Term
| What is another name for Dipole-Dipole interaction? |
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Definition
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Term
| What is another name for Dipole-induced Dipole interaction? |
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Definition
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Term
| What is another name for Induced dipole-induced Dipole interaction? |
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Definition
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Term
| Describe Dipole-Dipole interactions |
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Definition
The strongest of the van der Waals forces; interaction is between permanent dipole molecules.
Raise boiling point.
Ex. Water, HCl, alcohol, and acetone |
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Term
| Describe Dipole-induced Dipole interactions |
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Definition
The interaction is between permanent dipole and temporary dipole molecules.
A polar molecule (e.g. HCl) can produce a temporary dipole in nonpolar molecules that are easily polarizable such as ethylacetate, methylene chloride, and ether. |
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Term
| Describe Induced dipole-induced Dipole interactions |
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Definition
The weakest of the van der Waals forces. The interaction is between temporary dipole molecules.
Temporary dipoles are formed by nonpolar molecules during transient electron cloud distortions. |
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Term
| Where do you see Dipole-induced Dipole interactions? |
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Definition
| They are involved with the solubility of some nonpolar compounds in ethanol, and propanolol. |
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Term
| Where do you see Induced dipole-induced Dipole interactions? |
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Definition
| These forces are responsible for the liquefaction of nonpolar gases (e.g. O2) and are present in phospholipid bilayers of cell membranes. |
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Term
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Definition
Hydrogen bonding is the attractive interaction of a hydrogen atom with an electronegative atom such as N, O or F.
These bonds can be intermolecular or intramolecular. |
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Term
| Why is the boiling point of water so high? |
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Definition
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Term
| List four intermolecular forces other than Hydrogen bonds or Van der Waal's |
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Definition
Ion-Ion e.g. Na+ and Cl- in water
Ion-Dipole e.g. Na+ and HCl
Ion-Charged surface e.g. packaging bottles used in pharmacy
Dipole-Charged surface e.g. packaging bottles used in pharmacy |
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Term
| Describe the ideal gas law |
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Definition
PV=nRT
P= pressure in atm
V=Volume in liters
n=Moles of gas
R=.0821
T=temperature in Kelvin (C+273) |
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Term
| In the ideal gas law, what else can n equal besides the moles of gas? |
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Definition
| Weight of gas/ molecular weight of gas |
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Term
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Definition
Ptotal = p1 + p2 +…+pn
p=partial pressure of gas=moles gas x pressure exerted by gas |
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Term
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Definition
Charged, ionized matter that is not solid, liquid, or gas
Ex. lightning, neon lights |
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Term
| Define "system" in terms of thermodynamics |
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Definition
| A part of the universe under consideration. |
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Term
| Define "surrounding" in terms of thermodynamics |
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Definition
| The entire universe except the system. A boundary separates the system from the surrounding. |
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Term
| What is the difference between an open and a closed system? |
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Definition
Open system: energy and matter can be exchanged with the surrounding.
Closed system: only energy can be exchanged with the surrounding |
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Term
| What is the difference between an isolated and a closed system? |
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Definition
In an isolated, neither energy nor matter can be exchanged with the surrounding
In closed, energy can be exchanged |
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Term
| What is the 1st law of thermodynamics? |
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Definition
| Energy can neither be created nor destroyed but only transferred from one form to the other |
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Term
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Definition
| A measure of the total energy of a system. It is also referred to as heat content |
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Term
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Definition
| The change of heat content in a reaction when 1 mole of a compound is formed from its elements in STP |
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Term
| What is ΔHf of an element in its standard state? (Ex. O2 is in its standard state) |
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Definition
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Term
| How do you solve for ΔHr (enthalpy/heat of reaction)? |
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Definition
| ΔHr = ΔHf (products) – ΔHf (reactants) |
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Term
| If the ΔHr of a reaction is positive, is it exothermic or endothermic? |
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Definition
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Term
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Definition
| The change in enthalpy (ΔH) of a reaction depends on the initial and final states of the system, and is independent of the number of steps or pathway required to complete the process. |
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Term
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Definition
| A factor that provides the quantitative description of randomness or disorder of the system. It is fundamental in predicting the spontaneity of chemical reactions. |
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Term
| What is the 2nd law of thermodynamics? |
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Definition
For any spontaneous process in an isolated system, there is an increase in entropy
ie, disorder increases |
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Term
| What is the 3rd law of thermodynamics? |
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Definition
The entropy of a pure crystalline substance is zero at absolute zero.
ie, at absolute zero there is no thermal energy or heat, and therefore the molecules do not move, and hence there is no disorder. A pure perfect crystal will have only one possible configuration. |
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Term
| Define Gibb's free energy (G) |
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Definition
| The potential which causes a chemical reaction to move forward under isothermal/isobaric conditions. As such, it is a criterion of spontaneity for processes with constant temperature and pressure. |
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Term
| If the ΔG of a reaction is negative, is the reaction spontaneous? |
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Definition
Yes, (-)ΔG=spontaneous
(+)ΔG=nonspontaneous |
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Term
| What are the equations to solve the change in free energy of solute associated with change in concentration? |
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Definition
ΔG = n RT x ln(a2/a1)
ΔG = 2.303n RTxlog(a2/a1) |
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Term
| Define heat of vaporization |
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Definition
The heat absorbed when 1g or 1mol of a liquid is vaporized
(This number will be higher if the liquid is less readily vaporized) |
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Term
| How is the vapor pressure and boiling point of a liquid related? |
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Definition
| They are inversely related |
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Term
| How is the vapor pressure and temperature of a liquid related? |
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Definition
| They are directly related |
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Term
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Definition
| The heat required to increase the molecular distance in the solid phase to form the liquid phase |
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Term
| What three states do solids exist in? |
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Definition
| Crystalline, amorphous, and polymeric |
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Term
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Definition
| The molecules or atoms are arranged in repetitious three-dimensional lattice structure. They have a definite geometric form with six common structures, and a definite boiling point |
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Term
| Define polymorphic and give an example |
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Definition
Having more than one crystalline structure
Cocoa butter |
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Term
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Definition
| A polymorphic solid that can reversibly change its crystal structure, usually a result of temperature or solvent changes in the system. |
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Term
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Definition
| A quality of a solid when a polymorphic form irreversibly converts to a different crystal |
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Term
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Definition
| The product when solvent becomes trapped in the crystal lattice of a solid (in a fixed molar ratio) |
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Term
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Definition
| A solvate when the solute is water |
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Term
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Definition
| Solids without definite order of arrangement of atoms or molecules. They have no definite m.p. as the temperature for transition to a liquid is a range of several degrees. |
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Term
| Give a drug example where amorphous and crystalline forms are used |
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Definition
| The amorphous form of insulin is used for rapid action, while the crystalline form is used for long action. |
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Term
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Definition
Large units of repeating molecules connected by covalent bonds, usually carbon based if drug related
Can help solubility of drugs |
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Term
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Definition
| The point where the melting point of two mixed solids is lower than the separate melting points |
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Term
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Definition
| A mixture of two solids that is liquid (due to lower m.p.) even though separate the solids would not have melted |
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