Chemistry bonding 3.0 / 5 based on 1 rating ? ChemistryBonding & shapesASAQA Created by: francesca_321Created on: 21-05-15 17:49 What is the definition of bonding? An ionic bond is the electrostatic force of attraction between oppositely charged ions formed by electron transfer 1 of 22 When is the ionic bonding stronger and the melting point is higher? The ions are smaller 2 of 22 What is a covalent bond? A shared pair of electrons 3 of 22 What is a dative covalent bond? It forms when the pair of electrons in a covalent bond come from only one of the bonding atoms. 4 of 22 What is the definition of a metallic bond? The electrostatic force of attraction between the positive metal ions and the delocalised electrons 5 of 22 What are the three main factors that affect the strength of a metallic bond? Number of protons, number of delocalised electrons and the size of the ion 6 of 22 What is an ionic bond? Electrostatic force of attraction between oppositely charged ions 7 of 22 For example? Sodium chloride, magnesium oxide 8 of 22 What is the structure of a covalent bond? Simple molecular 9 of 22 With what forces? intermolecular forces(van der waals, permanent dipoles and hydrogen bonds between molecule 10 of 22 for example? iodine, ice, carbon dioxide, water and methane 11 of 22 What are examples of a macromolecule? Diamond Graphite, silicon dioxide and silicon 12 of 22 What is metallic bonding? Electrostatic forces between the metal posistive ions and delocalised electrons 13 of 22 for example? Magnesium, sodium- giant metallic structure 14 of 22 Why does a molecular structure have low BP/MP? Because of weak intermolecular forces between molecules(eg; van der waals/ hydrogen 15 of 22 why are metals malleable? The positive ions in the lattice are identical so the planes can slide easily over eachother 16 of 22 Why can graphite conduct electricity? Free delocalised electrons between layers 17 of 22 what is the definition of electronegativity? The relative tendency of an atom in a covalent bond to attract electrons in a covalent bond to itself 18 of 22 Why does electronegativity increase across a period? The number of protons increases 19 of 22 Why does the atomic radius decrease? The electrons in the same shell are pulled in more 20 of 22 What happens down a group? decreases down a group because the distancebetween the nucleus and the outer electrons increases and the shieldingof inner shell electrons increases. 21 of 22 Why is I2 a solid and CL2 a gas? Increasing number of electrons in the bigger molecules causing an increase in the size of van der waals between molecules 22 of 22
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