1.2.1 ELECTRON STRUCTURE 0.0 / 5 ? ChemistryBonding & shapesASOCR Created by: upsidedown1004Created on: 16-05-16 12:43 What is the first ionisation energy? the energy required to remove one electron from each atom in one mole of gaseous atoms 1 of 19 what is the second ionisation energy? the energy required to remove one electron from each ion in one mole of +1 ions 2 of 19 Describe successive ionisation energies they increase as electrons being removed on inner shells are harder to remove 3 of 19 How are successive ionisation energies useful? illustrate information about electron structure - how many shells etc. 4 of 19 What factors affect ionisation energies? Atomic shielding/radius // electron shielding // nuclear charge 5 of 19 How does atomic shielding/radius affect ionisation energies? in larger atoms, the outer electron is further away and less strongly attracted to the nucleus to easier to remove 6 of 19 How does electron shielding affect ionisation energies? more inner electrons shield the nuclear share from the outer electrons - electrons have the same charge so repel 7 of 19 How does nuclear charge affect ionisation energies? electrons closer the nucleus feel greater attraction / more protons in the nucleus, the greater the attraction 8 of 19 How do ionisation energies change down a group? they decrease as atomic radius and electron shielding increase 9 of 19 How do ionisation energies change across a period? increases across as nuclear charge increases, electrons are added to the same shell, electrons are attracted more strongly 10 of 19 When removing an electron from the next shell of an atom what happens? ionisation energy increases greatly 11 of 19 What is the equation for finding how many electrons there are in each shell? 2(n^2) 12 of 19 How many electrons can be held in shells 1,2,3 and 4? 1 = 2 // 2 = 8 // 3 = 18 // 4 = 32 13 of 19 What is an orbital? a region of space that can hold up to two electrons, with opposite spins 14 of 19 What is an s-orbital? spherical shape 15 of 19 describe the shape of a p-orbital lobe/dumbbell shaped, right angles to each other 16 of 19 What is the order of the orbitals? s, p, d, f 17 of 19 How many electrons can each orbital hold? s = 2 // p = 6 // d = 10 // f =14 18 of 19 Describe the features of shell 3 electrons fill the 4s subshells before filling the 3d subshells due to a lower relative energy 19 of 19
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