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52 Cards in this Set
- Front
- Back
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Which states are considered condensed states?
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solids and liquids because they are highly incompressible and their atoms/ions/molecules are closer together than in gases
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Which states are considered fluids?
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liquids and gases because they easily flow
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Intermolecular attraction is strong in...
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solids an dliquids
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If we compare the strengths of interactions among particles and the degree of ordering of particles, we see that...
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Gases<Liquids<Solids
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Define Ion-ion interactions (typically in ionic compounds)
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The force of attraction between two oppositely charged ions is governed by Coulomb’s law.
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Coulomb’s law determines _____________ and ____________
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The melting and boiling points of ionic compounds and the melting and boiling points of ionic compounds
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Define Dipole-dipole interactions
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Interaction of the positive end, δ+, of a polar molecule with the negative end, δ-, of another polar molecule
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Define Hydrogen bonding
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special type of dipole-dipole interaction which occurs among polar covalent molecules containing H bonded to one of the three small, highly electronegative elements – F, O, or N
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Define Dispersion Forces (van der Waals forces)
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They are the weakest of the intermolecular forces, is the only attractive force in nonpolar molecules, and exists in all substances
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Arrange the four types of intermolecular attractions by strength
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Ion-ion > hydrogen-bonding > dipole-dipole > dispersion forces
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Strength of _____________________ increases with increasing size of compound
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Dispersion forces
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Viscosity is....
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the resistance to flow
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Surface tension is.....
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a measure of the unequal attractions that occur at the surface of a liquid
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Evaporation is...
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the process in which molecules escape from the surface of a liquid and become a gas
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Vapor Pressure is...
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the pressure exerted by a liquid’s vapor on its surface at equilibrium
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Boiling Point is...
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the temperature at which the liquid’s vapor pressure is equal to the applied pressure
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Normal boiling point is...
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the boiling point when the pressure is exactly 1 atm
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Molar heat of vaporization or ΔHvap is...
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the amount of heat required to change 1.00 mole of a liquid to a gas at constant temperature
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What is the relationship between intermolecular force of attraction?
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Stronger intermolecular force of attraction higher molar heat of vaporization or ΔHvap
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Normal melting point is...
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the temperature at which the solid melts (liquid and solid in equilibrium) at exactly 1.00 atm of pressure
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The melting point ___________________ as the strength of the intermolecular attractions increases
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increases
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Molar heat of fusion or ΔHfusion is...
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is the amount of heat required to melt a mole of a substance at its melting point
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In the _____________________ the solid transforms directly to the vapor phase without passing through the liquid phase
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Sublimation process
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Amorphous solids do not have a well ordered ______________________
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molecular structure
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Crystalline solids have well defined structures that consist of extended array of repeating units called ________________
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unit cells
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What determines vapor pressure of a liquid at a new T, determines what T we must heat something to get a specified vapor pressure, way to determine ΔHvap if we know pressure at 2 T’s, and determine boiling points at different pressures
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Clausius-Clapeyron equation
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Dissolving medium is called the ____________.
Dissolved species are called the ____________. |
solvent
solute |
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Two major factors affect dissolution of solutes are
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Change of energy content or enthalpy of solution, ΔHsolution
If ΔHsolution is exothermic (< 0) dissolution is favored. If ΔHsolution is endothermic (> 0) dissolution is not favored. Change in disorder, or randomness, of the solution (ΔSmixing) large increase in disorder – dissolution is favored |
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The best conditions for dissolution are.....
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For the solution process to be exothermic
ΔHsolution < 0 For the solution to become more disordered |
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Solvent-solute attractions, ____________, releases energy
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solvation
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The crystal lattice energy is....
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a measure of the attractive forces in a solid
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Dissolution is a competition between....
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Solute -solute attractions
crystal lattice energy for ionic solids Solvent-solvent attractions H-bonding for water Solute-solvent attractions Solvation or hydration energy |
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In an _____________ dissolution, energy is released when solute particles are dissolved
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exothermic
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In an _____________ dissolution, energy is absorbed when solute particles are dissolved
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endothermic
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_____________________: solution which cannot dissolve additional amounts of the solute; point of maximum concentration; saturation point
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Saturated solutions
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__________________ solutions have higher-than-saturated concentrations of dissolved solutes.
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Supersaturated
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Possible stresses to chemical systems include:
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Heating or cooling the system
Changing the pressure of the system Changing the concentrations of reactants or products |
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For ionic solids that dissolve endothermically dissolution is ____________ by heating
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enhanced
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For ionic solids that dissolve exothermically dissolution is enhanced by __________
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cooling
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Pressure changes have ___________________ on solubility of liquids and solids in liquids
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little or no effect
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Pressure changes have _________ effects on the solubility of gases in liquids
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large
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The effect of pressure on the solubility of gases in liquids is described by _______________
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Henry's Law
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Colligative properties are properties of solutions that depend solely on the _______________________ dissolved in the solution
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number of particles
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four common types of colligative properties are....
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Vapor pressure lowering
Freezing point depression Boiling point elevation Osmotic pressure |
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______________________ is the study of the changes in energy and transfers of energy that accompany chemical and physical processes
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Thermodynamics
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The enthalpy change, ΔH, is the change in heat content at _____________________
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constant pressure
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If ΔHrxn < 0 the reaction is __________________
If ΔHrxn > 0 the reaction is __________________ |
exothermic
endothermic |
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________________ of Heat Summation states that the enthalpy change for a reaction is the same whether it occurs by one step or by any (hypothetical) series of steps
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Hess's Law
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____________________ is the amount of energy required to break the bond and separate the atoms in the gas phase
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Bond Energy
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The total amount of heat energy that a system can provide to its surroundings at constant temperature and pressure is given by
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ΔH= ΔE + P ΔV
ΔH = change in enthalpy of system ΔE = change in internal energy of system PΔV = work done by system |
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Spontaneity is favored when....
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heat is released during the change(exothermic) and when the change causes an increase in the dispersal of energy and matter (increase in entropy)
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Spontaneous processes have two requirements:
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The free energy change of the system must be negative
The entropy of universe must increase |
