Textbook Question
Write a balanced net ionic equation for the reaction of the amphoteric oxide ZnO with:
a. Hydrochloric acid
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 22.31a
The following pictures represent various silicate anions. Write the formula and charge of each anion.
Verified step by step guidance1
insert step 1> Identify the type of silicate structure for each anion in the pictures. Common types include orthosilicates, pyrosilicates, cyclic silicates, chain silicates, and sheet silicates.
insert step 2> Determine the basic formula for each type of silicate anion. For example, orthosilicates have the formula SiO_4^{4-}, pyrosilicates have Si_2O_7^{6-}, etc.
insert step 3> Count the number of silicon (Si) and oxygen (O) atoms in each anion structure to verify the specific formula.
insert step 4> Calculate the charge of each anion by considering the oxidation state of silicon (+4) and oxygen (-2), and ensuring the overall charge matches the typical charge for that silicate type.
insert step 5> Write down the chemical formula and charge for each silicate anion based on your analysis from the previous steps.
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Key Concepts
Here are the essential concepts you must grasp in order to answer the question correctly.
Silicate Anions
Silicate anions are polyatomic ions composed of silicon and oxygen, typically represented by the general formula SiO4^n-. They form the basis of silicate minerals and can vary in structure and charge depending on the arrangement of silicon and oxygen atoms. Understanding the different types of silicate anions, such as orthosilicate (SiO4^4-) and pyrosilicate (Si2O7^6-), is essential for identifying their formulas and charges.
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Test for Anions
Polyatomic Ions
Polyatomic ions are ions that consist of two or more atoms bonded together, carrying a net charge due to the loss or gain of electrons. They play a crucial role in chemical reactions and compound formation. Recognizing the common polyatomic ions, including their formulas and charges, is vital for accurately writing the formulas of silicate anions and understanding their behavior in chemical contexts.
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Charge Balance in Ionic Compounds
In ionic compounds, the total positive charge must balance the total negative charge to achieve electrical neutrality. This principle is fundamental when writing chemical formulas, as it dictates the ratio of cations to anions. For silicate anions, knowing their charges allows for the correct combination with cations to form stable compounds, ensuring that the overall charge of the resulting formula is zero.
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Related Practice
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)
(a) Identify each binary hydride as ionic, covalent, or interstitial.
(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.
(a) Identify the nonfluorine atom in each case, and write the molecular formula of each fluoride.
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
Look at the location of elements A, B, C, and D in the following periodic table:
Which hydride has the lowest boiling point?