Textbook Question
The following pictures represent structures of the hydrides of four second-row elements:
(1)
(2)
(3)
(4)
(b) Which compound has the lowest boiling point?
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 22.89b
Select the group 4A element that best fits each of the following descriptions.
b. Is the least dense semimetal
Verified step by step guidance1
Identify the elements in group 4A (14) of the periodic table: Carbon (C), Silicon (Si), Germanium (Ge), Tin (Sn), and Lead (Pb).
Determine which of these elements are classified as semimetals (metalloids).
Recognize that Silicon (Si) and Germanium (Ge) are the semimetals in group 4A.
Compare the densities of Silicon and Germanium to determine which is the least dense.
Select the element with the lower density as the least dense semimetal in group 4A.
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Key Concepts
Here are the essential concepts you must grasp in order to answer the question correctly.
Group 4A Elements
Group 4A of the periodic table includes elements such as carbon (C), silicon (Si), germanium (Ge), tin (Sn), and lead (Pb). These elements exhibit a range of properties, including varying densities and metallic characteristics. Understanding the position of these elements in the periodic table helps in predicting their behavior and properties.
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Main Group Elements: Density Example
Semimetals
Semimetals, or metalloids, are elements that have properties intermediate between metals and nonmetals. They typically exhibit some metallic luster and electrical conductivity but are brittle and not malleable. In Group 4A, germanium (Ge) and silicon (Si) are commonly recognized as semimetals, making them important in electronics and materials science.
Density of Elements
Density is a physical property defined as mass per unit volume, and it varies significantly among elements. In the context of Group 4A, the density of semimetals can be compared to identify which is the least dense. For example, silicon has a lower density than germanium, making it the least dense semimetal in this group.
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Related Practice
Textbook Question
The following models represent the structures of binary hydrides of second-row elements:
b. Draw an electron-dot structure for each hydride. For which hydride is there a problem in drawing the structure? Explain.
Textbook Question
Look at the location of elements A, B, C, and D in the following periodic table:
Which hydride has the lowest boiling point?
Textbook Question
In the following pictures of binary hydrides, ivory spheres
represent H atoms or ions, and burgundy spheres represent
atoms or ions of the other element.
(1)
(2)
(3)
(4)
(b) What is the oxidation state of hydrogen in compounds (1), (2), and (3)? What is the oxidation state of the other
element?
Textbook Question
Consider the six second- and third-row elements in groups 4A–6A of the periodic table:
Possible structures for the binary fluorides of each of these elements in its highest oxidation state are shown below.
(b) Explain why the fluorides of nitrogen and phosphorus have different molecular structures but the fluorides of carbon and silicon have the same molecular structure.
Textbook Question
Complete and balance the equation for each of the following reactions.
b. Ca(s) + H2O(l) →