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Why is there a large jump between 10 and 11 ionization ehergies of magnisium?
Wiki User
∙ 13y ago
- the large jump is caused because magnisium is such a powerful element that if it was combined in an explosive it have the power of an atomic bomb
Wiki User
∙ 13y ago
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Between his large number of friends?
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When magnesium burns, it reacts with oxygen in the air to form magnesium oxide and produces a bright white light. This is a highly exothermic reaction, releasing a large amount of heat and energy. The resulting magnesium oxide residue is a white powder.
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Cl
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Francium would be expected to have the lowest ionization energy, as it is located in the alkali metal group at the bottom left of the periodic table. Alkali metals typically have the lowest ionization energies due to their large atomic size and low effective nuclear charge.
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Ionic bonds form between atoms with a large difference in electronegativity (generally between a metal and a nonmetal) because one atom will easily donate electrons to the other. Additionally, the atoms involved must have low ionization energy and high electron affinity to readily gain or lose electrons.
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Low ionization energies are typically characteristic of atoms that have large atomic size and few protons in their nucleus, such as alkali metals and alkaline earth metals. These atoms have loosely bound electrons that require less energy to remove.
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The biggest element in the alkali family is cesium. It has the largest atomic radius and is the most reactive alkali metal due to its large size and low ionization energy.
Why is there such a large jump in ionization enery between the second and third ionization energies for magnesium?
The jump in ionization energy between the second and third ionization energies for magnesium is due to the removal of an electron from a full electron shell. Removing an electron from a full shell requires significantly more energy as it disrupts the stable electron configuration of the atom.
