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Chapter 9: Problem 94

Consider a nitrogen atom in the ground state and comment on whether the following statements are true or false. (a) \(\mathrm{Z}_{\text {eff }}\) for an electron in a 2 s orbital is greater than that for the 1 s orbital. (b) The \(Z_{\text {eff for the } 2 p \text { and } 2 s \text { orbitals is the same. }}\) (c) More energy is required to remove an electron from a 2 s orbital than from the \(2 p\) orbital. (d) The 2 s electron is less shielded than the \(2 p\) electron.

Short Answer

Expert verified
Statement a) is false, b) is true, c) is true, and d) is true.

Step by step solution

01

Statement (a) analysis

The effective nuclear charge (\(Z_{eff}\)) is the attraction felt by an electron towards the nucleus. It is affected by two factors: the atomic number (in this case, nitrogen with atomic number 7) and the shielding effect of other electrons. The 2s electrons are farther from the nucleus than the 1s electrons, therefore the inner shell (1s) electrons shield the outer shell (2s) electrons from the nuclear charge. So, \(\mathrm{Z}_{\text {eff }}\) for an electron in a 2s orbital is actually less than that for the 1s orbital. Therefore, statement (a) is false.
02

Statement (b) analysis

In nitrogen atom, both the 2s and 2p orbitals are in the same shell (n=2) and thus have the same average distance from the nucleus, so they experience the same amount of shielding from the inner shell (1s) electrons. Therefore the effective nuclear charge (\(Z_{eff}\)) is the same for both orbitals. So, statement (b) is true.
03

Statement (c) analysis

Energy required to remove an electron from an atom is called ionization energy. In an atom, the 2s electrons are closer to the nucleus and more tightly bound than the 2p electrons, thus they are shielded less effectively by the inner-shell electrons and experience a higher \( Z_{eff} \). As a result, it requires more energy to remove an electron from a 2s orbital than from a 2p orbital. Therefore, statement (c) is true.
04

Statement (d) analysis

Shielding effect relates to the ability of an electron in an atom to shield other electrons from the positive charge of the nucleus. Since 2s electrons are closer to the nucleus and more tightly bound, they are shielded less effectively by the inner shell (1s) electrons than the 2p electrons, which are farther from the nucleus. Consequently, the 2s electron is less shielded than the 2p electron. Therefore, statement (d) is true.

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Most popular questions from this chapter

For the atom \(^{119} \mathrm{Sn}\), indicate the number of (a) protons in the nucleus; (b) neutrons in the nucleus; (c) \(4 d\) electrons; (d) 3s electrons; (e) 5 \(p\) electrons; (f) electrons in the valence shell.

Listed below are two atomic properties of the element germanium. Refer only to the periodic table on the inside front cover and indicate probable values for each of the following elements, expressed as greater than, about equal to, or less than the value for Ge. $$\begin{array}{lcc} \hline \text { Element } & \text { Atomic Radius } & \begin{array}{c} \text { First lonization } \\ \text { Energy } \end{array} \\ \hline \mathrm{Ge} & 122 \mathrm{pm} & 762 \mathrm{kJ} / \mathrm{mol} \\ \mathrm{Al} & ? & ? \\ \mathrm{In} & ? & ? \\ \mathrm{Se} & ? & ? \\ \hline \end{array}$$

In your own words, define the following terms: (a) isoelectronic; (b) valence- shell electrons; (c) metal; (d) nonmetal; (e) metalloid.

The following species are isoelectronic with the noble gas krypton. Arrange them in order of increasing radius and comment on the principles involved in doing so: $\mathrm{Rb}^{+}, \mathrm{Y}^{3+}, \mathrm{Br}^{-}, \mathrm{Sr}^{2+}, \mathrm{Se}^{2-}.$

Arrange the following in expected order of increasing radius: $\mathrm{Br}, \mathrm{Li}^{+}, \mathrm{Se}, \mathrm{I}^{-} .$ Explain your answer.
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