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.
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 22.21b
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?
Verified step by step guidance1
Identify the general rule for the oxidation state of hydrogen in binary hydrides, which is typically +1 when bonded to non-metals and -1 when bonded to metals.
Examine compound (1) and determine if hydrogen is bonded to a metal or non-metal to assign its oxidation state.
Examine compound (2) and determine if hydrogen is bonded to a metal or non-metal to assign its oxidation state.
Examine compound (3) and determine if hydrogen is bonded to a metal or non-metal to assign its oxidation state.
For each compound, use the known oxidation state of hydrogen to deduce the oxidation state of the other element, ensuring the sum of oxidation states equals the overall charge of the compound, which is zero for neutral compounds.
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Key Concepts
Here are the essential concepts you must grasp in order to answer the question correctly.
Oxidation State
The oxidation state, or oxidation number, is a theoretical charge assigned to an atom in a compound, reflecting its degree of oxidation or reduction. It helps in understanding electron transfer in chemical reactions. For hydrogen, the oxidation state is typically +1 when bonded to nonmetals and -1 when bonded to metals.
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Oxidation Numbers
Binary Hydrides
Binary hydrides are compounds formed between hydrogen and one other element, typically a metal or a nonmetal. The properties and oxidation states of hydrogen in these compounds can vary based on the nature of the other element. Understanding the type of bonding and the electronegativity of the other element is crucial for determining oxidation states.
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Electronegativity
Electronegativity is a measure of an atom's ability to attract and hold onto electrons in a chemical bond. It plays a significant role in determining the oxidation states of elements in compounds. In binary hydrides, the relative electronegativities of hydrogen and the other element dictate whether hydrogen will have a positive or negative oxidation state.
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Related Practice
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
Select the group 4A element that best fits each of the following descriptions.
b. Is the least dense semimetal
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) →
Textbook Question
Which compound in each of the following pairs is more ionic?
(b) P4O6 or Ga2O3