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Chapter 8: Problem 90

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

Short Answer

Expert verified
The element is Fluorine (F).

Step by step solution

01

Understanding the question context

The question asks us to identify the element that reacts with all other elements in the periodic table, barring He, Ne and Ar. This element must exhibit a high level of reactivity and bonding capacity.
02

Identifying the element

The element that fits this description is Fluorine (F). Fluorine is a halogen that is located in Group 17 of the periodic table. It is the most active non-metal. Due to its high electronegativity and reactivity, Fluorine can form compounds with almost all elements in the periodic table, except the noble gases He, Ne, and Ar.

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Most popular questions from this chapter

Predict the atomic number and ground-state electron configuration of the next member of the alkali metals after francium.

Write a balanced equation that predicts the reaction of rubidium (Rb) with (a) \(\mathrm{H}_{2} \mathrm{O}(l)\) (b) \(\mathrm{Cl}_{2}(g)\) (c) \(\mathrm{H}_{2}(g)\)

In halogen displacement reactions a halogen element can be generated by oxidizing its anions with a halogen element that lies above it in the periodic table. This means that there is no way to prepare elemental fluorine, because it is the first member of Group 7A. Indeed, for years the only way to prepare elemental fluorine was to oxidize \(\mathrm{F}\) ions by electrolytic means. Then, in \(1986,\) a chemist reported that by reacting potassium hexafluoromanganate(IV) \(\left(\mathrm{K}_{2} \mathrm{MnF}_{6}\right)\) with antimony pentafluoride \(\left(\mathrm{SbF}_{5}\right)\) at \(150^{\circ} \mathrm{C},\) he had generated elemental fluorine. Balance the following equation representing the reaction: $$ \mathrm{K}_{2} \mathrm{MnF}_{6}+\mathrm{SbF}_{5} \longrightarrow \mathrm{KSbF}_{6}+\mathrm{MnF}_{3}+\mathrm{F}_{2} $$

State whether each of the following properties of the representative elements generally increases or decreases (a) from left to right across a period and (b) from top to bottom within a group: metallic character, atomic size, ionization energy, acidity of oxides.

As a group, the noble gases are very stable chemically (only \(\mathrm{Kr}\) and Xe are known to form compounds). Use the concepts of shielding and the effective nuclear charge to explain why the noble gases tend to neither give up electrons nor accept additional electrons.
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