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Presentation On Giant Structures

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Published in: Chemistry
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This PPT is suitable for the IGCSE and O Level Chemistry students. It only provides theoretical background of the topic. The practice questions, worksheets and topical questions will be discussed during the tutoring sessions

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  1. Giant Structures Chemistry (IGCSE / O-Level)
  2. What will you learn in this lesson? • Giant ionic lattice structures • Giant covalent lattice structures • Giant metallic lattices formed by metallic bonding • Properties of metals
  3. Giant Structures These are lattices where the structure repeats itself in all directions. The forces involved are the same in all direction holding the whole structure There are three types of giant structure 1. Giant ionic lattices 2. Giant covalent structures 3. Giant metallic lattices
  4. Giant Ionic Lattices • A lattice held together by the electrostatic force of attraction between positive and negative ions • In NaCl, each Na+ ion is surrounded by six Cl- ions. Overall, there are equal number of positive and negative ions • The arrangement of ions depend on the number of ions involved and their structure. • The ionic compound is overall neutral
  5. Giant Ionic Lattices (contd.) Ionic crystals are hard but much more brittle than other types of crystal lattice. Pushing one layer against another causes repulsion and gets fractured easily force .pplied here e ee ee In Ionic crystals, when ane tayer Is forced to slide against another. repulsions cause the crystal to fracture.
  6. Giant Ionic Lattices (contd.) Water can also disrupt the ionic lattice. Water surrounds the ions of the lattice Ions in solution can conduct electric current as they are free to move. This is also true when melted mr rru:iecuks (red *tel strraund meal (VOW) and ms. Ths (e.g. c—. Nacn to Osofve in water. For those ionic compounds that do not dissolve in water have strong bonds
  7. Giant Covalent Structures Giant molecular crystals are held together by strong covalent bonds Diamond and Graphite: properties Dark grey, shiny solid Uses ppearance ardness ectrical conductiv properties colourless, transparent crystals that sparkle In light The hardest natural substance Does not conduct electricity In Jewellery and omamental objects In drill bits, diamond saws and glass-cutters Soft — the layers can slide In pencils, and as a over each other — end lubricant solid has a slippery feel Conducts electricity As electrodes and for the brushes in electric motors
  8. Giant Covalent Structures (contd.) Diamond: Each carbon atom is bonded covalently with four other carbon atoms Diamond has very high melting point because the bonding exists throughout the structure Much more brittle than giant metallic lattices Tetrahedral Structure There are no free electrons
  9. Giant Covalent Structures (contd.) Graphite: Graphite is a different kind of carbon that conducts electricity Each carbon atom has strong covalent bond with three other carbon atoms but between the layer there are weaker force of attraction. That helps them to slide over one another There are free electrons between the layers, not used for covalent bonding by atoms Why graphite has a slippery touch? one Byer how the layers fittogether Flat hexagonal layered structure of graphite Why graphite despite being a form of carbon conducts electricity?
  10. Giant Covalent Structures (contd.) Silicon(lV) Oxide, Si02: Silicon has a very similar tetrahedral structure as that of diamond. Each silicon atom is combined to four oxygen atoms and each oxygen atom is combined to two silicon atoms Si02 has similar physical properties as that of diamond. They both are very hard, have high melting points and do not conduct electricty silicon(lV) oxide
  11. Metal lic Bonding An electrostatic force of attraction between the mobile 'sea' of delocalized (not restricted to orbiting the positive ion)electrons and the regular array of positive metal ions within a solid metal i:uooooo 00000 In metallic bonding. the mew Ions are surrounded by a 'sea' of delocalised electrons that are free to move about.
  12. Physical Properties of Metals • Most metals have high melting points and boiling points • Metals are good conductors of electricity • Metals are easily bent and shaped (malleable) or stretched into wires (ductile) Before After formed a is apphed to the layers can slide over each otherwithout the structure being broken. Why metals have high melting and boiling points? Why metals are good conductors of electricity?
  13. Summary of Chemical Bonding in Elements and Compounds metals ELEMENTS bonding Covalent, metallic giant ionic simple giant molecular lattices separate atoms (noble gases) bonding covalent bondtng 1. Covalent bonding 2. Ionic bonding 3. Metallic bonding metal + non-metal(s) COMPOUNDS metal(s)

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