Bond Polarity 0.0 / 5 ? ChemistryBonding & shapesA2/A-levelAQA Created by: emma.davisonCreated on: 05-11-18 11:32 Give the definition for electronegativity. Power of an atom to attract the pair of electrons in a covalent bond 1 of 14 How and why does an increased nuclear charge effect electronegativity? Increased - more protons in nucleus so a stronger attraction to the bonding pair 2 of 14 How and why does an increased number of electron shells effect electronegativity? Decreased - bonding electrons are more shilded from nuclear charge so weaker attraction 3 of 14 How and why does an increased atomic radius effect electronegativity? Decreased - nucleus is further from bonding pairs and so a weaker attraction 4 of 14 Explain the trend of electronegaitiviy down a group. Decreasing - number of electron shells increases, more electron shielding so less attraction. Atoms get larger, so BP futher from nucleus. 5 of 14 Explain the trend of electronegativity across a period. Increasing - uincreased nucluear charge, so more protons in nucleus so stronger attractions. Atoms decrease in size so nucleus is clsoer to BP. 6 of 14 What is the definition for polarity? Unequal sharing of electrons in a bond 7 of 14 When does a non-polar covalent bond occur? When two atoms have the same electronegativity. 8 of 14 What does a non-polar covalent bond mean? Covalent bond where two electrons are shared equally. 9 of 14 Give an example of a non-polar covalent bond. Cl-Cl 10 of 14 When does a polar covalent bond occur? When two atoms have different electronegativities. 11 of 14 What does a polar covalent bond mean? Covalent bond where two electrons are not shared equally 12 of 14 Which atom are the electrons closer to in a polar covalent molecule? The more electronegative molecule 13 of 14 Give an example of a polar covalent bond. HCl 14 of 14
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