### Comparing Bromine (Br₂) and Chlorine (Cl₂)#### Question:Compare bromine (Br₂) and chlorine (Cl₂). One is a gas at room temperature while the other is a liquid. Which do you think is more likely to be a liquid and why?### Options:1. **Br₂** because Br-Br bonds are stronger than Cl-Cl bonds and require more energy to break upon vaporization.2. **Cl₂** because Cl-Cl bonds are stronger than Br-Br bonds and require more energy to break upon vaporization.3. **Br₂** because the intermolecular forces (IMFs) in bromine are stronger than the IMFs in chlorine and require more energy to overcome upon vaporization.4. **Cl₂** because the IMFs in chlorine are stronger than the IMFs in bromine and require more energy to overcome upon vaporization.#### Answer Choices:- ○ 3- ○ 2- ○ 1- ○ 4There are no graphs or diagrams included in this image. The text focuses on comparing the molecular properties and intermolecular forces between bromine and chlorine to determine which is more likely to be in a liquid state at room temperature.

At room temperature, chlorine exists as gas where as bromine exists as liquid.

Compare bromine (Br₂) and chlorine (Cl₂). One is a gas at room temperature while the other is a liquid. Which do you think is more likely to be a liquid and why? 1. Br₂ because Br-Br bonds are stronger than CI-CI bonds and require more energy to break upon vaporization. 2. Cl₂ because CI-CI bonds are stronger than Br-Br bonds and require more energy to break upon vaporization. 3. Br₂ because the IMFs in bromine are stronger than the IMFs in chlorine and require more energy to overcome upon vaporization. 4. Cl₂ because the IMFs in chlorine are stronger than the IMFs in bromine and require more energy to overcome upon vaporization. O 3 02 01 04

Compare bromine (Br₂) and chlorine (Cl₂). One is a gas at room temperature while the other is a liquid. Which do you think is more likely to be a liquid and why? 1. Br₂ because Br-Br bonds are stronger than CI-CI bonds and require more energy to break upon vaporization. 2. Cl₂ because CI-CI bonds are stronger than Br-Br bonds and require more energy to break upon vaporization. 3. Br₂ because the IMFs in bromine are stronger than the IMFs in chlorine and require more energy to overcome upon vaporization. 4. Cl₂ because the IMFs in chlorine are stronger than the IMFs in bromine and require more energy to overcome upon vaporization. O 3 02 01 04

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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