普通化学(全英文)教学大纲 Syllabus for general chemistry () ClassWebpagehttp://www.chemistry.fudan.edu.cn/mnetteacher/gfzheng/teaching.html 1. Introduction( Chapter 1-3) 1. 1. Elements, compounds and mixtures 12. Atoms. molecules and ions 1.3. SI units and converting units nd intensive prope 1.5. Amount of substance 16. Law of conservation of matter 1.7. Mass relationships in chemical reactions 18. Balancing the chemical reaction 1.9. Limiting reactants 1. 10. Empirical formula 2. Electronic Structures and the Periodic table(chapter 7-8) 2.1. Atomic structure, Isotope 2.2. The period ic table (a). Main groups, metals and non-metals (b). S-block, p-block, d-block elements 23. Electron cloud and Atomic orbitals 2 4. Electron configurations (a). 4 quantum numbers: n, l,m,ms (b). Pictures of the orbitals: S, px, py, pz (c). How to fill electrons in different orbitals (d). Be able to draw the electron configuration of the first 20 elements (e). Unpaired electrons, Spin, Paramagnetic and Diamagnetism 2.5. Comparing the atomic orbitals with Bohr's model of atoms( Classical but incorrect) 2.6. Electron's states a). Each state is related to specific energy (b). e" will transit between states when absorbing/giving off energy, in a form of" light (c). Ground state, Excited states, the first excited state (d). Energy of light": relationship among wavelength, frequency, and photon's energy (e). Absorption spectrum and Emission spectrum (f). Red shift and blue shift Materials color
普通化学（全英文）教学大纲 Syllabusfor General Chemistry (I) Class Webpage: http://www.chemistry.fudan.edu.cn/m_netteacher/gfzheng/teaching.html 1．Introduction (Chapter 1—3) 1.1．Elements, compounds, and mixtures 1.2．Atoms, molecules and ions 1.3．SI units and converting units 1.4．Extensive and intensive properties 1.5．Amount of substance 1.6．Law of conservation of matter 1.7．Mass relationships in chemical reactions 1.8．Balancing the chemical reaction 1.9．Limiting reactants 1.10．Empirical formula 2．Electronic Structures and the Periodic Table (Chapter 7—8) 2.1．Atomic structure, Isotope 2.2．The periodic table (a)．Main groups, metals and non-metals (b)．s-block, p-block, d-block elements 2.3．Electron cloud and Atomic orbitals 2.4．Electron configurations (a)．4 quantum numbers: n, l, m, ms (b)．Pictures of the orbitals: s, px, py, pz (c)．How to fill electrons in different orbitals (d)．Be able to draw the electron configuration of the first 20 elements (e)．Unpaired electrons, Spin, Paramagnetic and Diamagnetism 2.5．Comparing the atomic orbitals with Bohr’s model of atoms (Classical but incorrect) 2.6．Electron’s states (a)．Each state is related to specific energy (b)．e - will transit between states when absorbing/giving off energy, in a form of “light” (c)．Ground state, Excited states, the first excited state (d)．Energy of “light”: relationship among wavelength, frequency, and photon’s energy (e)．Absorption spectrum and Emission spectrum (f)．Red shift and blue shift (g)．Materials’ color
2.7. Atomic and ionic rad i 2.8. Ionization energy: the first, second,.. ionization energy 2.9. Electron affinity (Note here we use a different definition of the electron affinity from the textbook.) 2.10. Exothermic and Endothermic reactions 3. Chemical Bonds, Valence Bond, and Molecular Shape(Chapter 9) 31. Valence electrons 3.2. Ionic bond 33. Covalent bond 3. 4. Lewis structures (a). Octet rule (b). Single, double, and triple bonds (c). Bond order, bond length, and bond energy Be able to calculate the heat of a reaction from the given bond energies (d). Lone pair electrons, Coordinate bond (e). Be able to write Lewis structures of common molecules ( f. Exception of the octet rule: more than 8 e"; fewer than 8e"; odd number of e (g). Resonance structures (h ). Formal charges -a way to select the most effective Lewis structure(s) (. Failure of Lewis structure: octet rule exception; resonance structure; paramagnetism 3.5. Electronegativity 3.6. Nonpolar and polar covalent bonds 3.7. Valence Bond (VB)method (a). Definition of the valence bond method (b). g bond andπbond How o bond and T bond are made from S, px, py, pz orbitals? How o bond and bond relate to single/double/triple bonds (c). Hybrid orbitals(only applied to central atoms ): sp, sp, sp, spd (d ). Bond angle and the shape of molecules (e). Cis-and Trans-isomerism(sp- hybrid f). VSEPR method: predict the electron pair shapes and molecular shapes How to calculate the hybrid type of the central atom(s) How to arrange lone pair electrons and bonding electrons (g). Advantages and disad vantages of the Vb method 3.8. Molecule's polarity: sum of all bonds' dipoles 3.9. Brief introduction to organic molecules
2.7．Atomic and ionic radii 2.8．Ionization energy: the first, second, … ionization energy 2.9．Electron affinity (Note here we use a different definition of the electron affinity from the textbook.) 2.10．Exothermic and Endothermic reactions 3．Chemical Bonds, Valence Bond, and Molecular Shape (Chapter 9) 3.1．Valence electrons 3.2．Ionic bond 3.3．Covalent bond 3.4．Lewis structures (a)．Octet rule (b)．Single, double, and triple bonds (c)．Bond order, bond length, and bond energy: Be able to calculate the heat of a reaction from the given bond energies (d)．Lone pair electrons, Coordinate bond (e)．Be able to write Lewis structures of common molecules (f)．Exception of the octet rule: more than 8 e- ; fewer than 8 e- ; odd number of e- (g)．Resonance structures (h)．Formal charges – a way to select the most effective Lewis structure(s) (i)．Failure of Lewis structure: octet rule exception; resonance structure; paramagnetism 3.5．Electronegativity 3.6．Nonpolar and polar covalent bonds 3.7．Valence Bond (VB) method (a)．Definition of the valence bond method (b)．σ bond and π bond How σ bond and π bond are made from s, px, py, pz orbitals? How σ bond and π bond relate to single/double/triple bonds? (c)．Hybrid orbitals (only applied to central atoms): sp, sp2 , sp3 , sp3d (d)．Bond angle and the shape of molecules (e)．Cis- and Trans- isomerism (sp2 hybrid) (f)．VSEPR method: predict the electron pair shapes and molecular shapes How to calculate the hybrid type of the central atom(s) How to arrange lone pair electrons and bonding electrons (g)．Advantages and disadvantages of the VB method 3.8．Molecule’s polarity: sum of all bonds’ dipoles 3.9．Brief introduction to organic molecules
4. Molecular Orbital(MO) Method( Chapter 10) 41. Introduction to the mo method (a). Bonding, Antibond ing, and Nonbonding MOs (b). g bond andπbond Compare" o bond and T bond"in VB method and in MO method 4.2. Bond orders, unpaired electrons (a). Compare"Bond order"definitions in Lewis structure, VB, and MO method (b). Compare"Lone pair electrons"in Lewis structure, VB, and MO method (c). Predict the stability of molecules/ions (d). Predict paramagnetism/diamagnetism of a molecule 4.3. Homonuclear diatomic molecules(1st and 2nd period elements) 44. Heteronuclear d atomic molecules 4.5. Conjugated II bond and electron delocalization (a). Be able to judge whether a molecule has a conjugated II bond (b). Draw the molecular shape, and jud ge the p-orbitals and p-electrons (c). Calculate the IInm 46. HOMO and LUMO 4.7. Band theory of bonding in solids (a). Valence band, conduction band, band gap (b). Metal, semiconductor and insulator 48. Inter-molecular interactions (a). van der Waals interaction: polar VS. nonpolar molecules (b). Hydrogen bond (c). Bond energy: chemical bond > hydrogen bond> van der Waals interaction (d). Relationship of Inter-molecular interactions with Melting, boiling point, hardness (e). Hydrophobic and hydrophilic interaction 4.9. Introduction to proteins and nucleic acids (a). Amino acid Peptide Protein: which interactions are involved in each step? (b). Oligonucleotide, Single strand DNA,Double strand DNA: which interactions?
4．Molecular Orbital (MO) Method (Chapter 10) 4.1．Introduction to the MO method (a)．Bonding, Antibonding, and Nonbonding MOs (b)．σ bond and π bond Compare “σ bond and π bond” in VB method and in MO method 4.2．Bond orders, unpaired electrons (a)．Compare “Bond order” definitions in Lewis structure, VB, and MO method (b)．Compare “Lone pair electrons” in Lewis structure, VB, and MO method (c)．Predict the stability of molecules/ions (d)．Predict paramagnetism/diamagnetism of a molecule 4.3．Homonuclear diatomic molecules (1st and 2nd period elements) 4.4．Heteronuclear diatomic molecules 4.5．Conjugated Π bond and electron delocalization (a)．Be able to judge whether a molecule has a conjugated Π bond (b)．Draw the molecular shape, and judge the p-orbitals and p-electrons (c)．Calculate the Πnm 4.6．HOMO and LUMO 4.7．Band theory of bonding in solids: (a)．Valence band, conduction band, band gap (b)．Metal, semiconductor and insulator 4.8．Inter-molecular interactions (a)．van der Waals interaction: polar vs. nonpolar molecules (b)．Hydrogen bond (c)．Bond energy: chemical bond >> hydrogen bond > van der Waals interaction (d)．Relationship of Inter-molecular interactions with Melting, boiling point, hardness (e)．Hydrophobic and hydrophilic interaction 4.9．Introduction to proteins and nucleic acids (a)．Amino acid → Peptide → Protein: which interactions are involved in each step? (b)．Oligonucleotide → Single strand DNA → Double strand DNA: which interactions?
5. Acids and Bases( Chapter 15, 16.1--16.4) 5. 1. The Bronsted-Lowry definitions(H, OH transfer) (a). Strong acid(base)and Weak acid(base) (b). Conjugated acid-base pair Note in each acid-base reactions, there are two conjugated acid-base pairs (c). Poly-protic acid(base), and amphoteric substance 5.2. Lewis acid-base definition (transfer of lone pair electrons to an empty orbital) 5.3. lon pro ater,Kw=[H3O]x [OH-]=10-4(@25C (a). Kw is a constant in all aqueous solution(under a constant temperature) (b).[H3O]>10M→ acidic;田H3O=107M→ neutral;田H3O+<10M→ basic (c). pH=-logIo [H30*]: pOH=-log1o [OH]; pH pOH= 14 (d). Definition of Ka, Kb Calculate the Ka, Kb of their conjugated acid/base 5.4. Calculation of H3 in acid solution(s Every calculation is indeed based on"Initial-Change-Equilibrium"for setting up a quadratic equation of equilibrium constant (a). strong acid only Let the strong acid dissociate completely first, and then see whether thewater dissociation matters, i.e. whether [H3O*]from the strong acid>10-5M? (b). weak acid only Consider the Kal only( for poly-protic acid) If Cacid/Ka>100>[H30]=v(Cacid X Ka) If Cacid/Ka< 100> need to solve the quadratic equation (c). one strong acid+ one weak acid Let the strong acid dissociate completely first, and then setup the" ICE equation of the weak acid's dissociation (d). one weak acid its conjugated base(it is a buffer Ina buffer [H30]=Ka(Cacid/Cbase) (e). one acid one bas Let the acid-base reaction go into completion first. (Need to find out the limiting reactants! Then the remaining species will belong to one of the 5.5. Calculation of oH-l in base solution(s) 5.6. Hydrolysis of salt (a). How to quickly judge whether a salt is acidic, neutral or basic (b). Calculate the pH value of a salt solutio 5.7. Buffer solutions Note for a good buffer, its acid/base ratio should be 0. 1-10 5.8.Tt (a). Titration curve: use a strong base to titrate a strong acid (b). Titration curve: use a strong base to titrate a weak acid
5．Acids and Bases (Chapter 15, 16.1—16.4) 5.1．The Bronsted-Lowry definitions(— H+ , OHtransfer) (a)．Strong acid (base) and Weak acid (base) (b)．Conjugated acid-base pair Note in each acid-base reactions, there are two conjugated acid-base pairs (c)．Poly-protic acid (base), and amphoteric substance 5.2．Lewis acid-base definition (— transfer of lone pair electrons to an empty orbital) 5.3．Ion product of water, Kw = [H3O+ ] × [OH- ] = 10-14 (@ 25 oC) (a)．Kw is a constant in all aqueous solution (under a constant temperature) (b)．[H3O+ ] > 10-7 M → acidic; [H3O+ ] = 10-7 M → neutral; [H3O+ ] < 10-7 M → basic (c)．pH = – log10 [H3O+ ]; pOH = – log10 [OH- ]; pH + pOH = 14 (d)．Definition of Ka, Kb. Calculate the Ka, Kb of their conjugated acid/base 5.4．Calculation of [H3O+ ] in acid solution(s) Every calculation is indeed based on “Initial–Change–Equilibrium” for setting up a quadratic equation of equilibrium constant. (a)．strong acid only Let the strong acid dissociate completely first, and then see whether thewater dissociation matters, i.e. whether [H3O+ ] from the strong acid > 10-5 M? (b)．weak acid only Consider the Ka1 only (for poly-protic acid) If Cacid/Ka > 100 → [H3O+ ] = √(Cacid × Ka) If Cacid/Ka ≤ 100 → need to solve the quadratic equation (c)．one strong acid + one weak acid Let the strong acid dissociate completely first, and then setup the “ICE” equation of the weak acid’s dissociation. (d)．one weak acid + its conjugated base (it is a buffer!) In a buffer: [H3O+ ] = Ka × (Cacid / Cbase) (e)．one acid + one base Let the acid-base reaction go into completion first. (Need to find out the limiting reactants!) Then the remaining species will belong to one of the previous categories. 5.5．Calculation of [OH- ] in base solution(s) 5.6．Hydrolysis of salt (a)．How to quickly judge whether a salt is acidic, neutral or basic (b)．Calculate the pH value of a salt solution 5.7．Buffer solutions Note for a good buffer, its acid/base ratio should be 0.1~10. 5.8．Titration (a)．Titration curve: use a strong base to titrate a strong acid (b)．Titration curve: use a strong base to titrate a weak acid
Outline for general Chemistry (lD) 6A. Solution( Chapter 4) 1 class 61. Solute solvent. and solution 6.2. Solubility(S)and molarity(C) a). Solubil ity: grams of solute /100 g solvent; Molarity: moles of solute /1 L solution (b). Be able to convert between solubility and molarity of a given solution 6.3. Electrolyt (a). Strong electrolyte: fully dissociate into cations and anions in solution or melt (b). Weak electrolyte: partially dissociate(with a dissociation factor between 0-1), and majority remains as molecules 64. Acid base and salt Note that"insoluble salt" is still a strong electrolyte 6.5. Reaction/calculation between ions in solution (a). Water solubility of different acids, bases and salts (b). Find out the limiting reactants for calculation 6.6. Ionic equation 6B. Precipitate(Chapter 16.5--16.8) I class 6.7. Solubility product (a). Ksp=[cation]m x [anion]n,(where m, n are coefficients of ions in the precipitate's dissociation reaction) (b). Convert between solubility product(Ksp)and solubility(s) 6.8. Pred ict the solubility formation Compare the magnitude of ion product, [cation]m x [anion]n, with the Ksp (a). cation]m x [anion<Ksp> under saturated solution, No precipitate (b). [cation]m x [anion]n=Ksp> saturated solution, Start to precipitate (c). [cation]m x [anion]n>Ksp)Over saturated solution, Precipitate is formed 6.9. The common ion effect 6.10. Calculation of ion concentrations in solution When more than one precipitate can be formed, which one will precipitat When the 2nd precipitate starts to form, what is the remaining ion concentration for the 1st ion? 7. Oxidation-Reduction Reaction( Chapter Il) 2 class 7.1. Oxidation numbers(Oxidation state) 7.2. Rules for assigning the oxidation number Apply the 5 steps in order
Outline for General Chemistry (II) 6A．Solution (Chapter 4) 1 class 6.1．Solute, solvent, and solution 6.2．Solubility (S) and molarity (C) (a)．Solubility: # grams of solute / 100 g solvent; Molarity: # moles of solute / 1 L solution (b)．Be able to convert between solubility and molarity of a given solution 6.3．Electrolyte (a)．Strong electrolyte: fully dissociate into cations and anions in solution or melt (b)．Weak electrolyte: partially dissociate (with a dissociation factor between 0~1), and majority remains as molecules 6.4．Acid, base, and salt Note that “insoluble salt” is still a strong electrolyte 6.5．Reaction/calculation between ions in solution (a)．Water solubility of different acids, bases and salts (b)．Find out the limiting reactants for calculation 6.6．Ionic equation 6B．Precipitate (Chapter 16.5—16.8) 1 class 6.7．Solubility product: (a)．Ksp = [cation]m × [anion]n , (where m, n are coefficients of ions in the precipitate’s dissociation reaction) (b)．Convert between solubility product (Ksp) and solubility (S) 6.8．Predict the solubility formation – Compare the magnitude of ion product, [cation]m × [anion]n , with the Ksp (a)．[cation]m × [anion]n < Ksp → under saturated solution, No precipitate (b)．[cation]m × [anion]n = Ksp → saturated solution, Start to precipitate (c)．[cation]m × [anion]n > Ksp → Over saturated solution, Precipitate is formed 6.9．The common ion effect 6.10．Calculation of ion concentrations in solution When more than one precipitate can be formed, which one will precipitate first? When the 2nd precipitate starts to form, what is the remaining ion concentration for the 1st ion? 7．Oxidation-Reduction Reaction (Chapter 11) 2 class 7.1．Oxidation numbers (Oxidation state) 7.2．Rules for assigning the oxidation number Apply the 5 steps in order