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Chapter 4: Problem 5

Using grammatically correct English sentences: a) provide a possible explanation for why \(\mathrm{IE}_{1}\) for \(\mathrm{He}\) is greater than \(\mathrm{IE}_{1}\) for \(\mathrm{H}\). b) provide a possible explanation for why \(\mathrm{IE}_{1}\) for \(\mathrm{Li}\) is less than \(\mathrm{IE}_{1}\) for He.

Short Answer

Expert verified
a) \(\mathrm{IE}_{1}\) for \(\mathrm{He}\) is greater than \(\mathrm{IE}_{1}\) for \(\mathrm{H}\) because Helium has more electrons in the same shell which are tightly bound to the nucleus. b) \(\mathrm{IE}_{1}\) for \(\mathrm{Li}\) is less than \(\mathrm{IE}_{1}\) for \(\mathrm{He}\) because the third electron in Lithium is in a higher energy level, further from the nucleus and less tightly held.

Step by step solution

01

Understanding IE for Hydrogen and Helium

\(\mathrm{IE}_{1}\) for \(\mathrm{He}\) is greater than \(\mathrm{IE}_{1}\) for \(\mathrm{H}\) because Helium has 2 electrons in the 1s shell, while Hydrogen has only one. Both electrons in Helium share the same shell and are thus tightly bound to the nucleus, causing it to have a higher ionization energy than Hydrogene. It takes more energy to remove an electron from Helium as it is more tightly held than in Hydrogen.
02

Understanding IE for Lithium and Helium

\(\mathrm{IE}_{1}\) for \(\mathrm{Li}\) is less than \(\mathrm{IE}_{1}\) for \(\mathrm{He}\) because Lithium has three electrons with the third electron existing in a higher energy level (2s) compared to Helium's two electrons (in the 1s level). The electron in the 2s level in Lithium is less tightly held as it's further from the nucleus, hence it requires less energy to remove it compared to removing an electron from Helium.

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Most popular questions from this chapter

The value of the ionization energy of He given in Table 1 is described as being consistent with two electrons in a "shell" approximately the same distance from the nucleus as the one electron in H. Use the Coulombic Potential Energy equation, \(V=\frac{\mathrm{kq}_{1} \mathrm{q}_{2}}{\mathrm{~d}}\) to explain how this conclusion can be reached. Hint: recall the relationship between \(V\) and \(\mathrm{IE}_{1}\).

For atoms with many electrons, not all electrons are at the same distance from the nucleus. In this case, which electron would have the lowest ionization energy: the electron that is closest to the nucleus or the electron that is farthest from the nucleus? Explain.

Recall that the IE of \(\mathrm{H}\) is \(1.31 \mathrm{MJ} / \mathrm{mole}\). If all three electrons in Li were in the first shell at a distance equal to that of hydrogen, which of the following values would be the better estimate of the IE of Li: 3.6 MJ/mole or 0.6 MJ/mole? Explain.

Predict the relationship between \(\mathrm{IE}_{1}\) and atomic number by making a rough graph of IE \(_{1}\) vs. atomic number. DO NOT PROCEED TO THE NEXT PAGE UNTIL YOU HAVE COMPLETED THIS GRAPH.

Is the amount of energy required to remove one of the electrons from the first shell of Li greater than, less than, or equal to the \(\mathrm{IE}_{1}\) for Li? Explain your reasoning.
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