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Chapter 4: Problem 10

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.

Short Answer

Expert verified
The energy required to remove an electron from the first shell of Li is greater than the \( \mathrm{IE}_{1} \) for Li. This is because electrons in the first shell are more tightly bound to the nucleus due to greater attractive forces.

Step by step solution

01

Understanding Ionization Energy

The ionization energy (IE) of an atom is the minimum energy required to remove an electron from the ground state of the isolated gaseous atom. The first ionization energy (\( \mathrm{IE}_{1} \)) refers to removing the first, or outermost, electron.
02

Recognizing Position of Electrons

The first shell of the atom is closest to the nucleus. Given that the nucleus contains protons, it has a positive charge. Electrons, being negatively charged, are attracted to this positive charge. This means electrons in shells closer to nucleus are generally more strongly attracted, and therefore more difficult to remove.
03

Comparing Ionization Energies

Since the first shell electron is held more tightly to the nucleus due to the attractive forces, it requires more energy to remove than an electron from higher energy levels. Thus, the ionization energy to remove an electron from the first shell is greater than \( \mathrm{IE}_{1} \) for Li.

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Most popular questions from this chapter

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.

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.

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.
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