(a)
Interpretation:
The types of intermolecular forces present in
Concept Introduction:
The forces of attraction between the molecules are the forces that keep them close or bonded together and they are called intermolecular forces.
There are generally 3 types of intermolecular forces-
- London-dispersion forces- The electrons within a molecule are constantly moving and sometimes this leads to uneven distribution of electrons for a very small interval of time. This unsymmetrical distribution can distort the nearby molecule also leading to the induced dipole−induced dipole interactions between the two molecules. As all the molecules have moving electrons, thus all types of molecules exhibit these forces.
- Dipole-dipole interactions- When two dipoles (polar molecules) come nearby, then the positive end of one dipole interacts with the negative end of the other dipole or vice-versa. Such interactions are referred to as the dipole-dipole interactions.
- Hydrogen bonding-It exists when hydrogen bonded to a highly electronegative atom such as O, F or N is attracted by the lone pair on another electronegative atom.
(b)
Interpretation:
The types of intermolecular forces present in
Concept Introduction:
The forces of attraction between the molecules are the forces that keep them close or bonded together and they are called intermolecular forces.
There are generally 3 types of intermolecular forces-
- London-dispersion forces- The electrons within a molecule are constantly moving and sometimes this leads to uneven distribution of electrons for a very small interval time. This unsymmetrical distribution can distort the nearby molecule also leading to the induced dipole −induced dipole interactions between the two molecules. As all the molecules have moving electrons, thus all types of molecules exhibit these forces.
- Dipole-dipole interactions- When two dipoles (polar molecules) come nearby, then the positive end of one dipole interacts with the negative end of the other dipole or vice-versa. Such interactions are referred to as the dipole-dipole interactions.
- Hydrogen bonding-It exists when hydrogen bonded to a highly electronegative atom such as O, F or N is attracted by the lone pair on another electronegative atom.
(c)
Interpretation:
The types of intermolecular forces present in
Concept Introduction:
The forces of attraction between the molecules are the forces that keep them close or bonded together and they are called intermolecular forces.
There are generally 3 types of intermolecular forces-
- London-dispersion forces- The electrons within a molecule are constantly moving and sometimes this leads to uneven distribution of electrons for a very small interval time. This unsymmetrical distribution can distort the nearby molecule also leading to the induced dipole −induced dipole interactions between the two molecules. As all the molecules have moving electrons, thus all types of molecules exhibit these forces.
- Dipole-dipole interactions- When two dipoles (polar molecules) come nearby, then the positive end of one dipole interacts with the negative end of the other dipole or vice-versa. Such interactions are referred to as the dipole-dipole interactions.
- Hydrogen bonding-It exists when hydrogen bonded to a highly electronegative atom such as O, F or N is attracted by the lone pair on another electronegative atom.
(d)
Interpretation:
The types of intermolecular forces present in
Concept Introduction:
The forces of attraction between the molecules are the forces that keep them close or bonded together and they are called intermolecular forces.
There are generally 3 types of intermolecular forces-
- London-dispersion forces- The electrons within a molecule are constantly moving and sometimes this leads to uneven distribution of electrons for a very small interval time. This unsymmetrical distribution can distort the nearby molecule also leading to the induced dipole −induced dipole interactions between the two molecules. As all the molecules have moving electrons, thus all types of molecules exhibit these forces.
- Dipole-dipole interactions- When two dipoles (polar molecules) come nearby, then the positive end of one dipole interacts with the negative end of the other dipole or vice-versa. Such interactions are referred to as the dipole-dipole interactions.
- Hydrogen bonding-It exists when hydrogen bonded to a highly electronegative atom such as O, F or N is attracted by the lone pair on another electronegative atom.
(e)
Interpretation:
The types of intermolecular forces present in
Concept Introduction:
The forces of attraction between the molecules are the forces that keep them close or bonded together and they are called intermolecular forces.
There are generally 3 types of intermolecular forces-
- London-dispersion forces- The electrons within a molecule are constantly moving and sometimes this leads to uneven distribution of electrons for a very small interval time. This unsymmetrical distribution can distort the nearby molecule also leading to the induced dipole −induced dipole interactions between the two molecules. As all the molecules have moving electrons, thus all types of molecules exhibit these forces.
- Dipole-dipole interactions- When two dipoles (polar molecules) come nearby, then the positive end of one dipole interacts with the negative end of the other dipole or vice-versa. Such interactions are referred to as the dipole-dipole interactions.
- Hydrogen bonding-It exists when hydrogen bonded to a highly electronegative atom such as O, F or N is attracted by the lone pair on another electronegative atom.
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Chapter 7 Solutions
General, Organic, and Biological Chemistry - 4th edition
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- 8.43 Identify the kinds of intermolecular forces (London dispersion, dipoledipole, or hydrogen bonding) that are the most important in each of the following substances. (a) methane (CH4) , (b) methanol (CH4OH) , (c) chloroform (CHCl3) , (d) benzene (C6H6) , (e) ammonia (NH3) , (f) sulfur dioxide (SO2)arrow_forwardConsider the iodine monochloride molecule, ICI. Because chlorine is more electronegative than iodine, this molecule is a dipole. How would you expect iodine monochloride molecules in the gaseous state to orient themselves with respect to each other as the sample is cooled and the molecules begin to aggregate? Sketch the orientation you would expect.arrow_forward
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