explain why elemental chlorine (Cl2) is a gas at room temperature and pressure while iodine (I2) is a solid despite the...
explain why elemental chlorine (Cl2) is a gas at room temperature and pressure while iodine (I2) is a solid despite the fact that both have similar lewis structures. explain based on the relative strength of their intermolecular forces of attraction
Homework Answers
Basically the I2 molecule is heavier than the Cl2 molecule.
So the dispersion forces (London forces) are strong enough in I2 to keep it in the solid state where as Cl2 dispersion forces are not strong enough. So, Cl2 is in gas state.
The Dispersion forces in Cl2 are not strong enough to keep the molecules held together. So that Cl2 molecule is in gas state and I2 molecule is in solid state.
Relative strength of inter molecular forces of attraction of I2 molecule is higher than that of Cl2 molecule.
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explain why elemental chlorine (Cl2) is a gas at room temperature and pressure while iodine (I2) is a solid despite the...
explain why elemental chlorine (Cl2) is a gas at room tempeature and pressure while iodine (I2)...
explain why elemental chlorine (Cl2) is a gas at room tempeature and pressure while iodine (I2) is a solid despite the fact that both have similar lewis structures. explain based on the relative strength of their intermolecular forced of attraction.
A. Physical State of Halogens at Room Temperature 1. Samples of the elemental halogens are provided....
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Consider the reaction between iodine gas and chlorine gas to form iodine monochloride: I2(g)+Cl2(g)⇌2ICl(g)Kp=81.9 (at 298...
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1. Select the two compounds that are more likely to be a gas at room temperature...
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Elemental iodine (12) is a solid at room temperature. What is the dominant attractive force that exists between 12 molecules in the solid? London forces Hydrogen bonds Halogen forces Dipole dipole forces Covalent bonds
INTERMOLECULAR FORCES INTRODUCTION LEARNING OBJECTIVES To relate the effecet of intermolecular forces on relative melting points and vapour pressures of some organic substances THEORY Weak attractive forces that occur between individual molecules in substances are called intermolecular forces. These include London dispersion forces, dipole-dipole forces and hydrogen-bonding forces. Collectively, the three types of intermolecular forces are referred to as Van der Waals forces. These attractive forces are much weaker than the chemical bonds between atoms in a molecule. Note that...
Applications 5.91 Would behave more like an ideal gas at Skor SOK? Explain your reasoning. 592 Would co behave more like an ideal gas at 2 atm or 20 atm? Explain your reasoning. The Liquid State Foundations 5.93 Compare the strength of intermolecular forces in liquids with those in gases. Compare the strength of intermolecular forces in liquids with those in solids. What is the relationship between the temperature of a liquid and the vapor pressure of that liquid? 5.96...
2. Identify the strongest type of intermolecular forces in acetone, ethanol, water and hexane. (Structures listed on page 15.) Experiment 2 Intermolecular Forces There are three general types of intermolecular forces. All substances exhibit London Dispersion Forces (LDF), and they are generally the weakest of the three types. These London forces are due to the attractions between small, temporary dipoles that arise from the constant, random movement of the electrons in a substance. As molar mass increases, the size of...
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