Textbook Question
A common form of elemental phosphorus is the tetrahedral P4 molecule, where all four phosphorus atoms are equivalent:
(b) How many P-P bonds are there in the molecule?
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Ch.8 - Basic Concepts of Chemical Bonding
Brown14th EditionChemistry: The Central ScienceISBN: 9780134414232
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Table of contents
- Ch.1 - Introduction: Matter, Energy, and Measurement140
- Ch.2 - Atoms, Molecules, and Ions192
- Ch.3 - Chemical Reactions and Reaction Stoichiometry172
- Ch.4 - Reactions in Aqueous Solution156
- Ch.5 - Thermochemistry151
- Ch.6 - Electronic Structure of Atoms137
- Ch.7 - Periodic Properties of the Elements127
- Ch.8 - Basic Concepts of Chemical Bonding143
- Ch.9 - Molecular Geometry and Bonding Theories167
- Ch.10 - Gases147
- Ch.11 - Liquids and Intermolecular Forces97
- Ch.12 - Solids and Modern Materials129
- Ch.13 - Properties of Solutions126
- Ch.14 - Chemical Kinetics175
- Ch.15 - Chemical Equilibrium107
- Ch.16 - Acid-Base Equilibria127
- Ch.17 - Additional Aspects of Aqueous Equilibria133
- Ch.18 - Chemistry of the Environment88
- Ch.19 - Chemical Thermodynamics140
- Ch.20 - Electrochemistry137
- Ch.21 - Nuclear Chemistry99
- Ch.22 - Chemistry of the Nonmetals66
- Ch.23 - Transition Metals and Coordination Chemistry69
- Ch.24 - The Chemistry of Life: Organic and Biological Chemistry11
Brown14th EditionChemistry: The Central ScienceISBN: 9780134414232Not the one you use?Change textbook
Chapter 8, Problem 105c2
Acetylene (C2H2) and nitrogen (N2) both contain a triple bond, but they differ greatly in their chemical properties. (c) Write balanced chemical equations for the complete oxidation of N2 to form N2O5(g) and of acetylene to form CO2(g) and H2O(g). Write a balanced chemical equation for the complete oxidation of acetylene to form CO2(g) and H2O(g).
Verified step by step guidance1
Identify the reactants and products for the oxidation reactions. For nitrogen, the reactant is \( N_2 \) and the product is \( N_2O_5 \). For acetylene, the reactant is \( C_2H_2 \) and the products are \( CO_2 \) and \( H_2O \).
Write the unbalanced chemical equations for each reaction. For nitrogen: \( N_2 + O_2 \rightarrow N_2O_5 \). For acetylene: \( C_2H_2 + O_2 \rightarrow CO_2 + H_2O \).
Balance the nitrogen oxidation equation. Start by balancing the nitrogen atoms, then balance the oxygen atoms. Adjust the coefficients to ensure the same number of each type of atom on both sides of the equation.
Balance the acetylene oxidation equation. Begin by balancing the carbon atoms, then the hydrogen atoms, and finally the oxygen atoms. Adjust the coefficients to ensure the same number of each type of atom on both sides of the equation.
Verify that both equations are balanced by counting the atoms of each element on both sides of the equations. Ensure that the total number of atoms for each element is equal on the reactant and product sides.
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Key Concepts
Here are the essential concepts you must grasp in order to answer the question correctly.
Balancing Chemical Equations
Balancing chemical equations is essential in chemistry to ensure that the law of conservation of mass is upheld. This means that the number of atoms of each element must be the same on both sides of the equation. To balance an equation, coefficients are adjusted in front of the chemical formulas, allowing for the correct stoichiometric relationships between reactants and products.
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Balancing Chemical Equations
Combustion Reactions
Combustion reactions involve the reaction of a substance with oxygen to produce energy, typically in the form of heat and light. For hydrocarbons like acetylene, complete combustion results in carbon dioxide (CO2) and water (H2O) as products. Understanding the stoichiometry of these reactions is crucial for writing balanced equations and predicting the amounts of reactants and products involved.
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Oxidation States
Oxidation states (or oxidation numbers) are used to keep track of electron transfer in chemical reactions, particularly in redox reactions. In the context of the question, nitrogen in N2 has an oxidation state of 0, while in N2O5, it has a +5 oxidation state. Recognizing changes in oxidation states helps in understanding the nature of the reaction and the products formed during oxidation.
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Related Practice
Textbook Question
A common form of elemental phosphorus is the tetrahedral P4 molecule, where all four phosphorus atoms are equivalent:
Draw a Lewis structure for a linear P4 molecule that satisfies the octet rule. Does this molecule have resonance structures?
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Textbook Question
Acetylene (C2H2) and nitrogen (N2) both contain a triple bond, but they differ greatly in their chemical properties. (e) Both N2 and C2H2 possess triple bonds with quite high bond enthalpies (Table 8.3). Calculate the enthalpy of hydrogenation per mole for both compounds: acetylene plus H2 to make methane, CH4; nitrogen plus H2 to make ammonia, NH3.
Textbook Question
Acetylene (C2H2) and nitrogen (N2) both contain a triple bond, but they differ greatly in their chemical properties. (b) By referring to Appendix C, look up the enthalpies of formation of acetylene and nitrogen. Which compound is more stable?
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Textbook Question
One scale for electronegativity is based on the concept that the electronegativity of any atom is proportional to the ionization energy of the atom minus its electron affinity: electronegativity = k1I - EA2, where k is a proportionality constant. (b) Why are both ionization energy and electron affinity relevant to the notion of electronegativity?
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