CHEM 1211 Final Exam Study Guide Lectures 1 24 Lecture 1 January 9 Atoms Compounds and Molecules Reminder E mc2 E Energy M Mass C Light C 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 2N A Alloy Mixture of two or more molecules o Alloys are solutions o Example H N H H 3NH3 3N 9H N H 1 3 ALWAYS B States of Matter o Kinetic Molecular Theory Theory that makes up matter a 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 conserved Lecture 2 January 14 Mixtures Properties and Measurements I Chemical and Physical Properties A Chemical 1 Rusting oxidation 2 Chemical reactions B Physical 1 Changes in state 2 Density color solubility C Extensive properties depend on quantity D Intensive properties do not depend on quantity II Common Conversion Factors a Length 1 1m 39 37 inches 2 2 54 cm 1 inch EXACT b Volume 1 1 Liter 1 06qt 2 1qt 0 946 Liters III Rules for Sig Figs A Rule 1 All non zero digits are significant a 123 mm 3 sig figs B Rule 2A Leading zeros are never significant a 0 000357 3 sig figs C Rule 2B Trailing zeros are significant ONLY if decimal point is present a 1300 ambiguous or 2 sig figs D Rule 2C Imbedded zeros are ALWAYS significant a 1300 033 7 sig figs E Rule 3 Exact numbers have infinite numbers of sig figs a 15 eggs infinite F Rule 4 use scientific notation to remove doubt a 2 40 x 103 mantissa 3 sig figs b 5 003 x 106 4 sig figs Lecture 3 January 16 Percentage Density Specific Gravity Subatomic Particles Exact Figures 10mm 1cm 2 54cm 1 inch 1 yard 3 feet 1 Gallon 4 qts 1qt 2 pints o V l x w x h Cube l w h Vcube a3 A V Cube A Percentage Amount of Substance x 10x x 2 pph Total amount of sample x 3 ppt x 4 ppm PPH percent in part per hundred B Density Mass Volume C Specific Gravity o Unitless o Example 1 31 0 g piece of chromium dropped in 5 00 mL of water What is SG of chromium if water level rises to 9 32 mL V 9 32 mL 5 00 mL V 4 32 mL D 31 0g 4 32 mL 7 18 g mL SG 7 18 1 00 7 18 D Subatomic particles a 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 Z b Neutrons No charge Located in the Nucleus Mass 1 009 u c Electrons Located in the space around the nucleus Relative mass 0 0005 u of protons of electrons Lecture 4 January 21 Isotopes Atomic Weight the Periodic Table I Nuclide Structure A 14 Si 28 0855 X A Mass Number Z of Protons All Atomic masses are based on Carbon 12 12C 12amu 12 1 99265 x 10 23g 1 66 x 10 24g C Mass of Carbon 1 99265 x 10 23g 6 12amu 1 99265 x 10 26kg Isotopes Same element different mass Z II 14 Atomic Number Si Symbol of Element 28 0855 Mass Number 35 17 x 37 17 x X Cl Same Element Different number of neutrons different masses A Mass Spectrum Isotopes Chemically of same reactivity B Natural Abundance Cl 35 100 132 x 100 75 7 75 3 1 Ratio Cl 37 32 132 x 100 24 2 25 Cl 35 100 Cl 37 32 Atomic Weight AW Ne 20 19 9924u Ne 21 20 9938u Ne 22 21 9914u III The Periodic Table Lecture 5 January 23 Nomenclature Ionic Compounds Groups of the Periodic Table Metal Non Metal Properties A Natural States Metal Na s Na s Cl2 g Ionic Compound NaCl s Non Cl2 g Molecular Nomenclature o Greek Prefixes Mono 1 Di 2 A Examples Tri 3 1 CH4 methane and carbon carbon tetrahydride Tetra 4 2 CH3CH2OH ethanol Penta 5 3 SO3 sulfur trioxide Hexa 6 4 P2O5 diphosphourous pentaoxide Hepta 7 Octa 8 Nona 9 Deca 10 Ionic Compounds A Cation Positive Charge Can be metal polyatomic B Anion Negative Charge Can be non metal polyatomic C Chemical Formula cation then anion See list of Ions you should know at bottom of page Carbon Atoms C 12 Atom Mass 2 0 x 10 23g 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 Lecture 6 January 28 Moles Formula Weight Percent Elemental Composition o Moles V l x w x h or a x h 12 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 10 23 How do we calculate formula weight of a compound The molecular weight of C4H10 H 10 10 amu 10 x 1 01 C 48 04 amu 4 x 12 01 1 mol of C4H10 54 14g EXAMPLE Calcium Carbonate chalk Ca2 CO32 2 958g 29 58 2 740 0 218g CaCO3 used After writing on the board 2 740g Ca 40 08 C 12 01 O 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 chalkboard 2 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 board 1 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 board 2 17 x 10 3mol CaCO3 40 08 gCa 1 mol Ca 0 0869gCa Mass of Ca left on board o Percent Composition gElement molar mass x 100 weight percentage o 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 Name Group IA Cations Li 1 Lithium Na 1 Sodium K 1 Potassium Rb 1 Rubidium Cs 1 Cesium Group IIA Cations 2 Mg 2 Magnesium Ca2 2 Calcium 2 Sr 2 Strontium 2 Ba 2 Barium Group IIIA Cation 3 Al 3 Aluminum Transition Metal Cations Cu 1 Copper I 2 …