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D & F-BLOCK ELEMENTS in 1 Shot - All Concepts with PYQs | Class 12 NCERT

NCERT Wallah・2 minutes read

Ayush Kumar Gupta explores the significance of D block elements in organic chemistry, emphasizing their electronic configurations, properties, and oxidation states, while also introducing the concept of coordination compounds. The text highlights key features such as the classification of elements, the importance of memorizing configurations for exams, and the behaviors of transition metals, ultimately stressing the need for a thorough understanding of these concepts for success in chemistry.

Insights

  • Ayush Kumar Gupta introduces the first chapter on "D Block Elements" in organic chemistry, noting that it will be followed by a chapter on "Coordination Compounds," highlighting the structured approach to the syllabus and the importance of these topics in understanding complex chemical behaviors.
  • The text emphasizes the significance of electronic configurations in D block elements, stating that these configurations are crucial for understanding properties like oxidation states, magnetic characteristics, and color, which are essential for mastering the behavior of transition metals.
  • The classification of D block elements is detailed, with 10 groups identified, and the distinction between transition elements and non-transition elements is made clear, noting that elements like Zinc and Silver do not qualify as transition metals due to their fully filled d subshells.
  • The chapter discusses the trends in atomic size across the D block, explaining that atomic size generally decreases from left to right due to increasing nuclear charge, while also addressing the shielding effect and effective nuclear charge, which influence atomic behavior and reactivity.
  • The concept of variable oxidation states in transition metals is highlighted, with examples like chromium and copper illustrating how these states are influenced by electron configurations, which allows these metals to participate in diverse chemical reactions and form complex ions.
  • The text concludes by stressing the importance of memorizing key properties and electron configurations of transition metals for academic success, suggesting the use of mnemonics and regular practice to retain this information, which is vital for understanding and applying chemistry concepts effectively.

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Recent questions

  • What are D block elements?

    D block elements are transition metals characterized by their electron configurations, specifically those with partially filled d orbitals. These elements, found in groups 3 to 12 of the periodic table, exhibit unique properties such as variable oxidation states, the ability to form complex ions, and distinct magnetic characteristics. The d block includes metals like iron, copper, and chromium, which are essential in various chemical reactions and industrial applications. Understanding their electronic configurations is crucial for predicting their behavior in chemical processes, as these configurations influence their reactivity, color, and conductivity.

  • How do transition metals behave?

    Transition metals exhibit a range of behaviors due to their unique electronic configurations, particularly the presence of unpaired electrons in their d orbitals. This allows them to participate in various oxidation states, typically ranging from +1 to +7, which is significant in redox reactions. Their ability to form complex ions and engage in coordination chemistry is also notable, as it leads to diverse applications in catalysis and materials science. Additionally, transition metals are known for their magnetic properties, which can be calculated based on the number of unpaired electrons. Overall, their behavior is influenced by their electron configurations, making them versatile in chemical reactions.

  • What is oxidation state in chemistry?

    The oxidation state, or oxidation number, is a concept in chemistry that indicates the degree of oxidation of an atom in a compound. It reflects the number of electrons an atom gains, loses, or shares when forming chemical bonds. Transition metals are particularly notable for exhibiting multiple oxidation states, which allows them to participate in various chemical reactions. For example, iron can exist in +2 and +3 states, while manganese can reach up to +7. Understanding oxidation states is crucial for predicting the reactivity and properties of elements, especially in redox reactions where electron transfer occurs.

  • Why are electron configurations important?

    Electron configurations are essential in chemistry as they provide insight into the arrangement of electrons around an atom's nucleus, influencing its chemical properties and behavior. For transition metals, the configuration of d orbitals plays a critical role in determining their oxidation states, reactivity, and ability to form complex ions. Knowledge of electron configurations helps predict how elements will interact in chemical reactions, their magnetic properties, and their conductivity. Additionally, understanding these configurations is vital for mastering concepts in inorganic chemistry, particularly when studying transition metals and their unique characteristics.

  • What is hydration energy?

    Hydration energy refers to the amount of energy released or absorbed when ions are surrounded by water molecules during the process of solvation. This energy is crucial in determining the stability and reactivity of metal ions in aqueous solutions. For instance, the hydration energy of copper ions significantly influences their solubility and reactivity. High hydration energy indicates strong interactions between the ion and water, making the ion more stable in solution. Understanding hydration energy is essential for predicting how different metal ions behave in chemical reactions, particularly in processes involving transition metals, where hydration can affect their oxidation states and overall reactivity.

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Summary

00:00

Understanding D Block Elements in Chemistry

  • Ayush Kumar Gupta introduces the topic of the first chapter, focusing on "D Block Elements" in organic chemistry, and mentions that the second chapter will cover "Coordination Compounds."
  • The chapter discusses the deletion of certain topics, specifically mentioning that KMnO4 and Cr2O7 have been removed from the syllabus, along with a focus on electronic configurations and oxidation states.
  • The D block elements are defined as those with electrons filling the d subshell, and the electronic configuration is crucial for understanding their properties.
  • The text explains the classification of elements into groups, specifically noting that there are 10 groups in the D block, ranging from group 3 to group 12.
  • It describes the shapes of orbitals, particularly the "double dumbbell" shape of d orbitals, and how these shapes relate to the arrangement of electrons.
  • The maximum number of electrons in the d block is stated to be 10, with a detailed explanation of how these electrons are distributed among the orbitals.
  • Transition elements are defined as those with an incomplete d subshell, and the text emphasizes the importance of understanding their oxidation states, which typically range from +1 to +2.
  • The configuration of transition elements is discussed, with specific examples such as Scandium (Sc) and Copper (Cu), highlighting their electronic configurations and how they relate to their classification as transition elements.
  • The text notes that not all elements in the d block are considered transition elements, specifically mentioning Zinc (Zn) and Silver (Ag) as exceptions due to their fully filled d subshells.
  • Finally, the chapter emphasizes the significance of electronic configuration in understanding the properties of transition elements, including their magnetic properties and color, and encourages memorization of these configurations for better comprehension.

24:11

Understanding Transition Metals and Their Properties

  • The text discusses the classification of elements, specifically focusing on the transition metals, which are categorized as D block elements, and highlights that there are 32 elements in total, with 30 being significant in the context of the discussion.
  • It mentions that the maximum number of electrons in an orbital is two, and emphasizes the importance of understanding electron configurations, particularly for transition elements, which are defined by their unique properties and positions in the periodic table.
  • The D block elements are introduced, with a focus on their general electronic configuration, which typically follows the pattern of filling the 3D, 4D, and 5D orbitals across different periods, specifically from the 3rd to the 7th period.
  • The text outlines the first series of transition elements, starting from Scandium (atomic number 21) to Zinc (atomic number 30), and provides a mnemonic to help remember the order of these elements.
  • It explains the significance of oxidation states in transition metals, noting that they can exhibit multiple oxidation states, which is crucial for understanding their chemical behavior and reactions.
  • The second series of transition elements is mentioned, which includes elements from Yttrium (atomic number 39) to Cadmium (atomic number 48), and emphasizes the need to memorize their configurations and properties.
  • The third series, covering elements from Lanthanum (atomic number 57) to Lutetium (atomic number 71), is also discussed, highlighting the importance of knowing their atomic numbers and electron configurations.
  • The text stresses the importance of memorizing the properties and configurations of elements, particularly for exams, and suggests using songs or mnemonics as effective study aids to retain this information.
  • It provides specific examples of electron configurations for various transition metals, such as Chromium (atomic number 24) and Copper (atomic number 29), detailing how to derive their configurations based on the removal of electrons from their outer shells.
  • Finally, the text encourages students to practice and review the configurations and properties of transition metals regularly, as this knowledge is essential for mastering chemistry concepts related to these elements.

50:08

Properties and Trends of D Block Metals

  • The discussion focuses on the physical properties of metals, particularly those in the D block of the periodic table, emphasizing their characteristics and behaviors in various conditions.
  • Mercury is highlighted as the only metal that is liquid at room temperature, and it can be manipulated into thin sheets, showcasing its unique properties compared to other metals.
  • The text mentions that metals like silver and copper are excellent conductors of electricity, with copper being specifically noted for its use in wiring due to its high conductivity.
  • Iron is emphasized for its strength and utility in construction, with a recommendation to use it for building durable structures, as it is both shiny and sonorous.
  • The concept of atomic size is introduced, explaining that atomic size decreases from left to right across a period in the D block due to increasing nuclear charge, which attracts electrons more strongly.
  • The shielding effect is described, where inner electrons repel outer electrons, affecting the overall size of the atom and its reactivity; this is crucial for understanding atomic behavior.
  • The effective nuclear charge is defined as the net positive charge experienced by valence electrons, which influences their attraction to the nucleus and thus the size of the atom.
  • The text outlines a trend in atomic size across the 3D series, noting that as atomic number increases, the size generally decreases due to increased nuclear charge and effective attraction.
  • The relationship between atomic size and electron configuration is discussed, particularly how filling electron shells affects the size and properties of elements in the D block.
  • Finally, the text concludes with a note on the size trends in the 4D and 5D series, indicating that while size generally increases, there are exceptions based on electron filling and nuclear charge interactions.

01:12:42

Understanding Size Trends in Elemental Chemistry

  • The text discusses five mistakes related to the size of elements in a chart, emphasizing that if social factors increase, the size should also increase, particularly in the context of 5D elements, which are noted to be 240 in size and can rot in half at 253.
  • It mentions that the size of certain elements remains almost the same, specifically referencing a size of 9 inches for a length related to the "Feeling of Forest" and how this impacts the overall understanding of size in the context of 5D elements.
  • The text highlights that the size of elements can decrease due to various factors, including the influence of valence electrons, and provides a specific example of how the size of the T-20 series was reduced initially, with copper and zinc showing an increase in size.
  • It explains that as atomic numbers increase, the size of elements generally decreases, with a specific focus on the behavior of elements in the 3D, 4D, and 5D series, noting that the size remains almost equal in certain groups.
  • The text outlines the relationship between positive charge and size, indicating that a greater positive charge results in a smaller size, using magnesium and iron as examples to illustrate how size decreases with increasing positive charge.
  • It discusses the concept of ionization energy, stating that as size decreases, ionization energy increases, with a specific mention of how this trend is observed across different series, particularly in the D block.
  • The text emphasizes the irregularities in size trends within the D block series, noting that while size generally decreases from left to right, there are exceptions, particularly in the case of chromium and copper.
  • It mentions the energy required to remove electrons from elements, specifically highlighting that removing the third electron from iron requires a significant amount of energy, quantified as 307 kilojoules.
  • The text also addresses the oxidation states of transition metals, indicating that the first and last members of a series do not show variable oxidation states, while others do, with specific examples provided for scandium and zinc.
  • Finally, it touches on electrode potential in electrochemistry, noting that the behavior of the 3D series is not regular, with specific values provided for electrode potentials, indicating a trend that deviates at certain points.

01:35:38

Metals Properties and Behaviors Explained

  • Understanding the state of metals involves recognizing their solid state and the process of electron removal, which is essential for manipulating their properties. This requires knowledge of sublimation, where a solid directly transitions to gas without becoming liquid, necessitating energy input at the right time.
  • The concept of hydration energy is crucial, as it determines how much energy is needed to change the state of a metal, such as copper, which has two electrons that can be removed to form a copper ion (Cu²⁺). The hydration energy for this process is approximately 140 kJ/mol.
  • The process of oxidation and reduction is fundamental in chemistry, where oxidation involves losing electrons and reduction involves gaining them. For example, chromium can exist in multiple oxidation states, such as Cr²⁺ and Cr³⁺, depending on the electron configuration.
  • The density of metals increases from left to right in the periodic table, influenced by both mass and volume. As the atomic size decreases, the density tends to increase, which is important for understanding the physical properties of metals.
  • The strength of metallic bonds is directly proportional to the number of unpaired electrons; more unpaired electrons result in stronger bonds and higher melting points. For instance, metals with higher unpaired electron counts exhibit greater hardness and stability.
  • The magnetic properties of metals can be calculated using the formula for magnetic moment, which is based on the number of unpaired electrons. The formula is n√(n+2), where n is the number of unpaired electrons.
  • Transition metals, such as copper and chromium, can exhibit multiple oxidation states due to their electron configurations, which allows them to participate in various chemical reactions and form complex ions.
  • The process of complex formation in transition metals is significant, as it allows for the creation of various compounds with unique properties. For example, iron is used in the Haber process to synthesize ammonia from nitrogen and hydrogen.
  • The hydration energy and the energy required for electron removal are critical in determining the reactivity of metals. For example, the hydration energy for copper ions is a key factor in its solubility and reactivity in aqueous solutions.
  • Understanding the properties and behaviors of transition metals, including their ability to form complexes and exhibit variable oxidation states, is essential for applications in chemistry, materials science, and industrial processes.

02:00:38

Chemical Processes and Properties of Materials

  • High nickel is utilized in hydrogenation processes, particularly for converting vegetable oil, which is a key theme in the text. The process involves using a P DC adapter and specific tools for effective conversion.
  • The production of polythene requires a high-temperature environment, and it is recommended to use a specific type of potato to achieve the desired results in polymer creation.
  • The text discusses the significance of unpaired electrons in color translation within compounds, emphasizing that the presence of these electrons can lead to color changes in materials, such as the pink or purple hues observed in potassium permanganate.
  • The concept of charge transfer is introduced, explaining that when electrons are transferred, it can result in color changes in various compounds, including silver bromide and silver iodide, which exhibit yellow coloration due to polarization.
  • Polarization is further explained, noting that smaller ions lead to greater polarizing power, which affects the color and properties of compounds, with specific mention of silver chloride turning white when certain conditions are met.
  • The text highlights the importance of the size difference between metals when creating alloys, stating that the size difference should not exceed 15% for optimal mixing, which is crucial in the production of materials like gold jewelry.
  • Transition metals are discussed in the context of interstitial compounds, where smaller atoms can occupy spaces within the metal lattice, affecting the properties of the resulting material.
  • The energy required for various reactions, such as sublimation and ionization, is emphasized, with specific energy values mentioned, such as 126 kilojoules for certain reactions involving transition metals.
  • The role of fluorine as a stabilizer in oxidation states is explained, particularly how it stabilizes higher oxidation states in elements like manganese, while lower oxidation states can lead to instability.
  • The text concludes with a discussion on copper's oxidation states, detailing how copper(I) iodide behaves as a reducing agent, and the implications of copper's oxidation states in chemical reactions, including the transition from copper(II) to copper(I).

02:23:48

Hydration Energy and Oxidation States in Metals

  • Hydration of copper releases significant energy, specifically when comparing Copper(II) to Copper(I), with the former exhibiting a higher hydration energy release, quantified at 500 units of energy.
  • The process of removing electrons from Copper(II) requires energy, indicating that the hydration energy plays a crucial role in the stability and reactivity of copper ions.
  • Manganese, as an element, has a group number that indicates its oxidation states, with the highest being +7, which is relevant in reactions involving fluoride.
  • The acidity of a solution increases with the oxidation state of the metal, meaning that as the oxidation state rises, the acid character of the solution also intensifies.
  • Transition metals, such as chromium and titanium, exhibit varying oxidation states, with chromium showing +3 and +6 states, which are important in redox reactions.
  • Copper does not react with dilute sulfuric acid due to its position below hydrogen in the reactivity series, which is supported by its positive reduction potential of +0.341.
  • The hydration energy of ions like Nickel(II) is notably high, which affects their reactivity and stability in solution, making them strong oxidizing agents.
  • The electronic configuration of transition metals is crucial for understanding their chemical behavior, with the last electron entering the d-orbital, influencing their oxidation states and reactivity.
  • Lanthanide contraction occurs as atomic numbers increase, leading to a slight decrease in atomic size, which affects the physical and chemical properties of the elements in this series.
  • Common oxidation states for transition metals typically include +2 and +3, with some elements also exhibiting +4 and +6 states, which are significant in various chemical reactions and applications.

02:46:48

Understanding Chemical Elements and Their Reactivity

  • The text discusses the properties and behaviors of various chemical elements, particularly focusing on electron configurations and the reactivity of transition metals. It mentions that noble gases have stable electron configurations and that the release of electrons can affect the chemical characteristics of elements, with specific reference to the electron configurations of copper and nickel, including their hydration energies and oxidation states.
  • It highlights the importance of understanding interstitial compounds and their formation, noting that small items can spoil over time in interstitial spaces. The text also emphasizes the significance of knowing the melting points and conductivity of certain materials, suggesting that these properties are crucial for identifying the reactivity of chemicals, particularly in the context of transition elements.
  • The text concludes with a reminder of the necessity to grasp key concepts and numerical data for effective preparation for examinations, including the importance of understanding oxidation states and the ability to form multiple bonds in chemical reactions. It encourages students to familiarize themselves with charts and concepts to answer questions accurately, indicating that a solid grasp of these topics is essential for success in chemistry.
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