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(s) mole (mol) Kelvin (K) Temperature: Luminous Intensity: candela (cd) Electric current: Ampere (A) Fundamental Concepts IF YOU DONT KNOW YOUR CONVERSION FACTORS NSTRUCTO YOU'RE GONNA HAVE A BAD TIME quickmeme.com The Microscope Head Nosepiece Objective turret Stage. Iris Diaphragm. Condenser Illumination System Base Fundamental Concepts Eyepiece Eyepiece Tube Objectives Frame Coarse Focus Fine Focus Illumination Intensity Knob JT 000 10000 00- E = mc² Illll V2 Bea LITT DIH H₂O QUESTION Significant Figures and Scientific Notation 1. 0.00567 has how many significant figures? A. 3 B. 4 C. 5 D. 6 2. If the same number is expressed in scientific notation, how many significant figures are there? A. 3 B. 4 C. 5 D. 6 000 M- E = mc² 1-001 HO Illll VZ A DOH H₂0 Sege ANSWER Significant Figures and Scientific Notation 1. 0.00567 has how many significant figures? A. 3 B. 4 C. 5 D. 6 2. If the same number is expressed in scientific notation, how many significant figures are there? A. 3 B. 4 C. 5 D. 6 JT ITM 000 H 0000 E = mc² 00 21lll Vz DIA H₂O Read QUESTION Properties of Matter Which of the following properties is different from the other properties? A. Density B. Specific heat C. Mass D. Color J 000 00 00- 00 E = mc² PUR VZ DIA H₂0 ANSWER Properties of Matter Which of the following properties is different from the other properties? A. Density B. Specific heat C. Mass D. Color JT 000 00- 0000 E = mc² 2lll Vz BER DIAH H₂O QUESTION Units and Conversion At what value are Fahrenheit and Celsius units equal? A. -20 degrees B. 0 degrees C. 20 degrees D. -40 degrees 000 D E = mc² 1-001 Illll V2 LTT DOH H₂0 ANSWER Units and Conversion At what value are Fahrenheit and Celsius units equal? A. -20 degrees B. 0 degrees C. 20 degrees D. -40 degrees Atomic Theories Dalton's Atomic Theory debunked ● All matter is consisted of indivisible particles called atoms : proton, electron Atoms of an element are identical in mass and properties and has different from other elemental atom properties : isotopes, radioactivity The Atom "Marble" (Dalton - 1803) "Pudding" (Thompson - 1904) "Nuclear" (Rutherford 1911) "Planetary" (Bohr - 1913) Quantum Wave Function (Schrodinger - 1926) Quantum Atomic Theory ● C The Atom Electrons behave both as particle and wave. Heisenberg's Uncertainty Principle: the exact position and momentum of an electron is IMPOSSIBLE to determine at the same time. Pauli's Exclusion Principle: two electrons may not occupy same quantum state. Each orbital may be occupied by maximum of two electrons with different spin. Hund's Rule: when several orbitals of equal energy are available, electrons enter singly with parallel spins (minimizes repulsion) Quantum Atomic Theory energy level 2pº 2s² 111 number of electrons in orbital Examples: Phosphorus 15P 3p³ 15² 1 10 -type of ort ital 3s²111 11 n=3, 1=1, m=+1 correct ##++- 19 29² 2p² Sulfur 16S 2p 2s²111 កស 11 The Atom incorrect ### 18 28 3p4 3ş² 11 1 14 2p² "electrons-in-boxes" Quantum Numbers Quantum numbers: set of numbers to describe electron's orbital Symbol Range of Values Name Principal : Primary Azimuthal : Angular Momentum Magnetic : Projection of Angular Momentum Spin n 1 mi Ms Orbital Meaning Shell (main energy level) Subshell (orbital) S=0, p=1, d=2, f=3 Orientation of subshell shape Spin of electron n≥1 0≤1≤n-1 The Atom -1≤m, ≤ +1 Example n = 1, 2, 3, …... for n=3: L = 0, 1, 2 (s, p, d) For = 1 (p-orbital) m₁ = -1, 0, +1 Px, Py, Pz 1/2 = clockwise -1/2 = counter-clockwise Electronic Configuration Noble Gas Configuration Octet rule (of thumb): Atoms tend to combine in a way that they each have eight electrons in their valence shells, giving them the same electronic configuration as a noble gas (applicable to the main-group elements, except helium). ● C Noble gas: Na -e 11 1s²2s² 2p 3s1 +e 9F 1s²2s²2p5 The Atom 10 Ne 1s²2s²2p6 Na+ 1s²2s²2p6 1s²2s²2p6 J ITM 000 00- E = mc² 21llle Vz BER DIAH H₂O QUESTION Quantum Numbers Which of the following set of quantum number is impossible? Format: n, l, m₁, ms S A. 2, 2, 1, -1/2 B. 2, 1, 0, 12 C. 4, 2, -1, 12 D. 3, 0, 0, 1 000 E = mc² -01 10 All VZ Peg LTT S DIA H₂0 ANSWER Quantum Numbers Which of the following set of quantum number is impossible? Format: n, l, m₁, ms A. 2, 2, 1, -12 B. 2, 1, 0, 1/2 C. 4, 2, -1, 12 D. 3, 0, 0, 12 JT 000 0000 00- E = mc² 00 2llll Vz DIH H₂O QUESTION Electronic Configuration What is the correct electron configuration of Chloride ion? Atomic number of Cl = 17. A. 1s² 2s² 2p 3s² 3p5 B. 1s² 2s² 2p 3s² 3p4 C. 1s² 2s² 2p 3s² 3p6 D. 1s² 2s²2p5 3s² 3p5 E. 1s² 2s² 2p 3s² 3p5 4s¹ π 000 HO E = mc² 00 Illll VZ TT DIA H₂O ANSWER Electronic Configuration What is the correct electron configuration of Chloride ion? Atomic number of Cl = 17. A. 1s² 2s² 2p 3s² 3p5 B. 1s² 2s² 2p6 3s² 3p4 C. D. 1s² 2s² 2p 3s² 3p6 1s² 2s²2p5 3s² 3p5 E. 1s² 2s² 2p 3s² 3p5 4s¹ JT 000 00- 0000 f.of E = mc² 21lll V2 ARTIT DIAH H₂O Read QUESTION Quantum Numbers Which of the following orbitals is not allowed? A. 5f B. 2s C. 2d D. 3p E. 1s J 000 E = mc² 2|||| V2 DIH H₂0 ANSWER Quantum Numbers Which of the following orbitals is not allowed? A. 5f B. 2s C. 2d D. 3p E. 1s Structure of the Periodic Table H Hydrogen 1.01 Li Lithium 6.94 19 1 K Potassium 39.10 37 11 12 Na Mg Sodium Magnesium 22.99 24.31 Rb Rubidium 85.47 55 Cs Cesiam 132.91 4 87 Be Beryllium 9.01 2 20 21 Ca Sc Calcium 40.08 56 Ba Barium 137.33 88 Fr Ra Francium Radium 223.02 226.03 3 Scandium 44.96 22 57 Alkali Metal 4 Ti Titanium 47.88 23 5 O Carbon Nitrogen Oxygen 12.01 14.01 15 16.00 16 Al Si P 7 25 8 26 10 28 26.98 31 Aluminum Silicon Phosphorus Sulfur 28.09 30.97 32.06 32 33 34 24 27 29 30 Cr Mn Fe Co Ni Cu Zn Ga Ge As Se Br Kr Nickel Copper Zinc 58.69 63.55 65.38 46 47 48 Gallium Germanium Arsenic Selenium Bromine 69.72 72.63 74.92 78.97 79.90 49 51 52 53 Krypton 84.80 54 38 39 40 50 Sr Y Zr Nb Mo Tc Ru Rh Pd Ag Cd In Sn Sb Te I Xe Strontium Yttrium Zirconium Niobium Molybdenum Technetium Ruthenium 87.62 88.91 91.22 92.91 95.95 98.91 57-71 72 Lanthanides Rhodium Palladium Siver Cadmium Indiam Tin Antimony Telluriam 101.07 102.91 106.42 107.87 112.41 114.82 118.71 121.76 127.6 76 77 78 79 80 81 82 83 84 lodine 126.90 85 Xenon 131.29 86 73 75 Hf W Re Os Ir Pt Au Hg Tl Pb Bi Po At Rn Hafniam 178.49 89-103 104 Ta Tantalam Tungsten Rhenium Osmium Indiam 180.95 183.85 186.21 190.23 192.22 105 106 107 108 109 Platinum Gold Mercury Thallium Lead 195.08 196.97 200.59 204.38 207.20 110 111 112 113 114 Bismuth Polonium Astatine 208.98 [208.98] 209.98 115 116 117 Radon 222.02 118 Rf Db Sg Bh Hs Mt Ds Rg Cn Nh FI Mc Lv Ts Og Actinides Intherfordam Dubnium Seaborgium Bohriem [261] Hassium [269] Meitnerium Darmstadtum Roentgenium Copemicum Nihonium [278] [262] [266] [264] 58 Periodic Table of the Elements 6 74 V Vanadium Chromium Manganese Iron Cobat 50.94 51.99 54.94 55.85 58.93 41 42 43 44 45 9 Actinium Thorium Protatiniam Uranium Neptanium 227.03 232.04 231.04 238.03 237.05 Alkaline Earth Transition Metal Basic Metal Metalloid 11 12 Nonmetal 5 13 Halogen Boron 10.81 13 6 BCN 14 14 C 15 Noble Gas 16 The Periodic Table 9 Lanthanide 17 Fluorine 19.00 17 Actinide 59 60 61 62 63 64 65 66 67 68 69 70 71 La Ce Pr Nd Pm Sm Eu Gd Tb Dy Ho Er Tm Yb Lu Cerium Praseodymium Neodymium Promethium Samarium Lanthanam 138.91 89 Europium Gadoliniam Tertium Dysprosium Holmium 140.12 140,91 144.24 144.91 150.36 151.96 157.25 158.93 162.50 164.93 90 91 92 93 94 95 96 97 98 99 Erbiam Thurun Ytterbiam Lutetium 167.26 168.93 173.06 174.97 100 101 102 103 Ac Th Pa U Np Pu Am Cm Bk Cf Es Fm Md No Lr Plutonium Americium Curiem Berkeliam Califomiam Einsteinium 244.06 243.06 247.07 247.07 251.08 [254] Chorine 35.45 35 Fermium Mendeleviem Nobelium 257.10 258.10 259.10 He Helium 4.00 10 Ferovium Moscovium Livermorium Tennessine Oganesson [281] [280] [285] [286] [289] [289] [293] [294] [294] 18 Ne Mean 20.18 18 Ar Argon 39.95 36 Lawrencem [262] Trends Across the Periodic Table Atomic radius Ionization energy Electron affinity Nonmetallic character Metallic character Atomic radius C The Periodic Table Electron affinity Ionization energy Trends Across the Periodic Table atomic radius: radius of atoms ionization energy: energy required to remove an electron from a neutral atom in its gaseous phase ● ● electron affinity: ability of an atom to accept an electron; quantitative measurement of energy change that occurs when electron is added to a neutral gas atom. electronegativity: atom's ability to attract and bind with electrons metallicity: how readily an atom can lose an electron Atomic radius C The Periodic Table Ionization energy Electron affinity Nonmetallic character Metallic character Atomic radius Electron affinity Ionization energy Atomic Number, Mass Number and Atomic Mass Mass number Number of protons and neutrons in atom Atomic number Number of protons in atom 12 6 A Z 6 protons 6 neutrons 6 electrons 0 Atomic symbol Abbreviation used to represent atom in chemical formulas C The Periodic Table Oh my gosh, I've lost a neutron! Don't worry; you can get a new one "free of charge." Amount of Substance ● ● ● Molecular Mass: the mass of a molecule (mM) of a chemical compound is the sum of the atomic masses of the constituting elements. Amount of Substance (mole): the mass m of a portion related to the Molar Mass M of the substance. Avogadro's Number: An amount of substance n = 1 mol contains always the same number of particles: Avogadro's Number N: 1 mol » N = 6x1023 particles C Stoichiometry Calculating with the Amount of Substance m=M⋅n< m M=" n n m M JT ITM 000 00 E = mc² 21lll Vz DIH H₂O Read QUESTION The Periodic Table Element Infinitium has 9 protons and 12 neutrons. Its atomic number is which is equal to the A. 9, number of protons B. 12, number of neutrons C. 9, number of electrons 21, sum of protons and neutrons D. E. 12 number of electrons π 000 00- E = mc² Illll V2 DIA H₂0 ANSWER The Periodic Table Element Infinitium has 9 protons and 12 neutrons. Its atomic number is which is equal to the A. 9, number of protons B. 12, number of neutrons C. 9, number of electrons 21, sum of protons and neutrons D. E. 12 number of electrons JT ITM 000 E = mc² 21lll Vz Bea DIH H₂O QUESTION The Periodic Table Element Infinitium has 9 protons and 12 neutrons. Its mass number is which is equal to the A. 9, number of protons B. 12, number of neutrons C. 9, number of electrons D. E. 12 number of electrons 21, sum of protons and neutrons J E = mc² Illll V2 DIA H₂0 ANSWER The Periodic Table Element Infinitium has 9 protons and 12 neutrons. Its mass number is which is equal to the A. 9, number of protons B. 12, number of neutrons C. 9, number of electrons D. 21, sum of protons and neutrons E. 12 number of electrons J ITO 000 0 E = mc² 00 2llll Vz DIH H₂O Read QUESTION Trends Across the Periodic Table Consider the elements of Group II A, which of the following is correct according to increasing atomic size? A. H, Li, Na B. Mg, Ca, Sr C. Ca, Ba, Sr D. Na, Li, K 000 00- E = mc² All V2 Peg LTT DIA H₂0 ANSWER Trends Across the Periodic Table Consider the elements of Group II A, which of the following is correct according to increasing atomic size? A. H, Li, Na B. Mg, Ca, Sr C. Ca, Ba, Sr D. Na, Li, K JT ITM 000 00- E = mc² 00 21lll Vz Bea DIAH H₂O QUESTION Trends Across the Periodic Table Which of the following elements has the lowest electronegativity? A. Fluorine B. lodine C. Barium D. Aluminum E. Carbon 000 www E = mc² 00 Illll VZ LTT DIA H₂0 ANSWER Trends Across the Periodic Table Which of the following elements has the lowest electronegativity? A. Fluorine B. lodine C. Barium D. Aluminum E. Carbon JT 000 E = mc² 00 21llle Vz DIA H₂O Read QUESTION Trends Across the Periodic Table Within a given period of the periodic table, the element with the highest ionization energy is: A. Noble gas B. Transition Metal C. Alkali Metal D. Halogen E. Metalloid J 000 00- w E = mc² All V2 TTT DOH H₂0 Ma ANSWER Trends Across the Periodic Table Within a given period of the periodic table, the element with the highest ionization energy is: A. Noble gas B. Transition Metal C. Alkali Metal D. Halogen E. Metalloid Intermolecular Forces of Attraction Nonbonding (Intermolecular) Ion-dipole H bond Dipole-dipole Ion-induced dipole Dipole-induced dipole Dispersion (London) 8 -A-H.:B- Ion charge- dipole charge Polar bond to H- dipole charge (high EN of N, O, F) Dipole charges Ion charge- polarizable e cloud Dipole charge- polarizable e cloud Polarizable e clouds C 40-600 10-40 5-25 3-15 2-10 Chemical Bonds Na+ 'Н Ö-HÖ-H | H H Fe²+....0₂ H I-CI-CI H-CI CI-CI 0.05-40 F-FF-F Intermolecular Forces of Attraction ● Hydrogen bonds: attractive interaction of a hydrogen atom with an electronegative atom (N, O, F) that comes from another molecule or chemical group. d+ H 8+ H C Hydrogen Bonding between Ammonia and Water 8+ N H Chemical Bonds 8- 8+ Η ο δ- H 8+ Hydrogen bond Intermolecular Forces of Attraction Dipole-dipole interactions: electrostatic interactions of permanent dipoles in molecules (asymmetrical polar bonds; e. g. H20, HCI, HF). Attractive force between positive part of molecule and negative part of neighbored molecule 8+ 8 S+ C S+ to (a) Attraction S+ (c) Repulsion Chemical Bonds S+ 8+ S8+ (b) Attraction 8448 (d) Repulsion 8+ Intermolecular Forces of Attraction ● London dispersion forces (LDF): also called Van-der-Waals forces; weak intermolecular interactions arising from induced instantaneous polarization by random fluctuation of the electron density. The LDF between molecules increases with surface: ex: pentane 2-methyl butane 2,2- dimethyl propane Attraction Repulsion Repulsion + + Chemical Bonds € + + • electron groups notation e-group geometry AX2 Linear AX3 Trigonal planar AX4 Tetrahedral AX5 Trigonal bipyramid AX6 Octahedral 2 3 4 VSEPR: Electron Group Geometry and Molecular Group Geometry 5 6 tetrahedral trigonal pyramidal hybridization sp sp2 sp3 sp3d sp3d2 trigonal bipyramidal angle of separation 180 degrees 120 109.5 90, 120, 180 90, 180 octahedral Chemical Bonds linear trigonal planar linear bent or angular J 000 00- 0000 E = mc² 21lll Vz ATTIT DIA H₂O Read QUESTION VSEPR Determine the molecular shape of the following compounds: I. PF3 II. SbF5 III. COCI₂ 000 E = mc² All V2 DA H₂0 M ANSWER VSEPR Determine the molecular shape of the following compounds: I. PF3 - Trigonal pyramidal II. SbF5 - Trigonal bipyramidal III. COCI₂ - Trigonal planar Theories ● ● Arrhenius Acids: Produce H+ when in water Base: Produce OH- when in water ● Bronsted Lowry Theory Acid: Proton (H+) donor Base: Proton (H+) acceptor ● ● Amphoteric Conjugate acid-base pairs Lewis Theory • Acid: electron pair acceptor ● Base: electron pair donor ● Acids and Bases pH and pOH ● Water Equilibrium Pure water contains very small amounts of hydronium and hydroxide ions. These small amounts result in the autoionization of water • Kw = [H+][OH-] W Acids and Bases Dissociation of water results in one mole H* and one mole OH-, thus their concentrations are the same ([H+] = [OH-] = 1 x 107) pH Scale ● pH = -log[H+] pOH = -log[OH-] pH + pOH = 14 ● Strength ● ● ● C ● Acids and Bases STRONG ACIDS Completely dissociate thus, have very large values of Ka ● • The conjugate base of strong acids are very weak bases. Ex: HNO3, H₂SO4, HI, HBR, HCI, HCIO3, HCIO4 WEAK ACIDS Remain largely undissociated and have relatively small values of Ka STRONG BASES Quantitatively converted into hydroxide ion in aqueous solution. • Ex. NaOH, KOH, Ca(OH)2 and Mg(OH)2 ● WEAK BASES partially react with water to produce hydroxide ions. Rules for Predicting the pH of Aqueous Solutions In General: Neutral lons: Acids: Bases: C Acids and Bases Aqueous solutions of covalent oxides are acidic All Group 1A and 2A cations Anions which are conjugates of strong acids Uncharged strong or weak acids Metal cations other than those of Groups 1A and 2A Cationic conjugates of nitrogen bases The two anions HSO4 and H₂PO4 All anions not listed above Uncharged nitrogen bases J ITM 000 00- E = mc² Illll Vz DIH H₂0 Read QUESTION Acids and Bases Which of the following compounds acts as an acid in this reaction? 4 LiH + AICI → LIAIH4 + 3 LICI 3 I. LiH A. I, III B. C. D. II, IV I, IV II, III II. AICI 3 III. LIAIH4 IV. LICI 000 E = mc² -01 00- 2|ll| V2 DIA H₂O ANSWER Acids and Bases Which of the following compounds acts as an acid in this reaction? 4 LiH + AICI → LIAIH4 + 3 LICI 3 I. LiH A. B. C. D. I, III II, IV I, IV II, III II. AICI 3 III. LIAIH4 IV. LICI JT IYM 000 00- E = mc² 00 21lll Vz Bea DIA H₂O QUESTION Acids and Bases Which of the theories was applied in here? 4 LIH+ AICI → LIAIH4 + 3 LICI A. Lewis B. Bronsted-Lowry C. Arrhenius 000 E = mc² 1-01 H0 00 21||||| V2 geo DIA H₂0 ANSWER Which of the theories was applied in here? Acids and Bases 4 LIH+ AICI → LIAIH4 + 3 LICI A. Lewis B. C. Arrhenius Bronsted-Lowry J IYM 000 0000 00- E = mc² Illll Vz Bea ARTIS RIH H₂O QUESTION Acids and Bases 4 Upon investigation of a HCIO solution, it was found out that it has a pH of 2. What is the value of the concentration of H+ ions in the solution? A. 0.001 M B. 1 x 10¹2 M C. 0.01 M D. 1 x 1010 M 000 H0 E = mc² 21||||| V2 TTT DOH H₂0 Mama ANSWER Acids and Bases 4 Upon investigation of a HCIO solution, it was found out that it has a pH of 2. What is the value of the concentration of H+ ions in the solution? A. 0.001 M B. 1 x 10¹2 M C. 0.01 M D. 1 x 1010 M JT ITM 000 H 0000 E = mc² 2llle VZ DIA H₂O Read QUESTION Acids and Bases What is the value of the concentration of OH- ions in the solution? What is the pOH of the solution? A. 1 x 10-12 M, 2 B. 0.001 M, 2 C. 1 x 10-12 M, 12 D. 0.001 M, 12 000 HO E = mc² Illll VZ DA H₂O Mama ANSWER Acids and Bases What is the value of the concentration of OH- ions in the solution? What is the pOH of the solution? A. 1 x 10-12 M, 2 B. 0.001 M, 2 C. 1 x 10-12 M, 12 D. 0.001 M, 12 Chemical Reactions Limiting Reagent Excess Reagent Percent Yield Theoretical Yield Stoichiometry Empirical Formula Molecular Formula Molecular and Empirical Formula Steps: C Stoichiometry 1. Assume 100g of sample 2. Calculate moles of elements in 100g 3. Write tentative formula based on number of moles 4. Divide all mole numbers by smallest mole number 5. Write the new formula. Chemical Reactions ● Balance reactions Limiting reactant is consumed entirely Excess reactant is in excess Stoichiometry When you forget to balance the chemical reaction I have failed you. Sorry Thanos..... Types of Reactions ● ● ● ● ● C Synthesis: elements are joined to form compounds Decomposition: a compound breaks into parts Single Replacement: an element replaces another element in a compound Double Displacement: elements from two compounds 'switch' places Combustion: the formation of by products such as CO₂ and water Redox Reactions: ● Chemical Reactions Oxidation (LEORA): Lose Electrons, Oxidized, Reducing Agent Reduction (GEROA): Gain Electrons, Reduced, Oxidizing Agen Equilibrium C Chemical Reactions • Presence of backward and forward reaction ● • At equilibrium, no observable MACROSCOPIC change occurs however the forward and backward reactions still occur simultaneously Le Chatelier's Principle states that when a disturbance in a system in equilibrium occurs, the system adjusts to restore the state of equilibrium. Reactions ● C ● Chemical Reactions Activation energy ● • The minimum amount of energy reactants should possess in order for the reaction to proceed May be overcome via easier reactions with the use of catalysts Arrhenius equation Reaction constant depends on temperature and activation energy Reaction rates • A model of how fast a reaction proceeds Depends on reaction constant and concentration/pressure J ITM 000 H E = mc² 00 21lll Vz DIA H₂O QUESTION Stoichiometry In the production of methanol, the following reactions schemes are followed. ΔΗ CO₂ + 3H₂ CH3OH + H₂O AH 298K = -49.6 kJ/mol CH3OH AH 298K = -90.8 kJ/mol ΔΗ CO + 2H₂ There are 12 moles of H₂(g), present in the system while there are 2 moles of CO₂ and 4 moles of CO. Which of the following is the limiting reagent? A. Hydrogen gas B. Carbon monoxide C. Carbon dioxide D. Methanol J E = mc² 1-001 00 00- 2llll V2 TTT DIA H₂0 ANSWER Stoichiometry In the production of methanol, the following reactions schemes are followed. ΔΗ CO₂ + 3H₂ CH3OH + H₂O AH298K = -49.6 kJ/mol CO + 2H₂ → CH3OH AH 298K = -90.8 kJ/mol ΔΗ → There are 12 moles of H₂(g), present in the system while there are 2 moles of CO₂ and 4 moles of CO. Which of the following is the limiting reagent? A. Hydrogen gas B. Carbon monoxide C. Carbon dioxide D. Methanol J ITM 000 10000 f:.of E = mc² 00 Illlll Vz Bea ARTIT DIA H₂O QUESTION Stoichiometry Vitamin C is essential for preventing scurvy. Combustion of a 0.2 g sample of this compound yields 0.2998 g of carbon dioxide and 0.0819 g of water. What is the empirical formula of Vitamin C? J 00- E = mc² 00 Illll V2 Peg TTT DOH H₂0 ANSWER Stoichiometry Vitamin C is essential for preventing scurvy. Combustion of a 0.2 g sample of this compound yields 0.2998 g of carbon dioxide and 0.0819 g of water. What is the empirical formula of Vitamin C? Empirical formula: C3H403 JT ITM 000 00- E = mc² 00 21lll Vz T DIH H₂O tego QUESTION Stoichiometry Hydrogenation of carbon dioxide to form methanol is an exothermic reaction, meaning that heat is expelled from the system as the reaction proceeds. CO₂ + 3H₂ CH3OH + H₂O CH₂OH+H₂O AH298K = -49.6 kJ/mol ΔΗ, Which effect would result due to the addition of heat? A. Production of more carbon dioxide B. Production of more methanol C. Lower energy requirement D. No effect since the reaction is already in equilibrium π 00 E = mc² 2lll V2 TTT DIA H₂0 ANSWER Stoichiometry Hydrogenation of carbon dioxide to form methanol is an exothermic reaction, meaning that heat is expelled from the system as the reaction proceeds. CH₂OH+H₂O AH298K = -49.6 kJ/mol ΔΗ, CO₂ + 3H₂ CH3OH + H₂O Which effect would result due to the addition of heat? A. Production of more carbon dioxide B. Production of more methanol C. Lower energy requirement D. No effect since the reaction is already in equilibrium J ITM 000 E = mc² 2lll VZ FITNE DIH H₂O QUESTION Stoichiometry In the production of methanol, the following reactions schemes are followed. CO2 + 3H2 + CH3OH + H₂O CO + 2H₂ CH3OH ΔΗ, AH 298K ΔΗ 298Κ = -49.6 kJ/mol = -90.8 kJ/mol There are 12 moles of H2(g), present in the system while there are 3 moles of CO₂ and 3 moles of CO. Which of the following is in excess if 6 moles of hydrogen react with the carbon monoxide? A. Hydrogen gas B. Carbon monoxide C. Carbon dioxide D. Methanol 000 00- E = mc² Illll VZ Peo LTT DOH H₂0 Ma ANSWER Stoichiometry In the production of methanol, the following reactions schemes are followed. ΔΗ, AH 298K -49.6 kJ/mol AH298K = -90.8 kJ/mol There are 12 moles of H2(g), present in the system while there are 3 moles of CO₂ and 3 moles of CO. Which of the following is in excess if 6 moles of hydrogen react with the carbon monoxide? A. Hydrogen gas B. Carbon monoxide C. Carbon dioxide D. Methanol CO2 + 3H2 + CH3OH + H₂O CO + 2H₂ CH3OH = Gas Laws Law Boyle's Law Charles' Law Gay-Lussacs Law Description At constant temperature, as pressure decreases, volume increases. At constant pressure, volume changes directly with temperature. At constant volume, pressure increases with temperature C P1V1= P2V2 V1/T1= V2/T2 P₁/T1= P2/T2 Gases Formula Ideal Gas Law Variable P V T R N Ideal Gas Law Equation PV = nRT Name Pressure Volume Temperature Ideal Gas Law Constant Moles Definition The force per unit area that the gas exerts on the any surface. The amount of space occupied. The measure of the average kinetic energy in a system 0.0821 8.31 LokPa mol K mol K 6.022 X1023 Particles Units atm, mmHg, kPa L K Mol Measured by: Gases Barometer, pressure gauge Graduated Cylinder Thermometer Calculated Number of particles in 12 grams of carbon-12. JT 000 0000 H E = mc² 21lll Vz BER RIA H₂O QUESTION Gases What is the temperature of 50g of oxygen gas in atmospheric pressure contained in a 0.05 cubic meter container? Molecular weight of oxygen gas: 32 g/mol R = 0.0821 L-atm/mol K A. 390 K B. 390 C C. 195 K D. 195 C 000 00 00- E = mc² Ylli V2 DOH H₂0 Ma ANSWER Gases What is the temperature of 50g of oxygen gas in atmospheric pressure contained in a 0.05 cubic meter container? Molecular weight of oxygen gas: 32 g/mol R = 0.0821 L-atm/mol K A. 390 K B. 390 C C. 195 K D. 195 C JT ITM 000 E = mc² 00 21lll VZ BER DIH H₂O QUESTION Gases A container contains 5 moles of Argon at room temperature (25°C) and atmospheric pressure (1 atm). If the gas is heated to a temperature thrice the initial temperature, by what factor should the pressure change for the system to maintain it's volume? A. -1/3 B. -3 C. 1/3 D. 3 J 000 E = mc² 1-001 00- -0-0- 2|ll| VZ TTT DA H₂0 ANSWER Gases A container contains 5 moles of Argon at room temperature (25°C) and atmospheric pressure (1 atm). If the gas is heated to a temperature thrice the initial temperature, by what factor should the pressure change for the system to maintain it's volume? A. -1/3 B. -3 C. D. 3 1/3 Solubility Rules for lonic Compounds ● Solubility Almost all salts of the Group 1A (alkali metals) and of NH4+ are soluble in water. All nitrates are soluble in water. Most chlorides, bromides and iodides are soluble, the exceptions are those of Ag+ and Hg₂2+ Most sulfates are soluble, the major exceptions being those of barium, lead, mercury, bismuth and tin. Calcium sulfate is sparingly soluble. Most carbonates, oxides, hydroxides, phosphates and sulfides are insoluble. Exceptions are the alkali metals (rule 1). Calcium and barium hydroxides are fairly soluble. 000 0000 JT E = mc² 21lll VZ DIH H₂O QUESTION Solubility Which of the following metals when mixed with sulfate, will not dissolve in water? I. Sr²+ II. Hg2+ III. Pb²+ IV. Ba²+ A. I, II, IV only B. I, III, IV only C. III, IV only D. I, II, III, IV 000 00- E = mc² Yll V2 DIA H₂0 ANSWER Solubility Which of the following metals when mixed with sulfate, will not dissolve in water? I. Sr²+ II. Hg2+ III. Pb²+ IV. Ba²+ A. I, II, IV only B. I, III, IV only C. III, IV only D. I, II, III, IV System vs. Surroundings ● ● ● "Energy is neither created nor destroyed, it can only be transformed from one form to another." System vs Surroundings • system + surroundings universe = Thermodynamics Values are hard to obtain, thus reference states to which values are set arbitrarily Reversible and irreversible reactions • Egg and ice analogy ● Terms ● ● ● Internal Energy: total heat content of system Heat (q) (+) heat INTO system ● (-) heat OUT of system Work • (+) work done TO system (-) work done BY system Thermodynamics Entropy: overall entropy is always positive Spontaneity: AG = AH - TAS • If positive, spontaneous. If negative, non-spontaneous. ● JT ITM 000 00- E = mc² 00 2llll VZ BER DIH H₂O QUESTION Thermodynamics A movable constant pressure piston contains 3 moles of air with temperature of 25C. The piston is then heated up to 80°C. What is the value of the change in internal energy? Assume ideal gas. R = 8.314 J/mol.K Molecular weight of air: 29 g/mol. Heat capacity of air (constant pressure): Heat capacity of air (constant volume): A. 140.14 kJ B. 138.77 kJ C. 1.37 kJ D. 14.1 kJ 29 J/mol.K 20.8 J/mol-K J 00- E = mc² 2lll V2 LTT DA H₂O ANSWER Thermodynamics A movable constant pressure piston contains 3 moles of air with temperature of 25C. The piston is then heated up to 80°C. What is the value of the change in internal energy? Assume ideal gas. R = 8.314 J/mol.K Molecular weight of air: 29 g/mol. Heat capacity of air (constant pressure): Heat capacity of air (constant volume): A. 140.14 kJ B. 138.77 kJ C. 1.37 kJ D. 14.1 kJ 29 J/mol K 20.8 J/mol.K JT ITM 000 E = mc² 21lll Vz Bea DIH H₂O QUESTION Thermodynamics 50g of boiling water (100°C) is contained inside a calorimeter. A 83.5g strip of copper with temperature 25°C is then put in the calorimeter for cooling. What is the final temperature of the system? Specific heats: water: 4.184J/g.K; copper: 0.385 J/g. K A. 20°C B. 28°C C. 53°C D. 90°C J 00- E = mc² -0-0 All V2 ALTINIS DIA H₂0 ANSWER Thermodynamics 50g of boiling water (100°C) is contained inside a calorimeter. A 83.5g strip of copper with temperature 25°C is then put in the calorimeter for cooling. What is the final temperature of the system? Specific heats: water: 4.184J/g.K; copper: 0.385 J/g. K A. 20°C B. 28°C C. 53°C D. 90°C Functional Groups Functional Groups - The Main Players H₂ H₂C-C alkane CH 3 -N(H, R) 2 amine alkene alcohol ether =H ester alkyne i i i b aldehyde ketone carboxylic acid :::: benzene ring (phenyl) alkyl halide thiol N(H,R) 2 amide -CEN: Functional Groups - Supporting Actors nitrile C anhydride H Organic Chemistry epoxide nitro disulfide imine acid chloride sulfide (thioether) ● ● ● alkanes = CnH2n+2 alkenes = CnH2n alkynes = CnH2n-2 Organic Chemistry ADMIT IT. IT DOESN'T MATTER IF YOU UNDERSTAND ORGANIC CHEMISTRY OR NOT 0 BUT DRAWING BENZENE GIVES A GREAT PLEASURE J 000 0000 00- E = mc² 2llll Vz ARTI DIH H₂0 Read QUESTION Organic Chemistry Which of the following functional groups are present in the thiamine, the compound shown below? A. ketone, imine, amine B. alcohol, sulfide, amine C. alcohol, imine, amide D. ketone, sulfide, amide N CI™ *N* S NH₂ thiamine -OH π E = mc² -0-0- Illll V2 ALTINIS DOH H₂O ANSWER Organic Chemistry Which of the following functional groups are present in the thiamine, the compound shown below? A. ketone, imine, amine B. alcohol, sulfide, amine C. alcohol, imine, amide D. ketone, sulfide, amide N CI *N* S NH₂ thiamine -OH wi √2 |||| H- ANF = mc² H₂O T ALL I AM CYCLOPROPANE UNDER TOO MUCH STRESS AND PROBABLY SHOULD HAVE FALLEN APART BUT SOMEHOW STILL HERE 000 M U VZ VILDRE 18.0 معه Ins n DIS H₂O