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Transition Elements
This document discusses transition series elements and their properties. It describes how transition elements have electrons that enter the (n-1)d orbitals, giving them variable oxidation states up to +8. Their atomic radii decrease across periods but increase down groups. Transition metals can conduct heat and electricity well and can be alloyed to improve strength. Some have magnetic properties depending on unpaired electrons. Their colored complexes are due to electron transitions between d orbitals. Common applications include stainless steel, bronze, and uses of copper and nickel in coins, batteries, and turbines.
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Introduces Shri. Dr. R.G. Rathod Arts and Science College and the focus on studying transition series elements.
Discusses the historical context of alchemy and defines transition (d-block) elements placed between s and p-block.
Explains atomic radius, ionization energy, oxidation states, and highlights trends in these properties across transition metals.
Highlights physical properties, alloys, and magnetic properties of transition metals, and discusses color absorption in complex ions.
Discusses applications of nickel, bronze, copper, and stainless steel, emphasizing their usage in various industries.
Highlights the vital role of iron in biology, specifically its function in hemoglobin and energy transport in cells.
Includes a closing slide soliciting attention, summing up the information presented.
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Transition Elements
- 1. Shri. Dr. R.G.Rathod Arts and Science college, Murtizapur Presented by, Dr. Gopalkrushna H. Murhekar Shri Dr. R. G. Rathod Arts and Science, College Murtizapur
- 2. Study of Transition SeriesElements
- 3. ALCHEMISTS Alchemist tried tomake lead into gold. They studies many materials and used mysterious symbols to represent these materials.
- 4. TRANSITION ELEMENTS Theelements in which differentiating electron enter in (n-1)d orbitals of (n-1)th main shell are called transition elements. These elements are also known as bridge elements as they are lying between s and p bolck elements in a periodic table. Because the differenting electron in these elements enter in d orbital so these elements are called as d-block elements.
- 5. Atomic Radius Thedistance from centre of nucleus to the valence shell of electron in an atom is known as atomic radius. Atomic radius is measured in cm. Atomic radii actually decrease across a row in the periodic table. Due to an increase in the effective nuclear charge. Within each group (vertical column), the atomic radius tends to increase with the atomic number number.
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- 7. OXIDATION STATES Variable Up to+8 in Os & Ru Re has widest range: -3 +7 !
- 8. EXPLANATION The transitionmetals can form a variety of ions by losing one or more electrons. For the first five metals the maximum possible oxidation state corresponds to the loss of all the 4s and 3d electrons. Toward the right end of the period, maximum oxidation state are not observed, in fact 2+ ions are the most common because the 3d orbital become lower in energy as the nuclear charge increases, and the electrons become increasingly difficult to remove.
- 9. IONIZATION ENERGY Ionizationenergy, Ei: minimum energy required to remove an electron from the ground state of atom (molecule) in the gas phase. M(g) + h M+ + e. Increase across row But increase smaller than for main-group elements Also, 3rd transition row has higher ionization E (generally) than first 2 rows Runs counter to main- group elements Due to outer e-’s being held more tightly
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- 11. PHYSICAL PROPERTIES OFMETALS 1. Efficient conduction of heat and electricity 2. Malleability (they can be hammered into thin sheets) 3. Ductility (they can be pulled into wires) 4. A lustrous (shiny) appearance 5. All transition elements are metal at room temperature except mercury which is liquid at room tempeture. Platinum Sliver Gold Copper
- 12. ALLOYS Alloys area mixture of metals to improve strength. Examples of alloys include: Gold jewelry (Au and Ag) Bronze – Cu and Sn Brass – Cu and Zn Sterling silver – Cu and Ag
- 13. MAGNETIC PROPERTIES • Althoughan electron behaves like a tiny magnet, two electrons that are opposite in spin cancel each other. Only atoms with unpaired electrons exhibit magnetic susceptibility • A paramagnetic substance is one that is weakly attracted by a magnetic field, usually the result of unpaired electrons. • A diamagnetic substance is not attracted by a magnetic field generally because it has only paired electrons.
- 14. COLOR OF COMPLEXIONS The color wheel: absorption of color appears as complementary color Color in causes lower d- orbital e- to go up to higher d-orbital state Specific wavelength of light kicked out The complement of color absorbed Colorless complexes are either d0 or d10 Don’t have d-orbital e- ’s to move up
- 15. e- inpartially filled d sublevel absorbs visible light moves to slightly higher energy d orbital
- 17. Applications of Nickel Turbineengine Electroplating Batteries
- 18. TRANSITION METALS Elementsin groups 3-12 Less reactive harder metals Includes metals used in jewelry and construction. Metals used “as metal.”
- 19. BRONZE Copper alloys containingtin, lead, aluminum, silicon and nickel are classified as bronzes. Cu-Sn Bronze is one of the earliest alloy to be discovered as Cu ores invariably contain Sn. Stronger than brasses with good corrosion and tensile properties; can be cast, hot worked and cold worked. Wide range of applications: ancient Chinese cast artifacts, skateboard ball bearings, surgical and dental instruments.
- 20. COPPER The secondlargest use of Cu is probably in coins. The U.S. nickel is actually 75% copper. The dime, quarter, and half dollar coins contain 91.67% copper and the Susan B Anthony dollar is 87.5% copper. The various Euro coins are made of Cu-Ni, Cu-Zn-Ni or Cu-Al-Zn- Sn alloys.
- 21. APPLICATIONS OF STAINLESS STEELS •Stainless steels - A group of steels that contain at least 11% Cr. Exhibits extraordinary corrosion resistance due to formation of a very thin layer of Cr2O3 on the surface. Categories of stainless steels: Ferrite Stainless Steels – Composed of ferrite (BCC) Martens tic Stainless Steels – Can be heat treated. Austenitic Stainless Steels – Austenite ( ) phase field is extended to room temperature. Most corrosion resistant. Duplex Stainless Steels – Ferrite + Austenite
- 22. Biological Importance ofIron Plays a central role in almost all living cells. Component of hemoglobin and myoglobin. Involved in the electron-transport chain.
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