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Chapter 4: Problem 50

What is a metalloid? Where are the metalloids found on the periodic table?

Short Answer

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A metalloid is an element that possesses properties of both metals and non-metals, and they are also known as semimetals. On the periodic table, metalloids are found along the diagonal line separating metals and non-metals, known as the "stair-step line" or "metalloid staircase" in the p-block. Common metalloids include boron (B), silicon (Si), germanium (Ge), arsenic (As), antimony (Sb), tellurium (Te), and polonium (Po). Their properties include intermediate electrical conductivity, variable reactivity, lustrous yet brittle appearance, ability to form alloys with metals, and acting as semiconductors.

Step by step solution

01

Definition of Metalloids

A metalloid is an element that possesses properties of both metals and non-metals. They are also commonly referred to as 'semimetals'. Metalloids generally display a combination of metallic characteristics, such as electrical conductivity, and non-metallic characteristics, such as brittleness.
02

Metalloids on the Periodic Table

Metalloids can be found on the periodic table, lying along a diagonal line that separates metals and non-metals. This line is often referred to as the "stair-step line" or "metalloid staircase," and it is located in the p-block of the periodic table. Elements touching or in close proximity to this line are considered metalloids.
03

List of Metalloids

There are commonly seven elements considered as metalloids, which include: 1. Boron (B) 2. Silicon (Si) 3. Germanium (Ge) 4. Arsenic (As) 5. Antimony (Sb) 6. Tellurium (Te) 7. Polonium (Po) These elements are found in Groups 13, 14, 15, and 16 of the periodic table, along the "stair-step line."
04

Properties of Metalloids

Some properties of metalloids that distinguish them from metals and non-metals include: 1. They have intermediate electrical conductivity that can be modified by changing their temperature, pressure, or by adding impurities. 2. They are generally less reactive than metals and more reactive than non-metals. Their reactivity depends on the particular element and the conditions in which they are present. 3. Metalloids often possess a lustrous or metallic appearance, but they are brittle and break easily. This contrasts with metals, which are generally more malleable and ductile when solid. 4. Some metalloids can form alloys with metals, while others cannot. 5. They can act as semiconductors, making them widely used in electronics and modern technology.

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Key Concepts

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

Periodic Table
The periodic table is a powerful tool in chemistry and science. It categorizes all known elements based on their atomic number, electron configurations, and recurring chemical properties. This organization makes it easier to understand and predict the properties of elements and their interactions with each other.
Elements in the periodic table are arranged in order of increasing atomic number from left to right and top to bottom.
  • Each element is placed in a specific location due to its atomic structure.
  • The table is divided into rows, known as periods, and columns, known as groups or families.
Periods represent elements with the same number of electron shells, while groups contain elements with similar configurations in their outer electron shell, resulting in similar chemical properties.
The table's design also separates metals, non-metals, and metalloids. Metalloids lie along the diagonal 'stair-step' line, bridging the metals and non-metals. Their unique position signifies their dual properties.
Semiconductors
Semiconductors are materials that have electrical conductivity between that of conductors (like metals) and insulators (like non-metals). Metalloids, especially silicon and germanium, are typical semiconductors.
  • They are the backbone of modern electronics, found in devices like computers, smartphones, and solar cells.
  • Semiconductors have the unique ability to control electrical current flow, enabling the creation of complex electrical circuits.
By adding impurities鈥攁 process called doping鈥攖he electrical properties of semiconductors can be altered. Doping involves introducing small amounts of other elements to boost conductivity.
This flexibility makes semiconductors essential for integrated circuits, which are critical for the operation of electronic devices, ranging from simple calculators to advanced microprocessors.
Properties of Elements
Each element possesses distinct properties that determine its chemical behavior and its role in the natural world. These properties are generally categorized into physical and chemical properties.
  • Physical properties: Include appearance, state of matter, melting and boiling points, density, and electrical and thermal conductivity.
  • Chemical properties: Describe an element's reactivity and ability to form compounds, such as acidity/basicity, oxidation states, and types of bonds formed.
For example, metalloids share properties of both metals and non-metals.
They may appear shiny and conduct electricity like metals but often behave like non-metals in chemical reactions. This duality allows them to serve specific functions in technology, such as their use in semiconductors. Understanding these properties helps chemists and engineers to choose the appropriate element for specific applications, maximizing the efficiency and performance of the materials used in technology and industry.

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Most popular questions from this chapter

What two common types of particles are found in the nucleus of the atom? What are the relative charges of these particles? What are the relative masses of these particles?

For the following pairs of ions, use the concept that a chemical compound must have a net charge of zero to predict the formula of the simplest compound that the ions are most likely to form. a. \(\mathrm{Fe}^{3+}\) and \(\mathrm{P}^{3-}\) b. \(\mathrm{Fe}^{3+}\) and \(\mathrm{S}^{2-}\) c. \(\mathrm{Fe}^{3+}\) and \(\mathrm{Cl}^{-}\) d. \(\mathrm{Mg}^{2+}\) and \(\mathrm{Cl}^{-}\) e. \(\mathrm{Mg}^{2+}\) and \(\mathrm{O}^{2-}\) f. \(\mathrm{Mg}^{2+}\) and \(\mathrm{N}^{3-}\) g. \(\mathrm{Na}^{+}\) and \(\mathrm{P}^{3-}\) h. \(\mathrm{Na}^{+}\) and \(\mathrm{S}^{2-}\)

Positive ions are called __________, whereas negative ions are called _________.

For the following processes that show the formation of ions, use the periodic table to indicate the number of electrons and protons present in both the ion and the neutral atom from which the ion is made.a. \(\mathrm{Ca} \rightarrow \mathrm{Ca}^{2+}+2 \mathrm{e}^{-}\) b. \(P+3 e^{-} \rightarrow P^{3-}\) c. \(\mathrm{Br}+\mathrm{e}^{-} \rightarrow \mathrm{Br}^{-}\) d. \(\mathrm{Fe} \rightarrow \mathrm{Fe}^{3+}+3 \mathrm{e}^{-}\) e. \(A l \rightarrow A l^{3+}+3 e^{-}\) f. \(\mathrm{N}+3 \mathrm{e}^{-} \rightarrow \mathrm{N}^{3-}\)

How are ions produced from an atom? Does the formation of a simple ion involve changes to the atom's nucleus?
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