Trends in the periodic table 0.0 / 5 ? Chemistrychapter 3 unit 1 Scottish HighersSQA Created by: lindseyreidxoCreated on: 14-05-16 14:00 Covalent Radius a measure of the size of atom, half the distance between the nuclei of two covalently bonded atoms 1 of 16 Going across a period, covalent radius.... decreases 2 of 16 Going down a period, covalent radius.... increases 3 of 16 covalent radius, decreases Going across a period because of increasing nuclear charge 4 of 16 covalent radius, increases Going down a period because of the number of filled electron shells increase, (shielding effect) 5 of 16 electronegativity is a measure of attraction for electrons in a covalent bond 6 of 16 the higher the electronegativity the stronger attraction for the electrons 7 of 16 Going down a period, electronegativity.... decreases 8 of 16 Going across a period, electronegativity.... increases 9 of 16 electronegativity,decreases Going down a period because of the number of filled electron shells increase, screening effect which means that electrons are less strongly attracted to the atom 10 of 16 electronegativity,increases Going across a period because of increase in nuclear charge causes the atom to attract to bonded electrons more strongly 11 of 16 ionisation energy the energy required to move one mole of electrons from one mole of gaseous atoms 12 of 16 going down a group, ionisation energy .. decreases 13 of 16 going across a group, ionisation energy .. increases 14 of 16 going down a group, ionisation energy decreases because.. an electron is being removed from the layer of electrons which is furthest from the nucleus 15 of 16 going across a group, ionisation energy increases because.. the nuclear charge is increasing, the outermost electrons are therefore more strongly held . 16 of 16
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