Stuff to Know for the Final Exam I

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Valentine Eugene Powers
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1 Exam I Kinetics Rates; relationships Rate Laws Reaction Orders Rate versus time; 1st and 2nd order linear equations and graphs Half life; 1st and 2nd order E a, transition state, ΔE, E profile Arrhenius equation (k vs. T) Mechanisms, elementary reactions, intermediates, catalysts Rate determining step Catalysts Enzymes 2

Exam I K eq expression, solids and liquids

2 Exam I K eq expression, solids and liquids K c, K p, relationship Meaning of large/small K Manipulation of multistep reaction K eq s and overall K eq Relationship of Q to K Le Chatelier s Principle Change in pressure Change in concentration Change in temperature 3

Up to 20 n=p stable Above AN 83 alpha decay High n/p beta decay Low n/p light nuclei, positron High n/p, heavy, e -

3 Stuff to Know for For the Final Exam 1 Nuclear Chemistry Nucleon symbols, 5 types of decay Balance nuclear reactions Stability; Compare isotope in P.T. Up to 20 n=p stable Above AN 83 alpha decay High n/p beta decay Low n/p light nuclei, positron High n/p, heavy, e - capture Detection of radioactivity Effects of radioactivity Kinetics Rate (k) in dps per atom Half life and k Ratio of Nt/No Binding Energy Fusion and Fission Nuclear Reactors, Atomic bombs Medical Applications, 4

Exam 2 Acids and Bases: Qualitative Conjugate Acids and Bases, relative strength Memorize 7 Strong Acids Memorize 7 Strong Bases Auto-ionization of Water, K w K a for weak

Identify Lewis acids and bases Acids and Bases: Quantitative Calculation of ph for strong acids and bases, relationship to [H + ] Calculation of poh, relationship to ph and pk

4 Exam 2 Acids and Bases: Qualitative Conjugate Acids and Bases, relative strength Memorize 7 Strong Acids Memorize 7 Strong Bases Auto-ionization of Water, K w K a for weak acids, acid dissociation reaction K b for weak bases, base hydrolysis reaction K a K b = K w Identify acidic or basic ions in salts Correlate acid strength with structure Identify Lewis acids and bases Acids and Bases: Quantitative Calculation of ph for strong acids and bases, relationship to [H + ] Calculation of poh, relationship to ph and pk w Calculation of ph for weak acids and bases: equilibrium problem solving (ice) Calculation of concentrations/ph for polyprotic acids, K a1 vs. K a2 etc. Calculate ph of salt solutions 5

ions Effective Nuclear Charge Formation of ions Trends in metallic character Trends

5 Exam 2 Periodicity (Ch. 7, 22) Ionization Energy Electron Affinity Compare radii of atoms Compare radii of ions Effective Nuclear Charge Formation of ions Trends in metallic character Trends in reactivity Trends in electronegativity Metallic character Reactions of hydroxides with H 2 O Identify acidic or basic hydroxides or oxides 6

6 Exam 2 Buffers and Titrations (Ch. 17) Common ion effect, LeChatelier s Principle Definition of buffer, identify components Define buffer capacity and range Calculate ph of a buffer H-H equation Interpret graph of titration curve Identify components and balanced reaction at any point during a titration Find ph of acid/base mixture at any point during a titration Identify and define equivalence point Choose appropriate indicator Polyprotic acid titrations 7

Exam 2 Spontaneity Define spontaneity, reversibility of reactions Define absolute entropy Define ΔS, relationship to q rev Identify which substance has more absolute entropy Second Law of

7 Exam 2 Spontaneity Define spontaneity, reversibility of reactions Define absolute entropy Define ΔS, relationship to q rev Identify which substance has more absolute entropy Second Law of Thermodynamics; describe the ΔS of a spontaneous process Define microstate, and how it relates to entropy changes Predict which process or reaction has a positive entropy change Third Law; Define absolute entropy at 0K Calculate entropy change for a process Identify effect of volume change, temperature change, or pressure change on entropy 8

8 Useful Information (Exam 2) Acid Dissociation HA(aq) H + (aq) + A - (aq) Equilibrium constant = K a K a = [H + ][A ] [HA] Base Hydrolysis B(aq)+H 2 O( ) HB + (aq) + OH(aq) Equilibrium constant = K b K b = [HB+ ][OH ] [B] 9

Useful Information (Exam 2) ph = log 10 [H + ]

9 Useful Information (Exam 2) ph = log 10 [H + ] low ph = acidic high ph = basic poh= log 10 [OH ] at 25 C = 298K K w = [H + ][OH ] = 1.0 x pk w = log 10 K w = 14 pk w = ph + poh = 14 = log 10 [H + ] + log 10 [OH ] [H + ] [OH - ] = K a K b = K w ph + poh = pk a +pk b = pk w 10

both mean weak acid and not much dissociation. GIVEN a mixture: what is left in solution? Strong acid? strong base?

10 Acid/Base Basics YOU SHOULD KNOW GIVEN FIND ph [H + ], [OH - ], poh [H + ] or [OH - ] ph List of pk a s or K a s Weaker /Stronger K a or pk a and [HX] ph, [H + ], [OH - ] ph and [HX] K a Salt ph Buffer ph Recall that a small K a high pk a, and both mean weak acid and not much dissociation. GIVEN a mixture: what is left in solution? Strong acid? strong base? weak acid or base? Buffer? Then FIND ph. 3 definitions of acids and bases Identify conjugate acid base pairs Identify Lewis acids and bases. 11

of a common ion Calculate solubility given the ph Identify when ph affects solubility Describe Lewis acid/base interactions and metal

11 Exam 3 Solubility & Precipitation (Ch. 17) Write K sp expression and corresponding balanced reaction Define solubility Calculate solubility Calculate solubility in the presence of a common ion Calculate solubility given the ph Identify when ph affects solubility Describe Lewis acid/base interactions and metal complexes Write K f expression and corresponding balanced reaction Calculate concentrations using K f Define amphoteric Compare Q to K sp, predict solubility Predict which ion of a mixture precipitates first at a given ph and concentration 12

Exam 3 Thermodynamics: Define Free Energy ΔG = Δ H T ΔS ΔG and Spontaneity

equilibrium, relationship to K eq Standard Free Energy, conditions Free Energy

Energy of reaction using individual ΔG f Variation of ΔG with temperature;

12 Exam 3 Thermodynamics: Define Free Energy ΔG = Δ H T ΔS ΔG and Spontaneity Sign of ΔG Qualitative prediction of ΔG, affect of temperature Value of ΔG at equilibrium, relationship to K eq Standard Free Energy, conditions Free Energy of Formation, value for pure elements under standard state conditions Free Energy of reaction using individual ΔG f Variation of ΔG with temperature; predict boiling point or melting point Calculate ΔG under non-standard conditions using Q 13

Exam 3 Redox Chemistry Rules for assigning Oxidation States Balance

! Voltaic cells, spontaneity What is Cathode, Anode, e - flow direction,

each electrode E cell, E o, SHE Oxidizing and Reducing agents, strengths of

13 Exam 3 Redox Chemistry Rules for assigning Oxidation States Balance Reactions/half rxns KNOW THE RULES!! Voltaic cells, spontaneity What is Cathode, Anode, e - flow direction, effect of changing concentrations or electrode size What are products at each electrode E cell, E o, SHE Oxidizing and Reducing agents, strengths of each Dependence on K, Q, ΔG, work Nernst eq., Concentration cells Electrolytic cells, predict products Quantitative electrochem 14

Exam 3 Redox Chemistry: Batteries; balance reactions, identify anode and cathode, know description of fuel cell, calculate voltage Cathodic protection, corrosion

14 Exam 3 Redox Chemistry: Batteries; balance reactions, identify anode and cathode, know description of fuel cell, calculate voltage Cathodic protection, corrosion Calculate amount of current, time required, work, energy, predict g of product, amount of power Metallurgy Sources of metals Oxidation states of metals in minerals Definitions (hydrometallurgy, pyrometallurgy, calcination, etc.) Apply concepts to metallurgy e.g. complex ion formation as means of obtaining metals like Ag and Au Use of electrolysis to reduce metals Use of acid base chemistry (in processing of Al, and smelting of iron( Given metallurgical process, what is being oxidized and reduced? 15

Transition Metals Electron configuration Neutral metal Metal ions Number Valence

ions, charge on metal Mono-dentate, poly-dentate Coordination number Chelating

(octahedral geometry) Diamagnetic, Paramagnetic Color absorbed/transmitted

15 Transition Metals Electron configuration Neutral metal Metal ions Number Valence electrons Lewis acids and bases Complex Ions Coordination of Ligands Complex ions, charge on metal Mono-dentate, poly-dentate Coordination number Chelating Ligands # coordination sites, charge Chelate effect Crystal Field Theory (octahedral geometry) Diamagnetic, Paramagnetic Color absorbed/transmitted Crystal Field Splitting Energy Electron configurations Spin pairing energy High spin/low spin 16

Compare strength of IMF s Use phase diagram, know definitions Identify crystalline or amorphous solid Predict type of crystal formed;

16 Stuff to Know for Final Molecular Orbital Theory Shapes of orbitals Identify bonding, antibonding, sigma, pi, node, star Know relative energy of molecular orbitals Use MO diagram to determine bond order and number of unpaired electrons Bonding and Structure of Solids Compare strength of IMF s Use phase diagram, know definitions Identify crystalline or amorphous solid Predict type of crystal formed; molecular, atomic, network covalent, metallic, ionic Know properties of types of solids; ability to conduct electricity, hardness, MP/BP comparison 17

17 Periodicity (Ch. 7, 22) Ionization Energy Electron Affinity Compare radii of atoms Compare radii of ions Effective Nuclear Charge Formation of ions Trends in metallic character Trends in reactivity Trends in electronegativity Metallic character Reactions of hydroxides with H 2 O Identify acidic or basic hydroxides or oxides Period 2 versus 3 bonding trends 18

Stuff to Know for Final Chemistry of the Elements Occurrence of elements

Nonmetals Metals (metallurgy) Periodic Trends Size Ionization energy and

properties Trends in oxidation states Trends in bonding Period II vs.

18 Stuff to Know for Final Chemistry of the Elements Occurrence of elements Abundance Where in nature State of elements Isolation and purification Nonmetals Metals (metallurgy) Periodic Trends Size Ionization energy and Electron affinity electronegativity Metallic Character Trends in Acid/base properties Trends in oxidation states Trends in bonding Period II vs. Period III Know the trends! Effects of Bonding: Hydrides Summary of Periodic Trends For Groups I, II, II, IV and V 19

properties of Ceramics Structure of Metals Mechanical Properties Malleability of metals and alloys

19 Bonding in Metals Electrical Properties Bonding in metals Band theory Electrical conductivity Semiconductors Examples (n-type and p-type) Semiconductor devices (diodes and LEDs) Electrical properties of Ceramics Structure of Metals Mechanical Properties Malleability of metals and alloys Real-world example (high-strength Al) Defects in metals Hardening of metals/alloys Alloys Iron and steel Amorphous alloys 20

20 Modern Materials Polymers Polymer synthesis Polymers: properties Ceramics Silicates: Glasses Aluminosilicates: Zeolites 21

Miami Dade College CHM Second Semester General Chemistry

Miami Dade College CHM Second Semester General Chemistry Miami Dade College CHM 1046 - Second Semester General Chemistry Course Description: CHM 1046 is the second semester of a two-semester general chemistry course for science, premedical science and engineering