Quiz Grades Rewrite your answer to question 1 on the back of your quiz. If it is correct, I will add...
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![Page 1: Quiz Grades Rewrite your answer to question 1 on the back of your quiz. If it is correct, I will add up to 20% to your quiz grade (maximum score: 100%).](https://reader030.fdocuments.in/reader030/viewer/2022032702/56649ca35503460f949639d6/html5/thumbnails/1.jpg)
Quiz Grades
• Rewrite your answer to question 1 on the back of your quiz. If it is correct, I will add up to 20% to your quiz grade (maximum score: 100%).
• Due next class
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Ionisation Energies
p. 63-67
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Ions and electron configuration
• Li: 1s22s1
• Li+: 1s2
• He: 1s2
• Cl: 1s22s22p63s23p5
• Cl-: 1s22s22p63s23p6
• Ar: 1s22s22p63s23p6
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Ionisation Energy• the amount of energy required to remove
an electron from a gaseous atom to form a gaseous ion.
• Q(g) Q+(g) + e-
• Second ionisation energy: energy required to remove a second electron
• Q+(g) Q2+
(g) + e-
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• Energy is required to remove an electron (endothermic)
Factors affecting ionisation energy
1. Charge on the nucleus
2. Repulsion (pushing away) or “shielding” of electron from inner orbitals
3. Repulsion on the electron from other electrons in the valence shell
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Factors affecting ionisation energy
• Charge exerted on each electron by the positively charged nucleus
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Repel
AttractAttract
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Effective Nuclear Charge
• Charge exerted on each electron by the positively charged nucleus
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• Charge exerted on each electron by the positively charged nucleus
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Successive (next) Ionization Energies
• The more electrons that have been removed, the greater the energy required to remove the next electron.– because of lower electron-electron repulsions– greater nucleus-electron attraction
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Valence electrons repel
one another
No other electron in 3rd energy
level to repel the one remaining
electron
Remaining valence electron attracted more
strongly to nucleus
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Successive Ionization Energy of Mg
Big increase in ionization energy when the next electron is removed from a filled inner energy level. This electron has a much higher effective nuclear charge on itself.
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Stop.
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Ionisation Energy - Groups• Going down a group on the periodic table,
ionisation energy decreases– successive electrons are lost from higher
energy levels• further from the nucleus• less attraction to nucleus
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Ionization Energy - Periods
• Ionisation energy increases across a period– effective nuclear charge increases– not a smooth increase
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Ionization Energy Increases
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• Ionization energy decreases when going from the second to the third element in each period (Be to B, Mg to Al)– Because of which sub-level the electron
comes from (2p1 is higher energy than 2s2)– Lower ionization energy if removing one
electron from a doubly-filled orbital
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Isoelectronic Species
• Iso = same
• Atoms and ions that have the same electronic structure
• S2-, Cl-, Ar, K+, Ca2+