All About Metals - CHEM 010 Past Paper 2024 PDF

All About METAL CHEM 010  Marhainna Zacaria Ampatuan Presenter Cyra Jane D. Cabasog s: Aveniel Lumacad Princess Nicole Malones Christian Laurilla Charmane Goma Christian Jay B. Turque...

All About METAL CHEM 010  Marhainna Zacaria Ampatuan Presenter Cyra Jane D. Cabasog s: Aveniel Lumacad Princess Nicole Malones Christian Laurilla Charmane Goma Christian Jay B. Turqueza  Learning Objectives By the end of this lesson, students will be able to: 1st 2nd 3rd Define and identify Learn to list examples Analyze the chemical metals by of common metals and properties of metals, understanding their explain their key including their definition and physical properties, reactivity and distinguishing them such as conductivity, susceptibility to from nonmetals. malleability, etc. corrosion.  Learning Objectives By the end of this lesson, students will be able to: 4th 5th 6th Explore the Gain knowledge about Connect their categorization of metals alloys, their definitions, understanding of in the periodic table, and their importance in metals and alloys to such as alkali metals, improving the real-life applications in alkaline earth metals, properties of pure industries and everyday etc. metals. scenarios.  METALS Metals are natural compounds of earth’s crust, in which they are generally found in the form of metal ores, associated both with each other and with many other elements. They are also naturally present in the rocks washed by surface water and groundwater and in atmospheric dust.  Comparing Properties Metal Non- s Good electrical conductors Good heat conductors Metals Poor electrical conductors Poor heat conductors Shiny (lustrous) Dull in appearance High density Low density Malleable Brittle Ductile  Metal Examples Copper Iron Zinc Sodium Potassium Gold  Physical Properties of Metals  Metal Structure The key properties of metals, are due to their specific structure. Positive metal ions + + + + + + + + Delocalised electrons  Conductivity Metals are good conductors of electricity. Reas + + + + on are free to Delocalised electrons move around. When they move around, they carry electrical + + + + charge.  Malleability Metals are malleable. They can be hammered into shape. Reas + + + + on The metal atoms (or ions) slide over each other when a force is applied. This allow metals to + + + + change shape on impact.  Ductility The property of metal associated with the ability to be stretched into wire without breaking. Reas + + + + onbecause of their Metals are ductile atomic structure and metallic bonds. + + + +  Shiny Appearance Metals generally have a shiny (lustrous) appearance. Reas + + + + on Metals have delocalised electrons on the surface which + + + + reflect light energy.  Melting Point Metals have a high melting point. Reas + on There is a strong electrostatic attraction between the delocalized electrons and - the positive metal ions. A large amount of thermal energy is required to overcome this. In  Boiling Point Metals have high boiling points. Reas + + + + on Because of the strength of their metallic bonds, which are the + + + + chemical bonds that hold their atoms together.  Chemical Property of Metals  Reaction Of Metal With Oxygen Metals react with oxygen to form metal oxides. Metals donate electrons to oxygen for the formation of metal oxides. For example, 4K + O2 → 2 K2O  Reaction Of Metal With Metals like sodium andWater potassium are highly reactive. They react with water to form alkalis such as sodium hydroxide and potassium hydroxide. 2Na + 2H2O → Calcium also reacts2NaOH with water+ to H2 form calcium hydroxide and hydrogen. Ca + 2H2O → Ca(OH)2 + H2  Reaction Of Metal With Dilute Metals like sodium, Acidlithium and potassium, calcium react vigorously with dilute HCl and H2SO4 to form their metal salt and hydrogen. While magnesium, zinc, iron, tin and lead do not react vigorously with acids. Mg + HCl → MgCl2 + H2  Reaction Of Metal With Other Metals that are Metal more reactive will readily with Salts less reactive metals. More reactive metal displaces the less reactive metal from its oxides, chlorides or sulphides. Zn + CuSO4 → ZnSO4 + Cu Corrosion  What is CORROSION? Corrosion is one of the most common phenomena that we observe in our daily lives. It is basically defined as a natural process that causes the transformation of pure metals into undesirable substances when they react with substances like water or air. This reaction causes damage and disintegration of the metal, starting from the portion of the metal exposed to the environment and spreading to the entire bulk of the metal.  Do All Metals Corrode? Metals placed higher in the reactivity series, such iron, zinc, etc., get corroded very easily, and metals as placed lower in the reactivity series, like gold, platinum and palladium, do not corrode. The explanation lies in the fact that corrosion involves the oxidation of metals. As we go down, the reactivity series tendency to get oxidised is very low (oxidation potentials are very low). Factors Affecting the Rate of Corrosion 1. Reactive metals: In highly reactive metals, the rate of corrosion is very higher. 2. Temperature: Due to the increase in temperature, the rate of corrosion also increases. 3. Presence of impurities: The rate of corrosion increases when a metal is exposed to water especially saltwater. Metals in the Periodic table  Metals in the Periodic Table Metals are located on the left hand side and in the middle of the periodic table. The elements in N group 1 and 2 are on metals, as well as the -M Metals transition metals in et the middle. al s Alkali Metals It belong to the s-block elements occupying the leftmost side of the periodic table. Alkali elements are Lithium(Li), Sodium(Na), Potassium (K), Rubidium (Ru), Cesium (Cs) and Francium (Fr), occupying successive periods from first to seven. Transition Metals any of various metallic elements (such as chromium, iron, and nickel) that have valence electrons in two shells instead of only one. a chemical element in the d-block of the periodic table (groups 3 to 12), though the elements of group 12 (and less often group 3) are sometimes excluded.  Lanthanides The lanthanides are the elements in the top of the two rows located below the main body of the periodic table. Any of the series of 15 consecutive chemical elements in the periodic table from lanthanum to lutetium (atomic numbers 57– 71).  Actinides All actinide series elements are radioactive in nature, they release a large amount of energy on radioactive decay. series encompasses at least the 14 metallic chemical elements in the 5f series, with atomic numbers from 89 to 102, actinium through nobelium.  Metalloids Metalloids can be defined as chemical elements whose physical and chemical properties fall in between the metal and non-metal categories. Boron (B), Germanium (Ge), Silicon (Si), Antimony (Sb), Arsenic (As), Tellurium (Te) and Pollanium (Po) are the seven most widely recognized metalloids.  Other Metals The 7 elements classified as "other metals" or sometime called "typical metals" are located in groups 13, 14, and 15. While these elements are ductile and malleable, they are not the same as the transition elements. This group of "Other Metals" includes Aluminum (Al), Gallium (Ga), Indium (In), Tin (Sn), Thallium (Tl), Lead (Pb), and Bismuth (Bi). Alloy  What does ‘ALLOY' mean? Alloys are combinations of metals or metals and other elements. In order to impart certain properties to metals, or in order to strengthen some of their existing properties, certain other metals/elements can be added to the metals in specific ratios to form alloys. For example, pure aluminium is a relatively soft metal. Pure copper is also quite soft. However, when aluminium is alloyed with copper, the strength of the resulting alloy is far greater than that of its parent metals.  Alloy Examples Steel Nichrome Bronze Solder Duralumin Brass  Elements that are commonly used for Alloying Five common alloying elements are listed below. Chromium Vanadium Molybdenum Nickel Manganese  Thank you for listening All About Metals