Chemistry
Chemistry, 17.07.2019 21:00, SoccerHalo

What is ionization energy? a. the minimum energy required to remove one electron from an atom. b. the maximum energy required to remove one electron from an atom. c. the maximum energy required to move one electron to the valence shell. d. the minimum energy required to remove one electron from another electron.

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Chemistry, 17.07.2019 21:00, BrownBeauty4623
What is ionization energy? a. the minimum energy required to remove one electron from an atom. b. the maximum energy required to remove one electron from an atom. c. the maximum energy required to move one electron to the valence shell. d. the minimum energy required to remove one electron from another electron.
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Physics, 17.09.2019 06:00, ayoismeisalex
Elements are arranged in groups by similar atomic structure on the periodic table. this allows for an element's properties to be predicted based on general periodic trends. one of these trends, ionization energy, increases up a group and to the right along a period and can be defined as the a) energy required to add an electron b) energy required to excite an electron c) energy required to remove a core electron d) energy to required to remove a valence electron
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Chemistry, 19.09.2019 04:30, sunny3799
What is ionization energy? a. the minimum energy required to remove one electron from an atom. b. the maximum energy required to remove one electron from an atom. c. the maximum energy required to move one electron to the valence shell. d. the minimum energy required to remove one electron from another electron.
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Chemistry, 18.10.2019 18:30, hannahkharel2
When atoms lose more than one electron, the ionization energy to remove the second electron is always more than the ionization energy to remove the first. similarly, the ionization energy to remove the third electron is more than the second and so on. however, the increases in ionization energy upon the removal of subsequent electrons is not necessarily uniform. for example, consider the first three ionization energies of magnesium: first ionization energy 738kj/mol second ionization energy 1450kj/mol third ionization energy 7730kj/mol the second ionization energy is roughly twice the first ionization energy, but then the third ionization energy is over five times the second. use the electronic configuration of magnesium to explain why this is so? would you expect the same behavior in sodium? why or why not?
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