Textbook Question
Compare and contrast the properties of ammonia and phosphine.
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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 22.95
Give an example of an ionic carbide. What is the oxidation state of carbon in this substance?
Verified step by step guidance1
Identify the type of carbide: Ionic carbides are typically formed with metals from groups 1 and 2 of the periodic table.
Choose an example of an ionic carbide: Calcium carbide (CaC2) is a common example.
Determine the oxidation state of calcium: In CaC2, calcium is a group 2 metal, so it typically has an oxidation state of +2.
Set up the equation for oxidation states: The sum of oxidation states in a neutral compound must be zero. Therefore, for CaC2, the equation is: +2 (for Ca) + 2x (for each C) = 0.
Solve for the oxidation state of carbon: Rearrange the equation to find the oxidation state of carbon, x, in CaC2.
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Key Concepts
Here are the essential concepts you must grasp in order to answer the question correctly.
Ionic Compounds
Ionic compounds are formed when atoms transfer electrons, resulting in the formation of positively charged cations and negatively charged anions. These oppositely charged ions attract each other, creating a stable ionic bond. Understanding ionic compounds is essential for identifying their properties and predicting their behavior in chemical reactions.
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Ionic Compounds Naming
Carbides
Carbides are compounds composed of carbon and a less electronegative element, often a metal. They can be classified into ionic, covalent, and metallic carbides, with ionic carbides typically containing carbon in a -4 oxidation state. Recognizing the type of carbide helps in determining the oxidation states of the elements involved.
Oxidation States
The oxidation state of an element in a compound indicates the degree of oxidation or reduction it has undergone. It is a useful concept for understanding electron transfer in chemical reactions. In ionic carbides, the oxidation state of carbon can vary, but in ionic carbides like calcium carbide (CaC2), carbon has an oxidation state of -4, reflecting its role as an anion.
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Related Practice
Textbook Question
Using the shorthand notation of Figure 22.9, draw the structure of the cyclic silicate anion in which four SiO4 tetrahedra share O atoms to form an eight-membered ring of alternating Si and O atoms. Give the formula and charge of the anion.
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Textbook Question
Which of the following elements (X) will form a covalent hydride with the formula XH3 that is a gas at room temperature? (LO 22.4)
(a) Al (b) As (c) Ba (d) Se
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Textbook Question
Draw the electron-dot structure for CO, CO2, and CO32–, and predict which substance will have the strongest carbon–oxygen bond.
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Textbook Question
What is the hybridization and geometry around carbon atoms in graphene? Explain why graphene is an excellent conductor of electricity.
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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?
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