Chapter 11 – Intermolecular Forces, Liquids, and Solids Which factor(s) affect the physical properties of a substance? Why does water boil at 100°C and freeze at 0°C? Why does high pressure and low temperature solidify most gasses? Why can’t hydrogen be solidified? In this unit we will look at the factors that affect the physical properties of liquids and solids.

Intermolecular Forces, Liquids, and Solids Intermolecular Forces – Forces of attraction between 2 or more other molecules in a substance.

Intermolecular Forces, Liquids, and Solids Intermolecular Forces – 3 types: London Dispersion Forces (weakest), Dipole-Dipole, and Hydrogen Bonding (strongest).

Intermolecular Forces, Liquids, and Solids Intermolecular Forces – London Dispersion Forces: Weak forces of attractions caused by the attraction between the protons in one molecules and the electrons in another molecule.

Intermolecular Forces, Liquids, and Solids Intermolecular Forces o London Dispersion Forces: Generally, substances that only have LDF’s have low melting and vaporization points. But substances with higher molecular weights can have so many LDF’s that they will have high melting and vaporization points.

Intermolecular Forces, Liquids, and Solids Intermolecular Forces o London Dispersion Forces: HalogenMolecular Weight (amu) Boiling Point (K) F2F Cl Br I2I

Intermolecular Forces, Liquids, and Solids Intermolecular Forces o London Dispersion Forces: Noble GasMolecular Weight (amu) Boiling Point (K) He Ne Ar Kr

Intermolecular Forces, Liquids, and Solids Intermolecular Forces o Dipole - Dipole Forces: Weak forces of attractions caused by the attraction between the oppositely charged poles of two or more molecules.

Intermolecular Forces, Liquids, and Solids Intermolecular Forces o Dipole - Dipole Forces: Therefore, dipole-dipole interactions only develop within polar substances.

Intermolecular Forces, Liquids, and Solids Intermolecular Forces o Hydrogen Bonding: Forces of attractions between a hydrogen atom of one molecule and a fluorine, oxygen, or nitrogen, of another molecule.

Intermolecular Forces, Liquids, and Solids Intermolecular Forces o Hydrogen Bonding: Ammonia’s trigonal pyramidal shape allows the hydrogen atoms of one molecule to be attracted to the nitrogen on another.

Intermolecular Forces, Liquids, and Solids Intermolecular Forces o Hydrogen Bonding:

Intermolecular Forces, Liquids, and Solids Intermolecular Forces o Hydrogen Bonding: o Ice is less dense than liquid water due to hydrogen bonding. o When H-Bonding is maximized in the formation of ice, large open spaces are created.

Intermolecular Forces, Liquids, and Solids Intermolecular Forces Interacting Molecules or ion Polar Molecules? Ions Present? Polar Molecules and Ions Present? LDF’s Diplole H-Bonding Ion-Dipole Ionic Bonding Dipole Weakest IMF’s > Strongest IMF’s

Intermolecular Forces, Liquids, and Solids Properties of Liquids o Viscosity – The measure of the resistance of a liquid to flow.

Intermolecular Forces, Liquids, and Solids Properties of Liquids o Viscosity – Affect by temperature and molecular weight.  Temperature – IMF’s are overcome with higher temperature.  Molecular Weight – The larger the molecule, the more ‘tangled’ it becomes, thus resisting flow.

Intermolecular Forces, Liquids, and Solids Properties of Liquids o Surface Tension – A measure of the inward forces that must be exerted to overcome to expand the surface of a liquid.

Intermolecular Forces, Liquids, and Solids Properties of Liquids o Surface Tension – Cohesive vs Adhesive Forces  Cohesive Forces – Forces among molecules in a liquid due to IMF’s.  Adhesive Forces – Forces between the molecules of a substance and the surface of a material.

Intermolecular Forces, Liquids, and Solids Phase Changes

Intermolecular Forces, Liquids, and Solids Phase Changes o Heat of Fusion (ΔH fus ): The amount of energy to melt 1 mole of a substance. o What patter do you see in the heat of fusion of these substances? ΔH fus H2O = 6.01 kJ / mol ΔH fus C4H10 = 5.00 kJ / mol ΔH fus Hg = 23.0 kJ / mol

Intermolecular Forces, Liquids, and Solids Phase Changes o Heat of Vaporization (ΔH vap ): The amount of energy to vaporize 1 mole of a substance. o What pattern do you see in the heat of vaporization of these substances? ΔH vap H2O = 40.7 kJ / mol ΔH vap C4H10 = 24.0 kJ / mol ΔH vap Hg = 58.0 kJ / mol

Intermolecular Forces, Liquids, and Solids Heating curves and Cooling Curves

Intermolecular Forces, Liquids, and Solids Heating curves and Cooling Curves

Intermolecular Forces, Liquids, and Solids Heating curves and Cooling Curves

Intermolecular Forces, Liquids, and Solids Cooling Curve for Solutions

Intermolecular Forces, Liquids, and Solids Phase Diagrams Phase Diagrams for Carbon Dioxide

Intermolecular Forces, Liquids, and Solids Phase Diagrams

Intermolecular Forces, Liquids, and Solids Phase Diagrams Triple Point – The combination of temperature and pressure that a substance exists as a solid, liquid, and a gas at the same time. Critical point – The maximum temperature by which a substance can not longer be liquified

Intermolecular Forces, Liquids, and Solids Vapor Pressure The pressure exerted by the gas above a liquid once dynamic equilibrium has been established between the liquid molecules and gas molecules.

Intermolecular Forces, Liquids, and Solids Vapor Pressure Dynamic Equilibrium – The rate of evaporation equals the rate of condensation.

Intermolecular Forces, Liquids, and Solids Vapor Pressure vs Intermolecular Forces The stronger the IMF’s, the more difficult it is for a molecule to escape to the gas phase. Therefore its vapor pressure will be lower. The weaker the IMF’s, the higher the vapor pressure.

Intermolecular Forces, Liquids, and Solids Vapor Pressure

Intermolecular Forces, Liquids, and Solids Solids Amorphous Solids: Solids that lack any molecular organization.

Intermolecular Forces, Liquids, and Solids Solids Crystalline Solids: – Solids that have a high degree of molecular organization. – Crystals are three-dimensional shapes that have flat surfaces and angled corners.

Intermolecular Forces, Liquids, and Solids Solids Crystalline Solids: Geodes

Intermolecular Forces, Liquids, and Solids Solids Crystalline Solids: – Unit Cells: The repeating three-dimensional shape of a crystalline solid. – Crystal Lattice: Many unit cells making an overall crystal.

Intermolecular Forces, Liquids, and Solids Solids Crystalline Solids: – All ionic compounds can be explained with 7 different types of unit cells. – We will take a close look at 3 common types; primitive cubic, body-centered cubic, and face-centered cubic.

Intermolecular Forces, Liquids, and Solids Crystalline Solids Primitive Cubic

Intermolecular Forces, Liquids, and Solids Crystalline Solids Body-Centered Cubic

Intermolecular Forces, Liquids, and Solids Crystalline Solids

Intermolecular Forces, Liquids, and Solids Crystalline Solids  Close Packing Spheres

Intermolecular Forces, Liquids, and Solids Crystalline Solids  Coordination Number – The number of particles that surround one specific particle in solid.

Intermolecular Forces, Liquids, and Solids Crystalline Solids  Coordination Number – What is the coordination numbers for the following examples?

Intermolecular Forces, Liquids, and Solids Crystalline Solids  Hollow Spheres  Rice University (1985): A 60-Carbon hollow ball of carbon is discovered.

Intermolecular Forces, Liquids, and Solids Crystalline Solids  Hollow Spheres  These structures were called buckminsterfullerenes or ‘buckyballs’.  Buckminster Fuller: Architect who created geodome shapes.

Intermolecular Forces, Liquids, and Solids Crystalline Solids  Hollow Spheres  These structures were called ‘buckyballs’.  Buckminster Fuller: Architect who created geodome shapes.

Intermolecular Forces, Liquids, and Solids Crystalline Solids  Hollow Spheres  Buckyballs are found in nature and even been identified in deep outer space in clouds surrounding stars.

Intermolecular Forces, Liquids, and Solids Crystalline Solids  Hollow Spheres  Buckyballs have potential uses in medicine, lubricants, and computers.

Intermolecular Forces, Liquids, and Solids Crystalline Solids  Buckminsterfullerenes  Nanotubes

Intermolecular Forces, Liquids, and Solids Covalent Network Solids  Molecular substances in which all of the atoms are connected by a network of covalent bonds.

Intermolecular Forces, Liquids, and Solids Covalent Network Solids  Diamonds versus graphite

Intermolecular Forces, Liquids, and Solids Summary of Crystalline solids Type of SolidParticlesForcesPropertiesExamples MolecularAtoms or Molecules LDF, dipole- dipole, H- Bonding Soft, low melting points Ar, CH 4, CO 2, ice Covalent Network Atoms connected by covalent bonds Covalent BondsVery hard, very high metltng points Diamonds, quartz, graphite, glass (SiO 2 ) IonicCations and anions Electrostatic Interactions Hard, brittle, high melting points NaCl, Ca(NO 3 ) 2 MetallicatomsMetallic BondsSoft or hard, low or high melting points Cu, Fe, Al