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Chapter 8: Problem 100

Little is known of the chemistry of astatine, the last member of Group \(7 \mathrm{~A}\). Describe the physical characteristics that you would expect this halogen to have. Predict the products of the reaction between sodium astatide (NaAt) and sulfuric acid. (Hint: Sulfuric acid is an oxidizing agent.).

Short Answer

Expert verified
As a member of the halogens, astatine is expected to manifest metallic characteristics, being volatile with a dark, lustrous appearance. When Sodium astatide (NaAt) reacts with sulfuric acid (H2SO4), it is predicted to form astatine gas (At), water (H2O) and Sodium sulfate (Na2SO4) since sulfuric acid acts as an oxidizing agent.

Step by step solution

01

Understand Astatine Properties

Astatine is a halogen, meaning it belongs to Group 7A. Halogens veer towards a non-metallic nature as you move down the group. So, it can be described that astatine, being the heaviest halogen, would have metallic characteristics. However, since it's at the bottom of the group, expect it to be quite volatile with a dark, lustrous appearance.
02

Predict Reaction Products

Predicting the products of the reaction between Sodium astatide (NaAt) and sulfuric acid (H2SO4) relies on the knowledge that sulfuric acid acts as an oxidizing agent. Typical reactions with halides and sulfuric acid often produce a halogen gas, water, and a sulfate salt. With Sodium astatide, this trend is expected to hold, forming astatine gas (At), water (H2O) and Sodium sulfate (Na2SO4).
03

Write out the Chemical Reaction

NaAt + H2SO4 -> At(g) + H2O(l) + Na2SO4

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Most popular questions from this chapter

The ionization energy of a certain element is \(412 \mathrm{~kJ} / \mathrm{mol}\). When the atoms of this element are in the first excited state, however, the ionization energy is only \(126 \mathrm{~kJ} / \mathrm{mol}\). Based on this information, calculate the wavelength of light emitted in a transition from the first excited state to the ground state.

Write ground-state electron configurations for these transition metal ions: (a) \(\mathrm{Sc}^{3+}\) (b) \(\mathrm{Ti}^{4+}\) (c) \(\mathrm{V}^{5+}\) (d) \(\mathrm{Cr}^{3+}\) , (e) \(\mathrm{Mn}^{2+},\) (f) \(\mathrm{Fe}^{2+}\) (h) \(\mathrm{Co}^{2+}\) (g) \(\mathrm{Fe}^{3+}\) (i) \(\mathrm{Ni}^{2+}\) (i) \(\mathrm{Cu}^{+}\) (k) \(\mathrm{Cu}^{2+}\) (1) \(\mathrm{Ag}^{+}\) \((\mathrm{m}) \mathrm{Au}^{+}\) (n) \(\mathrm{Au}^{3+},\) (o) \(\mathrm{Pt}^{2+}\)

Draw a rough sketch of a periodic table (no details are required). Indicate where metals, nonmetals, and metalloids are located.

Why do elements that have high ionization energies usually have more positive electron affinities?

Explain why alkali metals have a greater affinity for electrons than alkaline earth metals do.
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