Group iv elements
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The document discusses the Group IV elements carbon, silicon, germanium, tin, and lead. Group IV elements have a full s orbital and two electrons in the p orbital. The elements range from the nonmetal carbon to the weakly metallic lead. Carbon and silicon form acidic oxides, while tin and lead form amphoteric oxides. Carbon occurs naturally as diamond and graphite. Silicon is abundant as silica but not as the free element. Germanium is a rare element found in coal products. Tin is obtained commercially from its oxide cassiterite. Lead is extracted from its sulfide ore by roasting and heating with limestone and coal in a blast furnace.
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1) Potassium nitrate oxidizes carbon and sulfur fuels to produce carbon dioxide, sulfur dioxide, and oxygen gases, providing an upward thrust.
2) The gases heat metallic salts, exciting their electrons and producing light of different wavelengths and colors depending on the metal.
3) Various metals like lithium, calcium, sodium, copper, and magnesium produce the colors red, orange, yellow, blue, and silver seen in fireworks through electron excitation and emission.
Metals 2
Iron is extracted from its main ore, haematite, in a blast furnace. Haematite, coke, and limestone are fed into the top of the blast furnace where temperatures reach 1500°C. The main reducing agent, carbon monoxide, reduces the iron(III) oxide to iron. The molten iron collects at the bottom and is tapped off, while the limestone removes sandy impurities to form a slag.
Chapter 12 Redox Reaction
1. Redox reactions involve the transfer of electrons between oxidizing and reducing agents, resulting in a change in oxidation state.
2. Rusting of iron is a redox reaction where iron is oxidized by oxygen, releasing electrons. Water and oxygen gain electrons to form hydroxide ions.
3. When iron is in contact with more electropositive metals like magnesium or zinc, rusting is inhibited as the more reactive metal undergoes oxidation instead of the iron. Contact with less electropositive metals like copper or tin accelerates rusting as iron is more easily oxidized.
Nickel and its extraction
1). The document summarizes information about nickel, including its extraction from ores, properties, advantages, disadvantages, and classifications of nickel alloys. Nickel is extracted via pyrometallurgical or hydrometallurgical processes depending on the ore. 2). Important nickel alloys include nickel-copper alloys, nickel-chromium alloys, and nickel-base superalloys used in applications requiring high heat resistance. 3). Nickel has properties like corrosion resistance and is used to make alloys for applications across many industries.
Redox reaction Group C
This document discusses oxidation and reduction reactions. It defines oxidation as a reaction where oxygen combines with an element/compound or where an element loses hydrogen or electrons. Reduction is defined as a reaction where an element gains oxygen, hydrogen, or electrons. Common reducing agents are listed such as lithium aluminium hydride and sodium borohydride. The concept of oxidation state is introduced, which is the charge an atom would have if it existed as an ion in a compound. Rules for determining oxidation states are provided. An example of finding the oxidation states of elements in ammonium sulfate is worked out.
Blast furnace presentation
The blast furnace is a counter-current heat exchanger used to smelt iron from iron ore for steel production. Reactions inside reduce iron oxides to molten iron and separate impurities into a slag. The furnace operates at over 1500°C, using coke as the reducing agent and limestone as a flux. Key reactions include the reduction of iron oxides to iron and carbon monoxide, and the removal of impurities like sulfur. The process produces molten iron, known as pig iron, and a slag byproduct. The composition of the pig iron depends on the burden chemistry and furnace operating temperature.
Trends in group 2 part 3 chemical properties
Group 2 metals produce characteristic flame colors when burned due to the metal ions present. Flame tests can be used to identify these metal ions based on the colors they produce: magnesium is white, calcium is orange/red, strontium is red/crimson, and barium is green/yellow-green. Group 2 metals react with oxygen, chlorine, and water through redox reactions where the metal is oxidized and the other substance is reduced. Reactivity increases down the group as it is easier to remove electrons and form ions with a 2+ charge. Carbonates and nitrates of group 2 metals also become more stable to thermal decomposition as you go down the group due to the decreasing charge density of the metal ions
Inner transition series element
The document discusses inner transition elements (f-block elements) and actinides. It provides definitions and general properties of actinides. Actinides have the electronic configuration of 2,8,18,32,5s2,p6d10f0-14,6s2p6d0-2,7s2. Their common oxidation states are +2, +3, +4, +5, +6 and, in some cases, +7. The document also discusses metallurgy and describes the steps involved - crushing/pulverization, concentration, calcination, roasting, smelting and refining. Finally, it explains the differences between pyrometallurgy and
Chemistary ppt by group b
This document provides information on the chemical properties of metals. It discusses how metals react with oxygen, water, acids, and metal salt solutions. It explains that the reactivity of metals varies, with metals like sodium and potassium being the most reactive due to losing their outer shell electrons easily. The document also discusses the formation of ionic compounds through the transfer of electrons from metals to non-metals, and provides examples of how ionic compounds like NaCl and MgCl2 are formed.
Metals and Non-metals
This document provides an overview of metals and non-metals. It discusses their physical and chemical properties, including how metals react with oxygen, water, acids, and other substances. Metals are solid, malleable, ductile, and good conductors of heat and electricity. They form basic oxides and react vigorously with acids. Non-metals do not have these properties and are usually gases or solids. The document also covers extraction methods for metals and corrosion prevention.
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Group iv elements
- 1. GROUP IV ELEMENTS Krisnawati Hidayah (06121010010) Ina Ayu Nengtyas (06121010013) Pujiati (06121010018
- 2. Group IV elements: C :Carbon Si :Silicon Ge :Germanium Sn :Tin Pb :Lead
- 3. SUMMARY OF GENERAL CHARACTERISTICS In this group the outer quantum level has a full s level and two electrons in the corresponding p level. As the size of the atom increases the ionization energy changes and these changes are reflected in the gradual change from a typical nonmetallic element, carbon, to the weakly metallic element, lead. Hence the oxides of carbon and silicon are acidic whilst those of tin and lead are amphoteric.
- 5. CARBON Pure carbon occurs naturally in two modifications, diamond and graphite. In both these forms the carbon atoms are linked by covalent bonds to give giant molecules
- 6. Appearances of the Group IV elements at room temperature and pressure: carbon (graphite)
- 9. SILICON After oxygen, silicon is the most abundant element in the earth's crust. It occurs extensively as the oxide, silica, in various forms, for example, flint, quartz, sand, and as silicates in rocks and clays, but not as the free element, silicon. Silicon is prepared by reduction of silica, SiO2
- 10. Appearances of the Group IV elements at room temperature and pressure: silicon
- 13. GERMANIUM GERMANIUM Germanium is a greyish-white, brittle solid, obtained by reducing the dioxide, GeO2, with hydrogen or carbon at red heat. Germanium is a rare element found in trace quantities in coke obtained from bituminous coal.
- 14. Appearances of the Group IV elements at room temperature and pressure: germanium
- 16. TIN The common ore of tin is tinstone or cassiterite, SnO2, found in Cornwall and in Germany and other countries. Tin is obtained from the tin dioxide, SnO2, by reducing it with coal in a reverbatory furnace: SnO2 + 2C -> 2COf
- 17. Appearances of the Group IV elements at room temperature and pressure: tin
- 20. Lead In the extraction of lead, the sulphide ore is first roasted together with quartz in a current of air: 2PbS + 3O2 -> 2PbO + 2SO2 Any lead(II) sulphate formed in this process is converted to lead(II) silicate by reaction with the quartz. The oxide produced is then mixed with limestone and coke and heated in a blast furnace. The following reactions occur: PbO + C -> Pb + CO PbO + CO -> Pb + CO2 PbSiO3 + CaO + CO -> Pb + CaSiO3 + CO2
- 21. Appearances of the Group IV elements at room temperature and pressure: lead
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