Textbook Question
Using the shorthand notation of Figure 22.9, draw the structure of the silicate anion in:
(a) K4SiO4 (b) Ag10Si4O13
What is the relationship between the charge on the anion and the number of terminal O atoms?
Ch.22 - The Main Group Elements
Chapter 22, Problem 26
Look at the location of elements A, B, C, and D in the following periodic table:
(a) Write the formula of the oxide that has each of these elements in its highest oxidation state.
Verified step by step guidance1
Identify the group number of each element A, B, C, and D in the periodic table.
Determine the highest oxidation state for each element based on its group number.
Recall that the highest oxidation state of an element in its oxide is typically equal to its group number.
Write the chemical formula for the oxide by balancing the charges of the element and oxygen.
Ensure that the total charge of the compound is zero by adjusting the subscripts of the elements in the formula.
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Key Concepts
Here are the essential concepts you must grasp in order to answer the question correctly.
Oxidation States
Oxidation states indicate the degree of oxidation of an atom in a compound, reflecting the number of electrons lost or gained. Elements can exhibit multiple oxidation states, particularly transition metals, and the highest oxidation state is often associated with the element's ability to form stable compounds. Understanding oxidation states is crucial for predicting the formulas of oxides formed by elements.
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02:42
Oxidation Numbers
Periodic Table Trends
The periodic table organizes elements based on their atomic number and electron configuration, revealing trends in properties such as electronegativity, ionization energy, and atomic radius. Elements in the same group typically exhibit similar chemical behaviors, including their common oxidation states. Recognizing these trends helps in determining the highest oxidation states of elements A, B, C, and D.
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00:38Periodic Trends
Formation of Oxides
Oxides are compounds formed when elements react with oxygen, and their formulas depend on the oxidation states of the elements involved. The general formula for an oxide can be represented as E_xO_y, where E is the element and x and y are determined by the oxidation states. Knowing how to derive these formulas based on the highest oxidation states of the elements is essential for answering the question.
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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)
(c) Which compounds yield H2 gas when they are mixed together?
Textbook Question
In the following pictures of oxides, red spheres represent O atoms or ions, and green spheres represent atoms or ions of a second- or third-row element in its highest oxidation state.
(1)
(2)
(3)
(b) Identify each oxide as ionic or covalent.
Textbook Question
The following models represent the structures of binary
oxides of second- and third-row elements in their highest
oxidation states:
(a) Identify the non-oxygen atom in each case, and write the molecular formula for each oxide.