Textbook Question
Write balanced equations for the formation of the following compounds from their elements.(c) Uranium hexafluoride (a solid at 25 °C)
Ch.22 - The Main Group Elements
McMurry8th EditionChemistryISBN: 9781292336145
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Table of contents
- Ch.1 - Chemical Tools: Experimentation & Measurement170
- Ch.2 - Atoms, Molecules & Ions160
- Ch.3 - Mass Relationships in Chemical Reactions169
- Ch.4 - Reactions in Aqueous Solution199
- Ch.5 - Periodicity & Electronic Structure of Atoms102
- Ch.6 - Ionic Compounds: Periodic Trends and Bonding Theory92
- Ch.7 - Covalent Bonding and Electron-Dot Structures61
- Ch.8 - Covalent Compounds: Bonding Theories and Molecular Structure59
- Ch.9 - Thermochemistry: Chemical Energy122
- Ch.10 - Gases: Their Properties & Behavior155
- Ch.11 - Liquids & Phase Changes54
- Ch.12 - Solids and Solid-State Materials73
- Ch.13 - Solutions & Their Properties120
- Ch.14 - Chemical Kinetics98
- Ch.15 - Chemical Equilibrium125
- Ch.16 - Aqueous Equilibria: Acids & Bases110
- Ch.17 - Applications of Aqueous Equilibria147
- Ch.18 - Thermodynamics: Entropy, Free Energy & Equilibrium86
- Ch.19 - Electrochemistry154
- Ch.20 - Nuclear Chemistry96
- Ch.21 - Transition Elements and Coordination Chemistry156
- Ch.22 - The Main Group Elements187
- Ch.23 - Organic and Biological Chemistry51
Chapter 22, Problem 98
How do the structures and properties of elemental silicon and germanium differ from those of tin and lead?
Verified step by step guidance1
Step 1: Understand the position of silicon, germanium, tin, and lead in the periodic table. Silicon (Si) and germanium (Ge) are in Group 14 and are metalloids, while tin (Sn) and lead (Pb) are also in Group 14 but are metals.
Step 2: Examine the crystal structures. Silicon and germanium both crystallize in a diamond cubic structure, which is a characteristic of covalent network solids. Tin and lead, on the other hand, have metallic structures; tin can exist in two forms: white tin (metallic) and gray tin (similar to silicon and germanium). Lead has a face-centered cubic structure.
Step 3: Compare the bonding and electronic properties. Silicon and germanium have strong covalent bonds due to their tetrahedral bonding, leading to high melting points and semiconducting properties. Tin and lead, being metals, have metallic bonds, which allow for electrical conductivity and malleability.
Step 4: Discuss the physical properties. Silicon and germanium are brittle and have high melting points due to their covalent network structures. Tin and lead are softer, more malleable, and have lower melting points due to their metallic bonding.
Step 5: Consider the applications and implications of these properties. Silicon and germanium are used in semiconductors and electronic devices due to their semiconducting properties. Tin is used in alloys and coatings, while lead is used in batteries and radiation shielding, reflecting their metallic nature.
Key Concepts
Here are the essential concepts you must grasp in order to answer the question correctly.
Elemental Properties of Group 14 Elements
Silicon (Si) and germanium (Ge) are metalloids, while tin (Sn) and lead (Pb) are metals, all belonging to Group 14 of the periodic table. The properties of these elements vary significantly due to their position in the periodic table, affecting their conductivity, malleability, and reactivity. Metalloids like Si and Ge exhibit intermediate properties, making them useful in semiconductor applications, whereas metals like Sn and Pb are characterized by high electrical conductivity and malleability.
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Crystal Structure and Bonding
Silicon and germanium crystallize in a diamond cubic structure, which contributes to their semiconductor properties, allowing them to control electrical conductivity. In contrast, tin and lead have a more metallic bonding structure, which results in different physical properties such as ductility and luster. The differences in crystal structure and bonding lead to distinct behaviors in electrical and thermal conductivity among these elements.
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Oxidation States and Chemical Reactivity
The oxidation states of these elements influence their chemical reactivity. Silicon and germanium typically exhibit oxidation states of +4 and +2, forming covalent compounds, while tin and lead can exhibit +2 and +4 oxidation states, often forming ionic compounds. This difference in oxidation states affects their reactivity with other elements and compounds, leading to varied applications in industry and technology.
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