The relationship between intermolecular force in a liquid and its boiling point and critical temperature has to be outlined. The reason for the greater critical temperature of water has to be outlined. Concept Introduction: Intermolecular force Intermolecular force refers to the attractive forces between the molecules of a substance. It is the force which holds the molecules together . Many physical properties of the substance such as – melting point, boiling point, surface tension, viscosity etc., are influenced by the strength of intermolecular force present in the substance. The three types of intermolecular forces are – London dispersion force, dipole-dipole force and Hydrogen bonding. They are collectively known as Van der Waals forces. London dispersion forces exist in all types of molecules. This is the force responsible for the condensation of non-polar compounds into liquids or solids under low temperature. Dipole-dipole forces exist in polar covalent compounds. Hydrogen bonding exists in polar covalent compounds containing Fluorine, Oxygen or Nitrogen directly bonded to Hydrogen. The strength of intermolecular forces is, London dispersion forces < Dipole-dipole forces < Hydrogen bonding Boiling point The temperature at which the vapor pressure of liquid becomes equal to atmospheric pressure is boiling point of the liquid . During boiling the molecules in liquid phase partly evaporates to vapor phase. The molecules in vapor phase and that of the liquid phase remain in equilibrium with each other. Critical temperature Critical temperature is defined as the temperature above which a gas cannot be liquefied irrespective of the external pressure.
The relationship between intermolecular force in a liquid and its boiling point and critical temperature has to be outlined. The reason for the greater critical temperature of water has to be outlined. Concept Introduction: Intermolecular force Intermolecular force refers to the attractive forces between the molecules of a substance. It is the force which holds the molecules together . Many physical properties of the substance such as – melting point, boiling point, surface tension, viscosity etc., are influenced by the strength of intermolecular force present in the substance. The three types of intermolecular forces are – London dispersion force, dipole-dipole force and Hydrogen bonding. They are collectively known as Van der Waals forces. London dispersion forces exist in all types of molecules. This is the force responsible for the condensation of non-polar compounds into liquids or solids under low temperature. Dipole-dipole forces exist in polar covalent compounds. Hydrogen bonding exists in polar covalent compounds containing Fluorine, Oxygen or Nitrogen directly bonded to Hydrogen. The strength of intermolecular forces is, London dispersion forces < Dipole-dipole forces < Hydrogen bonding Boiling point The temperature at which the vapor pressure of liquid becomes equal to atmospheric pressure is boiling point of the liquid . During boiling the molecules in liquid phase partly evaporates to vapor phase. The molecules in vapor phase and that of the liquid phase remain in equilibrium with each other. Critical temperature Critical temperature is defined as the temperature above which a gas cannot be liquefied irrespective of the external pressure.
Solution Summary: The author explains the relationship between intermolecular force in a liquid and its boiling point and critical temperature.
The relationship between intermolecular force in a liquid and its boiling point and critical temperature has to be outlined.
The reason for the greater critical temperature of water has to be outlined.
Concept Introduction:
Intermolecular force
Intermolecular force refers to the attractive forces between the molecules of a substance. It is the force which holds the molecules together. Many physical properties of the substance such as – melting point, boiling point, surface tension, viscosity etc., are influenced by the strength of intermolecular force present in the substance.
The three types of intermolecular forces are – London dispersion force, dipole-dipole force and Hydrogen bonding. They are collectively known as Van der Waals forces.
London dispersion forces exist in all types of molecules. This is the force responsible for the condensation of non-polar compounds into liquids or solids under low temperature.
Dipole-dipole forces exist in polar covalent compounds. Hydrogen bonding exists in polar covalent compounds containing Fluorine, Oxygen or Nitrogen directly bonded to Hydrogen.
The temperature at which the vapor pressure of liquid becomes equal to atmospheric pressure is boiling point of the liquid. During boiling the molecules in liquid phase partly evaporates to vapor phase. The molecules in vapor phase and that of the liquid phase remain in equilibrium with each other.
Critical temperature
Critical temperature is defined as the temperature above which a gas cannot be liquefied irrespective of the external pressure.
Which does NOT describe a mole? A. a unit used to count particles directly, B. Avogadro’s number of molecules of a compound, C. the number of atoms in exactly 12 g of pure C-12, D. the SI unit for the amount of a substance
5
What would the complete ionic reaction be if aqueous solutions of potassium sulfate and barium acetate were mixed?
ed
of
Select one:
O a
2 K SO4 + Ba2 +2 C₂H3O21
K+SO4 + Ba2+ + 2 C2H3O21
K+SO42 + Ba2 +2 C2H3O2
BaSO4 +2 K+ + 2 C2H3O
estion
Ob.
O c.
Od.
2 K SO4 +Ba2 +2 C₂H₂O₂
BaSO4 + K+ + 2 C2H3O
BaSO4 + K + 2 C2H301
→Ba² +SO42 +2 KC2H3O
s page
(28 pts.) 7. Propose a synthesis for each of the following transformations. You must include the
reagents and product(s) for each step to receive full credit. The number of steps is provided.
(OC 4)
4 steps
4 steps
OH
b.
Author:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell
Author:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell