Bonding Unit 2 Chemistry 0.0 / 5 ? ChemistryStructure and bondingGCSEAQA Created by: SunsetCreated on: 05-01-14 13:21 Why do GIANT IONIC STRUCTURES have high melting and boiling points? Lots of attraction required to overcome strong attraction 1 of 11 Why don't SIMPLE COVALENT STRUCTURES conduct electricity? They have no charge 2 of 11 Why is DIAMOND hard? Each carbon atom is bonded to 4 others by strong covalent bonds and there are no layers 3 of 11 Why does GRAPHITE conduct electricity? Each carbon atom is bonded to three others leaving one free electron which is delocalised and able to carry charge 4 of 11 What type of atom does COVALENT BONDING happen between? Non-metals 5 of 11 Why are METALS malleable? They are arranged in layers which can slide over one another 6 of 11 Why do METALS have high melting and boiling points? There is a strong electrostatic attraction between the positive ions and delocalised electrons which requires a lot of energy to break 7 of 11 Why are ALLOYS harder than pure metals? The different sized atoms disrupt the pattern preventing the layers from slidingw 8 of 11 Why don't Thermosetting Plastics soften when heated? They have strong covalent bonds which require a lot of energy to break 9 of 11 What charged ion would a group 2 atom make? +2 10 of 11 Lithium has atomic number 12 and oxygen has atomic number 8. They are ionically bonded. What is the formula of the ionic compound that they form? Li2O 11 of 11
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