intermolecular forces p. 45 - grey college · 2020-04-03 · the intermolecular forces in hcl are...
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Intermolecular forces
p. 45
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Ion-induced Dipole forces
An ion that is close to an atom or molecule, canturn the electron cloudand cause a temporary
dipole
-
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Dipole-Dipole forcesSimilar to hydrogen forces,
but weaker dipoles.
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Dipole-induced Dipole forces
A dipole that is close to an atom or molecule, canturn the electron cloudand cause a temporary
dipole
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Induced dipole forces
(London forces) Temporary dipole.Very weak forces.
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Hydrogen bondsH bond with N, O, F
NH3, H2O, HF
Relatively strong bonds
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Metals Ionic crystal
structures
Molecules
• Metal bonds • Electrostatic
forces
• Hydrogen
bonds
• Van der Waals
forces(Dipole-dipole, Ion-
dipole and London
forces)
Cu Cu Cu Cu Cu Cu
Cu Cu Cu Cu Cu Cu
Cu Cu Cu Cu Cu Cu
Mg
O
Mg
O
Mg
O
Mg
O
Mg
O
Mg
O
H F
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HomeworkExercise 5p. 433, 8, 11
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3.1 Forces that prevent ice blocks to adopt the shape of the container?
3.2 Forces overcome when ice melts
3.3 Forces overcome when water evaporates?
3.4 Forces overcome when converting water into a gas state of hydrogen gas and oxygen gas.
3. Which type of force - between atoms or between molecules are involved in the following?
Intermolecular
Intermolecular
Intermolecular
Interatomic
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11. Arrange the following in order of increasing strength of intermolecular forces in the pure matter. Ne, CH4, CO and CCl4. Give a reason for your answer.
Ne - London (weak)
CH4 - London (weak)
CO - dipole-dipole (weak)
CCl4 - London (weak)
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3. Complete the following table.
Compound Intermolecular force Weak or strong
3.1 HBr
3.2 HF
3.3 SO2
3.4 CO2
3.5 H2O
Dipole-dipoleWeak
Hydrogen bonds Strong
Dipole-dipoleWeak
London forces Weak
Hydrogen bonds Strong
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4. Complete the following table.
Elements Type of interatomic bonds Formula
4.1Sodium and
chlorine
4.2Magnesium and
oxygen
4.3Hydrogen and
oxygen
4.4Carbon and
oxygen
4.5 Copper atoms
Ionic bondNaCl
Ionic bond MgO
Covalent bond H2O
Covalent bond CO2
Metal bond Cu
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4. Complete the following table.
Elements Type of interatomic bonds Formula
4.6 Carbon atoms
4.7Hydrogen and
fluorine
4.8One iron and one
oxygen atom
4.9Magnesium and
chlorine
4.10Calcium and
chlorine
Covalent bondC
Covalent bond HF
Ionic bond FeO
Ionic bond MgCl2
Ionic bond CaCl2
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Phases of molecules p 47Solid – strong forces
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Phases of molecules Solid - heated
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Phases of molecules Solid - melting
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Phases of molecules Liquid – start to flow
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Phases of molecules Gas – weak forces between particles
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Size of molecules
F Cl Br I
• More electrons• Stronger dipole• Stronger intermolecular forces(Size of molecule only influences Van der Waals forces)
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DensityDensity decreases when strength of intermolecular forces decreases
Water is an exception
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Boiling and melting pointsStronger intermolecular forces --> more energy is needed to overcome the intermolecular forces.Boiling and melting points increase.
Cl
H
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ViscosityViscosity is an indication of the fluidity of a substance(NB. it is not the fluidity of the substance!)
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Thermal expansionExpansion when material is heated.E.g. train tracks, thermometers...
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HomeworkExercise 6p. 595, 6, 8.1, 8.2, 13
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5.1
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5.2
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5.3
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6.1
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6.2
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8.1
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8.2
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13
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5. Choose from the following list the substance that best matches the description.
Br2, I2, F2, N2, O2, Cl25.1 Highest boiling point
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5. Choose from the following list the substance that best matches the description.
Br2, I2, F2, N2, O2, Cl25.2 Highest melting point
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5. Choose from the following list the substance that best matches the description.
Br2, I2, F2, N2, O2, Cl25.3 Greatest intermolecular force
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5. Choose from the following list the substance that best matches the description.
Br2, I2, F2, N2, O2, Cl25.4 Largest molecule
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5. Choose from the following list the substance that best matches the description.
Br2, I2, F2, N2, O2, Cl25.5 Arrange according to decreasing size of atom
I2, Br2, Cl2, F2, O2, N2
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5. Choose from the following list the substance that best matches the description.
Br2, I2, F2, N2, O2, Cl25.5 Arrange according to increasing strength of intermolecular forces
N2, O2, F2, Cl2, Br2, I2
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6. Consider the following substances.
Cu, S, NH3, NaBr6.1 Which of the substances is the best conductor of electricity at room temperature?
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6. Consider the following substances.
Cu, S, NH3, NaBr6.2 Which of the substances has the lowest boiling point?
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6. Consider the following substances.
Cu, S, NH3, NaBr6.3 Which of the substances has hydrogen bonds between molecules?
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7. Study the following graph showing the melting points of hydrogen halides.
7.1 Explain why HF has a higher melting point than HCl.
The intermolecular forces in HF are stronghydrogen bonds.The intermolecular forces in HCl are weak Van der Waals forces.Hydrogen bonds are stronger than Van der Waals forces. Therefore HF has a higher boiling point, because more energy is needed to break the intermolecular forces.
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7. Study the following graph showing the melting points of hydrogen halides.
7.2 Give a reason for the tendency of increasing melting points after HCℓ, moving down in the group.
The intermolecular forces in HCℓ, HBr and HI are Van der Waals forces which increase with increasing molar mass. The melting points increase with increasing strength in intermolecular forces. Stronger forces need more energy to be broken.