List all of the different intermolecular interactions (IMFs) that are possible in a solution of CaCl2...
List all of the different intermolecular interactions (IMFs) that are possible in a solution of CaCl2 in methanol (CH3OH). Explain how/why these are possible
Homework Answers
Answer: CaCl2 has inonic bond within the molecule.
Methanol (CH3OH) has hydrogen bonding between another molecule while within the molecule it has covalent linkage.
When CaCl2 in dissolved in methanol the solubility is due to formation of ion-dipole forces. This is due to fact that this force develops because of the interaction of ions and polar molecule.
The slightly negative Oxygen of methanol is attarcted towards Ca2+ while slightly positive Hydrogen gets attracted to Cl-.
Add Answer to:
List all of the different intermolecular interactions (IMFs)
that are possible in a solution of CaCl2...
Several methanol (CH3OH) dimers are drawn below, and several proposed intermolecular bonding interactions are highlight...
Several methanol (CH3OH) dimers are drawn below, and several
proposed intermolecular bonding interactions are highlighted in
green. if highlighted interaction is a valid hydrogen bond, leave
it unaltered. if the interaction IS NOT a valid hydrogen bond,
delete the gree bond to yiled two non-interacting alcohol
molecules.
11. Consider an ideal liquid mixture (solution) of A and B, where the intermolecular interactions between...
11. Consider an ideal liquid mixture (solution) of A and B, where the intermolecular interactions between A molecules are same strength as the intermolecular interactions between B molecules, and these are the same size as intermolecular interactions between A and B molecules. This means that upon mixing, AH = 0. Now for comparison, consider a nonideal mixture solution) of A and B, where the intermolecular interactions between A and B molecules are much weaker than the intermolecular interactions between either...
INTERMOLECULAR FORCES INTRODUCTION LEARNING OBJECTIVES To relate the effecet of intermolecular fo...
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...
1. Describe and compare the motion and interactions of molecules in the three different phases of...
1. Describe and compare the motion and interactions of molecules in the three different phases of matter 2. Explain the relationship between temperature and intermolecular forces as it affects the phase of matter. 3. List the steps necessary to determine the intermolecular forces present in a pure substance.
For the following compounds and b.p. data, consider the intermolecular forces involved (and review the chapter...
For the following compounds and b.p. data, consider the intermolecular forces involved (and review the chapter on intermolecular forces in a first year chemistry textbook if necessary). methane (CH4) b.p. = -164 0C decane (C10H22) b.p. = 174 0C methanol (CH3OH) b.p. = 65 0C 1-decanol (C10H21OH) b.p. = 229 0C explain why the b.p. of methanol is nearly 230 0C higher than that of methane; explain why the b.p. of 1-decanol is 55 0C higher than that...
1. All of the following are electrolytes in solution except a) CaCl2 b) CH3OH c) Na3PO4...
1. All of the following are electrolytes in solution except a) CaCl2 b) CH3OH c) Na3PO4 d) NH4I e) Zn (NO3)2
b) Describe the strongest intermolecular interactions occurring between carboxylic acids and explain how the affects the...
b) Describe the strongest intermolecular interactions occurring between carboxylic acids and explain how the affects the boiling point of carboxylic acids.
Lecture 3. Intermolecular interactions. What sort of changes are related with monomolecular reactions? Under what conditions...
Lecture 3. Intermolecular interactions. What sort of changes are related with monomolecular reactions? Under what conditions can a bimolecular reaction become a first order reaction? What is activation energy of a chemical reaction? What is reflected by the factor A in the Arrhenius equation? What are the possible causes of kinks in the Arrhenius plot? How does Arrhenius plot look like and what parameters are used for its expression? What is the van’t Hoff factor? What are its values for...
Consider 1.00 mole of each of the following substances: 1) NaCl (sodium chloride) 2) CaCl2 (calcium...
Consider 1.00 mole of each of the following substances: 1) NaCl (sodium chloride) 2) CaCl2 (calcium chloride) 3) CH3OH (methanol) 4) Naphthalene (C10H8) Answer the following questions: A) Which one of the above substances would likely not change the freezing point of water at all? Explain. B) Which one of the above substances would likely lower the freezing point of water the most? Explain.
In class work. Help? Date Lab Partner EXPERIMENT 12 Intermolecular Forces substance | tmax (°C) |...
In class work. Help?
Date Lab Partner EXPERIMENT 12 Intermolecular Forces substance | tmax (°C) | tmin (°C) ?T (tmax-tmin) Ethanol l-propanol Predicted Explanation I-butanol npentane Methanol n-hexane The molecular weights for n-pentane and 1-butanol are similar but the liquids have significantly different ?? values. Explain why the values are different I. 2. Which of the alcohols studied has the strongest intermolecular forces of attraction? Explain
Several methanol (CH3OH) dimers are drawn below, and several
proposed intermolecular bonding interactions are highlighted in
green. if highlighted interaction is a valid hydrogen bond, leave
it unaltered. if the interaction IS NOT a valid hydrogen bond,
delete the gree bond to yiled two non-interacting alcohol
molecules.
11. Consider an ideal liquid mixture (solution) of A and B, where the intermolecular interactions between A molecules are same strength as the intermolecular interactions between B molecules, and these are the same size as intermolecular interactions between A and B molecules. This means that upon mixing, AH = 0. Now for comparison, consider a nonideal mixture solution) of A and B, where the intermolecular interactions between A and B molecules are much weaker than the intermolecular interactions between either...
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...
1. Describe and compare the motion and interactions of molecules in the three different phases of matter 2. Explain the relationship between temperature and intermolecular forces as it affects the phase of matter. 3. List the steps necessary to determine the intermolecular forces present in a pure substance.
1. All of the following are electrolytes in solution except a) CaCl2 b) CH3OH c) Na3PO4 d) NH4I e) Zn (NO3)2
b) Describe the strongest intermolecular interactions occurring between carboxylic acids and explain how the affects the boiling point of carboxylic acids.
In class work. Help?
Date Lab Partner EXPERIMENT 12 Intermolecular Forces substance | tmax (°C) | tmin (°C) ?T (tmax-tmin) Ethanol l-propanol Predicted Explanation I-butanol npentane Methanol n-hexane The molecular weights for n-pentane and 1-butanol are similar but the liquids have significantly different ?? values. Explain why the values are different I. 2. Which of the alcohols studied has the strongest intermolecular forces of attraction? Explain
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