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Chapter 8: Problem 106

A student is given samples of three elements, \(\mathrm{X}, \mathrm{Y}\), and \(\mathrm{Z}\), which could be an alkali metal, a member of Group \(4 \mathrm{~A},\) and a member of Group \(5 \mathrm{~A} .\) She makes the following observations: Element X has a metallic luster and conducts electricity. It reacts slowly with hydrochloric acid to produce hydrogen gas. Element \(Y\) is a light-yellow solid that does not conduct electricity. Element \(Z\) has a metallic luster and conducts electricity. When exposed to air, it slowly forms a white powder. A solution of the white powder in water is basic. What can you conclude about the elements from these observations?

Short Answer

Expert verified
Based on the properties and reactions described, it could be concluded that Element X is an alkali metal, Element Y is from Group 5A (the Nitrogen group), and Element Z is part of Group 4A (the Carbon group).

Step by step solution

01

Identify characteristics of Element X

Element X has metallic luster, conducts electricity and reacts slowly with hydrochloric acid to produce hydrogen gas. These characteristics suggest that Element X is an alkali metal. Alkali metals are characterized by their metallic qualities and noticeably slow reaction rate with acid to produce hydrogen.
02

Identify characteristics of Element Y

Element Y is described as a light-yellow solid and a non-conductor. The non-metallic properties of this element suggest that it belongs to Group 5A, known as the Nitrogen group. These elements are found in various physical states including gas, liquid, and solids. The most well-known element in this group (Nitrogen) is a gas, but solids are also found, as mentioned (for example, phosphorus), which may appear in several colors, including yellow-white.
03

Identify characteristics of Element Z

Element Z has a metallic luster, conducts electricity, and forms a basic water solution when its white powder is exposed to air. This matches the properties of Group 4A elements, known as the Carbon group. Some elements in this group appear metallic and can form basic (alkaline) oxides, leading to a basic solution in water.

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Most popular questions from this chapter

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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