board: 2.740gCa = 40.08 C = 12.01O = 16.00 x 3 = 48.00= 100.09 g CaCo3 /mol CaCo3 0.218 g CaCO3 x 1 mol CaCO3/100.09g CaCO3= 2.17 x 10-3 mol CaCO3 : Left on chalkboard2.17 x 10-3 mol CaCO3 x 6.022 x 1023 f.u. / 1 mol CaCO3=1.31 x 1021 f.u. : formula units of chalk on board1 mol CaCO3 = 1 mol Ca2+2.17 x 10-3 mol CaCO3 x ( 1 mol Ca2+ / 1 mol CaCO3) = 2.17 x 10-3mol Ca2+ : atoms of Ca left on board2.17 x 10-3mol CaCO3 ( 40.08 gCa / 1 mol Ca) = 0.0869gCa: Mass of Ca left on boardo Percent CompositiongElement / molar mass x 100% = weight percentageo Elemental Composition**Lowest whole number ration: empirical formula (determined by finding % comp.)1. Ethane C2H6 = CH3***Aikenes all have Emp. Form. of CH2**Ions you should know!!**Formula Charge NameGroup IA CationsLi+1+LithiumNa+1+SodiumK+1+PotassiumRb+1+RubidiumCs+1+CesiumGroup IIA CationsMg2+2+MagnesiumCa2+2+CalciumSr2+2+StrontiumBa2+2+BariumGroup IIIA CationAl3+3+AluminumTransition Metal CationsCu+1+Copper(I)Cu2+2+Copper(II)Fe2+2+Iron(II)Fe3+3+Iron(III)Zn2+2+ZincAg+1+SilverGroups VIIA (Halogens) AnionsF-1-FluorideCl-1-ChlorideBr-1-BromideI-1-IodideGroup VIA AnionsO2-2-OxideS2-2-SulfidePseudo Monoatomic Ions/Conjugate Acids/Base AnionsOH-1-HydroxideCN-1-CyanideCH3COO-1-Acetate NH4+1+AmmoniumOxyacid AnionsNO3-1-NitrateHSO3-1-Hydrogen sulfite (bisulfite)SO32-2-SulfiteHSO4-1-Hydrogen