* Shade a pair of circles representing atoms that are covalently bonded together. * Breaking intramolecular forces (covalent bonds) requires 192.9 kJ Brz(g) → 2Br (g) Is this reaction exothermic (releasing energy) or endothermic (absorbing energy)? Why? Explain 8. * Draw a curve around a pair of molecules that are held together in the liquid phase. * Breaking intermolecular forces requires 30.9 kJ Br2(1) → Br2 (g) Is this reaction exothermic or endothermic? Why? Explain
* Shade a pair of circles representing atoms that are covalently bonded together. * Breaking intramolecular forces (covalent bonds) requires 192.9 kJ Brz(g) → 2Br (g) Is this reaction exothermic (releasing energy) or endothermic (absorbing energy)? Why? Explain 8. * Draw a curve around a pair of molecules that are held together in the liquid phase. * Breaking intermolecular forces requires 30.9 kJ Br2(1) → Br2 (g) Is this reaction exothermic or endothermic? Why? Explain
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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![The image provides an educational exercise on chemical bonding, focusing on intramolecular and intermolecular forces. It features two sets of diagrams and instructions.
1. **Top Diagram: Intramolecular Forces**
- Illustration: A box filled with circles, some of which are shaded in pairs, representing atoms covalently bonded.
- Instruction: "Shade a pair of circles representing atoms that are covalently bonded together."
- Task: Breaking intramolecular forces (covalent bonds) requires 192.9 kJ, illustrated by the reaction:
\[
\text{Br}_2(g) \rightarrow 2\text{Br}(g)
\]
- Question: Determine if this reaction is exothermic (releasing energy) or endothermic (absorbing energy), and explain why.
2. **Bottom Diagram: Intermolecular Forces**
- Illustration: Another box filled with circles, with a curve drawn around pairs of circles, representing molecules held together in the liquid phase.
- Instruction: "Draw a curve around a pair of molecules that are held together in the liquid phase."
- Task: Breaking intermolecular forces requires 30.9 kJ, depicted by the reaction:
\[
\text{Br}_2(l) \rightarrow \text{Br}_2(g)
\]
- Question: Determine if this reaction is exothermic or endothermic, and explain why.
These illustrations and exercises test the understanding of energy changes associated with chemical bonding and phase changes.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F6d43ccb7-7359-44f4-9027-62e63eace4bf%2F7bd7bd6e-b1e6-46f9-8ead-d68bb9f2c02d%2Feq4gxan_processed.jpeg&w=3840&q=75)
Transcribed Image Text:The image provides an educational exercise on chemical bonding, focusing on intramolecular and intermolecular forces. It features two sets of diagrams and instructions.
1. **Top Diagram: Intramolecular Forces**
- Illustration: A box filled with circles, some of which are shaded in pairs, representing atoms covalently bonded.
- Instruction: "Shade a pair of circles representing atoms that are covalently bonded together."
- Task: Breaking intramolecular forces (covalent bonds) requires 192.9 kJ, illustrated by the reaction:
\[
\text{Br}_2(g) \rightarrow 2\text{Br}(g)
\]
- Question: Determine if this reaction is exothermic (releasing energy) or endothermic (absorbing energy), and explain why.
2. **Bottom Diagram: Intermolecular Forces**
- Illustration: Another box filled with circles, with a curve drawn around pairs of circles, representing molecules held together in the liquid phase.
- Instruction: "Draw a curve around a pair of molecules that are held together in the liquid phase."
- Task: Breaking intermolecular forces requires 30.9 kJ, depicted by the reaction:
\[
\text{Br}_2(l) \rightarrow \text{Br}_2(g)
\]
- Question: Determine if this reaction is exothermic or endothermic, and explain why.
These illustrations and exercises test the understanding of energy changes associated with chemical bonding and phase changes.
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