Chemistry
Chemistry, 22.07.2019 06:30, denym58

Atoms with low ionization energy tightly hold their electrons true or false

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Chemistry, 27.06.2019 22:30, Cocco
How is the number of valence electrons related to the ionization energy of an element? (1 point) low ionization energy correlates to elements with fewer valence electrons. elements with higher ionization energy tend to have less valence electrons. atoms with nearly full valence electron shells have lower ionization energy. high ionization energy indicates a low likelihood to gain valence electrons.
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Chemistry, 02.08.2019 00:00, anyaimartinez1901
Ionization energy is a measure of how strongly an atom holds onto its electrons. a higher ionization energy indicates that more energy would be needed to remove an electron. atoms that have a smaller atomic radius tend to have higher ionization energies because their electrons are closer to the nucleus. based on the periodic table, which element would be expected to have the lowest ionization energy? a) calcium (ca) b) cesium (cs) c) sodium (na) d) strontium (sr) wrong answers will be reported.
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Chemistry, 17.10.2019 11:30, tonytashaqua
How is the number of valence electrons related to the ionization energy of an element? a) low ionization energy correlates to elements with fewer valence electrons. b) elements with higher ionization energy tend to have less valence electrons. c) atoms with nearly full valence electron shells have lower ionization energy. d) high ionization energy indicates a low likelihood to gain valence electrons.
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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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Atoms with low ionization energy tightly hold their electrons true or false...

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