Textbook Question
The following pictures represent various silicate anions. Write the formula and charge of each anion.
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 22.20b
Look at the location of elements A, B, C, and D in the following periodic table:
Which hydride has the lowest boiling point?
Verified step by step guidance1
Identify the elements A, B, C, and D on the periodic table.
Determine the group and period of each element to understand their properties.
Recall that hydrides are compounds formed between hydrogen and another element.
Consider the type of hydride each element forms: ionic, covalent, or metallic.
Understand that boiling points of hydrides are influenced by molecular weight, intermolecular forces, and hydrogen bonding.
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Key Concepts
Here are the essential concepts you must grasp in order to answer the question correctly.
Periodic Trends
Periodic trends refer to the predictable patterns in the properties of elements as you move across or down the periodic table. Key trends include atomic size, ionization energy, electronegativity, and boiling points. Understanding these trends helps in predicting the behavior of elements and their compounds, including hydrides.
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00:38
Periodic Trends
Hydride Properties
Hydrides are compounds formed between hydrogen and other elements. The boiling points of hydrides can vary significantly based on the electronegativity and size of the other element involved. Generally, hydrides of lighter elements tend to have lower boiling points, while those of heavier elements exhibit higher boiling points due to increased van der Waals forces.
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02:00Ionic Hydrides
Intermolecular Forces
Intermolecular forces are the forces of attraction or repulsion between molecules. These forces, including hydrogen bonding, dipole-dipole interactions, and London dispersion forces, play a crucial role in determining the physical properties of substances, such as boiling points. Stronger intermolecular forces typically lead to higher boiling points, while weaker forces result in lower boiling points.
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Related Practice
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?
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
Select the group 4A element that best fits each of the following descriptions.
b. Is the least dense semimetal
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.