Textbook Question
Look at the location of elements A, B, C, and D in the following periodic table:
(a) Write the formula of the simplest binary hydride of each element.
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 21
Look at the location of elements A, B, C, and D in the following
periodic table:
(c) Which hydrides react with water to give H2 gas? Write a balanced net ionic equation for each reaction.
Verified step by step guidance1
Identify the elements A, B, C, and D on the periodic table. Determine their group and period.
Recognize that elements in groups 1 and 2 (alkali and alkaline earth metals) typically form hydrides that react with water to produce hydrogen gas.
For each element that forms a hydride reacting with water, write the general reaction: MH_x + H_2O \rightarrow M(OH)_x + H_2, where M is the metal and x is the number of hydrogens in the hydride.
Convert the general reaction into a net ionic equation by removing spectator ions. For example, for a group 1 metal hydride, the net ionic equation is: MH + H_2O \rightarrow M^+ + OH^- + H_2.
Ensure the net ionic equations are balanced in terms of both mass and charge.
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Key Concepts
Here are the essential concepts you must grasp in order to answer the question correctly.
Hydrides
Hydrides are compounds formed between hydrogen and another element. They can be classified into different types, such as ionic, covalent, and metallic hydrides. The reactivity of hydrides with water varies based on their composition; for instance, alkali metal hydrides typically react vigorously with water to produce hydrogen gas and a corresponding hydroxide.
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Ionic Hydrides
Net Ionic Equations
A net ionic equation represents the chemical species that are involved in a reaction, excluding spectator ions that do not participate in the reaction. This type of equation is useful for simplifying reactions in aqueous solutions, allowing chemists to focus on the actual chemical changes occurring. To write a net ionic equation, one must first write the balanced molecular equation and then remove the spectator ions.
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Reactivity of Elements in Water
The reactivity of elements with water is influenced by their position in the periodic table. Alkali metals and some alkaline earth metals readily react with water, often producing hydrogen gas and a hydroxide. Understanding the trends in reactivity, such as increasing reactivity down a group, is essential for predicting which hydrides will react with water to release hydrogen gas.
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Related Practice
Textbook Question
Look at the location of elements A, B, C, and D in the following periodic table:
(d) Which hydrides react with water to give an acidic solution, and which give a basic solution?
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.
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?