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10 Cards in this Set
- Front
- Back
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Are the 4p orbitals in iodine smaller in size than that in Ge? Explain.
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The 4p orbital in iodine is clearly smaller in size because of the greater effective nuclear charge
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Ionization Energy
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Highest in the right corner. How much the atom wants to keep it's atom
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Shielding
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Electrons closer to nucleus sheilds/stops electrons furtur away
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Reduced
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Losses electrons
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Oxidized
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Gains Electrons
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Bond order
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Number of bonding Electrons - Number of antiboding electrons divided by 2
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Bigger bond order
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Stronger, more stable
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Explain why Mg has a positive electron affinity whereas that of Na is negative.
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Because the 3s shell of Mg is closed and the shielding is almost complete for the nuclear charge. Therefore, there is little attraction between Mg and a free electron. On the other hand, the effective nuclear charge on the 3s electron in Na is greater than 1, making it possible to attract other free electrons nearby.
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Explain why Cl has the highest electron affinity and F has the highest electronegativity.
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Cl is bigger and the electron attached to it has a large room to stay away from other electrons already there. Or you can say that 3p orbitals are bigger than 2p orbitals. So the repulsion between the attached electrons and the rest is smaller in Cl case. F has very high ionization energy as well as electron affinity, making it the highest electronegative element.
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Name two benefits of fulfilling the octet rule.
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Energetic stability and becoming chemically inert
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