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Ionization Energy

Ionization Energy. Clint Ko John Kaczor Tommy Jasionowskiz AP. Ionization Energy. Ionization energy is the energy required to remove an electron from an atom in the gas phase. Atom in ground state (g)  Atom + (g) + e -. Δ E = ionization energy, IE.

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Ionization Energy

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  1. Ionization Energy Clint Ko John Kaczor Tommy Jasionowskiz AP

  2. Ionization Energy Ionization energy is the energy required to remove an electron from an atom in the gas phase. Atom in ground state (g)  Atom+ (g) + e- ΔE = ionization energy, IE All elements besides hydrogen have subsequent ionization energies (first, second, third, etc). The IE increases because the atom becomes more positively charged as you remove more electrons. Thus, the nucleus-electron attraction increases. IE1 = 738 kJ/mol IE2 = 1451 kJ/mol IE3 = 7733 kJ/mol Mg Mg+Mg2+

  3. Periodic trends As you move from left to right on the periodic table, the IE increases. This is because the effective nuclear charge, Z*, increases across a period. Thus increasing the extent of the nuclear-electron attraction. Also, because atomic radii decrease across a period, the electrons are closer to the nucleus and exhibit a stronger attractive force, increasing IE and requiring more energy to remove.

  4. Group Trends IE decreases down a group. This trend occurs because the electrons removed is further from the nucleus, thus reducing the nucleus-electron attractive force. This makes it easier to remove an electron, decreasing the energy required (IE).

  5. Variations Variations can occur across a period or down a group. These variations occur due to electron orbitals or differences in energy levels. Across a period, 2p electrons are slightly higher in energy that 2s electrons, thus the IE for boron is lower than that of beryllium. Also comparing O and N, O has one pair of paired electrons in its first 2p orbitals, which causes electron-electron repulsions. nitrogen, on the other had, is fully paramagnetic, or has three unpaired electrons. This means that electron-electron repulsions are at a minimum. Thus, the IE of O is lower than that of N.

  6. Ionization Energy

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