Ionization Energy and Electron Affinity
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Transcript of Ionization Energy and Electron Affinity
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Ionization Energy and Electron Affinity
Section 7.4-7.5
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Objectives
• Examine periodic trends in ionization energy
• Examine periodic trends in electron affinity
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Key Terms
• Ionization energy
• Electron Affinity
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Ionization Energy
• Ease at which electrons can be removed from an atom or ion• First ionization energy, I1, is the energy
required to remove the first electron from neutral atom
• Second ionization energy, I2, is the energy required to remove the second electron from a +1 ion
• Greater the I, the more difficult to remove the electron
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Trends of Ionization Energy
• I1< I2 < I3 < I4
• With each removal, the ion becomes more positive • Strengthens nucleus’s hold on its electrons
• Sharp increase in I when inner-shell electrons are removed• Table 7.2 on page 271
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Periodic Trends in I1
• Within rows, I1 increases with atomic number• Slight irregularities
• Within columns, I1 decreases with increasing atomic number
• Representative elements show larger range of I1 values than transition metals• Transitions slowly increase across rows
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Factors Affecting Trends
• More energy is needed to remove an electron as:• Effective Nuclear Charge increases• Atomic Radius decreases
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Irregularities
• I does not always increases across rows• Decrease from Be to B
Be: [He] 2s2
B: [He]2s2 2p1
• The most easily removed electron in B is that in the 2p orbital, higher in energy than the 2s electrons in Be
• 2p electron of B needs less energy for total removal than does the 2s electron of Be
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Irregularities
• O is lower than N• N: [He]2s2 2p3• O: [He]2s2 2p4
• Important difference in the way electrons are distributed
• Hund’s rule: 3 e- in the 2p orbitals of a nitrogen atom all have the same spin, but e- are paired in one of the 2p orbitals of oxygen• Electrons try to stay as far apart as possible to minimize
repulsion
• Force of repulsion between these electrons is minimized to some extent by pairing electrons• Slightly easier to remove an electron
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Electron Affinities
• Energy change that occurs when electron are added to a gaseous atom
• Measure of the attraction of an atom to an electron
• Negative values (energy is released during process)
• kJ/mol
• More negative affinity = greater attraction
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Trends in Affinities
• Not as evident as that of ionization energy
• Halogens have the greatest affinities (1 e- shy of a filled p subshell)
• Noble gases have affinities of 0
• Group 2A and 5A have very little affinity
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Electron Affinities (kJ/mol)
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Putting it all together
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Homework
• 7.35, 7.42, 7.44, and 7.46 on page 294