Chemistry Unit 2~ Bonding,Structure and Properties of matter 0.0 / 5 ? ChemistryStructure and bondingIGCSEAQA Created by: TharvCreated on: 12-11-18 17:45 Ionic Bonding -Involves the tranfer of electrons between Metals and non-metals -To create an Ion, Atoms either lose or gain electrons. -Electrons don't vanish or appear, they get transfered to one another creating the ions. -Positive and negative ions > attracted by Electrostatic Attraction. 1 of 14 Ionic Compounds -Have a structure- Giant Ionic Lattice. - Ions form a tightly packed Lattice where all strong electrostatic forces between them are in all directiins. 2 of 14 Properties of Ionic Formula -Strong forces > high melting and boiling points. -When solid, can't conduct electricity (until they melt- ions are free moving. -Dissolve easily in water > ions are free moving. 3 of 14 Convalescent Bonding -Atoms share elements -Bonds between Non-metals and Metals > Gain a full outer shell. - Bonds are very strong. 4 of 14 Simple Covalent Structrues - Very strong -Intermolecular forces between molecules are weak. > Very low melting and boiling point. >Usually liquids/gases room temp. > Bigger molecule get > strong the intermol. forces get. > More energy is needed to break them. 5 of 14 Polymers -Made from small molecules -Covalently joined to form long chains of repeating Molecules e.g Polyethane. 6 of 14 Properties of Polymers - Intermolecular forces between are large - Means it takes alot more energy to break them apart. - Forces are still weaker than ionic or covalent bonding. - Lower boiling/ melting points than ionic and giant covalent structures 7 of 14 Giant Covalent Structures. -Strong Covalent Bonds -High melting/boiling points, need lots of energy to break them down. - Don't conduct electricity except Graphite 8 of 14 Metallic Bonding - Decolonised Electrons (Free moving) - Strong electrostatic forces between the metal ion (+) and shared electrons (-) 9 of 14 Properties of Metallic Bonding - High melting and boiling points > Solid at room temp. - Delconised electrons conduct electricity and good conductors of heat. - Layers of atoms can slide over each other > Can be shaped. 10 of 14 Alloys - Mixture of atoms. - Stronger than metals > Different sized atoms in their structure > Atoms distort layers so they can't slide over eachother. 11 of 14 Allotopes of Carbon - Structually different forms of the same element in the same state. - For e.g Carbon Graphene - Thin sheet of carbon - Very strong - Incredibly light 12 of 14 Grpahene Graphene - Thin sheet of carbon - Very strong - Incredibly light - Conduct electricity with decolonised electrons - Good for you in electronics 13 of 14 Fullerenes - Molecules of Carbon - Carbon > mainly arranged in hexagons - Can be used to deliver drugs in body - Can form nanotubes - They have properties that make them useful in electronics. 14 of 14
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