1) D-block elements are those whose last electron enters the d orbital, lying between s- and p-block elements.
2) Not all d-block elements are transition elements, which are defined as having partially filled d orbitals, while all transition elements are d-block.
3) General properties of d-block elements include high melting/boiling points due to strong metallic bonds, variable oxidation states, and many forming colored ions or complexes.
The document discusses the group 16 (oxygen family) elements of the periodic table. It covers their general electronic configuration of ns2np4, trends in periodic properties like atomic radius and ionization energy decreasing down the group. It describes the common oxidation states of -2, +2, +4 and +6. It also discusses the formation of hydrides, halides, oxides and reactions with air, acids, alkalis and metals for these chalcogen elements.
d-block elements are those in which the valence electrons enters the d orbital. d- block elements are also called transition elements. Transition elements have partially filled d orbitals.
This document discusses the properties of transition elements and their coordination compounds. It begins by defining transition elements and inner transition elements based on their location in the periodic table. It then examines the properties of transition metals such as their colored and paramagnetic nature. Several trends in atomic properties across and within periods are described, including trends in atomic size, ionization energy, and oxidation states. Coordination compounds and bonding are also briefly mentioned.
The document discusses inner transition elements, specifically the lanthanide and actinide series. It provides details on their electronic configurations, oxidation states, properties such as color and magnetism, extraction from monazite sand, and separation methods. It also compares the lanthanides and actinides, noting they both show lanthanide/actinide contractions and have similar properties, but the actinides exhibit more variable chemistry and are all radioactive.
p-BLOCK ELEMENTS,Boron Family (Group 13 Elements )
Compounds of Boron,Orthoboric acid (H3BO3),Borax (sodium tetraborate) Na2B4O7. 10H2O,Diborane,Compounds of Aluminium,Aluminium Oxide or Alumina (Al2O3),
Aluminum Chloride AlCl3,Carbon Family (Group 14 Elements):
Compounds of Carbon,Carbon Monoxide,Carbon di-oxide,
Carbides, Nitrogen Family (Group 15 Elements),
Ammonia (NH3),Phosphorus,Phosphorous Halides,Oxides of Phosphorus,Oxy – Acids of Phosphorus,Oxygen Family (Group 16 Elements) , Allotropes of Sulphur,Halogen Family ( Group 17 Elements,Inter halogen compounds,
Hydrogen Halides,Pseudohalide ions and pseudohalogens,Some important stable compound of Xenon
This document discusses the characteristic properties of s-block elements, which include the alkali metals (Group IA) and alkaline earth metals (Group IIA). Some key points discussed include:
- S-block elements have their outermost shell electrons in the s orbital.
- Alkali metals react vigorously with water to form alkaline hydroxides and hydrogen gas. Reactivity increases down the group.
- They form oxides, peroxides, and superoxides with oxygen. Oxidation states include -2, -1, and -1/2.
- Properties such as ionization energy, hydration energy, and metallic character generally decrease or increase moving down a group and across a period,
1) D-block elements are those whose last electron enters the d orbital, lying between s- and p-block elements.
2) Not all d-block elements are transition elements, which are defined as having partially filled d orbitals, while all transition elements are d-block.
3) General properties of d-block elements include high melting/boiling points due to strong metallic bonds, variable oxidation states, and many forming colored ions or complexes.
The document discusses the group 16 (oxygen family) elements of the periodic table. It covers their general electronic configuration of ns2np4, trends in periodic properties like atomic radius and ionization energy decreasing down the group. It describes the common oxidation states of -2, +2, +4 and +6. It also discusses the formation of hydrides, halides, oxides and reactions with air, acids, alkalis and metals for these chalcogen elements.
d-block elements are those in which the valence electrons enters the d orbital. d- block elements are also called transition elements. Transition elements have partially filled d orbitals.
This document discusses the properties of transition elements and their coordination compounds. It begins by defining transition elements and inner transition elements based on their location in the periodic table. It then examines the properties of transition metals such as their colored and paramagnetic nature. Several trends in atomic properties across and within periods are described, including trends in atomic size, ionization energy, and oxidation states. Coordination compounds and bonding are also briefly mentioned.
The document discusses inner transition elements, specifically the lanthanide and actinide series. It provides details on their electronic configurations, oxidation states, properties such as color and magnetism, extraction from monazite sand, and separation methods. It also compares the lanthanides and actinides, noting they both show lanthanide/actinide contractions and have similar properties, but the actinides exhibit more variable chemistry and are all radioactive.
p-BLOCK ELEMENTS,Boron Family (Group 13 Elements )
Compounds of Boron,Orthoboric acid (H3BO3),Borax (sodium tetraborate) Na2B4O7. 10H2O,Diborane,Compounds of Aluminium,Aluminium Oxide or Alumina (Al2O3),
Aluminum Chloride AlCl3,Carbon Family (Group 14 Elements):
Compounds of Carbon,Carbon Monoxide,Carbon di-oxide,
Carbides, Nitrogen Family (Group 15 Elements),
Ammonia (NH3),Phosphorus,Phosphorous Halides,Oxides of Phosphorus,Oxy – Acids of Phosphorus,Oxygen Family (Group 16 Elements) , Allotropes of Sulphur,Halogen Family ( Group 17 Elements,Inter halogen compounds,
Hydrogen Halides,Pseudohalide ions and pseudohalogens,Some important stable compound of Xenon
This document discusses the characteristic properties of s-block elements, which include the alkali metals (Group IA) and alkaline earth metals (Group IIA). Some key points discussed include:
- S-block elements have their outermost shell electrons in the s orbital.
- Alkali metals react vigorously with water to form alkaline hydroxides and hydrogen gas. Reactivity increases down the group.
- They form oxides, peroxides, and superoxides with oxygen. Oxidation states include -2, -1, and -1/2.
- Properties such as ionization energy, hydration energy, and metallic character generally decrease or increase moving down a group and across a period,
The document discusses the properties of group 14 elements. It notes that carbon and silicon are non-metals, germanium is a metalloid, and tin and lead are metals. It discusses their electronic configurations, atomic radii, ionization energies, electronegativity, oxidation states, and physical properties. Carbon exhibits allotropes like diamond, graphite and buckminsterfullerenes which have the same chemical composition but different physical properties. Diamond has a high melting point and hardness due to its strong covalent bonds.
The document discusses the d-block and f-block elements of the periodic table. It provides details about their electronic configurations, properties, and reactions. The d-block contains the transition metals whose d orbitals are filled from groups 3 to 12. The f-block contains the inner transition metals whose 4f and 5f orbitals are filled. Elements in these blocks can exhibit a variety of oxidation states and form complexes due to their electronic structure.
Crystal Field Theory explains the colors of transition metal complexes based on ligand-metal interactions. The electrostatic interaction between ligands and metal d-orbitals splits the d-orbital energies. For an octahedral complex, the d-orbitals point directly at ligands have higher energy than those that bisect ligands. This splitting pattern determines if the complex is high or low spin, which then dictates its color and magnetic properties. The spectrochemical series orders ligands by their ability to cause crystal field splitting, correlating ligand type with complex color.
The document summarizes key information about d-block and f-block elements. It discusses:
- The d-block elements have their d orbitals progressively filled in each period, while the f-block elements have their 4f and 5f orbitals filled in the latter two periods.
- Transition metals exhibit a variety of oxidation states, melting points, atomic radii, and magnetic properties due to their incompletely filled d orbitals.
- Properties vary periodically across each series as the nuclear charge increases, with factors like ionization energies and electronegativity influencing stability and reactivity.
Introduction, position in periodic table, transition elements & inner transition elements, lanthanoids & actinoids, General trends in properties, atomic radii, atomic volume, melting points, boiling points, density, standard electrode potentials, oxidation states, Some practice questions.
Group 15 of the periodic table consists of nitrogen, phosphorus, arsenic, antimony, and bismuth. These elements can be non-metals, metalloids, or metals. They have the general electronic configuration of ns2np3 and can form compounds with oxidation states of -3, +3, and +5. The reactivity and properties of the elements change as one goes down the group due to an increase in atomic size and metallic character.
The document discusses Crystal Field Theory, which explains the bonding in transition metal complexes. It describes how the electrostatic interaction between ligand electrons and metal d-orbitals results in a splitting of the d-orbital energies. In an octahedral field, the t2g orbitals are stabilized more than the eg orbitals. Crystal Field Theory can explain properties like electronic spectra, magnetic moments, and color of complexes. The magnitude of splitting depends on factors like the metal ion, its charge, the ligands, and can be represented by the crystal field splitting energy Δo.
- The elements in Group 15 show increasing covalent radius and decreasing ionization energy down the group, due to additional shells. Nitrogen behaves anomalously due to small size and high electronegativity.
- They form trihydrides (MH3), trioxides (M2O3), and pentoxides (M2O5) with decreasing acidity down the group. They also form trihalides and pentahalides.
- Oxygen is industrially produced from air or water and is essential for respiration and combustion. Ozone is a reactive allotrope produced from oxygen that is used for sterilization and bleaching.
This document discusses coordination chemistry concepts including different types of salts such as simple salts, double salts, and complex salts. It defines coordination compounds and complex ions, and describes Werner's coordination theory which proposed that metals have primary and secondary valences. Ligands are defined as electron-rich species that bond to metals. Different classifications of ligands and coordination numbers are provided. The coordination sphere and effective atomic number concept are also summarized.
Class 12 The d-and f-Block Elements.pptxNamanGamer3
The document provides information on various topics related to d-block elements or transition elements including:
- Their electronic configurations with d orbitals being progressively filled
- Properties like high melting points and variable oxidation states arising due to unfilled d orbitals
- Trends in properties across periods and groups like decreasing atomic size but similar atomic radii between 2nd and 3rd transition series due to lanthanide contraction
- Transition metals exhibiting magnetic properties when they contain unpaired electrons and forming colored ions through d-d transitions
This document provides information about important families of elements in the periodic table including halogens, noble gases, chalcogens, and alkali and alkaline earth metals. It also discusses the classes of elements, position and electronic configurations of transition metals, and trends in various properties like ionization energies, oxidation states, magnetic properties, and formation of colored ions and complex compounds. The document explains how transition metals exhibit a variety of properties due to their ability to adopt multiple oxidation states and form complexes through d-orbital involvement.
The elements in which the valence electron enters the s orbital are called s block elements.
The elements in which the valence electron enters the p orbital are called p block elements.
This document discusses various properties of transition metals including their melting points, boiling points, atomic and ionic radii, ionization energies, oxidation states, and magnetic properties. Some key points:
- Transition metals have high melting and boiling points due to strong metallic bonds and involvement of d-orbitals in bonding. Melting points first increase to a maximum and then decrease along a period.
- Atomic/ionic radii first decrease to a minimum, then remain constant, and increase toward the end of a period as electron-electron repulsion increases.
- Ionization energies generally increase along a period as nuclear charge increases, but the effect is partly canceled by d-orbital shielding.
- Transition
The document discusses various principles and processes involved in the isolation of elements through metallurgy. It describes how elements are found in nature, either in native state or combined state in minerals and ores. It then explains the metallurgical processes of crushing and grinding ores, concentrating the ore through various methods, converting the concentrated ore into metal oxides through calcination or roasting. Finally, it discusses reducing the metal oxides into metals through reduction processes using suitable reducing agents, based on the reactivity and position of metals in the Ellingham diagram.
The document provides information about the elements in Group 14 of the periodic table. It begins by introducing the group and listing the elements carbon, silicon, germanium, tin, and lead. It then provides details about each element, including their physical properties, oxidation states, occurrence in nature, and important uses. The document discusses topics like allotropes of carbon, silicon semiconductor applications, germanium use in electronics, tin uses in alloys and solder, and properties of lead like its low melting point.
Transition metals: Manganese, Iron and CopperSidra Javed
Transition metals such as manganese, iron, and copper can exist in multiple oxidation states. Manganese commonly exists as Mn2+, Mn4+, and Mn7+. Potassium manganate (VII), KMnO4, is a powerful oxidizing agent. Iron exists as Fe2+ and Fe3+ and acts as a catalyst in the Haber process. Copper exists as Cu+ and Cu2+. Compounds of Cu+ are generally colorless and insoluble while compounds of Cu2+ are blue and soluble, forming complexes with ligands like OH-, NH3, and CO32-.
This document summarizes Crystal Field Theory, which considers the electrostatic interactions between metal ions and ligands. It describes ligands and metal ions as point charges that can have attractive or repulsive forces. This causes the d orbitals of the metal ion to split into two sets depending on if the field created by the ligands is weak or strong. The theory explains color in coordination compounds as being caused by d-d electron transitions under the influence of ligands. However, it has limitations like not accounting for other metal orbitals or the partial covalent nature of metal-ligand bonds.
This document provides information about the boron family (Group 13) of the periodic table. It discusses the elements in Group 13 - boron (B), aluminium (Al), gallium (Ga), indium (In), and thallium (Tl). It details their electronic configurations, occurrence in nature, extraction methods, and chemical and physical properties. In particular, it focuses on the extraction of aluminium via the Bayer process and discusses the uses of aluminium and its environmental impacts.
The document discusses d-block and f-block elements. It provides information on:
1. The d-block elements have incompletely filled d orbitals and include elements from groups 3 to 12 in the periodic table.
2. Transition metals show variable oxidation states due to their ability to gain or lose ns and (n-1)d electrons. They form colored compounds and complexes due to their unpaired d electrons.
3. The f-block elements have incompletely filled 4f and 5f orbitals and include the lanthanides and actinides which follow lanthanum and actinium respectively.
1. The document discusses the properties of d-block elements, also known as transition elements. These elements have incompletely filled d orbitals and make up three rows in the periodic table corresponding to the filling of 3d, 4d, and 5d orbitals.
2. Transition elements have varying properties depending on their electronic configuration such as their atomic and ionic radii, densities, melting and boiling points, and tendencies to form complexes. They also exhibit variable oxidation states and many have characteristic colors that arise from electron excitation within their d orbitals.
3. Key trends noted include decreasing atomic radii down each group due to poor shielding of d electrons, higher melting and boiling points arising from strong bonding between s
The document discusses the properties of group 14 elements. It notes that carbon and silicon are non-metals, germanium is a metalloid, and tin and lead are metals. It discusses their electronic configurations, atomic radii, ionization energies, electronegativity, oxidation states, and physical properties. Carbon exhibits allotropes like diamond, graphite and buckminsterfullerenes which have the same chemical composition but different physical properties. Diamond has a high melting point and hardness due to its strong covalent bonds.
The document discusses the d-block and f-block elements of the periodic table. It provides details about their electronic configurations, properties, and reactions. The d-block contains the transition metals whose d orbitals are filled from groups 3 to 12. The f-block contains the inner transition metals whose 4f and 5f orbitals are filled. Elements in these blocks can exhibit a variety of oxidation states and form complexes due to their electronic structure.
Crystal Field Theory explains the colors of transition metal complexes based on ligand-metal interactions. The electrostatic interaction between ligands and metal d-orbitals splits the d-orbital energies. For an octahedral complex, the d-orbitals point directly at ligands have higher energy than those that bisect ligands. This splitting pattern determines if the complex is high or low spin, which then dictates its color and magnetic properties. The spectrochemical series orders ligands by their ability to cause crystal field splitting, correlating ligand type with complex color.
The document summarizes key information about d-block and f-block elements. It discusses:
- The d-block elements have their d orbitals progressively filled in each period, while the f-block elements have their 4f and 5f orbitals filled in the latter two periods.
- Transition metals exhibit a variety of oxidation states, melting points, atomic radii, and magnetic properties due to their incompletely filled d orbitals.
- Properties vary periodically across each series as the nuclear charge increases, with factors like ionization energies and electronegativity influencing stability and reactivity.
Introduction, position in periodic table, transition elements & inner transition elements, lanthanoids & actinoids, General trends in properties, atomic radii, atomic volume, melting points, boiling points, density, standard electrode potentials, oxidation states, Some practice questions.
Group 15 of the periodic table consists of nitrogen, phosphorus, arsenic, antimony, and bismuth. These elements can be non-metals, metalloids, or metals. They have the general electronic configuration of ns2np3 and can form compounds with oxidation states of -3, +3, and +5. The reactivity and properties of the elements change as one goes down the group due to an increase in atomic size and metallic character.
The document discusses Crystal Field Theory, which explains the bonding in transition metal complexes. It describes how the electrostatic interaction between ligand electrons and metal d-orbitals results in a splitting of the d-orbital energies. In an octahedral field, the t2g orbitals are stabilized more than the eg orbitals. Crystal Field Theory can explain properties like electronic spectra, magnetic moments, and color of complexes. The magnitude of splitting depends on factors like the metal ion, its charge, the ligands, and can be represented by the crystal field splitting energy Δo.
- The elements in Group 15 show increasing covalent radius and decreasing ionization energy down the group, due to additional shells. Nitrogen behaves anomalously due to small size and high electronegativity.
- They form trihydrides (MH3), trioxides (M2O3), and pentoxides (M2O5) with decreasing acidity down the group. They also form trihalides and pentahalides.
- Oxygen is industrially produced from air or water and is essential for respiration and combustion. Ozone is a reactive allotrope produced from oxygen that is used for sterilization and bleaching.
This document discusses coordination chemistry concepts including different types of salts such as simple salts, double salts, and complex salts. It defines coordination compounds and complex ions, and describes Werner's coordination theory which proposed that metals have primary and secondary valences. Ligands are defined as electron-rich species that bond to metals. Different classifications of ligands and coordination numbers are provided. The coordination sphere and effective atomic number concept are also summarized.
Class 12 The d-and f-Block Elements.pptxNamanGamer3
The document provides information on various topics related to d-block elements or transition elements including:
- Their electronic configurations with d orbitals being progressively filled
- Properties like high melting points and variable oxidation states arising due to unfilled d orbitals
- Trends in properties across periods and groups like decreasing atomic size but similar atomic radii between 2nd and 3rd transition series due to lanthanide contraction
- Transition metals exhibiting magnetic properties when they contain unpaired electrons and forming colored ions through d-d transitions
This document provides information about important families of elements in the periodic table including halogens, noble gases, chalcogens, and alkali and alkaline earth metals. It also discusses the classes of elements, position and electronic configurations of transition metals, and trends in various properties like ionization energies, oxidation states, magnetic properties, and formation of colored ions and complex compounds. The document explains how transition metals exhibit a variety of properties due to their ability to adopt multiple oxidation states and form complexes through d-orbital involvement.
The elements in which the valence electron enters the s orbital are called s block elements.
The elements in which the valence electron enters the p orbital are called p block elements.
This document discusses various properties of transition metals including their melting points, boiling points, atomic and ionic radii, ionization energies, oxidation states, and magnetic properties. Some key points:
- Transition metals have high melting and boiling points due to strong metallic bonds and involvement of d-orbitals in bonding. Melting points first increase to a maximum and then decrease along a period.
- Atomic/ionic radii first decrease to a minimum, then remain constant, and increase toward the end of a period as electron-electron repulsion increases.
- Ionization energies generally increase along a period as nuclear charge increases, but the effect is partly canceled by d-orbital shielding.
- Transition
The document discusses various principles and processes involved in the isolation of elements through metallurgy. It describes how elements are found in nature, either in native state or combined state in minerals and ores. It then explains the metallurgical processes of crushing and grinding ores, concentrating the ore through various methods, converting the concentrated ore into metal oxides through calcination or roasting. Finally, it discusses reducing the metal oxides into metals through reduction processes using suitable reducing agents, based on the reactivity and position of metals in the Ellingham diagram.
The document provides information about the elements in Group 14 of the periodic table. It begins by introducing the group and listing the elements carbon, silicon, germanium, tin, and lead. It then provides details about each element, including their physical properties, oxidation states, occurrence in nature, and important uses. The document discusses topics like allotropes of carbon, silicon semiconductor applications, germanium use in electronics, tin uses in alloys and solder, and properties of lead like its low melting point.
Transition metals: Manganese, Iron and CopperSidra Javed
Transition metals such as manganese, iron, and copper can exist in multiple oxidation states. Manganese commonly exists as Mn2+, Mn4+, and Mn7+. Potassium manganate (VII), KMnO4, is a powerful oxidizing agent. Iron exists as Fe2+ and Fe3+ and acts as a catalyst in the Haber process. Copper exists as Cu+ and Cu2+. Compounds of Cu+ are generally colorless and insoluble while compounds of Cu2+ are blue and soluble, forming complexes with ligands like OH-, NH3, and CO32-.
This document summarizes Crystal Field Theory, which considers the electrostatic interactions between metal ions and ligands. It describes ligands and metal ions as point charges that can have attractive or repulsive forces. This causes the d orbitals of the metal ion to split into two sets depending on if the field created by the ligands is weak or strong. The theory explains color in coordination compounds as being caused by d-d electron transitions under the influence of ligands. However, it has limitations like not accounting for other metal orbitals or the partial covalent nature of metal-ligand bonds.
This document provides information about the boron family (Group 13) of the periodic table. It discusses the elements in Group 13 - boron (B), aluminium (Al), gallium (Ga), indium (In), and thallium (Tl). It details their electronic configurations, occurrence in nature, extraction methods, and chemical and physical properties. In particular, it focuses on the extraction of aluminium via the Bayer process and discusses the uses of aluminium and its environmental impacts.
The document discusses d-block and f-block elements. It provides information on:
1. The d-block elements have incompletely filled d orbitals and include elements from groups 3 to 12 in the periodic table.
2. Transition metals show variable oxidation states due to their ability to gain or lose ns and (n-1)d electrons. They form colored compounds and complexes due to their unpaired d electrons.
3. The f-block elements have incompletely filled 4f and 5f orbitals and include the lanthanides and actinides which follow lanthanum and actinium respectively.
1. The document discusses the properties of d-block elements, also known as transition elements. These elements have incompletely filled d orbitals and make up three rows in the periodic table corresponding to the filling of 3d, 4d, and 5d orbitals.
2. Transition elements have varying properties depending on their electronic configuration such as their atomic and ionic radii, densities, melting and boiling points, and tendencies to form complexes. They also exhibit variable oxidation states and many have characteristic colors that arise from electron excitation within their d orbitals.
3. Key trends noted include decreasing atomic radii down each group due to poor shielding of d electrons, higher melting and boiling points arising from strong bonding between s
The document summarizes key points about d-block and f-block elements. It discusses the electronic configuration of transition metals and inner transition elements. It also provides information about the preparation of potassium dichromate and potassium permanganate. Some questions and answers related to the properties of transition metals and inner transition elements are also included.
D-block elements are those elements belonging to groups 3 through 12 that have their last electron entering the d subshell. Transition elements are defined as elements that have partially filled d orbitals. While all transition elements are d-block elements, not all d-block elements are transition elements as some like zinc have a filled d10 configuration. D-block elements form complex compounds by binding metal ions to anions or neutral molecules through available d orbitals. They also commonly show paramagnetism and catalytic properties due to unpaired electrons in their d orbitals.
d & f-block elements 12th Chemistry.pdfKapilPooniya
The document discusses trends in the electronic configurations and properties of elements in the d-block of the periodic table. It notes that chromium and copper have anomalous electronic configurations that can be explained by extra stability from half-filled or completely filled subshells. It also describes how atomic radii, density, ionic radii, oxidation states, and magnetic properties generally trend across and down the d-block in the periodic table.
The document discusses d-block elements and transition elements. It provides definitions and explanations around these topics.
1) d-block elements are those in the periodic table between groups 3 to 12, where the last electron enters the d subshell. Not all d-block elements are transition elements.
2) Transition elements are defined as those with incompletely filled d orbitals. Zn, Cd and Hg are not considered transition elements as they have fully filled d orbitals.
3) d-block elements and transition elements show various physical and chemical properties due to their electron configuration, including colored ions, catalytic activity, and ability to form complexes and interstitial compounds.
d and f block elements ppt 2021-22 (1).pptxmanormatanwar3
The document discusses the d-block and f-block elements of the periodic table. It provides details about:
1) The d-block contains elements where the d orbitals are progressively filled in each period, while the f-block contains elements where the 4f and 5f orbitals are filled.
2) Transition metals are defined as metals that have incomplete d subshells, while zinc, cadmium, and mercury are not considered transition metals as they have full d10 configurations.
3) The f-block elements are called inner transition or lanthanide elements, with electronic configurations of [Xe] 4f1-14 5d0,1 6s2.
The document discusses the electronic configurations and properties of d-block elements. It begins by defining transition metals as elements whose atoms have partly filled d-orbitals. It then discusses exceptions to the general electronic configuration formula due to energy differences between orbitals. Subsequent paragraphs explain how to write electronic configurations of ions and discuss properties related to ionization energies and oxidation states. The document also discusses crystal field splitting of d-orbitals and how this relates to the formation of colored transition metal complexes. It compares the oxidizing powers of KMnO4 and K2Cr2O7 and discusses the common and stable oxidation states of lanthanides.
8. the d and f block elements anil-hssliveTariq Beigh
Transition elements have partially filled d orbitals. They are divided into four series based on which atomic orbital their valence electrons fill. Transition elements have varying properties based on their position in the periodic table, including decreasing then increasing atomic radius, increasing then decreasing melting points, and variable but regularly changing ionization energies. They form colored ions and complexes due to their partially filled d orbitals, and exhibit magnetic properties based on unpaired electrons. Transition elements also act as catalysts and form interstitial compounds and alloys.
This document discusses the properties of d-block elements. It explains that d-block elements have incompletely filled d orbitals which results in variable oxidation states and properties like catalytic activity, color, and paramagnetism. It also describes trends in properties across the periods and down groups, such as density increasing due to nuclear charge while size decreases, and higher melting points due to metallic and covalent bonding.
The d-block elements have d orbitals that are progressively filled in each period. They form three transition metal series (3d, 4d, 5d) and two inner transition metal series (4f, 5f). Transition metals are defined as having incompletely filled d orbitals. They have high melting and boiling points due to strong metallic bonding. They exhibit a variety of oxidation states and can form stable complexes and interstitial compounds.
Class XII d and f- block elements (part 2)Arunesh Gupta
This part contains ionisation enthalpies, oxidation states, metal oxides & oxocations, magnetic properties, coloured ions of d block elements, catalysts, interstitial compounds, alloy formation & some important conceptual questions with answers as hints. Also some reasoning questions are given to test the understanding of properties of d block elements.
The document discusses electronic spectra and color of transition metal complexes. It explains that the color of complexes is due to electronic transitions between split d-orbital energy levels of the metal ion. Crystal field theory is used to describe the splitting of d-orbitals in an octahedral ligand field, which determines the color. Complexes with strong field ligands have large splitting and absorb at higher energies, appearing more intensely colored.
This document provides information about the characteristics of d-block elements, also known as transition elements. It discusses their electronic configuration, variable valence, magnetic properties, catalytic properties, and ability to form complexes. It describes the first, second, and third transition series and provides examples of common oxidation states for elements in each series. The document also discusses the importance of d-block elements in applications such as metals, magnets, batteries, paints and more. It provides tables of typical oxidation states for different transition element groups.
Transition elements have several key characteristics:
(1) They exhibit variable oxidation states unlike s-block and p-block elements.
(2) Many of their compounds are colored due to electron transitions between d-orbital energy levels.
(3) They have a great tendency to form complex compounds due to their small, highly charged ions and vacant low energy d-orbitals.
The document discusses the chemistry of elements in the second and third transition series. It summarizes that the second transition series spans elements from yttrium to silver, and the third spans elements from lanthanum to gold. It describes trends in properties across the transition series, including increasing metallic radii, atomic weights proportional to densities, increasing melting/boiling points with atomic number, and medium ionization energies. Heavier transition elements form more stable higher oxidation states and prefer low spin configurations with paired electrons.
This document describes the properties of transition elements and their ions. Transition elements have variable oxidation states because their 4s and 3d orbitals are close in energy. They form colored complexes due to d-d transitions absorbing visible light. The color depends on the identity and oxidation state of the metal ion and the ligands present, which influence the splitting of d orbitals. Transition metals also show paramagnetism and some are ferromagnetic due to unpaired d electrons.
Transition elements have an electronic configuration of (n-1)d1-10ns1-2. They form many coordination complexes due to their size, charge density, and vacant orbitals that can accept electrons from ligands. Transition metal ions are often paramagnetic due to their unpaired electrons. They also commonly act as catalysts due to their variable valencies and surface properties. Transition elements form interstitial compounds by trapping smaller atoms in their crystal lattices, and they can form alloys by substituting positions in each other's crystal lattices. Their compounds are often colored due to electron transitions within the d-orbitals that absorb and emit visible light.
Hardy Weinberg law
Hardy Weinberg Equilibrium with Solved Questions|CSIR NET|Life Sciences|GATE|JRF|ICMR|
Video link: https://youtu.be/CUKGoxpptM8
Hardy Weinberg Law along with the assumptions the law is based on. Calculation of allelic and genotypic frequencies. Application of Hardy Weinberg law to different cases viz Multiple alleles, Polyploidy, Inbreeding and X-linked + Questions are discussed.
The Hamilton rule predicts whether natural selection will favor altruistic acts. It is favored when the cost (c) incurred by the altruist is outweighed by the benefit (b) received by recipients, multiplied by their coefficient of relatedness (r). Kin selection favors altruism when the benefit received outweighs the cost incurred, and organisms are more likely to behave altruistically towards close relatives like family due to higher relatedness. For half siblings with r=0.25, the altruistic act would be favored if 0.25b is greater than the cost c incurred.
Flowering in plants(Arabidopsis) ABC ModelFreya Cardozo
Flowering in plants(Arabidopsis) ABC Model
My youtube videos:
https://youtu.be/9SxSpNEQj_g
https://youtu.be/-D6OGm8YbXc
Set of four genes class A, B & C are involved in giving identity of different whorls. 4 pathways are involved - Photoperiodism, autonomous pathway, vernalization & giberlleic acid
Synthesis of oligonucleotides by phosphoramidite methodFreya Cardozo
Oligonucleotides are chemically synthesis by the Phosphoramidite method. It involves four main steps- Detritylation, Coupling, Oxidation and Capping.
Advantages and Disadvantages of the method are also discussed. Happy Learning!
Pullulan- Industrially Important Biopolymer(Exopolysaccharide)Freya Cardozo
Pullulan: Industrially Important Biopolymer- Exopolysaccharide Structure & Industrial Production
Pullulan is an industrially important polymer produced from a fungus Aerobasidium pullulans. The industrial process of production(Upstream and Downstream are discussed) and applications are explained in detail.
This document describes biochemical tests used to identify bacteria, including the Indole test, Methyl Red test, Voges-Proskauer test, and Citrate test.
The Indole test detects the production of indole from tryptophan. A positive result is indicated by a yellow or cherry red color change with Kovac's reagent.
The Methyl Red test identifies stable acid production from glucose in MR-VP broth, indicated by a red color with methyl red indicator.
The Voges-Proskauer test detects acetyl methyl carbinol production from glucose, shown as a pinkish red color change when alpha-naphthol and potassium hydroxide are added.
This document provides an overview of nuclear chemistry and radioactivity. It defines nuclear chemistry as the study of reactions involving changes in atomic nuclei. It describes the basics of atomic structure and the components of the nucleus. It then covers various nuclear reactions like radioactive decay, and types of radiation emitted. Key concepts discussed include radioactive half-life, rate of decay, and factors affecting nuclear stability. Classification of nuclides and various nuclear reactions like alpha, beta, and gamma decays are also summarized.
The document provides information on nuclear chemistry and radioactivity. It defines nuclear chemistry as the study of reactions involving changes in atomic nuclei. It describes the basic structure of the atom and defines key terms like isotopes, nuclides, and nuclear reactions. The document also discusses the classification of nuclides based on stability and magic numbers, as well as the forces that bind nucleons together and concepts like binding energy, mass defect, and radioactive decay.
Solution colligative properties 12th HSC Maharashtra state boardFreya Cardozo
The document discusses solution colligative properties. It defines a solution as a homogeneous mixture of two or more pure substances, with the solvent present in larger quantity than the solute. Solution properties like vapor pressure, boiling point, and freezing point depend on the number of solute particles rather than their identity, and are known as colligative properties. Vapor pressure of a solution is lower than the pure solvent due to the solute particles replacing solvent molecules at the surface and preventing their vaporization. The degree of vapor pressure lowering depends on the mole fraction of solute particles.
This document provides an overview of basic chemistry concepts including:
- Matter can be classified as mixtures or pure substances. Pure substances have a definite composition while mixtures do not.
- Elements are pure substances that cannot be broken down further, and are classified as metals, nonmetals, and metalloids. Compounds are also pure substances but have elements combined in fixed proportions.
- Chemical properties describe reactions that change a substance's composition, while physical properties can be observed without chemical changes.
Coordination compounds (12th Maharashtra state board)Freya Cardozo
As per revised textbook 2019-2020. Ligands, Werners theory, Valence bond theory, Crystal field splitting theory, Application of coordination compounds, IUPAC
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The document discusses the structure of the atom and the discovery of subatomic particles like electrons, protons, and neutrons. It describes experiments done by scientists like J.J. Thompson, Ernest Rutherford, and James Chadwick that led to the discovery of these fundamental particles. Key findings include the discovery of electrons as negatively charged particles in cathode rays, Rutherford's discovery of the nucleus through alpha particle scattering experiments, and Chadwick's discovery of the neutron through experiments with beryllium radiation.
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The document discusses ionic equilibrium and acid-base theories. It provides examples of different types of salts based on the strength of acids and bases involved:
1) Salts of strong acids and bases, like NaCl, are neutral as they do not undergo hydrolysis.
2) Salts of strong acids and weak bases, like CuSO4, are acidic due to hydrolysis of the metal cation.
3) Salts of weak acids and strong bases, like CH3COONa, are basic due to hydrolysis of the anion.
4) Salts of weak acids and weak bases can be acidic, basic or neutral depending on whether the Ka or Kb is greater and the extent of hydro
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Transport of drugs across the membrane, Passive Diffusion, carrier mediated, Facilitated, Endocytosis, Ion transport and pH trapping.
Blood brain barrier and(BBB) stratergies to overcome BBB
Solid state 12th Maharashtra state boardFreya Cardozo
- Solids can be crystalline or amorphous. Crystalline solids have long-range order while amorphous solids have short-range order.
- There are four main types of crystalline solids: ionic, molecular, metallic, and covalent networks. They differ in the type of particles that make them up and the nature of bonding between the particles.
- Crystalline solids can form different crystal structures depending on how the particles are packed together in the lattice. Common structures include simple cubic, body-centered cubic, and face-centered cubic.
Gender and Mental Health - Counselling and Family Therapy Applications and In...PsychoTech Services
A proprietary approach developed by bringing together the best of learning theories from Psychology, design principles from the world of visualization, and pedagogical methods from over a decade of training experience, that enables you to: Learn better, faster!
বাংলাদেশের অর্থনৈতিক সমীক্ষা ২০২৪ [Bangladesh Economic Review 2024 Bangla.pdf] কম্পিউটার , ট্যাব ও স্মার্ট ফোন ভার্সন সহ সম্পূর্ণ বাংলা ই-বুক বা pdf বই " সুচিপত্র ...বুকমার্ক মেনু 🔖 ও হাইপার লিংক মেনু 📝👆 যুক্ত ..
আমাদের সবার জন্য খুব খুব গুরুত্বপূর্ণ একটি বই ..বিসিএস, ব্যাংক, ইউনিভার্সিটি ভর্তি ও যে কোন প্রতিযোগিতা মূলক পরীক্ষার জন্য এর খুব ইম্পরট্যান্ট একটি বিষয় ...তাছাড়া বাংলাদেশের সাম্প্রতিক যে কোন ডাটা বা তথ্য এই বইতে পাবেন ...
তাই একজন নাগরিক হিসাবে এই তথ্য গুলো আপনার জানা প্রয়োজন ...।
বিসিএস ও ব্যাংক এর লিখিত পরীক্ষা ...+এছাড়া মাধ্যমিক ও উচ্চমাধ্যমিকের স্টুডেন্টদের জন্য অনেক কাজে আসবে ...
it describes the bony anatomy including the femoral head , acetabulum, labrum . also discusses the capsule , ligaments . muscle that act on the hip joint and the range of motion are outlined. factors affecting hip joint stability and weight transmission through the joint are summarized.
Philippine Edukasyong Pantahanan at Pangkabuhayan (EPP) CurriculumMJDuyan
(𝐓𝐋𝐄 𝟏𝟎𝟎) (𝐋𝐞𝐬𝐬𝐨𝐧 𝟏)-𝐏𝐫𝐞𝐥𝐢𝐦𝐬
𝐃𝐢𝐬𝐜𝐮𝐬𝐬 𝐭𝐡𝐞 𝐄𝐏𝐏 𝐂𝐮𝐫𝐫𝐢𝐜𝐮𝐥𝐮𝐦 𝐢𝐧 𝐭𝐡𝐞 𝐏𝐡𝐢𝐥𝐢𝐩𝐩𝐢𝐧𝐞𝐬:
- Understand the goals and objectives of the Edukasyong Pantahanan at Pangkabuhayan (EPP) curriculum, recognizing its importance in fostering practical life skills and values among students. Students will also be able to identify the key components and subjects covered, such as agriculture, home economics, industrial arts, and information and communication technology.
𝐄𝐱𝐩𝐥𝐚𝐢𝐧 𝐭𝐡𝐞 𝐍𝐚𝐭𝐮𝐫𝐞 𝐚𝐧𝐝 𝐒𝐜𝐨𝐩𝐞 𝐨𝐟 𝐚𝐧 𝐄𝐧𝐭𝐫𝐞𝐩𝐫𝐞𝐧𝐞𝐮𝐫:
-Define entrepreneurship, distinguishing it from general business activities by emphasizing its focus on innovation, risk-taking, and value creation. Students will describe the characteristics and traits of successful entrepreneurs, including their roles and responsibilities, and discuss the broader economic and social impacts of entrepreneurial activities on both local and global scales.
How to Make a Field Mandatory in Odoo 17Celine George
In Odoo, making a field required can be done through both Python code and XML views. When you set the required attribute to True in Python code, it makes the field required across all views where it's used. Conversely, when you set the required attribute in XML views, it makes the field required only in the context of that particular view.
B. Ed Syllabus for babasaheb ambedkar education university.pdf
d and f block elements/Transition and inner transition elements
1. TRANSITION AND INNER TRANSITION ELEMENTS
PRESENTE
D BY:
FREYA
CARDOZO
BY FREYA CARDOZO
2. TRANSITION ELEMENTS
THE GENERAL ELECTRONIC CONFIGURATION OF TRANSITION ELEMENTS IS
(N-1)D1-10 NS1-2.
THE TRANSITION ELEMENTS ARE PLACED IN THE PERIODS 4 TO 7 AND GROUPS 3 TO 12
THOSE CONSTITUTE 3D,4D,5D AND 6D SERIES
BY FREYA CARDOZO
3. WHAT ARE TRANSITION ELEMENTS
Elements that have a partially filled d orbital in their ground state or one of its oxidation state.
G.R why Zn is not a transition element but Cu is.
Since zinc has completely filled (n - 1)d orbital in the ground state (3d104s2) and (3d10) in its common
oxidation state +2, it is not regarded as transition element.
Copper in the elementary state (3d104s1) contains filled 3d orbitals but in the +2 oxidation state it has partly
filled 3d orbital (3d9), hence copper is a transition element.
BY FREYA CARDOZO
6. GIVE REASON
Why Cu and Cr show anomalous E.C
Mainly due to the fact that half filled and fully filled orbitals have extra stability
The general electronic configuration of the elements of the 3d series is 3d1-10 4s2 with the exceptions of
Cr and Cu.
The 3d and 4s orbitals are close in energy and in order to gain extra stability the last electron instead of
occupying 4s orbital occupies the 3d orbital that assigns Cr the 3d5 4s1 and Cu 3d10 4s1configuration
BY FREYA CARDOZO
7. PHYSICAL PROPERTIES
They are hard, lustrous, malleable and ductile
They are good conductors of heat and electricity
They possess high MP BP
Except Zn, Cd, Hg and Mn, all the other transition elements have one or more typical metallic structures
at ambient temperature.
These transition metals (with the exception of Zn, Cd and Hg) are very hard and have low volatility
BY FREYA CARDOZO
8. IONIC RADIUS
For the same oxidation state, with an increase of nuclear
charge a gradual decrease in ionic radii was observed.
The trend is pronounced for the divalent ions of the first
transition series (Cr2⊕ - 82 pm, Cu2⊕ - 72 pm).
The oxidation states of the same element shows
difference of one unit such as M⊕, M2⊕, M3⊕,M4⊕ and so
on.
With higher oxidation state the effective nuclear charge also
increases and hence, decrease of ionic radii can be observed
from M2⊕ to M3⊕
BY FREYA CARDOZO
9. ATOMIC RADII DECREASES GRADUALLY
ACROSS THE PERIOD
As we move across a transition series from left to right the nuclear charge increases by one unit at a
time.
The last filled electron enters a penultimate (n-1)d subshell.
However, d orbitals in an atom are less penetrating or more diffused and, therefore d electrons offer
smaller screening effect.
The result is that effective nuclear charge also increases as the atomic number increases along a
transition series.
Hence the atomic radii decrease gradually across a transition series from left to right.
BY FREYA CARDOZO
Size decreases across a period
10. IONIZATION ENTHALPY
The I.E for d block elements lies between the s and p blocks
Across the group as the size decrease
Ionization enthalpy increases
IE3>IE2> IE1
Depending on condition the type of bond is decided
Lower O.S – Ionic bond
High o.s – Covalent bond
BY FREYA CARDOZO
Ionization energy or Ionisation
energy, denoted Eᵢ, is the minimum
amount of energy required to
remove the most loosely bound
electron, the valence electron, of an
isolated neutral gaseous atom or
molecule
Size decreases across a
period
I.E ↑
Acros
s the
period
11. IONISATION ENTHALPY
G.R ionization enthalpy for 3rd transition series is
more than 1st and 2nd series
The atoms of elements of third transition series
possess filled 4f- orbitals. 4f orbitals show poor
shielding effect on account of their peculiar diffused
shape.
As a result, the valence electrons experience greater
nuclear attraction.
A greater amount of energy is required to ionize
elements of the third transition series
BY FREYA CARDOZO
12. METALLIC CHARACTER
Metallic character is due to the :
1. VACANT d orbitals
2. Low ionisation enthalpy
Hardness of metals is due to the covalent bond which is possible because of the unpaired (n-1)d
electrons in these elements
Mostly they show HCP, ccp, bcc lattice structure
Hardness, high melting points and metallic properties of the transition elements indicate that the metal
atoms are held strongly by metallic bonds with covalent character.
BY FREYA CARDOZO
13. MAGNETIC PROPERTIES
They show magnetic properties due to the unpaired electrons
3 types
1. Dimagnetic – Replled by magnetic field
2. Paramagnetic- attracted to mag field
3. Ferromagnetic- strongly attracted. EG. Fe, Co, Ni
Magnetic moment is sum of spin angular momentum and orbital angular momentum
µ= n(n + 2) BM
n = no.of unpaired ELECTRONS
BY FREYA CARDOZO
Paired e- : Diamagnetic
Unpaired e-:
Paramagnetic
14. QUESTIONS
Which one of the following is dimagnetic
a. Cr2⊕ b. Fe3⊕
c. Cu2⊕ d. Sc3⊕
Magnetic moment of a metal
complex is 5.9 B.M. Number of
unpaired electrons in the complex is
a. 2 b. 3
c. 4 d. 5
BY FREYA CARDOZO
15. QUESTIONS
What is the magnetic moment for Cr3+
a. equal to 1.73 BM,
b. less than 1.73 BM or
c. more than 1.73 BM ?
Why salts of Sc3⊕, Ti4⊕, V5⊕ are colourless ?
Calculate the spin only magnetic moment of divalent cation of a transition metal with atomic number 25.
BY FREYA CARDOZO
18. A substance appears coloured if
it absorbs a portion of visible light. The colour
depends upon the wavelength of absorption in
the visible region of electromagnetic radiation
BY FREYA CARDOZO
19. REASONS FOR COLOR IN TRANSITION METALS
1. presence of unpaired d electrons
2. d - d transitions
3. nature of ligands attached to the metal ion
4. geometry of the complex formed by the
metal ion
BY FREYA CARDOZO
20. UNPAIRED ELECTRONS AND D-D TRANSITION
REASON FOR COLOUR- d-d transition
BY FREYA CARDOZO
21. GEOMETRY OF COMPLEX ION
When cobalt chloride (Co2⊕) is dissolved in water, it forms a pink solution of the complex
[Co(H2O)6]2⊕ which has octahedral geometry.
But when this solution is treated with concentrated hydrochloric acid, it turns deep blue.
This change is due to the formation of another complex [CoCl4]2 which has a tetrahedral structure.
BY FREYA CARDOZO
22. CHARGE TRANSFER
MnO4- ion has an intense purple colour in solution.
In MnO4- , an electron is momentarily transferred from oxygen (O) to metal, thus momentarily changing
O2 to Oand reducing the oxidation state of manganese from +7 to +6.
For charge transfer transition to take place, the energy levels of the two different atoms involved should
be fairly close.
Colours of Cr2O7
2- , CrO4 , Cu2O and Ni-DMG (where DMG = dimethyl glyoxime) complex are other
examples
BY FREYA CARDOZO
23. CATALYTIC PROPERTIES
because of their ability to participate in different oxidation-reduction steps of catalytic reactions.
This possible due to
1. unpaired e-s in incomplete d orbitals
2. variable o.s
3. Large surface area
In homogeneous catalysis reactions, the metal ions participate by forming unstable intermediates.
In heterogeneous catalysis reactions on the other hand, the metal provides a surface for the reactants to
react.
BY FREYA CARDOZO
24. EXAMPLES OF IMPORTANT CATALYST
Mo/Fe – Habers process
Co-Th Fischer Tropsch process --- gasoline synthesis
Ni – cataylic hydrogenation
Platinised asbestos- solid catalyst --- contact process for manu of sulfuric acid from SO2 and O2
Fe-Cr – production of CO2 frm CO
BY FREYA CARDOZO
25. INTERSTITIAL COMPOUNDS
When small atoms like hydrogen, carbon or nitrogen are trapped in the interstitial spaces within the
crystal lattice, the compounds formed are called interstitial compounds
Steel and cast iron are examples of interstitial compounds of carbon and iron
Properties
1. Good conduction
2. MP BP higher than parent
3. Density less than parent
carbides of metals are inert and hard
hydrides of transition metals are Powerful reducing agents
BY FREYA CARDOZO
26. ALLOYS
Alloys are mixtures of metals
classification
1. Ferrouss alloys have atoms of other elements distributed randomly in atoms of
iron in the mixture.
As percentage of iron is more, they are termed ferrous alloys eg. nickel steel,
chromium steel, stainless steel etc. All steels have 2% carbon
2. Non-ferrous alloys are formed by mixing atoms of transition metal other than iron
with a non transition element.
eg. brass, which is an alloy of copper and zinc. Ferrous and non-ferrous alloys are
of industrial importance.
BY FREYA CARDOZO
27. USES
Bronze=Cu+Tin Tough, strong and corrosion resistant
Cupra nickel – machine parts of ships
stainless steel – air crafts
Nichrome=Ni+Cr – turbine engines
Titanium alloys --- can withstand high temp
Components of Nichrome alloy are
are
a. Ni, Cr, Fe b. Ni, Cr, Fe, C
c. Ni, Cr d. Cu, Fe
BY FREYA CARDOZO
28. PREPERATION OF POTASSIUM DICHROMATE
K2CR2O7
1. Chromite ore =FeO.Cr2O3 to Sodium chromate Na2CrO4 --- anhydrous
sodium carbonate And flux of like in air
2. Sodium chromate to Sodium dichromate Na2Cr2O7 ---- Sulphuric acid
and water
3. Sodium dichromate to potassium dichromate K2Cr2O7 --- Potassium
chloride
BY FREYA CARDOZO
FeO.Cr2O3
Na2CrO4
Na2Cr2O7
K2Cr2O7
OUTLINE
32. CHEMICAL PROPERTIES OF POTASSIUM
DICHROMATE
Reactant Colour
(Before)
K2SO4 Cr2(SO4)3 H2O Special
byproduct
Color
K2Cr2O7+H2SO
4
KI
Potassium
iodide
Orange ✓ ✓ ✓ I2 Brown
K2Cr2O7+H2SO
4
H2S
Hydrogen
sulphide
Orange ✓ ✓ ✓ S Green
solution
+
Yellow
ppt
BY FREYA CARDOZO
33. REACTION WITH KI
The oxidation of KI with acidified potassium dichromate produces I2
This changes the solution to brown
Potassium dichromate is reduced to chromic sulphate
BY FREYA CARDOZO
34. REACTION WITH H2S
The reaction leads to the pptn of S which appears as pale yellow ppt
Potassium dichromate is reduced to chromic sulphate
Due to the production of chromic sulphate the orange solution turns green
BY FREYA CARDOZO
35. KMNO4 – POTASSIUM PERMANGANATE
Preparation method
1. Chemical oxidation
2. Electrolytic oxidation
BY FREYA CARDOZO
36. CHEMICAL METHOD
MnO2 manganese dioxide K2MnO4 Potassium mangante(green) –
1. Caustic potash KOH
2. Potassium chlorate KClO3 – oxidising agent
Dispropotionation in neutral or acidic medium KMnO4 + MnO2
Filteration to glass wool
BY FREYA CARDOZO
37. ELECTROLYTIC OXIDATION
Alkaline solution of manganate ion is electrolysed between iron electrodes seperated by a diaphram
At anode the oxygen evolved is used to reduce manganate to permanganate
Overall reaction
The solution is evaporated and filtered to obtain the crystals
BY FREYA CARDOZO
38. CHEMICAL PROPERTIES OF KMNO4
In acidic medium- Oxidising action
1. Iodide to Iodine
2. Fe2+ to Fe3+
3. H2S to S
4. Oxidation of oxalic acid H2C2O4
In neutral medium or weakly alkaline medium
1. Iodide to Iodate
2. Oxidation of thiosulphate to sulphate
3. Manganous salt to manganese dioxide
BY FREYA CARDOZO
42. USES
Antiseptic
Test for unsaturation
Quantitative analysis- Halide detection
Volumetric analysis- For reducing agents
Oxidising agent- labs and industry
Why is KMnO4 such a good oxidising agent?
BY FREYA CARDOZO
44. INNER TRANSITION ELEMENTS
Orbital lies much inside the d orbital,in relation to the transition metals the f
block elements are called inner transition elements.
f – 1 to 14 electrons, d – 0 or 1 and s – 2 electrons
2 series : Lanthanoids and Actinoids
Lanthanoids – characterizied by filling of 4f
Actinoids - characterizied by filling of 5f
14 elements in each
BY FREYA CARDOZO
45. F BLOCK ELEMENTS
Those elements in which the outermost electrons enter the f subshell
They belong to the 6th and 7th period
Placed seperately at the bottom of the table
BY FREYA CARDOZO
46. PROPERTIES OF F BLOCK ELEMENTS
These metals are soft with moderate densities of about 7 g cm-3.
They have high melting point
They are quite reactive similar to the alkali metals than d block metals
common oxidation state for lanthanoids is +3
+2 is also very common among these, higher O.S like +4 is unusual (exptn- Ce)
BY FREYA CARDOZO
47. LANTHANOIDS- RARE EARTH ELEMENTS
They were know as rare because it was difficult to extract them economically from their ores
BY FREYA CARDOZO
48. G.R: LANTHANOIDS HAVE LOWER HEAT OF
ATOMIZATION THAN TRANSITION METALS.
The energy required to break up the metal lattice is heat of atomization.
This is because with d electrons, transition metals
are much harder and require high heat of
atomization.
Europium and ytterbium have the
lowest enthalpies of vaporization and largest
atomic radii of lanthanoids, resemble barium.
BY FREYA CARDOZO
49. RADII
Their ionic radii decrease from 117 pm of La to 100 pm for Lu.
This is because 5f orbitals do not shield the outer 5s and 5p electrons
effectively, leading to increase in effective
nuclear charge and decrease in the ionic size.
BY FREYA CARDOZO
50. REACTIONS WITH LN
Reactants Reactants Product
Ln C LnC
Ln H2O Ln(OH)3
Ln O2 Ln2O3
Ln N2 LnN
Ln X LnX3
Ln= Lanthanoids
BY FREYA CARDOZO
51. BASICITY OF LANTHANOIDS
All the lanthanoids form hydroxides ofthe general
formula Ln(OH)3
These are ionic and basic.
Since the ionic size decreasesfrom La3+ to Lu3+,
the basicity of hydroxides decreases.
La(OH)3 is the strongest base while Lu(OH)3 is the
weakest base.
BY FREYA CARDOZO
52. ELECTRONIC CONFIGURATION
Generally the E.C for lanthanoids is represented as [Xe] 4f0-14 5d0-1 6s2
Xe = Xenon, Z= 54
The E.C for Xe is 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s2 4d10
BY FREYA CARDOZO
53. EXCEPTIONS
The electrons first fill up the 6s
4f and 5d are very close in energy
In case of lanthanum the 5d oribtal has lower energy
In case of Gd and Yb the anamolous behaviour is
observed
As half filled and fully filled electrons have extra stability
Thus general E.C for lanthanoids is [Xe] 4f0-14 5d0-1 6s2
BY FREYA CARDOZO
54. IONISATION ENTHALPY
What is ionisation enthalpy?
As size increases, ionisation enthalpy decreases since the
last electron experiences lesser pull from the nucleus
Across the period, size decreases thus I.E increases
Why some elements have variable O.S states but others only
a few? Can ionisation enthalpy justify these?
BY FREYA CARDOZO
55. QUESTION
HINT:
-Energy required to remove unpaired electrons is lesser than that
to remove paired electrons
- Check the energy of subshell, lower the energy easy to remove
the last electron
- n+l lower: lesser energy the subshell has
BY FREYA CARDOZO
56. OXIDATION STATE
G.E.C = [Xe] 4f0-14 5d0-1 6s2
thus the common O.S is +3 i.e 2 e- from 6s and the order from d/f
subshell
The 4f electrons are shielded by the inner 5s and 5p orbitals, they are
tightly bond to the nucleus. Thus they do not take part in the bonding
Some show O.S +2 and +4 this is due to f0, f7, f14 E.C
BY FREYA CARDOZO
57. COLOUR
These elements are coloured due to the f-f
transition which corresponds to the energy in
the visible spectrum
The colour of ions with nf electrons= (14-n)f
electrons
COLOUR IN LANTHANOIDS
BY FREYA CARDOZO
58. WHAT IS SHIELDING EFFECT
The decrease in the net force of attraction between
the electrons present in the outer shell of an atom in
the direction of nucleus due to change in linearity of
the electric lines of forces between them due to the
presence of high election density in the inner shells
in the same atom is known as screening effect.
BY FREYA CARDOZO
59. ATOMIC RADII
Across the period the radii decreases as the size
decreases
The decrease in lanthanoids is very steady this is
called the LANTHANOID CONTRACTION
As we move left to right the nuclear charge
increases by +1 and an electron is added
The electron is added to the same 4f subshell
Due to their diffused shape the 4f electrons shield
each other poorly from the nuclear charge
With increasing atomic no. the effective nuclear
charge increases thus pulling the 4f shell closer,
causing it to cntract
BY FREYA CARDOZO
60. MAGNETIC MOMENT
µ=square root of n(n + 2) BM
n = no.of unpaired ELECTRONS
Calculate magnetic moment for La3+
La -57
[Xe]4f05d16s2 n=1
Magnetic moment
BY FREYA CARDOZO
61. APPLICATIONS In hybrid cars, superconductors and permanent magnets
Used in the colour tubes of computers and T.Vs since they
produce visible light over a small wavelength upon bombarding
with e-s
(Eu,Y)2O3 – red colour
There types of Ln are used to get 3 primary colours
Luminescent materials Nd: YAG laser
Applications of Lanthanoids
BY FREYA CARDOZO
63. ACTINOIDS
Starts with Thorium Z=90 and ends with Lawrencium Z=103
They are all radioactive and man-made
High M.P, B.P, density
The electronic configuration of actinoids is
[Rn] 5f0-14 6d0-2 7s2, where Rn is the electronic
configuration of radon.
most stable oxidation state in actinoids
is +3. The highest however actinoids show a variety of O.S from +2 to +8
BY FREYA CARDOZO
65. OXIDATION STATE
Early lanthanoids show variable O.S this is similar to transition
elements than lanthanoids
This pattern is seen mostly due to the ability of 5f orbital to
participate in bonding
A ready loss of 5f electrons by early actinoids indicates that these
electrons are much closer in energy to 7s and 6d electrons than
the 4f electrons to 6s and 5d electrons as in lanthanoids
G.E.C [Rn] 5f0-14 6d0-2 7s2
Eg. uranium has electronic configuration of [Rn]7s2 5f 36d1. The
formation of +6 oxidation state corresponds to an electronic
configuration of [Rn].
BY FREYA CARDOZO
66. Half filled and fully filled
orbitals have extra stability.
Thus one electron from f is
promoted to d
BY FREYA CARDOZO
67. The overall gradations
among the different blocks
of the periodic table
Transition elements- d
block
Lanthanoids-f block
Pre- transition – s block
BY FREYA CARDOZO
68. ACTINOID CONTRACTION
5f 6d 7s are almost same energy in actinoids
The 7s electrons shield the 5f and 6d orbitals from nuclear
charge , thus they expand a little. Therefore, they have size
greater than lanthanoids
But the decreases in radii is not as prominent, due to the
shielding effect of f orbitals
BY FREYA CARDOZO
69. APPLICATION OF ACTNOIDS
Half lives of Thorium & Uranium are so long that
the amount of radiation emitted is negiligble, thus
they can be used in everyday life.
Th(IV) oxide, ThO2 with 1% CeO2 was used as a
major source of indoor lighting before
incandescent lamps came into existence only
because these oxides convert heat energy from
burning natural gas to an intense light.
Even today, there is a great
BY FREYA CARDOZO
70. POSTACTINOID ELEMENTSPOST ACTINOID ELEMENTS
Elements with atomic number greater than 92 are called ‘Transuranium’.
Elements from atomic number 93 to 103 now are included in actinoid series and
those from 104 to 118 are called as postactinoid elements.
They are included as postactinoids because similar to actinoid elements, they can
be synthesized in the nuclear reactions.
So far, nine postactinoid elements have been synthesized.
Half life is in secs 2.8 x 10^-4, thus difficult to study reactions
Rutherfordium forms a chloride, RfCl4, similar to zirconium and hafnium in the +4
oxidation state.
Dubnium resembles to both, group 5 transition metal, niobium(V) and actinoid,
protactinium(V).
BY FREYA CARDOZO
71. Questions
ix. In which of the following series
all the elements are radioactive in
nature
a. Lanthanides b. Actinides
c. d-block elements d. s-block elements
x. Which of the following sets of ions
contain only paramagnetic ions
a. Sm3⊕, Ho3⊕, Lu3⊕ b. La3⊕, Ce3⊕, Sm3⊕
c. La3⊕, Eu3⊕, Gd3⊕ d. Ce3⊕, Eu3⊕, Yb3⊕
xi. Which actinoid, other than uranium,
occur in significant amount
naturally?
a. Thorium b. Actinium
c. Protactinium d. Plutonium
BY FREYA CARDOZO
73. DEFINITION
Mineral : naturally occuring substance found in the earth’s crust containing inorganic salts, solids,
siliceous matter etc, is called a mineral.
Ore: The mineral which contains high percentage of the metal and from which the metal can be
extracted economically is called an ore
DEFINITONS
BY FREYA CARDOZO
75. TYPES OF METALLURGY
Pyrometallurgy: A process in which the ore is reduced to
metal at high temperature using reducing agents like carbon,
hydrogen, aluminium, etc. is called pyrometallurgy.
Hydrometallurgy : The process of extracting metals from the
aqueous solution of their salts using suitable reducing agent
is called hydrometallurgy.
Electrometallurgy : A process in which metal is extracted by
electrolytic reduction of molten (fused) metallic compound is
called electrometallurgy
TYPES OF METALLURGY
BY FREYA CARDOZO
76. GENERAL METHODOLOGY
Extraction of ore
Concentration of ore – removing impurities of other metals, sand, dust
particles
impurities termed as gangue are removed from the ore and the ore gets
concentrated.
The sand, mud and other unwanted impurities which remain mixed with the
ore deposit are called gangue.
Methods –
1. Hydraulic classifiers
2. Froth floation
3. Magnetic seperation
Convert to its oxides – Can be done by either
1. Roasting .
2. Calcination
Obtaining pure metal
BY FREYA CARDOZO
78. EXTRACTION OF IRON Ore – Haematite ore (Fe2O3)
Gangue -SiO2 + Al2O3+ phosphates
Concentration – Hydraulic classifier
The powdered ore is washed in a powerful current of water introduced
into the hydraulic classifier.
The lighter gangue particles are separated and the concentrated ore is
collected at the bottom.
Converting into the oxide
Roasting : The concentrated ore is heated In a current of air. The sulfur
and arsenic impurties present in the ore get converted into their oxides
and escape as vapour. Ferrous oxide in the ore is converted to Fe2O3
4FeO + O2 -- 2 Fe2O3
STEPS IN EXTRACTION OF Fe ore
BY FREYA CARDOZO
81. BLAST FURNANCE- Smelting
Tall cylindrical steel tower lined with
refractory bricks.
The height=25 m and diameter =5 to10
m.
Working- counter current principle :
Charge comes down and hot gases move
up the tower.
The furnace is comprised of 3 parts –
1. Hearth, 2. Bosh and 3. Stack
Ore is introduced in the furnace through
a cup and cone arrangement
Ensures uniform distribution and
prevents loss of gases
A blast of preheated air is introduced into
the furnance below the bosh through
BY FREYA CARDOZO
83. 1.ZONE OF COMBUSTION
The formation of CO is exothermic and thus temperature is 2000K
Some CO decomposes to C
The hot CO gas moves upward and thus heats up the incoming charge
Therefore CO acts as a fuel and reducing agent
BY FREYA CARDOZO
85. ZONE OF SLAG FORMATION
The gangue present in the ore is converted to slag. This slag can be used for making road foundation.
Temperature of this zone is 1200 K. The gangue contains silica, alumina and phosphates. A removal of this
gangue is effected by adding lime-stone in the charge, which acts as flux. Limestone decomposes to give
CaO (quick lime)
3.Zone of slag formation
BY FREYA CARDOZO
86. • ZONE OF FUSION
MnO2 and Ca3(PO4)2 present in the iron ore are reduced to Mn and P. Some of the silica is also reduced to
Si.
The spongy iron coming down in the furnace melt absorbs impurities like C, Si, Mn, P and S. This molten
iron collects at the bottom in the furnace.
The slag which is lighter floats on the surface of molten iron. Molten slag and iron are collected through
separate outlets.
Molten iron is poured into moulds.
These solid blocks are called pigs. This iron contains about 4% of carbon.
When pig iron is remelted, run into moulds and cooled, it becomes cast iron. The waste gases containing
N2, CO and CO2 escape through the outlet at the top. These hot gases are used for preheating
the blast of air
BY FREYA CARDOZO
88. FACTORS AFFECTING EXTRACTION TECHNIQUE
Pure iron can be obtained by electrolytic refining of impure iron or other methods given in the flow chart.
The choice of extraction technique is governed by the following factors.
1. Nature of ore
2. Availability and cost of reducing agent, generally cheap coke is used
3. Availability of hydraulic power.
4. Purity of product (metal) required.
5. Value of byproducts for example, SO2 obtained during roasting of sulphide ores is vital for manufacture
of H2SO4. Knowledge of electrochemical series provides solutions to many problems.
BY FREYA CARDOZO