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Chapter 8: Problem 88

The \(\mathrm{H}^{-}\) ion and the He atom have two \(1 \mathrm{~s}\) electrons each. Which of the two species is larger? Explain.

Short Answer

Expert verified
The \(\mathrm{H}^{-}\) ion is larger than the He atom. This is due to the stronger nuclear charge of He, which pulls the electrons closer to the nucleus, resulting in a smaller atomic size compared to \(\mathrm{H}^{-}\) where the nuclear charge is less.

Step by step solution

01

Understand the atomic structure

Both the \(\mathrm{H}^{-}\) ion and a helium (He) atom have two electrons in the 1s orbital. However, a hydrogen ion has one proton in its nucleus while a helium atom has two.
02

Understand the electron shielding effect

Electron shielding describes the balance between the pull of the protons on the outermost electrons and the push of the other electrons. In the case of He, there is greater nuclear charge because it has two protons compared to H-, thus causing a stronger pull on the electrons.
03

Compare the size

Because of the stronger nuclear charge in He, the 1s electrons are pulled more closely to the nucleus, making He smaller compared to \(\mathrm{H}^{-}\). The \(\mathrm{H}^{-}\) ion, having a relatively smaller nuclear charge, has its electrons less tightly held and hence it is larger in size.

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Most popular questions from this chapter

Write formulas and give names for the binary hydrogen compounds of the second- period elements (Li to F). Describe the changes in physical and chemical properties of these compounds as we move across the period from left to right.

Specify in what group of the periodic table each of these elements is found: (a) [Ne]3s", (b) \([\mathrm{Ne}] 3 s^{2} 3 p^{3}\) (c) \([\mathrm{Ne}] 3 s^{2} 3 p^{6}\) (d) \([\mathrm{Ar}] 4 s^{2} 3 d^{8}\)

Name the element that forms compounds, under appropriate conditions, with every other element in the periodic table except He and Ne.

In the periodic table, the element hydrogen is sometimes grouped with the alkali metals (as in this book) and sometimes with the halogens. Explain why hydrogen can resemble the Group \(1 \mathrm{~A}\) and the Group 7A elements.

Without referring to a periodic table, write the electron configurations of elements with these atomic numbers: (a) \(9,\) (b) \(20,\) (c) \(26,\) (d) 33. Classify the elements.
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