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Chapter 12: Problem 40

Classify the solid states of the elements in the second period of the periodic table.

Short Answer

Expert verified
The solids in the second period of the periodic table include Lithium (Li), Beryllium (Be), Boron (B), and Carbon (C). In room temperature, Lithium and Beryllium have a metallic lattice structure, Boron has a rhombohedral lattice and Carbon exists as diamond and graphite.

Step by step solution

01

Identify the Elements of the Second Period

The first step is to establish what elements are in the second period of the periodic table. The second period includes the elements: Lithium (Li), Beryllium (Be), Boron (B), Carbon (C), Nitrogen (N), Oxygen (O), Fluorine (F) and Neon (Ne).
02

Determine the States of Elements

Among these elements, only Nitrogen (N), Oxygen (O), Fluorine (F), and Neon (Ne) are gases at room temperature. Therefore, the remaining elements, including Lithium (Li), Beryllium (Be), Boron (B), and Carbon (C) are all solids at room temperature.
03

Classifying the Solid State

Now, for the elements that are solid at room temperature, further classify them: Lithium (Li) and Beryllium (Be) are alkali and alkaline earth metals respectively, and both have a metallic lattice structure. Boron (B) is a metalloid having a rhombohedral lattice structure. Carbon (C) is a non-metal, which at room temperature exists in two forms. One is diamond, where each carbon atom is connected to four other carbon atoms to form a giant covalent structure. The other is graphite, another form of carbon, it has layers of carbon atoms arranged in hexagons, with weak forces between the layers.

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Key Concepts

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

Solid States
When we talk about solid states, we are describing how particles within an element or compound organize themselves in a rigid structure. This structural arrangement is known as a lattice, where atoms, ions, or molecules are fixed in successive patterns to form a defined shape and volume.

Solid states can be found in different forms, such as metallic, covalent, and molecular solids.
  • Metallic solids: These solids consist of metal atoms sharing a "sea" of electrons, giving the metal its characteristic properties such as electrical conductivity and malleability. Examples include Lithium (Li) and Beryllium (Be) in the second period.
  • Covalent solids: In covalent solids, atoms are linked by covalent bonds forming a giant network. A classic example is Diamond, an allotrope of Carbon (C), where each carbon atom is covalently bonded to four others forming an extremely hard structure.
  • Molecular solids: These consist of molecules held together by intermolecular forces like hydrogen bonding or van der Waals forces rather than true bonds, and hence are relatively soft. They are not common among second period elements classified as solids under normal conditions.
Understanding these classifications helps us to better grasp how different elements behave under normal conditions.
Second Period Elements
The second period of the Periodic Table comprises elements that play a crucial role in many core scientific concepts and real-world applications. This period includes eight elements: Lithium (Li), Beryllium (Be), Boron (B), Carbon (C), Nitrogen (N), Oxygen (O), Fluorine (F), and Neon (Ne).

Here are a few key points about these elements:
  • Li and Be: These are classified as metals with notable metallic properties. They are good conductors of electricity, strong, and shiny.
  • B and C: Boron acts as a metalloid, displaying properties of both metals and non-metals. Carbon, famous for its allotropes (like graphite and diamond), is a non-metal essential for organic chemistry.
  • N, O, F, and Ne: These elements are gases at room temperature. Nitrogen and Oxygen are vital to life, while Fluorine is highly reactive, used in many chemical reactions. Neon, known for its inactivity, is used in lighting.
Every element in the second period has unique features due to their increasing number of protons and electrons as you move across the period.
Covalent Structures
Covalent structures arise from covalent bonds, where atoms share pairs of electrons to achieve stable electronic configurations. These structures can significantly vary in form, from small molecules to large networks like in diamond or graphite.

In the context of the second period elements, covalent structures can be seen in the form of:
  • Giant Covalent Structures: These involve endless covalent bonds creating an "infinite" lattice, as seen in diamond, where carbon atoms bond in a tetrahedral arrangement, providing extreme hardness and high melting points.
  • Layered Covalent Structures: Graphite illustrates this type where carbon atoms form planar hexagonal rings. The layers slide over each other effortlessly because of weak forces between the layers, making graphite useful as a lubricant and in pencils.
    These diverse covalent structures explain why elements like Carbon have such varied applications and properties.

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Most popular questions from this chapter

Arrange the following compounds in order of increasing boiling point: \(\mathrm{RbF}, \mathrm{CO}_{2}, \mathrm{CH}_{3} \mathrm{OH}, \mathrm{CH}_{3} \mathrm{Br}\). Explain your arrangement.

Which of the following phase transitions gives off more heat: (a) 1 mole of steam to 1 mole of water at \(100^{\circ} \mathrm{C}\) or \((\mathrm{b}) 1\) mole of water to \(1 \mathrm{~mole}\) of ice at \(0^{\circ} \mathrm{C} ?\)

Argon crystallizes in the face-centered cubic arrangement at \(40 \mathrm{~K}\). Given that the atomic radius of argon is \(191 \mathrm{pm},\) calculate the density of solid argon.

Describe, with examples, these types of crystals: (a) ionic crystals, (b) covalent crystals, (c) molecular crystals. (d) metallic crystals.

The liquid-vapor boundary line in the phase diagram of any substance always stops abruptly at a certain point. Why?
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