Intermolcular
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the difference of physical properties (boiling point, freezing point) based on differences in intermolecular forces (van der Waals forces, London forces, and hydrogen bonding)
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Okay, let's break this down step-by-step:
* We are given: 1 mole of ice at -25°C
* Heat of fusion of ice = 6.01 kJ/mol
* Heat of vaporization of water = 40.7 kJ/mol
* Specific heat of ice = 2.09 J/g°C
* Specific heat of water = 4.18 J/g°C
1) Heat ice from -25°C to 0°C:
Q = m * c * ΔT
Q = (18 g) * (2.09 J/g°C) * (25°C) = 903 J
2) Heat
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Okay, let's break this down step-by-step:
* We are given: 1 mole of ice at -25°C
* Heat of fusion of ice = 6.01 kJ/mol
* Heat of vaporization of water = 40.7 kJ/mol
* Specific heat of ice = 2.09 J/g°C
* Specific heat of water = 4.18 J/g°C
1) Heat ice from -25°C to 0°C:
Q = m * c * ΔT
Q = (18 g) * (2.09 J/g°C) * (25°C) = 903 J
2) Heat
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Question 16 Given the following table of data, explain in terms of the Lennard-Jones potential, why the melting points and cohesive energies of noble gases increase with molecular weight [time4 minutes] Melting Point (K) 24 84 Solid Ne Ar Kr ?? Cohesive Energy (kJ/mol) 2.5 8.5 12 16 161
Solution
The melting and boiling points of noble gases are very low in comparison to those of other substances of comparable atomic and molecular masses. This indicates that only weak van der Waals forces or weak London dispersion forces are present between the atoms of the noble gases in the liquid or the solid state.
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intermolecular_forces.ppt
Okay, let's break this down step-by-step:
* We are given: 1 mole of ice at -25°C
* Heat of fusion of ice = 6.01 kJ/mol
* Heat of vaporization of water = 40.7 kJ/mol
* Specific heat of ice = 2.09 J/g°C
* Specific heat of water = 4.18 J/g°C
1) Heat ice from -25°C to 0°C:
Q = m * c * ΔT
Q = (18 g) * (2.09 J/g°C) * (25°C) = 903 J
2) Heat
intern_forc_biceps2.ppt
Okay, let's break this down step-by-step:
* We are given: 1 mole of ice at -25°C
* Heat of fusion of ice = 6.01 kJ/mol
* Heat of vaporization of water = 40.7 kJ/mol
* Specific heat of ice = 2.09 J/g°C
* Specific heat of water = 4.18 J/g°C
1) Heat ice from -25°C to 0°C:
Q = m * c * ΔT
Q = (18 g) * (2.09 J/g°C) * (25°C) = 903 J
2) Heat
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The document discusses different types of intermolecular forces including London dispersion forces, dipole-dipole forces, dipole-induced dipole forces, ion-dipole interactions, and hydrogen bonding. It provides examples of how these forces influence the properties of substances such as their melting and boiling points. Hydrogen bonding specifically is described as being an important intermolecular force that influences the properties of water, alcohols, and other polar molecules.
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- 1. Chemistry
- 2. Water ? Boiling point
- 3. have the same boiling point?? X Y
- 4. the difference of physical properties (boiling point, freezing point) based on differences in intermolecular forces (van der Waals forces, London forces, and hydrogen bonding).
- 5. There are three intermolecular forces Let’ssee
- 6. Quizz Which of the following has the lowest boiling point?O2 F2 Cl2 Fill the blank below.Boiling point and freezing point of polar molecules are ….. than non polar molecules. Higher Lower Which of the following has the highest boiling point?HI CH4 H2O
- 7. For non polar molecules, only intermolecular force of attraction is London force London force stronger for larger molecules, weaker for smaller molecules Which of the following has the lowest boiling point? O2 F2 Cl2
- 8. Which of the following has the lowest boiling point? O2 F2 Cl2 Atomic size decreases across a row (left to right). F is smaller than O. F2 is smaller than O2 Atomic size increases going down a column. F is smaller than Cl. F2 smaller than Cl2
- 9. relative molecular mass >> london force >> Boiling point and freezing point increase >> Butane Pentane
- 10. For polarmolecules, not only intermolecular force of attraction is London force. There is dipole-dipole force. intermolecular force in polarmolecules is stronger than intermolecular force in non polar molecules. Boiling point and freezing point of polarmolecules is higher than non polar molecules.
- 11. Freezing point Boiling point relative molecular mass
- 12. Hydrogen bonding is much stronger than the van der Waals force. Energy to break the hydrogen bond is about 15-40 kJ / mol while for the van der Waals force of about 2-20 kJ / mol. That is why the substances that have a hydrogen bond has a higher freezing point, and boiling point
- 13. Higher boiling point is due to stronger intermolecular forces. Lower boiling point is due to weaker intermolecular force. Hydrogen bonding Dipole-dipole force London force A B C 1st 2nd 3rd Which one that have highest boiling point?
- 14. Hydrogen bonding Dipole-dipole force London force H2O HI CH4 1st 2nd 3rd