Week 9 Ligands Workbook PDF - Monash S2 2024

10/25/24, 5:07 PM Week 9: Ligands - workbook | MonashELMS1 Week 9: Ligands - workbook Site: Monash Moodle1 Printed by: Kaltham Alzaabi...

10/25/24, 5:07 PM Week 9: Ligands - workbook | MonashELMS1 Week 9: Ligands - workbook Site: Monash Moodle1 Printed by: Kaltham Alzaabi Unit: CHM1022 - Chemistry II - S2 2024 Date: Friday, 25 October 2024, 5:07 PM Book: Week 9: Ligands - workbook https://learning.monash.edu/mod/book/tool/print/index.php?id=2780841 1/27 10/25/24, 5:07 PM Week 9: Ligands - workbook | MonashELMS1 Table of contents 1. Pre-workshop material 1.1. Introduction to Ligands 1.2. Ligands and coordination complexes 1.3. Ligand Exchange and Stability Constants 1.4. Activity 1 1.5. Naming Coordination Compounds 1.6. Activity 2 1.7. Putting it all together 1.8. Activity: Solutions 2. Summary 3. Preparation quiz 4. Online lectures 5. Workshops https://learning.monash.edu/mod/book/tool/print/index.php?id=2780841 2/27 10/25/24, 5:07 PM Week 9: Ligands - workbook | MonashELMS1 1. Pre-workshop material Please read Section 13.3 Chemistry, Blackman et al. (4th ed.) What are Ligands? We introduced you to ligands last week. They are molecules or ions which act as a Lewis base (an electron pair donor). Ligands have one or more donor atoms – these are atoms that have a lone pair of electrons that are able to be donated towards a metal ion. Ligands can be neutral molecules, such as water (H2O) or ammonia (NH3), or can be anionic, such as chloride (Cl-) or cyanide (CN-). Ligands can be classified by the number of donor atoms that attach to a metal centre. This classification is known as the concept of ‘denticity’. Ligands with one donor atom are called monodentate; ligands with two donor atoms are call bidentate; three = tridentate, etc. https://learning.monash.edu/mod/book/tool/print/index.php?id=2780841 3/27 10/25/24, 5:07 PM Week 9: Ligands - workbook | MonashELMS1 1.1. Introduction to Ligands Some examples of common monodentate ligands (which you should know) are shown in Figure 1. There are several shown that have more than one potential donor atom (shown in red), but coordinate through only one of these at any given time and are therefore monodentate. For example, the oxygen and nitrogen atoms on nitrite cannot both attach to a metal cation. Figure 1: Common monodentate ligands Bidentate ligands must have two donor atoms that are able to coordinate to a metal ion simultaneously. In the examples in Figure 2 both ligands form five-membered ‘chelate rings’ when they coordinate (i.e. a cycle of five atoms including the metal, two donor atoms and the ‘backbone’ of the ligand). In the third example, acetylacetonate (acac), forms a 6-membered chelate ring. Chelating ligands form more thermodynamically stable complexes than monodentate ligands. You should know the examples of bidentate ligands that are shown in Figure 2. Figure 2: Common bidentate ligands Bidentate ligands can be symmetrical or asymmetrical (i.e. have different types of donor atoms). Just because a ligand can act as a chelating ligand, does not mean that it always will (as shown in the iridium complex in Figure 3). https://learning.monash.edu/mod/book/tool/print/index.php?id=2780841 4/27 10/25/24, 5:07 PM Week 9: Ligands - workbook | MonashELMS1 Figure 3: Iridium complex with ethylenediamine and chloride ligands Tridentate ligands have three donor atoms. An example is diethylenetriamine (which can be thought of as an extended version of ethylenediamine) is shown in Figure 4. Figure 4: Tridentate ligand, diethylenetriamine Ligands with many donor atoms are sometimes called ‘polydentate’. This is a generic term and does not specify how many atoms are coordinating to a metal. For example, a common ligand used for extraction of metals is ethylenediaminetetraacetate (EDTA) – this can be thought of as ethylenediamine (Figure 2) with four acetates attached to it. EDTA4- can act as a hexadentate ligand and therefore only one is needed to fill the coordination sphere of an octahedral metal (Figure 5). EDTA complexes are very stable. Figure 5: Polydentate ligand, EDTA, bonding with cobalt A special class of polydentate ligands are ‘macrocyclic ligands’. As the name implies, these ligands are large ring-shaped molecules that have multiple donor atoms. 18-crown-6 and porphyrin are two examples of macrocyclic ligands (Figure 6). Derivatives of porphyrins bind iron in haemoglobin (protein responsible for O2 transport in mammals) and bind magnesium in chlorophyll (part of the light-harvesting cascade in photosynthesis). https://learning.monash.edu/mod/book/tool/print/index.php?id=2780841 5/27 10/25/24, 5:07 PM Week 9: Ligands - workbook | MonashELMS1 Figure 6: Macrocyclic ligands Some ligands are capable of coordinating simultaneously to multiple metals. These ligands act as a bridge between the metals and are therefore called ‘bridging ligands’. Bridging ligands can have one donor atom with multiple lone pairs (e.g. hydroxide) or multiple donor atoms that are positioned so that they can coordinate to multiple metals (e.g. cyanide). See Figure 7 for examples. Figure 7: Examples of bridging ligands https://learning.monash.edu/mod/book/tool/print/index.php?id=2780841 6/27 10/25/24, 5:07 PM Week 9: Ligands - workbook | MonashELMS1 1.2. Ligands and coordination complexes Common Ligands We will now look at some examples of complexes containing common ligands. We will be using correct chemical nomenclature here, this is explained later in this week’s workbook. Aqua (H2O) Complexes All first-row transition metals dissolve in water to form complexes with water or hydroxide (ligands). For example, NiCl2 + 6H2O → [Ni(OH2)6]2+ + 2Cl- (Figure 8). Similar complexes are known for the whole first row. Figure 8: Examples of aqua ligands forming a complex with nickel Hydroxido Complexes All metal ions are Lewis acids (electron pair acceptors) but their strength varies. Some are very strong Lewis acids (e.g. Fe3+, Ti3+) and pull electron pairs towards them very strongly. This property is roughly related to the charge density of the ion (charge density = charge / surface area) or effective nuclear charge (see Week 7). In instances where the metal ion is a strong Lewis acid, the following equilibrium exists and the solution becomes a Brønsted acid (the complex donates H+). The strength of the Lewis acidic metal draws the electrons from the aqua ligand very strongly, weakening one of the O-H bonds in the water ligand to the point of dissociation (Figure 9). These solutions can be quite strongly acidic, with pKa values comparable to acetic acid or stronger. Figure 9: Schematic of the relationship between strong Lewis acids and formation of Brønsted acids https://learning.monash.edu/mod/book/tool/print/index.php?id=2780841 7/27 10/25/24, 5:07 PM Week 9: Ligands - workbook | MonashELMS1 Once formed, complexes containing hydroxide typically combine to form complexes with increased ‘nuclearity’ – this means that they contain more than one metal ion. An example is shown below in Figure 10 for vanadium (similar chemistry occurs for chromium, iron and cobalt). Figure 10: Formation of multiple metal complexes. The OH- ligand becomes a bridging ligand. The "μ" in the chemical formula represents the bridging OH- ligands. Chlorido Complexes Reaction of transition metal aqua complexes with an excess of chloride (Cl-), i.e. in the presence of a high concentration of chloride, generally give tetrahedral chloride complexes (Figure 11). The same is generally true for bromide and iodide. This change from octahedral to tetrahedral is accompanied by a distinct colour change, for example the video below (we will understand more about colour changes in Week 11). The size of the halide ligands and charge repulsion gives preference to the tetrahedral geometry. Equilibrium in copper(II) chloride solution https://www.youtube.com/watch?v=fjfm0MTDtx8 Figure 11: Reaction of cobalt with dilute and concentrated HCl forms two different complexes. Cyanido Complexes The cyanide anion (N≡C-) usually binds through the carbon atom (this is the atom that carries the negative charge). This is the case in mononuclear complexes such as [Fe(CN)6]3- or [Fe(CN)6]4-. It is possible for the cyanide anion to coordinate through both the C and N atoms and act as a bridging ligand. https://learning.monash.edu/mod/book/tool/print/index.php?id=2780841 8/27 10/25/24, 5:07 PM Week 9: Ligands - workbook | MonashELMS1 For example, when [Fe(CN)6] is mixed with a solution containing aqueous Fe3+ a deep blue solid is immediately formed. This solid is 4- an infinite network of metal ions and CN- ligands and is called a coordination polymer. In this case, the material is Prussian Blue (Figure 12, structure on right hand side), one of the first known blue dyes from the 18th century (it can also be used as a qualitative test for cyanide). Figure 12: Formation of Prussian blue from the reaction of Fe3+ and cyanide ligands. Ammine Complexes Addition of aqueous ammonia to most [M(OH2)6]n+ complexes causes displacement of the aqua ligands. These displacement reactions are equilibrium reactions, and are written using equilibrium arrows to represent the exchange of ligands between species (Figure 13). We will explore this equilibrium process next. Figure 13: Equilibrium reactions between aqua complexes and NH3 to form aqua + ammine complex https://learning.monash.edu/mod/book/tool/print/index.php?id=2780841 9/27 10/25/24, 5:07 PM Week 9: Ligands - workbook | MonashELMS1 1.3. Ligand Exchange and Stability Constants Please read stability constants and the chelate effect of Chemistry, Blackman et al. (4th ed.) Ligand exchange is a dynamic process that occurs in an equilibrium. We can measure an equilibrium constant for these processes and compare them for different complexes. We will consider the example shown below in which ammonia replaces four of the aqua ligands from [Cu(OH2)6]2+. Any counter-anions are merely spectators and do not need to be considered. Figure 14: Overall equilibrium reaction between copper aqua complex and NH3 We can consider the exchange process happening in a step-wise manner, i.e. one aqua ligand is replaced at a time (Figure 15). We can then set up four separate equilibria and four separate equilibrium constants (one for each of the four exchange processes). These four expressions are shown below. The equilibrium constants are called ‘Kx’ where x is the step number (i.e. the first exchange process has the equilibrium constant k1). The equilibrium constant is calculated in the same way as any other exchange constant (for example, acid dissociation constant). The concentrations of the product(s) are divided by the concentrations of the reactant(s). Note that in the equation shown below the square brackets refer to concentration rather than defining a coordination complex (yes, this is confusing nomenclature!). In this example we do not put H2O as a product of the reaction; this is because the reaction is in water and there is effectively no change in the concentration of water as a result of those ligands being exchanged. Figure 15: Step-wise equilibrium reactions of aqua with another ligand "L" The overall equilibrium constant, also called the formation constant or stability constant, is called Kf (or βy where y is the number of individual stepwise constants). It is the product of the individual equilibrium constants. If you write out all of the individual expressions you should be able to derive the final expression as shown below (for the current example). Note that for the reactants (the denominator) the concentrations are multiplied, including the factor of 4 applied to the ammonia concentration (reflecting the stoichiometry of the reaction). The same would happen to the products if there were multiple species to be considered (as we will see in class). https://learning.monash.edu/mod/book/tool/print/index.php?id=2780841 10/27 10/25/24, 5:07 PM Week 9: Ligands - workbook | MonashELMS1 Figure 16: Overall equilibrium expression and constant The equilibrium constant can be used in the Gibbs free energy equation, whereby a large negative value of ΔG° indicates a complete forward reaction (Figure 17). Some Kf values for simple ligand exchanges are shown below, higher values indicate a more stable compound an indicate which ligands will displace others. Note: For CHM1022 exam, there will be no questions asking you to calculate ΔG or K. Figure 17: The mathematical relationship between Gibbs free energy and equilibrium constant K Additional information on chelating ligands and the chelate effect When a multidentate ligand coordinates to a metal ion using more than one donor atom (forming a ring with the metal), the ligand is said to be a chelating ligand and the resulting compound is said to be a chelate complex. Figure 18: Examples of multidentate ligands and their respective binding modes that are usually adopted during complex formation. The chelate complexes are more stable than non-chelate complexes. This effect is known as chelate effect, which can be explained by considering the formation of some non-chelated and chelated complex ions of the same metal. https://learning.monash.edu/mod/book/tool/print/index.php?id=2780841 11/27 10/25/24, 5:07 PM Week 9: Ligands - workbook | MonashELMS1 The value for ∆H (enthalpy) is negative and very similar for the three reactions because in each case four Pt-N bonds have been formed. If we consider number of reactants and products for each of the three reaction, it is clear that ΔS (entropy of change => the measure of disorder) for reaction (I) is zero (or close to it) as the number of the reactants (five: [Pt(OH2)4]2+ and 4xNH3) is the same as the number of products (five: [Pt(NH3)4]2+ and 4xH2O), while it is positive and increasing as we go to reaction (II) and then reaction (III). Thus, the order of entropy change in going from reactant to product side is ΔS reaction(I)< ΔS reaction(II)< ΔS reaction(III) Therefore, if we consider that ΔG = ΔH - TΔS then reaction (III) is more favourable (ΔG is more negative) than reaction (II) which is, in turn, more favourable than reaction (I) predominantly due to the relative values for ΔS of these reactions. This means that [Pt(trien)]2+ is more stable than [Pt(en)2]2+ , which is then more stable than [Pt(NH3)4]2+. https://learning.monash.edu/mod/book/tool/print/index.php?id=2780841 12/27 10/25/24, 5:07 PM Week 9: Ligands - workbook | MonashELMS1 1.4. Activity 1 Question 1 Here is a simple coordination complex. Which of the following statements is true? A: Ligands = ammonia; donor atoms = oxygen B: Ligands = water; donor atoms = oxygen C: Ligands = water; donor atoms = hydrogen D: Ligands = water; donor atoms = oxygen and hydrogen Question 2 Here is a coordination complex. Which of the following statements is true? A: There are six monodentate ligands B: There are three bidentate ligands C: There are two tridentate ligands D: There are three tridentate ligands Question 3 Which of the two complexes, [Mn(OH2)6]2+ or [Mn(OH2)6]3+, would you expect to form the solution with the lowest pH value (i.e. most acidic) and why? https://learning.monash.edu/mod/book/tool/print/index.php?id=2780841 13/27 10/25/24, 5:07 PM Week 9: Ligands - workbook | MonashELMS1 2+ A: [Mn(OH2)6] because the metal ion has a higher charge density B: [Mn(OH2)6]2+ because the metal ion has a lower charge density C: [Mn(OH2)6]3+ because the metal ion has a higher charge density D: [Mn(OH2)6]3+ because the metal ion has a lower charge density https://learning.monash.edu/mod/book/tool/print/index.php?id=2780841 14/27 10/25/24, 5:07 PM Week 9: Ligands - workbook | MonashELMS1 1.5. Naming Coordination Compounds Please read nomenclature of transition metal complexes of Chemistry, Blackman et al. (4th ed.)(page 770-774) Nomenclature Nomenclature, how to name compounds, is not an exciting topic but it is very important. An essential ability in any field of science that deals with chemicals is to be able to unambiguously tell another person the nature of a chemical. The International Union of Pure and Applied Chemistry (IUPAC) dictates a set of guidelines for the naming of compounds. There is a separate book for inorganic compounds (known as the Red Book). If you are interested, you can find the book by following this link https://iupac.org/cms/wp-content/uploads/2016/07/Red_Book_2005.pdf or you can find a simplified explanation by looking up the following journal paper from the library website, Pure and Applied Chemistry, 2015, 87, 1039-1049. We will explore how to name simple coordination complexes as part of this course. A brief segment of the IUPAC guide is shown below in Figure 18; this is a good flowchart to follow when naming compounds. Figure 18: A sample of the IUPAC instructions on naming coordination compounds Ways of Writing/Naming Compounds Coordination compounds can be expressed in three ways; (a) a chemical diagram, (b) a shorthand formula, or (c) a fully expressed systematic name. An example of a compound identified by these three methods is show below in Figure 19. Note that in all instance the cation comes before the anion. https://learning.monash.edu/mod/book/tool/print/index.php?id=2780841 15/27 10/25/24, 5:07 PM Week 9: Ligands - workbook | MonashELMS1 Figure 19: Three different ways to represent a coordination compound When we write out the formula or the full name we always place the ligands in alphabetical order as they are written. This means that the formula and name may have the ligands in a different order to each other (for example, when water is a ligand it is called ‘aqua’, starting with ‘a’, but in a formula it is written ‘OH2’, starting with ‘O’). The metal is given first in the formula, and last in the full name. When molecules or ions act as ligands, especially simple species, their name often changes to clearly denote that it is coordinated to a metal. The names of common ligands are shown in Figure 20. Note that for common anions an –ide suffix becomes –ido when acting as a ligand, and an –ate ending becomes –ato. Figure 20: IUPAC names of ligands A simple example of a complex is shown below in Figure 21. The name is hexaaquacobalt(II), written as [Co(OH2)6]2+. Figure 21: IUPAC name of this complex is hexaaquacobalt(II) We can learn a few rules from this example. 1. The number of ligands of a certain type is expressed by a numerical prefix (di, tri, tetra, penta, hexa, etc.). This is not needed when there is a single ligand of that type and the prefix is ignored when determining alphabetical order. 2. For the full name, the oxidation state of the metal is written as Roman numerals in brackets. The charge is given for the formula, so the oxidation state is implied (you can calculate it). 3. The formula always contains the complex in square brackets (as for the chemical drawing). 4. In the formula, the donor atom of the ligand is written first, OH2 rather than H2O https://learning.monash.edu/mod/book/tool/print/index.php?id=2780841 16/27 10/25/24, 5:07 PM Week 9: Ligands - workbook | MonashELMS1 Ligands with Multiple Potential Donor Atoms If a ligand can potentially coordinate through different donors atoms then we must be unambiguous about which is coordinating. An example is the thiocyanate anion, SCN-, which can coordinate through either the sulfur or the nitrogen atom. When writing a formula we simply write the donor atom first. [Cu(SCN)4]2- would contain ligands in which the S atom is the donor atom and [Cu(NCS)4]2- would contain ligands in which the N atom is the donor atom. When writing out full names, we denote the donor atom using kappa notation, employing the Greek symbol κ. The two compounds mention above would be called tetrathiocyanato-κS-cuprate(II) and tetrathiocyanato-κN-cuprate(II). Why have we written ‘cuprate’? See below… Naming Anionic Complexes If the metal complex has an overall negative charge then we add the suffix –ate to the name. For example, [ZnCl4]2- is called tetrachloridozincate. There are some elements that use the Latin root of their name when the complex is anionic, as for cuprate in the previous example. Other non-standard names are shown in Figure 22. Figure 22: IUPAC names of metals when the complex is a negative charge https://learning.monash.edu/mod/book/tool/print/index.php?id=2780841 17/27 10/25/24, 5:07 PM Week 9: Ligands - workbook | MonashELMS1 1.6. Activity 2 Question 1 For the ligand exchange equilibrium shown below (in aqueous solution), determine which is the correct formula for the formation constant. Question 2 What is the full chemical name for the compound shown below? A: dibromidetetraaquacobalt(III) bromide B: bromide tetaraquadibromidocobalt(III) C: dibromidotetraaquacobalt(II) bromine D: tetraaquadibromidocobalt(III) bromide https://learning.monash.edu/mod/book/tool/print/index.php?id=2780841 18/27 10/25/24, 5:07 PM Week 9: Ligands - workbook | MonashELMS1 1.7. Putting it all together Example We will look at one example that pieces together many of these naming rules and conventions. As with all ionic compounds, the cation is named first and the anion last. The metal comes first in the formula, last in full name. Ligands are listed alphabetically in both the formula and name (note how the order is different though). In the name, prefixes denote the number of a particular ligand and are ignored for determining naming order. Anionic ligands end in “ido”, neutral ligands are mostly not changed. If the complex is an anion, its ending is changed to –ate (not in this instance). The oxidation number of the metal is given as a Roman numeral in parentheses immediately after the name of the metal. The number of each ion is not specified in the name – it is implied by the oxidation state and our knowledge of charges on the ligands and counterions. Another example is the compound [Ni(en)3][FeCl4]2 which contains metal complexes as both the cation and the anion. This compound is named tris(ethylenediamine)nickel(II) tetrachloridoferrate(III). Some rules that can be observed here are: The cationic complex comes first. Because the name of the ligand ‘ethylenediamine’ already contains ‘di’ as part of the name, we use ‘tris’ (instead of ‘tri’) to avoid confusion and make sure that the ligand is named in brackets. We do not specify the ratio of cation:anion in the name, this is implied by the oxidation states and ligands. The anionic complex uses the form ‘ferrate’ to denote the charge. https://learning.monash.edu/mod/book/tool/print/index.php?id=2780841 19/27 10/25/24, 5:07 PM Week 9: Ligands - workbook | MonashELMS1 1.8. Activity: Solutions Activity 2 Question 1 For the ligand exchange equilibrium shown below (in aqueous solution), determine which is the correct formula for the formation constant. CORRECT ANSWER: (A) Question 2 What is the full chemical name for the compound shown below? https://learning.monash.edu/mod/book/tool/print/index.php?id=2780841 20/27 10/25/24, 5:07 PM Week 9: Ligands - workbook | MonashELMS1 A: dibromidetetraaquacobalt(III) bromide B: bromide tetaraquadibromidocobalt(III) C: dibromidotetraaquacobalt(II) bromine D: tetraaquadibromidocobalt(III) bromide CORRECT ANSWER: (D) https://learning.monash.edu/mod/book/tool/print/index.php?id=2780841 21/27 10/25/24, 5:07 PM Week 9: Ligands - workbook | MonashELMS1 2. Summary This week you will learn to recognize different ligands within coordination compounds, and to identify the manner in which they coordinate. The ability to accurately name compounds (or to identify compounds from their names) is very important, and the basic nomenclature associated with coordination compounds will be discussed. https://learning.monash.edu/mod/book/tool/print/index.php?id=2780841 22/27 10/25/24, 5:07 PM Week 9: Ligands - workbook | MonashELMS1 3. Preparation quiz Now that you have completed the pre-workshop material, attempt the following preparation quiz. These 10 questions give you a chance to test your knowledge and practice the skills that were covered in this week's pre-workshop material. This material is essential for this week's workshops and may be applied in your laboratory classes. You have two attempts at each quiz and your highest attempt will count towards your final grade. Preparation quiz for Week 9 https://learning.monash.edu/mod/book/tool/print/index.php?id=2780841 23/27 10/25/24, 5:07 PM Week 9: Ligands - workbook | MonashELMS1 4. Online lectures CHM1022-Week9-10-Intro These captions have been automatically generated. As such, the CHM1022-Week9-10-Intro quality is not 100% accurate. Accuracy may be affected by audio quality, topic under discussion and clarity of the speakers. Staff are not expected or required to edit or correct automatically- generated captions. It is best to not rely solely on captions when viewing video play_arrow content and to use them alongside other learning resources. Students who are registered with Disability Support Services should be in contact with them to discuss captioning if needed. Powered by Panopto get_app closed_caption fullscreen keyboard_arrow_up CHM1022-Week9-L1-A1 CHM1022-Week9-L1-A2 These captions have been automatically generated. As such, the CHM1022-Week9-L1-A2 quality is not 100% accurate. Accuracy may be affected by audio quality, topic under discussion and clarity of the speakers. Staff are not expected or required to edit or correct automatically- generated captions. It is best to not rely solely on captions when viewing video play_arrow content and to use them alongside other learning resources. Students who are registered with Disability Support Services should be in contact with them to discuss captioning if needed. Powered by Panopto get_app closed_caption fullscreen keyboard_arrow_up CHM1022-Week9-L1-A3 These captions have been automatically generated. As such, the CHM1022-Week9-L1-A3 quality is not 100% accurate. Accuracy may be affected by audio quality, topic under discussion and clarity of the speakers. Staff are not expected or required to edit or correct automatically- generated captions. It is best to not rely solely on captions when viewing video play_arrow content and to use them alongside other learning resources. Students who are registered with Disability Support Services should be in contact with them to discuss captioning if needed. Powered by Panopto get_app closed_caption fullscreen keyboard_arrow_up https://learning.monash.edu/mod/book/tool/print/index.php?id=2780841 24/27 10/25/24, 5:07 PM Week 9: Ligands - workbook | MonashELMS1 CHM1022-Week9-L1-A4 CHM1022-Week9-L2-A1pt1 These captions have been automatically generated. As such, the CHM1022-Week9-L2-A1pt1 quality is not 100% accurate. Accuracy may be affected by audio quality, topic under discussion and clarity of the speakers. Staff are not expected or required to edit or correct automatically- generated captions. It is best to not rely solely on captions when viewing video play_arrow content and to use them alongside other learning resources. Students who are registered with Disability Support Services should be in contact with them to discuss captioning if needed. Powered by Panopto get_app closed_caption fullscreen keyboard_arrow_up CHM1022-Week9-L2-A1pt2 These captions have been automatically generated. As such, the CHM1022-Week9-L2-A1pt2 quality is not 100% accurate. Accuracy may be affected by audio quality, topic under discussion and clarity of the speakers. Staff are not expected or required to edit or correct automatically- generated captions. It is best to not rely solely on captions when viewing video play_arrow content and to use them alongside other learning resources. Students who are registered with Disability Support Services should be in contact with them to discuss captioning if needed. Powered by Panopto get_app closed_caption fullscreen keyboard_arrow_up CHM1022-Week9-L2-A2pt1 These captions have been automatically generated. As such, the CHM1022-Week9-L2-A2pt1 quality is not 100% accurate. Accuracy may be affected by audio quality, topic under discussion and clarity of the speakers. Staff are not expected or required to edit or correct automatically- generated captions. It is best to not rely solely on captions when viewing video play_arrow content and to use them alongside other learning resources. Students who are registered with Disability Support Services should be in contact with them to discuss captioning if needed. Powered by Panopto get_app closed_caption fullscreen keyboard_arrow_up https://learning.monash.edu/mod/book/tool/print/index.php?id=2780841 25/27 10/25/24, 5:07 PM Week 9: Ligands - workbook | MonashELMS1 CHM1022-Week9-L2-A2pt2 Additional examples for Lecture 2 Activities 1 and 2 (optional) CHM1022-Week9-L2-A1pt3optional These captions have been automatically generated. As such, the CHM1022-Week9-L2-A1pt3optional quality is not 100% accurate. Accuracy may be affected by audio quality, topic under discussion and clarity of the speakers. Staff are not expected or required to edit or correct automatically- generated captions. It is best to not rely solely on captions when viewing video play_arrow content and to use them alongside other learning resources. Students who are registered with Disability Support Services should be in contact with them to discuss captioning if needed. Powered by Panopto get_app closed_caption fullscreen keyboard_arrow_up CHM1022-Week9-L2-A2pt3optional These captions have been automatically generated. As such, the CHM1022-Week9-L2-A2pt3optional quality is not 100% accurate. Accuracy may be affected by audio quality, topic under discussion and clarity of the speakers. Staff are not expected or required to edit or correct automatically- generated captions. It is best to not rely solely on captions when viewing video play_arrow content and to use them alongside other learning resources. Students who are registered with Disability Support Services should be in contact with them to discuss captioning if needed. Powered by Panopto get_app closed_caption fullscreen keyboard_arrow_up Online lecture slides can be downloaded from this link: Week 9 lecture slides https://learning.monash.edu/mod/book/tool/print/index.php?id=2780841 26/27 10/25/24, 5:07 PM Week 9: Ligands - workbook | MonashELMS1 5. Workshops CHM1022_Workshop Week 9 worksheet Week 9 Week 9 worksheet answers https://learning.monash.edu/mod/book/tool/print/index.php?id=2780841 27/27