UNIT - 1 - PERIODIC PROPERTIES

[Audio] Welcome to our presentation on the topic of periodic properties and coordination compounds. Our company, [Company Name], is honored to have the opportunity to share our knowledge on this subject, including basic principles, crystal field splitting, and factors that impact CFT. Our team has conducted research on coordinating compounds and their potential uses, which we will also be discussing. We are eager to delve into this intriguing topic and share our insights with you. Let's begin our first unit on this significant topic. So, without further ado, let's explore the realm of periodic properties and coordination compounds. Thank you for joining us..

[Audio] This is slide number 2 out of 23 of our UNIT-1-PERIODIC PROPERTIES presentation for BATCH-2. We will now introduce our team members who have contributed their unique skills and knowledge to make this project a success. Let's meet them: Srivatsan with RA2511003020502, Amrutha Varshni T- RA2511003020503, Shyam - RA2511003020504, P. Meghavarshnee - RA2511003020505, Sandeep M - RA2511003020506, Kiruthik Pranav JS - RA2511003020507, Pranav Kumaar Kartik - RA2511003020508, Jashwanth - RA2511003020509, Rithikroshan - RA2511003020510, Deepa - RA2511003020511, and Sanjana - RA2511003020512. Each team member has put in their best efforts to make this presentation informative and engaging. We hope you will find it valuable. Thank you for your attention..

[Audio] The third slide will cover the topic of coordination compounds, which are important in chemistry and have a significant role in industrial processes. This unit will cover the principles of coordination compounds, followed by an exploration of crystal field splitting and its impact. We will also discuss the various factors that influence crystal field splitting, including ligand size, charge, and spin. Understanding these factors will enhance our understanding of coordination compounds. Additionally, we will learn about the HSAB theory, which helps determine the reactivity of coordination compounds and is widely used in the field. Finally, we will look at the applications and limitations of coordination compounds, giving us a better understanding of their use in industries and the challenges they present. This concludes slide three and the table of contents for this unit on periodic properties. Please continue with the remaining slides to uncover more about the intriguing world of coordination compounds..

[Audio] Today, we will be discussing the topic of Introduction to Coordination Compounds. Coordination compounds are complex molecules that contain a central metal ion bonded to ligands. These ligands can be either neutral or negatively charged and they form coordinate covalent bonds with the central metal ion. An example of a coordination compound is [Cu(NH₃)₄]SO₄, where copper is the central metal ion and ammonia is the ligand. The concept of coordination compounds was first established by Alfred Werner's Coordination Theory. This theory introduced the concept of coordination numbers and geometries, which determine the arrangement of ligands around the central metal ion. This image illustrates a coordination complex with octahedral geometry, where the central metal ion is surrounded by 6 ligands. Coordination compounds are widely used in various fields, including medicine, agriculture, and industry. They have unique properties and play a significant role in many chemical reactions. This concludes our discussion on the introduction to coordination compounds. We will dive deeper into its properties and applications in the following slides..

[Audio] In this unit, we will discuss the basic principles of Crystal Field Theory (CFT), which involves a central metal ion surrounded by ligands. The metal-ligand bond in a complex is purely ionic and ligands can be categorized as true, negative, or neutral. This bond is purely repulsive and causes the five d-orbitals to split into two sets - t₂g and eₙ. This is known as splitting energy. One important concept of CFT is that it does not allow for electron sharing between the metal ion and ligands, meaning there is no overlapping of orbitals as seen in covalent bonds. The number and arrangement of ligands around the central ion determine the crystal field. These different crystal fields will have varying effects on the energies of the five d-orbitals, which is crucial in understanding the properties of complex compounds. Now, let's move on to the next slide to explore these effects further..

[Audio] We are now on the sixth slide of our presentation, Unit 1 - Periodic Properties for Batch 2. This slide will cover d-orbital shapes and energy. D-orbitals are a type of atomic orbital that can hold up to 10 electrons and are denoted by the letter 'd'. There are five degenerate d-orbitals: dxy, dyz, dxz, dx²−y², and dz². This means that all five orbitals have equal energy and electrons can occupy them without preference. However, when a metal atom is surrounded by ligands, the energy of the d-orbitals can be affected, known as splitting in a ligand field. Ligands can cause the degenerate d-orbitals to split, resulting in some orbitals having higher energy levels and others having lower energy levels. This allows for a more orderly arrangement of electrons, which can greatly impact the chemical and physical properties of the metal atom. In conclusion, d-orbitals have unique shapes and energies and the presence of ligands can affect their energy levels, which is crucial in understanding the behavior of metal atoms in chemical reactions. More informative slides will follow, thank you for your attention..

[Audio] Slide 7 out of 23 in this presentation discusses crystal field splitting, an important concept in understanding the interactions of transition metal complexes. It is essential to have knowledge of the spatial arrangement of d orbitals to fully comprehend this concept. When a negative ligand charge is applied, the fivefold degeneracy of d-orbitals in a free gaseous metal ion remains, but their energy changes due to a spherically symmetric crystal field. This creates an imbalance, known as crystal field splitting. In this presentation, we will delve deeper into this concept and its significance in transition metal complexes. Let's now move on to slide 8..

[Audio] We are currently discussing octahedral crystal field splitting in an octahedral coordination compound, where six ligands surround the metal atom/ion. This results in repulsion between the electrons in d orbitals and the ligand electrons, with the most significant repulsion occurring in the dx2-y2 and dz2 orbitals. As a result, these two orbitals have a higher energy level compared to the average energy in a spherical crystal field. On the other hand, the dxy, dyz, and dxz orbitals experience lower repulsion as they are directed between the axes, resulting in a lower energy level. This repulsion causes the d orbitals to split into two energy levels: the t2g set (dxy, dyz, and dxz) with lower energy and the eg set (dx2-y2 and dz2) with higher energy. Understanding this crystal field splitting is crucial in predicting the behavior and properties of coordination compounds. Please stay tuned for the next slide..

[Audio] Periodic properties are essential in understanding the behavior of elements in the field of chemistry. Our presentation will be focusing on these properties in Unit 1. Moving on to slide number 9, we will be discussing crystal field splitting, which refers to the separation of degenerate energy levels caused by ligands. This means that a ligand can affect the energy levels of a central metal ion, resulting in the split of energy levels into t2g and eg levels. The difference between these two sets is represented by the symbol "Δo" and is known as the crystal field splitting. It is worth noting that different ligands can have varying effects, with some creating stronger fields and larger crystal field splitting and others producing weaker fields and smaller splitting. This difference is crucial in understanding the behavior of elements in different ligand environments. This concludes slide 9, and we will continue to discuss periodic properties in our Unit 1 presentation. Thank you for your attention..

[Audio] Today's presentation covers tetrahedral crystal field splitting, an important concept in chemistry. In this type of crystal field, a metal ion's five degenerate d orbitals are split into two energy levels, T(d). The dx2-y2 and dz2 orbitals are affected less by ligands, resulting in a lower energy for those orbitals compared to the dxy, dyz, and dxz orbitals. The smaller number of ligands in Td complexes leads to a weaker ligand field and a smaller total negative charge, causing this split. Additionally, the orientation of the d orbitals and the approaching ligands is not symmetrical, leading to the splitting. This concept is crucial in understanding the properties and behaviors of coordination compounds, such as their color, magnetic properties, and reactivity. Next, we will discuss the effect of ligand strength on crystal field splitting in slide number 11..

[Audio] Transition metals in coordination compounds have unique properties due to their ability to form multiple bonds with ligands. This is because these metals have unfilled d orbitals in their outermost energy level. In a tetrahedral coordination compound, the repulsions result in two distinct energy levels: the t2 set, consisting of three orbitals (dxy, dyz, and dxz) with higher energy, and the e set, consisting of two orbitals (dx2-y2 and dz2) with lower energy. The crystal field splitting in a tetrahedral complex is smaller compared to an octahedral field, as there are only two-thirds as many ligands and they have a less direct effect on the d orbitals. The e set has a relative stabilizing effect of -6Dq, while the t2 set has a destabilizing effect of +4Dq. This unique energy level configuration allows transition metals to form a variety of coordination compounds, each with different properties and applications..

[Audio] We have now reached slide number 12 out of 23 in our presentation on "Unit - 1 - Periodic Properties, Batch - 2". This slide presents a table on Crystal Field Stabilization Energy, an important concept in the field of chemistry, especially when studying transition metal compounds. The values in the table vary depending on the type and arrangement of ligands around the transition metal ion and play a crucial role in determining the electronic and magnetic properties of the compounds. These values are measured in units of "Dq" which represents the energy difference between lower and higher levels of the d orbitals. A higher Dq value indicates a greater energy required to stabilize the compound. Additionally, Crystal Field Stabilization Energy affects the color and optical properties of the compounds as it influences the absorption of light. Understanding this concept is essential in predicting and comprehending the properties of transition metal compounds and their potential applications in various fields. This concludes our discussion on the Crystal Field Stabilization Energy Table. Please stay tuned for more information on other aspects of periodic properties in our presentation..

[Audio] Slide 13 discusses the factors that influence crystal field splitting in transition metal complexes. These factors include the nature of ligands, oxidation state of the metal ion, geometry, and electronic configuration. Strong field ligands, such as CN⁻ and CO, cause a larger splitting energy, while weak field ligands, like I⁻ and Br⁻, result in a lower splitting due to differences in electronic configuration and bonding strength. Higher oxidation states lead to an increase in splitting energy, as the metal ion has a stronger pull on the ligands. The geometry of the complex also plays a role, with octahedral complexes typically having greater splitting compared to tetrahedral complexes. The electronic configuration of the metal ion also affects the splitting, with high spin complexes having a larger splitting energy due to the distribution of electrons among the d-orbitals, and low spin complexes having a lower splitting energy. These factors are important to consider in order to understand and predict the properties of transition metal complexes..

[Audio] We are currently on slide number 14 out of 23, discussing the atomic properties of elements in our presentation on UNIT - 1 - PERIODIC PROPERTIES BATCH - 2. Let's begin by understanding the concept of atomic radii, which is the distance from the nucleus to the outermost electron shell. This distance varies among different elements and determines the size of an atom. Next, we have ionisation energy, which measures the energy required to remove an electron from a gaseous atom. It also shows the ease with which an atom can become a cation. Moving on, electronegativity is a measure of an atom's attraction to shared electrons in a chemical bond and is essential in understanding chemical bonds and element reactivity. Lastly, electron affinity is the energy released when a neutral atom gains an extra electron to form a negative ion, playing a significant role in explaining the formation of ionic compounds and atom stability. These atomic properties are crucial in understanding the behavior and reactions of elements. Let's now move on to the next slide..

[Audio] Today, we will discuss the spectrochemical series and its role in coordination complexes. The series arranges ligands in order of their ability to split the d-orbitals of a central metal ion, known as the crystal-field splitting energy. This has a significant impact on the electronic structure, color, and magnetic properties of the complex. Ligands are ranked from weak-field to strong-field based on the size of the splitting, with strong-field ligands causing a greater energy difference between the d-orbitals. This energy difference greatly influences the properties and reactivity of the complex. Understanding the spectrochemical series is crucial for predicting the behavior and designing coordination complexes with specific properties. It is a vital tool in inorganic chemistry. In conclusion, the spectrochemical series has a significant impact on the study of coordination chemistry and the properties of coordination complexes..

[Audio] Slide number 16 of our presentation on UNIT 1, Batch 2, "Periodic Properties" delves into the Introduction to HSAB Theory. The concept of hard and soft acids and bases is the focal point of this segment. Hard and soft classifications are based on three factors: charge density, polarizability, and the nature of interactions. Hard acids and bases have a high charge density, low polarizability, and tend to form more ionic bonds. Examples of hard acids include metal ions with high positive charges and small ionic sizes, while hard bases include small anions and neutral molecules. Oxygen and nitrogen atoms are commonly classified as hard. Further examples of hard acids and bases include H+, O2-, OH-, F-, Fe3+, and Al3+. We hope this further understanding of the HSAB Theory and the classification of hard acids and bases has been helpful. The remaining slides of our presentation will provide more information on this topic..

[Audio] Slide 17 out of 23 of our presentation on Unit 1 and Periodic Properties for Batch 2 will focus on "Soft Acids and Bases". This concept is important in the study of chemical bonding and reactivity. Soft acids and bases have a low charge density, meaning a low number of positive or negative charges in a given space. This makes them more polarizable and allows for the formation of strong covalent bonds. Typical examples of soft acids include transition metals with a +1 charge, such as Cu+ or those in the late 4d and 5d series like Cd2+ and Hg2+. Soft bases, on the other hand, are usually larger anions and neutral molecules, such as I- and S2-. Understanding soft acids and bases is crucial in predicting chemical reactions and comprehending the properties and behavior of different elements..

[Audio] In slide number 18, we will discuss the topic of isomerism. Isomerism refers to the occurrence of compounds that have the same molecular formula but differ in the arrangement of their atoms or groups. When it comes to coordination compounds, isomers differ in the structure or spatial arrangement of ligands around the central metal ion, resulting in different properties and behaviors of the compounds. There are two common types of isomerism in coordination compounds: structural and geometrical isomerism. Structural isomers have the same molecular formula but differ in the bonding order of the atoms, while geometrical isomers have the same molecular formula but differ in the spatial arrangement around the double bond. An understanding of isomerism is essential in studying coordination compounds, as it allows for the recognition and explanation of their various properties and behaviors. For further information on this topic, let's proceed to the next slide..

[Audio] We are currently on slide number 19, discussing three types of isomerism in coordination compounds. These are ionization isomerism, hydrate isomerism, and linkage isomerism. Ionization isomerism occurs when compounds produce different ions in solution, despite having the same composition. An example of this is when a compound can produce both a cation and an anion in solution. Hydrate isomerism, also known as solvate isomerism, is determined by the number of water molecules present inside or outside the coordination sphere of a compound. For instance, the same compound can have different numbers of water molecules attached to it. Lastly, linkage isomerism happens when a ligand can attach through two different donor atoms, known as an ambidentate ligand. For example, the same ligand can attach through two different atoms, resulting in different isomers. As we can see, isomerism has a significant impact on the properties and behavior of coordination compounds. We hope that this brief overview has provided a better understanding of these three types of isomerism. Stay tuned for the remaining slides as we continue exploring periodic properties in Batch 2 of our presentation..

[Audio] This slide will discuss coordination isomerism and coordination position isomerism, which are commonly found in compounds with cationic and anionic complexes. These isomerism types result from the exchange of ligands between the complexes, leading to different structures with the same chemical formula. An example of this can be seen in the compound shown. Additionally, coordination position isomerism occurs in polynuclear complexes where ligands can occupy different coordination sites, resulting in different structures with the same chemical formula. Understanding these isomerism types is crucial in coordination chemistry as they greatly impact the properties and behavior of compounds. By recognizing and analyzing these types of isomerism, we can gain a deeper understanding of the periodic properties of compounds and their behavior in various environments. Let's move onto the next slide for more information on this concept in our unit on periodic properties..

[Audio] Slide number 21 discusses geometrical isomerism in coordination compounds. This phenomenon is caused by the arrangement of ligands around the central metal ion. It is commonly seen in square planar and octahedral complexes. In square planar complexes with the formula MA₂B₂, there are two possible isomers - cis and trans. The cis-isomer has identical ligands adjacent to each other, while the trans-isomer has them on opposite sides of the metal ion. For example, a square planar complex with two ammonia (NH₃) ligands can have a cis or trans configuration. This concludes our discussion on geometrical isomerism in coordination compounds. Next slide for more information..

[Audio] We will now discuss octahedral complexes, specifically the MA₄B₂ and MA₃B₃ types, on slide number 22. These complexes exhibit cis/trans isomerism, where the ligand positions can impact the complex's properties and reactivity. For MA₃B₃ type complexes, there are two possible isomerism patterns: fac and mer. The fac isomer has three identical ligands on one face of the octahedron, while the mer isomer has three identical ligands on one meridian plane. To better understand, consider an example of an octahedral complex with the formula MA₃B₃, which can have both fac and mer isomers if the ligands are the same. This is a crucial aspect to consider when studying the properties and behavior of octahedral complexes. Our discussion on octahedral complexes has now concluded. Moving on, our final slide will wrap up our unit on periodic properties for Batch 2..

Thank You.