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Chapter 22: Problem 12

Identify cach of the following clements as a metal, nonmetal, or metalloid: (a) gallium, (b) molybdenum, (c) tellurium, (d) arsenic, (c) xenon, (f) ruthenium.

Short Answer

Expert verified
(a) Gallium is a metal. (b) Molybdenum is a metal. (c) Tellurium is a metalloid. (d) Arsenic is a metalloid. (e) Xenon is a nonmetal. (f) Ruthenium is a metal.

Step by step solution

01

(a) Gallium

Gallium is in Group 13 and Period 4 of the Periodic Table. Elements in Group 13 are commonly referred to as the 'Boron Group' or 'Post-transition metals'. In this case, gallium is a metal.
02

(b) Molybdenum

Molybdenum is in Group 6 and Period 5 of the Periodic Table. Elements in Group 6 are classified as 'Transition Metals'. Therefore, molybdenum is a metal.
03

(c) Tellurium

Tellurium is in Group 16 and Period 5 of the Periodic Table. Elements in Group 16 are referred to as 'Chalcogens'. Tellurium is a metalloid because it has properties that fall between metals and nonmetals.
04

(d) Arsenic

Arsenic is in Group 15 and Period 4 of the Periodic Table. Elements in Group 15 are known as 'Pnictogens'. Arsenic, having properties of both metals and nonmetals, is a metalloid.
05

(e) Xenon

Xenon is in Group 18 and Period 5 of the Periodic Table. Elements in Group 18 are part of 'Noble Gases' and are characterized by their full electron shell configuration. In this case, xenon is a nonmetal.
06

(f) Ruthenium

Ruthenium is in Group 8 and Period 5 of the Periodic Table. Elements in Group 8 are classified as 'Transition Metals'. Hence, ruthenium is a metal.

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Key Concepts

These are the key concepts you need to understand to accurately answer the question.

Metal Nonmetal Metalloid Characteristics
Understanding the characteristics of metals, nonmetals, and metalloids is essential when exploring the Periodic Table. Metals are typically shiny, good conductors of heat and electricity, malleable (can be hammered into thin sheets), and ductile (can be drawn into wires). Most elements on the table fall into this category. Nonmetals, on the other hand, are usually not lustrous, are poor conductors of heat and electricity, and are brittle in their solid form. They are found on the right side of the Periodic Table.

Metalloids have properties that fall somewhere between metals and nonmetals. They can conduct electricity better than nonmetals but not as well as metals, which makes them useful as semiconductors. The staircase-shaped line starting at boron (B) and extending down to polonium (Po) typically marks the border between metals and nonmetals and helps to identify metalloids.

Characteristic Examples

  • Metals: Gallium (Ga), Ruthenium (Ru)
  • Nonmetals: Xenon (Xe)
  • Metalloids: Tellurium (Te), Arsenic (As)
Transition Metals
Transition metals are elements found in Groups 3 through 12 of the Periodic Table. These metals are known for their ability to form various oxidation states and colorful compounds. One of the defining features of transition metals is their d-orbitals that are partially filled with electrons. This unique electron arrangement allows them to form an extensive array of complex ions and compounds.

Some common characteristics of transition metals include high melting and boiling points, high densities, and the presence of magnetic properties in some of them. They are also notably good conductors of heat and electricity and often have a high tensile strength. Transition metals play vital roles in industry and biochemistry, with many serving as catalysts in reactions.

Element Examples

  • Molybdenum (Mo)
  • Ruthenium (Ru)
Noble Gases
Noble gases constitute Group 18 of the Periodic Table and are odorless, colorless, and monatomic gases under standard conditions. Their unique feature is a full valence electron shell, which renders them largely inert and unreactive. This property makes noble gases very stable, and they typically do not form compounds with other elements.

Historically called inert gases, noble gases have since been found to form a limited number of compounds under specific conditions. They are used in various applications, such as neon lights, inert gas shielding in welding, and as refrigerants. Xenon, a noble gas, is used in high-intensity lamps and has even been used in medical imaging.

Element Example

  • Xenon (Xe)
Group Period Elements
In the Periodic Table, elements are organized into groups and periods. A Group refers to the vertical columns and represents elements that have similar chemical properties and the same number of electrons in their outermost shell. There are 18 groups in the Periodic Table. A Period refers to the horizontal rows and indicates the energy level of the valence electrons of the elements within that row; there are seven periods.

The position of an element in a group or period provides valuable information regarding its reactivity, electronegativity, atomic size, and other chemical properties. By examining an element's group and period, we can predict its behavior in chemical reactions and its role in various compounds.

Classifications Based on Group and Period

  • Gallium (Ga) - Group 13, Period 4: A metal
  • Tellurium (Te) - Group 16, Period 5: A metalloid
  • Argon (Ar) - Group 18, Period 3: A noble gas, specifically a nonmetal

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Most popular questions from this chapter

In aqueous solution, hydrogen sulfide reduces (a) \(\mathrm{Fe}^{3+}\) to \(\mathrm{Fe}^{2+}\), (b) \(\mathrm{Br}_{2}\) to \(\mathrm{Br}^{-}\), (c) \(\mathrm{MnO}_{4}^{-}\)to \(\mathrm{Mn}^{2+}\), (d) \(\mathrm{HNO}_{3}\) to \(\mathrm{NO}_{2}\). In all cases, under appropriate conditions, the product is elemental sulfur. Write a balanced net ionic equation for each reaction.

SOLUTION Analyze We must write balanced nuclear equations in which the masses and charges of reactants and products are equal. Plan We can begin by writing the complete chemical symbols for the nuclei and decay particles that are given in the problem. Solve (a) The information given in the question can be summarized as $$ { }_{80}^{201} \mathrm{Hg}+{ }_{-1}^{0} \mathrm{e} \longrightarrow{ }_{Z}^{A} \mathrm{X} $$ The mass numbers must have the same sum on both sides of the equation: $$ 201+0=A $$ Thus, the product nucleus must have a mass number of 201. Similarly, balancing the atomic numbers gives $$ 80-1=Z $$ Thus, the atomic number of the product nucleus must be 79 , which identifies it as gold (Au): $$ { }_{80}^{201} \mathrm{Hg}+{ }_{-1}^{0} \mathrm{e} \longrightarrow{ }_{79}^{201} \mathrm{Au} $$ (b) In this case we must determine what type of particle is emitted in the course of the radioactive decay: $$ { }_{90}^{231} \mathrm{Th} \longrightarrow{ }_{91}^{231} \mathrm{~Pa}+{ }_{\mathrm{Z}}^{\mathrm{X}} \mathrm{X} $$ From \(231=231+A\) and \(90=91+Z\), we deduce \(A=0\) and \(Z=-1\). According to Table \(21.2\), the particle with these characteristics is the beta particle (electron). We therefore write $$ { }_{90}^{231} \mathrm{Th} \longrightarrow{ }_{91}^{231} \mathrm{~Pa}+{ }_{-1}^{0} \mathrm{e} \text { or } \quad{ }_{90}^{231} \mathrm{Th} \longrightarrow{ }_{91}^{231} \mathrm{~Pa}+\beta^{-} $$

What does hydrogen have in common with the halogens? Explain.

Give a reason why hydrogen might be placed along with the group lA elements of the periodic table.

The dissolved oxygen present in any highly pressurized, high-temperature steam boiler can be extremely corrosive to its metal parts. Hydrazine, which is completely miscible with water, can be added to remove oxygen by reacting with it to form nitrogen and water. (a) Write the balanced equation for the reaction between gaseous hydrazine and oxygen. (b) Calculate the enthalpy change accompanying this reaction. (c) Oxygen in air dissolves in water to the extent of \(9.1\) Ppm at \(20^{\circ} \mathrm{C}\) at sea level. How many grams of hydrazine are required to react with all the oxygen in \(3.0 \times 10^{4} \mathrm{~L}\) (the volume of a small swimming pool) under these conditions?
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