Chemistry 1-7-09 2nd Ionization Energy
CHEMISTRY: Great job in class today! I really like it when we can have a dialog in class, and you really seemed to be with me today – and it was tough stuff. Good job! Here’s the lecture on second ionization energy.
January 7th, 2009 at 11:43 PM
Why is it that after electrons have been taken away it still retains its identity? Wouldn’t it be an isotope instead of an ion, or are they not the same thing?
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January 8th, 2009 at 8:16 AM
what exactly is 2nd ionization energy?
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January 8th, 2009 at 4:16 PM
what are the trends of electron affinity.
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January 8th, 2009 at 4:19 PM
what is the difference between 2nd and 3rd ionization energy?
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January 8th, 2009 at 4:22 PM
ok brandon: the difference is that the second ionization energy is to take the second electron and third is to take away the third and also the third ;is much greater than the first
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January 8th, 2009 at 4:23 PM
What is the trend of ionization energy going across the periodic table?
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January 8th, 2009 at 5:41 PM
Jalen,the trend for ionization energy going across the peridic table is energy INCREASING as you go across to the far right,but stop at the Noble Gases.!
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January 8th, 2009 at 7:03 PM
What is the trend of ionization going down periods?
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January 8th, 2009 at 7:04 PM
oh ok i get the 2nd and 3rd ionization energy now
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January 8th, 2009 at 7:06 PM
elizabeth: The 2nd ionization energy is the energy required to remove a second electron from an atom.
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January 8th, 2009 at 7:26 PM
Hey people! I was just doing my homework and I was just wondering-what chemical property decreases down the group and period? I was stumped.
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January 8th, 2009 at 8:18 PM
Aniah, an atom retains its identity because it’s identity is determined by how many protons it has, not electrons. Isotopes are atoms with different numbers of protons than neutrons. Ions are atoms with a different number of protons than electrons.
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January 8th, 2009 at 8:30 PM
Ionization energies increase moving from left to right across a period. Ionization energy decreases moving down a group.
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January 8th, 2009 at 8:33 PM
I have a question about electronegativity…the more negative the number on the table is, the higher the electronegativity is??
(I wasn’t quite sure how to state the question)
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January 8th, 2009 at 8:49 PM
oops. I meant electron affinity. I’ve confused myself
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January 8th, 2009 at 8:50 PM
how is the behavior of an atom different when it has a full outer energy level than when it doesnt? does anything change besides its charge?
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January 8th, 2009 at 9:23 PM
why does the negative atom become positive when you take an electron away?
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January 8th, 2009 at 10:26 PM
ok so if you take away an elements electron to make it stable how would that not change what the element is?
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January 9th, 2009 at 4:49 PM
kaele,
the element doesnt change because it still has the same number of protons.
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January 9th, 2009 at 4:23 PM
jake it becomes possitive bacause it begins with the same number of protons and electorns and if you take one or more electrons away then it becomes possitive because it has more protons then electrons.
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January 9th, 2009 at 9:51 PM
well Mackenzie, the atom becomes stable once it has a full outer energy level. it wont react with other atoms when it has a full outer energy level.
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