Question
Consider this set of successive ionization energies:IE1 = 578 kJ>mol IE2 = 1820 kJ>molIE3 = 2750 kJ>mol IE4 = 11,600 kJ>molTo which third-period element do these ionization values belong?
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The first ionization energy is the energy to remove the first electron, the second ionization energy is the energy to remove the second electron, and so on. Show more…
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Consider this set of successive ionization energies: $$ \begin{array}{ll}{\mathrm{IE}_{1}=578 \mathrm{kJ} / \mathrm{mol}} & {\mathrm{IE}_{2}=1820 \mathrm{kJ} / \mathrm{mol}} \\ {\mathrm{IE}_{3}=2750 \mathrm{kJ} / \mathrm{mol}} & {\mathrm{IE}_{4}=11,600 \mathrm{kJ} / \mathrm{mol}}\end{array} $$ To which third period element do these ionization values belong?
Consider this set of ionization energies. $\mathrm{IE}_{1}=578 \mathrm{~kJ} / \mathrm{mol}$ $\mathrm{IE}_{2}=1820 \mathrm{~kJ} / \mathrm{mol}$ $\mathrm{IE}_{3}=2750 \mathrm{~kJ} / \mathrm{mol}$ $\mathrm{IE}_{4}=11,600 \mathrm{~kJ} / \mathrm{mol}$ To which third-period element do these ionization values belong?
Consider the set of successive ionization energies: IE1: 496 kJ/mol IE2: 4562 kJ/mol IE3: 6910 kJ/mol IE4: 9543 kJ/mol Identify the element in period 3 that corresponds to this set of ionization energies. Na Mg Si Al
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