Term
| What are intramolecular forces? Give an example. |
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Definition
| Forces that occur between the individual atoms of a compound. For example, ionic and covalent bonding. |
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Term
| What are intermolecular forces? Name the three types. |
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Definition
| Forces that occur between molecules in a substance. The three types are: Dipole-Dipole, Hydrogen Bonds, and London (a.k.a. Dispersion, Van Der Waal) Forces. |
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Term
| What are Dipole-Dipole forces? |
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Definition
| A type of intermolecular force where molecules are attracted to other molecules opposite dipoles. |
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Term
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Definition
| A type of intermolecular force similar to dipole-dipole forces except it only takes place between Hydrogen and O, N, or F. |
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Term
| What does the strength of Dipole-Dipole forces depend upon? |
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Definition
| The distance between molecules. The greater the distance, the weaker the forces, so at low pressure and in the gas phase, these forces are relatively unimportant. |
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Term
| Why are Hydrogen Bonds so strong? |
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Definition
| These types of forces are so strong because they occur between such small, extremely electronegative molecules. |
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Term
| What is a characteristic of a molecule that is effected by hydrogen bonding? |
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Definition
| A compound being effected by this type of force will have a high boiling point. |
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Term
| What types of molecules experience London forces? |
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Definition
| All molecules experience these types of forces. |
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Term
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Definition
| The resistance of a liquid to an increase in its surface area. |
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Term
| What is capillary action? |
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Definition
| The spontaneous rising of a liquid in a narrow tube. |
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Term
| What are the two forces involved in capillary action? |
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Definition
| Cohesive and adhesive forces are responsible for this. |
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Term
| What are cohesive forces? |
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Definition
| the intermolecular forces among the molecules of their container. |
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Term
| What are adhesive forces? |
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Definition
| the forces between the liquid molecules and their container. |
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Term
| If a liquid's capillary action shows it 'creeping up the walls of it's container,' or it has a concave meniscus, what can we assume about it's adhesive and cohesive forces? |
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Definition
| In this case, we can assume that the liquid's adhesive forces towards it's container are stronger than it's cohesive forces to itself. |
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Term
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Definition
| A measure of a liquid's resistance to flow. |
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Term
| What factors affect a liquid's viscosity? |
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Definition
| The strength of intermolecular forces as well as the molecule's complexity affect it's ability to flow. |
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Term
| What type of intermolecular forces affect non polar molecules? |
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Definition
| ONLY London forces affect these types of molecules. |
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Term
| What shape (in relation to a liquid's surface tension), would be ideal and provide the smallest surface area? |
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Definition
| A sphere is the ideal shape for liquid's with high intermolecular forces. |
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Term
| What is a hydrophyillic surface? |
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Definition
| A surface which water tries to maximize surface contact. |
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Term
| What is a hydrophobic surface? |
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Definition
| A surface with which water tries to minimize surface contact. |
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Term
| What are ion-dipole interactions? |
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Definition
| When ions and polar molecules attach to one another. |
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Term
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Definition
| An instance of ion-dipole interactions where water molecules surround and bond to ions. |
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Term
| Which is stronger: Dipole-Dipole or Ion-Dipole interactions? |
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Definition
| Dipole-Dipole interactions are the stronger of these two forces. |
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Term
| What affects the number of water molecules that surround an ion? f |
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Definition
| Size and charge of the ion are factors in hydration. |
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Term
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Definition
| SOLUBILITY RULES (you can find this at the end of the 'IMF notes part 1' lecture) |
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Term
| In a class container, are polar molecules more likely to have strong or weak adhesive forces? |
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Definition
| In that type of container, polar molecules have strong adhesive forces. |
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Term
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Definition
| A solid which consists of ions. |
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Term
| What is a molecular solid? |
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Definition
| A solid that doesn't consist of ions. |
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Term
| What is the difference between ionic and molecular solids? |
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Definition
| Ionic solids conduct electricity when dissolved in water, while molecular solids do not. |
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Term
| What are atomic solids? Give an example. |
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Definition
| Substances with all atoms occupying the lattice points. For example: graphite, diamonds, silicon, all metals, and boron. |
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Term
| What determines the properties of a solid? |
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Definition
| They are determined by the nature of the forces that hold it together. |
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Term
| What are crystaline solids? |
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Definition
| Solids that have a generally repeating pattern. |
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Term
| What are some properties of crystalline solids? |
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Definition
| Are able to be cleaved, have constant intermolecular forces throughout, and sharp melting points are all properties of this type of solid. |
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Term
| What is an amorphous solid? |
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Definition
| Solids that have no uniform structure. |
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Term
| What are some properties of amorphous solids? |
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Definition
| varying intermolecular forces throughout, shatter or break into random lumps, broad melting points are all properties of this type of solid. |
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Term
| What are the four types of crystalline solids? |
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Definition
| Metallic, Ionic, Molecular, and Network are the four types of this type of solid. |
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Term
| What is the lattice unit for metals? |
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Definition
| The lattice unit for this type of solid is the 'electron sea' model. |
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Term
| What is the result of the 'electron sea' structure in metal solids? |
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Definition
| Metals are malleable, ductile, and good electric and thermal conductors as a result of this type of structure. |
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Term
| What is the lattice units for ionic solids? |
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Definition
| ions are the lattice units for this type of solid. |
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Term
| YOU SHOULD GET SOME HELP ON: |
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Definition
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Term
| What is the result of ions as the lattice structure of ionic solids? |
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Definition
| Poor thermal and electrical conductors (unless dissolved in water), high m.p. and b.p.s, hard and brittle are all results of this type of solid due to ions as the lattice unit. |
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Term
| What is the type of attraction between the lattice units in metallic solids? |
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Definition
| the electron 'sea' or bands is the type of attraction between the lattice units in this type of solid. |
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Term
| What is the type of attraction between the lattice units in ionic solids? |
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Definition
| Attraction of ions is the type of attraction between the lattice units in this type of solid. |
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Term
| What is the equation for lattice energy? |
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Definition
Lattice Energy= [k(Q1*Q2)]/r
Where:
r=distance between ions
k=constant for type of solid
Q1, Q2=charges on the ions |
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Term
| What does a higher lattice energy entail? |
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Definition
| Higher melting and boiling points are a result of this. |
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Term
| What are the lattice units in molecular solids? |
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Definition
| Molecules are the lattice units in this type of solid. |
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Term
| What type of attraction occurs between lattice units in molecular solids. |
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Definition
| London forces, dipole-dipole, and hydrogen bonding occur between the lattice units of molecular solids. |
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Term
| What is the result of the lattice structure of molecular solids? |
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Definition
| Softness, low melting and boiling points, poor electrical and thermal conductors, brittleness if pure are results of the lattice structure in this type of molecule. |
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Term
| What is important to remember about the properties of molecular solids? |
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Definition
| The properties of molecular solids vary from case to case and depend on the strength of each instance's intermolecular forces. |
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Term
| What are the lattice units of network solids? |
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Definition
| The lattice units in in this type of solid are atoms. |
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Term
| What type of attraction is present between the lattice units of network solids? |
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Definition
| covalent bonds are the attraction between lattice units in this type of solid. |
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Term
| What is the result of the lattice units in network solids? |
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Definition
| Poor thermal and electrical conductor, high m.p. and b.p., brittleness are the results of the lattice units in this type of solid. |
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Term
| What network solid is an exception to the general property of poor conductivity? |
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Definition
| Graphite is an exception to this network solid property. |
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