Textbook Question
The following models represent the structures of binary hydrides
of second-row elements:
(a) Identify the nonhydrogen atom in each case, and write the molecular formula for each hydride.
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 22.85
Explain why the properties of boron differ so markedly from the properties of the other group 3A elements.
Verified step by step guidance1
Step 1: Understand the periodic table. The periodic table is organized in such a way that elements with similar properties are grouped together. Boron is in Group 3A, along with aluminum, gallium, indium, and thallium.
Step 2: Consider the atomic structure. Boron has an atomic number of 5, which means it has 5 protons and, in its neutral state, 5 electrons. These electrons are arranged in two energy levels: 2 in the first level and 3 in the second. This configuration is different from the other elements in Group 3A, which have more energy levels and more electrons.
Step 3: Consider the size of the atom. Boron is a relatively small atom compared to the other elements in Group 3A. This means that the electrons are closer to the nucleus and more strongly attracted to it, which affects the chemical properties of the element.
Step 4: Consider the type of bonding. Boron is a metalloid, which means it has properties of both metals and nonmetals. It forms covalent bonds, unlike the other elements in Group 3A, which are metals and form ionic bonds.
Step 5: Consider the electron deficiency. Boron has fewer electrons than it has orbitals available for bonding, making it electron deficient. This leads to the formation of compounds with unusual structures and properties, further distinguishing boron from the other elements in Group 3A.
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Key Concepts
Here are the essential concepts you must grasp in order to answer the question correctly.
Group 3A Elements
Group 3A elements, also known as Group 13 in the periodic table, include boron, aluminum, gallium, indium, and thallium. These elements share similar valence electron configurations, typically having three electrons in their outer shell. However, their properties can vary significantly due to differences in atomic size, electronegativity, and the presence of d-orbitals in heavier elements, which influence their chemical behavior.
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Group 3A vs. Group 2A Elements
Boron’s Unique Properties
Boron is a metalloid, which gives it distinct properties compared to the metals in Group 3A. It has a high melting point, is a poor conductor of electricity, and forms covalent compounds, unlike the more metallic character of aluminum and other heavier elements. Boron's small atomic size and high ionization energy contribute to its unique behavior, making it less reactive and more stable in certain compounds.
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Chemical Bonding and Structure
The type of bonding and molecular structure significantly influence the properties of elements. Boron often forms covalent bonds and complex structures like boranes, which are different from the ionic or metallic bonding seen in aluminum and other heavier Group 3A elements. This difference in bonding leads to variations in physical properties such as hardness, melting points, and reactivity.
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Related Practice
Textbook Question
Which of the following oxides will be more soluble in acidic solution? (LO 22.14)
(a) SiO2 (b) NO2
(c) BaO (d) B2O3
Textbook Question
In what forms is oxygen commonly found in nature?
Textbook Question
Describe the structures of the white and red allotropes of phosphorus, and explain why white phosphorus is so reactive.
Textbook Question
Compare some of the physical properties of H2S, NaH, and PdHx.
Textbook Question
Which of the group 4A elements have allotropes with the diamond structure? Which have metallic allotropes? How does the variation in the structure of the group 4A elements illustrate how metallic character varies down a periodic group?