Final Exam- 9,10,11,16 Flashcards
Solids with highly ordered structures are said to be ___________
Crystalline
Physical properties of liquids and solids are due to _____________ _______.
These are ______ between _______
Intermolecular forces
forces
molecules
_______ _______ reflect intermolecular force strength.
_______ _______ also reflect intermolecular fore strength.
A high ___ ___ or ___ ___ indicates strong attractive forces.
Boiling Point
Melting Point
Collectively _________ forces are intermolecular forces that exist between natural molecules
van-der-waals
Van der waals forces include
______
______
______
Dispersion forces
dipole-dipole forces
hydrogen forces
For an instant, the electron cloud become distorted. In that instant a dipole i formed.
it is called an ___________ or momentary _____.
Instantaneous or momentary dipole
One instantaneous dipole can induce another instantaneous dipole in an adjacent molecule (or atom). These two ________ ____ attract each other.
Temporary dipoles
___________ is the ease with which an electron distribution can be deformed
Polarizability
Dispersion force ______ as molecular weight ______.
Increases
Increases
The _____ _____ ____ reflects the dipole-dipole forces present.
Higher boiling point
Polar molecules _______ ____ ____
Attract each other
The partially _____ end of one molecule attracts the partially _____ end of another.
Positive
Negative
Polar molecular need to be ____ ______ to form strong ____- ___ interactions
close together
dipole-dipole
If two molecules have similar mass and size, then dipole- dipole forces ______ with ______ _______.
Increase with increasing polarity.
_______ _______ is a special type of ________ _______. This is a special case of dipole-dipole interactions.
Hydrogen bonding
intermolecular attraction
H bonding require:
H Bonded to a small _______ ______.
Most important for compounds of _, _, and _.
electronegative element
F, O, & N
Bond energies of Hydrogen bonds vary from about 4kj/mol to 25kj/mol. They are much _____ than ______ ______ _____.
weaker than ordinary chemical bonds
An interesting consequence of H-bonding is that for such a low molar mass molecule (Mm = 18g/mol) water has an unusually:
a)____ ____ _____
b)____ ____ of __________
c)water is a liquid under most circumstances
makes life possible.
d)water is a _____ _____
e) The solid has a ____ density than the liquid, causing the ice to ____.
a) High surface tension
b) High heat of vaporization (makes possible evaporative cooling)
d) Is a Superior Solvent
e) Lower density, causing Ice to float.
The molecules in solids are usually more closely packed than those in liquids.
Therefore, solids are usually denser than liquids.
But a few molecules have their solids less dense than their liquids, like
Ice to water.
An ___-___ force is an interaction between an ion (e.g., Na+) and the partial change on the end of a polar molecule/dipole (e.g. water)
Ion-dipoles
H-bonding is the _____ of the intermolecular forces while Dispersion Force is the _______.
Strongest
weakest
Ion-Dipole interaction are _____ than H-bonds
Stronger
Intermolecular attractive force will generally be ______ in the substance with the ______ ______ _____.
greater
higher molecular weight
_______ is the resistance of a liquid to flow.
Viscosity
Viscosity depends on…
the attractive forces between molecules
________ ______.
Bulk molecules (those in the liquid) are equally attracted to all of their neighbors.
Surface molecules are only attracted inward towards the bulk of the molecules.
Surface Tension
______ ____ is the rise of liquids up very narrow tubes. The liquid climbs until adhesive and cohesive forces are balanced by gravity.
Capillary Action
______ _____ are intermolecular fores that bind molecules to one another.
Cohesive Force
____ _____ are intermolecular forces that bind molecules to a surface.
Adhesive Force
An example of Capillary action is the _____ in a tube filled with water.
Meniscus
Matter in one state is converted into another state
Phase change or change of state
Sublimation
Solid –> Gas
Melting or Fusion
Solid –>Liquid
Vaporization
Liquid –> Gas
Deposition
Gas –> Solid
Condensation
Gas –> Liquid
Freezing
Liquid –> Solid
Is any substance at a temperature and pressure above its critical point, where distinct liquid and gas phases do not exist.
Supercritical Fluid
when a liquid is cooled below its freezing point and its still remains a Liquid
Supercooling
ex: Glass
https://upload.wikimedia.org/wikipedia/commons/thumb/3/34/Phase-diag2.svg/300px-Phase-diag2.svg.png
https://upload.wikimedia.org/wikipedia/commons/thumb/3/34/Phase-diag2.svg/300px-Phase-diag2.svg.png
Plot of temperature change versus heat added is a _____ ____
Heating Curve
_______ _______ is the highest temperature at which a substance can exist as a liquid
Critical Temperature
_______ _______ is the pressure required for liquefaction at this critical temperature.
Critical Pressure
Supercritical fluid extraction is used to ______ ______ ______
Separate Complex Mixtures
Some of the molecules on the surface of a liquid have enough energy to….
escape the attraction of a bulk liquid.
_______ _____ of a liquid is the pressure exerted by its vapor when the liquid and vapor are in dynamic equilibrium.
Vapor Pressure
Liquids that evaporate easily are said to be ______.
Volatile
The _____ _____ of a liquid is the temperature at which the external pressure at the liquid surface equals the vapor pressure
Boiling Point
A ______ ______ is a plot of pressure vs temperature summarizing all equilibria between phases
Phase Diagram
Vapor-pressure curve
As temperature increases, vapor pressure increases.
Critical Point
critical temperature and pressure for the gas
Sublimation curve
Separates the solid and gas phases
Melting Curve
Separates the Solid and Liquid phases
Normal melting Point
1 atm
Triple Point
temperature and pressure at which all three phases are in equilibrium
Any temperature and pressure combination not on a curve represents a ______ _____
Single Phase
_______ _____Held together by delocalied “sea” of shared valence electrons
Metallic solids
______ _____Held together by mutual attraction between cations and anions.
Tend to be _____
_____ melting & boiling points
Ionic Solids
Brittle
High
______ _____Held together by relatively weak intermolecular forces
Tend to be ____
_____ melting & boiling points
Molecular Solids
Soft
Low
______ _____Have atoms and ions arranged in an orderly repeating pattern.
Crystalline Solids
ex: NaCl, quartz, Diamonds
_____ _____Lack the order of crystalline solids
Amorphous Solids
ex: Rubber, Glass
A ________ is a homogeneous mixture of solute and solvent.
Solution
Each substance present is a ________ of the solution
Component
The ______ is the component present in the largest amount
Solvent
The mixing of gases is a ___________ process
Spontaneous
________ is the thermodynamic quantity that measures the extent of the spreading of the molecules and their associated kinetic energies.
Entropy
_____ _____ of intermolecular interactions are involved in solution formation
Three kinds
______ _____ interactions between solute particles
Must be overcome in order to disperse the particles through the solvent.
Solute-solute
______ _____ interactions between solvent particles
Must be overcome to make room for the solute particle in the solvent
Solvent-solvent
______ _____ interactions between solvent and solute particles. Occur as particles mix
Solvent-solute
The opposite process of a solution is _________
Crystallization
If crystallization and dissolution are in equilibrium with undissolved solute, the solution is ______.
Saturated
_______ is the amount of the solute required to form a saturated solution.
Solubility
A solution is said to be _____________ if more solute is dissolve than in a saturated solution.
Supersaturated
The tendency of a substance to dissolve in another depends on: \_\_\_\_\_\_\_\_ \_\_\_\_\_\_\_\_ \_\_\_\_\_\_\_\_ \_\_\_\_\_\_\_\_
The nature of the Solute
& Solvent
The temperature
The Pressure (for gases)
Pairs of liquids that mix in any proportions are said to be ______
Miscible
In contrast, ________ liquids do not mix significantly
Immiscible
ex: Gas & water
____________: like dissolve like
Generalization
The solubility of most solids solutes in water ________ as the solution temperature increase
increases
The solubility of gas in water with increasing temperature
decreases
________ _______If lakes get to warm, CO2 and O2 become less soluble and are not available for plants or animals.
Thermal pollution
The terms _____ and _________ are qualitative ways to concentration.
Dilute
Concentrated
A _____ solution has relatively small concentration of solute
Dilute
A _________ solution has a relatively high concentration of solute
Concentrated
The most commonly used expressions for concentration are: \_\_\_\_\_\_\_\_\_ \_\_\_\_\_\_\_\_ \_\_\_\_\_\_\_\_ \_\_\_\_\_\_\_\_
Mass percentage (mass%)
Mole fraction (X)
Molarity (M)
Molality (m)
Acids taste ____ and cause certain dyes to change color
Sour
Bases taste _____ and feel soapy.
Bitter
In water, cluster of hydrated H+(aq) ions form.
the simplest cluster is ____, we call this a ___________ ___
H3O+
Hydronium Ion
In bronsted-Lowry, Acids ______ H+
& Bases _____ H+
Donates
Accepts
An _________ substance can behave either as an acid or as a base
Amphiprotic
whatever is left of the acid after the proton is donated is called its __________ base
Conjugate
X- is called the _________ base
Conjugate
Do strong or weak acids completely transfer their protons to water
Strong
Do strong or weak acids only partially dissociate in aqueous solution
weak
Substances with __________ acidity do not transfer a proton to water
Negligible
In pure water the following equilibrium is established, this process is called
Autoionization
__ is called the ion-product constant
Kw
Most ph levels fall between “#” & “#”
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